Chapter 11

The substance diethylamine is a weak nitrogenous base like ammonia. Write a net ionic equation to show how diethylamine, (C2H5)2NH, behaves as a base in water.

(C2H5)2NH (aq) + H2O (l)----->____> (C2H5)2NH2+ (aq) + OH- (aq)

An ion from a given element has 55 protons and 54 electrons

+1 cesium

What is the Ka of a particular acid if a 4.70×10-2 M aqueous solution of it has a pH of 3.14?

1.12×10-5

An ion from a given element has 20 protons and 18 electrons

+2 calcium

An ion from a given element has 27 protons and 25 electrons

+2 cobalt

An ion from a given element has 29 protons and 27 electrons

+2 copper

An ion from a given element has 25 protons and 23 electrons

+2 manganese

An ion from a given element has 38 protons and 36 electrons

+2 strontium

An ion from a given element has 13 protons and 10 electrons

+3 aluminum

An ion from a given element has 24 protons and 21 electrons

+3 chromium

An aqueous solution has a hydroxide ion concentration of 1.0×10-13 M (10-13 M) (1) What is the hydronium ion concentration in this solution? (2) What is the pH of this solution? (3) What is the pOH of this solution?

0.10 M 1 13

How many equivalents are contained in 0.25 moles of H2SO4?

0.50

Strontium-90 has a half-life of 28.1 years. Starting with 4.00 mg of this isotope, how much would remain after 84.3 years?

0.500 mg

How many 4s orbitals are there in an atom?

1

How many orbitals are there in the shell with n = 1 in an atom?

1

How many types of orbitals are there in the shell with n = 1 in an atom?

1

The element iodine would be expected to form

1

An aqueous solution has a pOH of 13 (1) What is the pH of this solution? (2) What is the hydronium ion concentration in this solution? (3) What is the hydroxide ion concentration in this solution?

1 10- 1 M 10 -13 M

An aqueous solution has a pOH of 13 (1) What is the pH of this solution? (2) What is the hydronium ion concentration in this solution? (3) What is the hydroxide ion concentration in this solution?

1 10- 1 M 10 -13 M

How many 5s orbitals are there in an atom? What is the maximum number of electrons possible in a set of 5s orbitals?

1 2

The element fluorine would be expected to form

1 covalent bond

What is the pH of 0.70 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13.

1.14

What is the pH of 0.66 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 3.6 x 10-13.

1.15

The hydronium ion concentration in an aqueous solution at 25°C is 9.5×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

1.1×10-13 M 1.02 12.98

The hydroxide ion concentration in an aqueous solution at 25°C is 8.8×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

1.1×10-13 M 12.94 1.06

The hydroxide ion concentration in an aqueous solution at 25°C is 9.5×10-2 M. The hydronium ion concentration is The pH of this solution is The pOH is

1.1×10-13 M 12.98 1.02

What is the pH of 0.37 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13.

1.28

A 0.58 M solution of an unknown amine base is found to be 1.8% ionized at equilibrium. Calculate the value for Kb for this amine.

1.8E-4

The hydronium ion concentration in an aqueous solution at 25°C is 5.6×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

1.8×10-13 M 1.25 12.75

The hydroxide ion concentration in an aqueous solution at 25°C is 5.5×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

1.8×10-13 M 12.74 1.26

The pH of a 0.353 M solution of the conjugate base, A-, of a weak acid, HA, is 10.40. What is the Kb for A-?

1.8×10-7

Sodium-24 has a half-life of 15 hours. Calculate the number of mg of an initial 48-mg sample that remains after one day and 10 hours

10 mg

An aqueous solution has a pOH of 3 . (1) What is the pH of this solution? (2) What is the hydronium ion concentration in this solution? (3) What is the hydroxide ion concentration in this solution?

11 10- 11 M 10 -3 M

Calculate the pH of a 0.033 M solution of trimethylamine (Kb = 7.4 x 10-5).

11.20

Calculate the pH of a 0.049 M solution of trimethylamine (Kb = 7.4 x 10-5).

11.28

Calculate how long will it take for a sample of a radionuclide with a half-life of 25.3 days decay to 1.0% of its original value.

168 days

What is the complete ground state electron configuration for the sulfur atom? What is the complete ground state electron configuration for the zinc atom?

1s22s22p63s23p4 1s22s22p63s23p64s23d10

The element oxygen would be expected to form

2

The radioactive isotope decays by beta emission. If the mass of a sample of thallium-209 decays from 62.4 micrograms to 15.6 micrograms in 4.40 minutes, what is the half-life of thallium-209?

2.20 minutes

The radioactive isotope carbon-14 is used for radiocarbon dating. The half-life of carbon-14 is 5.730×103 years. A wooden artifact in a museum has a 14C count that is 6.25×10-2 times that found in living organisms. Estimate the age of the artifact.

2.29×104 yrs

The hydroxide ion concentration in an aqueous solution at 25°C is 4.6×10-2 M. The hydronium ion concentration is The pH of this solution is The pOH is

2.2×10-13 M 12.66 1.34

The pH of a 0.289 M solution of the conjugate base, A-, of a weak acid, HA, is 11.40. What is the Kb for A-?

2.2×10-5

The pH of a 0.395 M solution of the conjugate base, A-, of a weak acid, HA, is 11.00. What is the Kb for A-?

2.5×10-6

Nitrogen-13 is used in tracers injected into the bloodstream for positron emission tomography (PET). The half-life of nitrogen-13 is 10.0 minutes. If you begin with 83.5 milligrams of nitrogen-13, how many milligrams will you have left after 50.0 minutes have passed?

2.61 mg

What is the pH of 7.7 × 10-3 M HF? The Ka for hydrofluoric acid is 7.2 × 10-4.

2.69

Fill in the nuclide symbol for the missing particle in the following nuclear equation The mass number of the reactant is 210 + 4 = 214 The atomic number of the reactant is 82 + 2 = 84. The element with atomic number 84 is polonium

214 Po 84

Write a balanced nuclear equation for the alpha decay of polonium-218

218Po84 --> 4He2 + 214Pb82

Fill in the nuclide symbol for the missing particle in the following nuclear equation.

226 Ra 88----> 4 He 2 + 222 Rn 86

The following Lewis diagram represents the valence electron configuration of a main-group element. X=2

2A cation charge of +2 If X is in period 4 , the ion formed has the same electron configuration as the noble gas: calcium Ca2+

The radioactive isotope Po decays by alpha emission. If the mass of a sample of polonium-218 decays from 52.7 micrograms to 13.2 micrograms in 6.10 minutes, what is the half-life of polonium-218?

3.05 minutes

Calculate the pH of a solution prepared by mixing 10.0 mL of 0.010 M HCl with 125.0 mL of 0.10 M HCN. For HCN, Ka = 1.0 × 10-10. Assume that the volumes are additive.

3.13

Gallium-67 is used medically in tumor-seeking agents. The half-life of gallium-67 is 78.2 hours. How many milligrams of a 52.7 milligram sample of gallium-67 will be lost by radioactive decay during 156.4 hours?

39.5 mg

To determine the number of equivalents of Al(NO3)3 in a 0.750 M solution, the conversion factor would be which of the following?

3eqAl(NO3)3/1 mole Al(NO3)3

How many orbitals are there in the shell with n = 2 in an atom?

4

The hydroxide ion concentration in an aqueous solution at 25°C is 2.5×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

4.0×10-13 M 12.40 1.60

The radioactive isotope decays by beta emission. If the mass of a sample of thallium-206 decays from 58.5 micrograms to 29.3 micrograms in 4.19 minutes, what is the half-life of thallium-206?

4.19 minutes

The hydronium ion concentration in an aqueous solution at 25°C is 2.3×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

4.3×10-13 M 1.64 12.36

The hydroxide ion concentration in an aqueous solution at 25°C is 2.2×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

4.5×10-13 M 12.34 1.66

The pH of a 0.419 M solution of the conjugate base, A-, of a weak acid, HA, is 11.14. What is the Kb for A-?

4.6E-6

What is the pKa of an acid with a Ka of 1.82 × 10−5?

4.74

Predict which of the following nuclides is most likely to be a stable nucleus

40 Ca 20

The hydronium ion concentration in an aqueous solution at 25°C is 1.9×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

5.3×10-13 M 1.72 12.28

The hydronium ion concentration in an aqueous solution at 25°C is 1.7×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

5.9×10-13 M 1.77 12.23

Fill in the symbol for the missing particle in the following nuclear equation.

56 Cr 24 ----> 0 e -1 + 56 Mn 25

The following Lewis diagram represents the valence electron configuration of a main-group element. X=6

6A anion -2 If X is in period 2 , the ion formed has the same electron configuration as the noble gas: oxygen O2-

Sodium-24 has a half-life of 15 hours. Calculate the number of mg of an initial 30-mg sample that remains after one day and 11 hours

6mg

Calculate the pH at the equivalence point when 20.0 mL of 0.450 M HCl is titrated with 20.0 mL of 0.450 M NaOH.

7

How many 4f orbitals are there in an atom? What is the maximum number of electrons possible in a set of 4f orbitals?

7 14

How many 5f orbitals are there in an atom? What is the maximum number of electrons possible in a set of 5f orbitals?

7 14

How much of a fissionable material is required to have a self-sustaining reaction?

A critical mass of fissionable material is required and varies depending on the identity of the fissionable material

Choose the species that can act as a Lewis acid. a. Fe3+ b. CCl4 c. NH3 d. CH3CH2NH2

A. Fe3+

The acid with the smallest pKa:

Acetic 1.8x10-5

Which salt shifts the pH when dissolved in water?

Al(NO3)3

Write a net ionic equation to show that hydrosulfuric acid, H2S, behaves as an acid in water. Consider only its first ionization. Classify hydrosulfuric acid as a monoprotic, diprotic or triprotic acid.

An acid forms the hydronium ion in water. In this case, H2S donates a proton to H2O to form HS- and H3O+. H2S (aq) + H2O (l)____>------>HS- (aq) + H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion. H2S is a diprotic acid because it has 2 ionizable protons. This is indicated by the two H atoms at the beginning of its formula. All sulfuric acids, including Hydrosulfuric acid, are diprotic acids.

The stronger acid is AH2CO3 4.2×10-7 BH3PO4 7.5×10-3

B

Which of the following buffers will have the lowest pH? A. a solution containing 0.15 M HC2H3O2 and 0.25 M NaC2H3O2 B. a solution containing 0.25 M HC2H3O2 and 0.15 M NaC2H3O2 C. a solution containing 0.20 M HC2H3O2 and 0.20 M NaC2H3O2 D. They all have the same pH.

B

What is the formula of the compound in which the atom combining ratios are: boron : hydrogen : chlorine = 4 : 9 : 1

B4H9Cl

What is the formula of the compound in which the atom combining ratios are: boron : hydrogen : chlorine = 5 : 8 : 1

B5H8Cl

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: C (s) + O2 (g) CO2 (g)

C (s) + O2 (g) CO2 (g)

Which is the explanation for the difference between the two isotopes of carbon, C-12 and C-14?

C-14 contains 2 more neutrons than does C-12

hich of the following chemical equations is a net ionic equation for the reaction between aqueous HCl and a weak base? H3O+(aq) + OH-(aq) 2 H2O(l) HCl(g) + NH3NH4Cl(aq) H3O+(aq) + F-(aq) HF(aq) + H2O(l) 2 HCl(aq) + Sr(OH)2(aq)SrCl2(aq) + 2 H2O(l) HCl(aq) + NaF(aq) NaCl(aq) + HF(aq)

C. H3O+(aq) + F-(aq) HF(aq) + H2O(l)

Which of the following chemical equations is a net ionic equation for the reaction between aqueous HCl and a weak base? A. H3O+(aq) + OH-(aq) → 2 H2O(l) B. HCl(g) + NH3 → NH4Cl(aq) C. H3O+(aq) + F-(aq) → HF(aq) + H2O(l) D. 2 HCl(aq) + Sr(OH)2(aq) → SrCl2(aq) + 2 H2O(l) E. HCl(aq) + NaF(aq) → NaCl(aq) + HF(aq)

C. H3O+(aq) + F-(aq) → HF(aq) + H2O(l)

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: C3H8 (g) + O2 (g) CO2 (g) + H2O (g)

C3H8 (g) + 5O2 (g) 3CO2 (g) + 4H2O (g)

Write a balanced chemical equation for the reaction of copper(II) carbonate with hydrochloric acid.

CuCO3(s) + 2 HCl(aq) → CuCl2(aq) + H2O(l) + CO2(g)

A solution is prepared by dissolving 4.66 g of KCl in enough distilled water to give 250 mL of solution. KCl is a strong electrolyte. How will the freezing point of the solution be different from that of pure water? (Note: Kf for water is 1.86°C/M.) a. Solution will be 0.930°C higher than pure water. b. Solution will be 0.475°C higher than pure water. c. Solution will be 0.475°C lower than pure water. d. Solution will be 0.930°C lower than water.

D

Which of the following buffers will have the lowest pH? A. a solution containing 0.20 M HC2H3O2 and 0.20 M NaC2H3O2 B. a solution containing 0.10 M HC2H3O2 and 0.10 M NaC2H3O2 C. a solution containing 0.30 M HC2H3O2 and 0.30 M NaC2H3O2 D. They all have the same pH.

D. all

Which of the following affects the half-life of a radioactive sample? A. the size of the sample B. the temperature of the sample C. the age of sample D. none of these

D. none of these

Write the net ionic equation for the reaction that occurs when 0.107 mol HBr is added to 1.00 L of the buffer solution.

F- + H3O+ HF + H2O

Write the net ionic equation for the equilibrium that is established when calcium fluoride is dissolved in water

F-(aq) + H2O HF(aq) + OH -(aq) BASIC

Write the net ionic equation for the equilibrium that is established when barium fluoride is dissolved in water

F-(aq) + H2O HF(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when potassium fluoride is dissolved in water

F-(aq) + H2O HF(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when potassium fluoride is dissolved in water.

F-(aq) + H2O HF(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when sodium fluoride is dissolved in water

F-(aq) + H2O HF(aq) + OH -(aq) basic

Which of the following reaction is a Bronsted-Lowry acid-base reaction?

F-(aq) + H2O(l) HF(aq) + OH-(aq)

Which of these is a strong acid? nitric acid citric acid oxalic acid sodium hydroxide phosphoric acid

Nitric

When solid sodium hydroxide is dissolved in water which of the following species is not present in the solution?

None, because H2O, OH-, Na+ are all PRESENT

The decay of Pb to Bi occurs through the emission of

a positron

HCN

is a weak acid

CH3OH (l) CH3OH(aq)

non

Which of the following is not a nuclear reaction?

redox

The substance dimethylamine is a weak nitrogenous base like ammonia. Write a net ionic equation to show how dimethylamine, (CH3)2NH, behaves as a base in water.

(CH3)2NH (aq) + H2O (l) = (CH3)2NH2+ (aq) + OH- (aq) The double arrow in the equation indicates that the reaction does not go to completion.

An ion from a given element has 29 protons and 28 electrons

+1 copper

An ion from a given element has 19 protons and 18 electrons

+1 potassium

An ion from a given element has 37 protons and 36 electrons

+1 rubidium

An ion from a given element has 11 protons and 10 electrons

+1 sodium

An ion from a given element has 30 protons and 28 electrons

+2 zinc

An ion from a given element has 26 protons and 23 electrons

+3 iron

An ion from a given element has 9 protons and 10 electrons. What is the charge on the ion? What is the name of the element?

-1 F

An ion from a given element has 9 protons and 10 electrons

-1 fluorine

An ion from a given element has 53 protons and 54 electrons

-1 iodine

An ion from a given element has 8 protons and 10 electrons

-2 oxygen

An ion from a given element has 34 protons and 36 electrons

-2 selenium

An ion from a given element has 7 protons and 10 electrons

-3 nitrogen

An ion from a given element has 15 protons and 18 electrons

-3 phosphorus

What is the pH of 3.8 × 10-4 M HF? The Ka for hydrofluoric acid is 7.2 × 10-4.

...3.56

Which of the following aqueous solutions are buffer solutions?

0.25 M NH4NO3 + 0.33 M NH3 0.32 M HNO2 + 0.30 M NaNO2 0.18 M CH3COOH + 0.10 M CH3CO 0.35 M NH4NO3 + 0.35 M NH3 0.14 M HCN + 0.17 M KCN 0.13 M HNO2 + 0.20 M KNO2 0.32 M CH3COOH + 0.29 M CH3COOK 0.34 M HF + 0.22 M KF 0.29 M NH4NO3 + 0.33 M NH3 0.19 M CH3COOH + 0.15 M CH3COO 0.18 M HNO2 + 0.14 M KNO2 0.33 M KBr + 0.24 M KNO3 0.18 M HF + 0.18 M KF 0.38 M HCN + 0.23 M NaCN 0.29 M NH4Br + 0.35 M NH3 0.14 M CH3COOH + 0.19 M CH3COO 0.34 M HCN + 0.28 M NaCN 0.31 M NH4Br + 0.38 M NH3 0.22 M HCN + 0.14 M KCN 0.22 M HCN + 0.11 M NaCN 0.32 M HClO + 0.26 M KClO 0.33 M CH3COOH + 0.22 M CH3COOK 0.21 M HCN + 0.11 M NaCN 0.26 M NH4Br + 0.33 M NH3 0.29 M NH4Br + 0.37 M NH3 0.15 M HClO + 0.15 M NaClO 0.36 M HClO + 0.26 M NaClO 0.11 M HNO2 + 0.10 M KNO2 0.11 M HCN + 0.20 M NaCN 0.30 M HClO + 0.22 M KClO 0.27 M NH4NO3 + 0.40 M NH3 0.13 M HClO + 0.17 M KClO 0.28 M NH4Br + 0.36 M NH3 0.21 M HClO + 0.13 M KClO 0.40 M CH3COOH + 0.23 M CH3COOK 0.33 M HCN + 0.27 M KCN 0.35 M NH4Br + 0.34 M NH3 0.13 M HF + 0.16 M KF 0.27 M NH4Br + 0.39 M NH3 0.17 M HNO2 + 0.11 M KNO2 0.21 M HClO + 0.13 M NaClO 0.40 M HCN + 0.26 M KCN 0.31 M CH3COOH + 0.29 M CH3COONa 0.30 M NH4Br + 0.33 M NH3 0.20 M HCN + 0.12 M KCN 0.26 M NH4Br + 0.39 M NH3 0.13 M HNO2 + 0.14 M KNO2 0.38 M HClO + 0.23 M NaClO 0.12 M HNO2 + 0.12 M NaNO2 0.11 M CH3COOH + 0.11 M CH3COO 0.25 M NH4Br + 0.32 M NH3 0.34 M HF + 0.22 M NaF 0.16 M HNO2 + 0.20 M NaNO2 0.27 M NH4Br + 0.40 M NH3 0.31 M HF + 0.24 M KF 0.11 M HCN + 0.18 M NaCN 0.34 M NH4Br + 0.38 M NH3 0.31 M HNO2 + 0.20 M KNO2 0.20 M HF + 0.12 M KF 0.15 M HCN + 0.18 M KCN 0.29 M NH4Br + 0.35 M NH3 0.10 M HF + 0.22 M KF 0.33 M HNO2 + 0.21 M KNO2 0.39 M HF + 0.24 M KF 0.21 M HCN + 0.16 M NaCN 0.28 M NH4Br + 0.31 M NH3 0.31 M NH4NO3 + 0.36 M NH3 0.18 M HNO2 + 0.16 M NaNO2 0.30 M CH3COOH + 0.23 M CH3COOK 0.18 M HClO + 0.18 M KClO

Which of the following statements concerning buffers is/are correct? (1) Buffers are resistant to changes in pH when diluted with water. (2) The pH of a buffer is normally within ±1 pH unit of the pKa of the weak acid from which it is made. (3) Buffers hold the pH at neutral; pH = 7.00

1 and 2

The element chlorine would be expected to form

1 covalent bond to obey octet rule

Strontium-90 has a half-life of 28.1 years. Starting with 4.00 mg of this isotope, how much would remain after 56.2 years?

1.00 mg

An aqueous solution has a hydroxide ion concentration of 1.0×10-13 M

1.0×10-1 M acidic

An aqueous solution has a hydrogen ion concentration of 1.0×10-13 M (1.0×10-13 M)

1.0×10-1 M basic

An aqueous solution has a hydroxide ion concentration of 1.0×10-4 M (10-4 M) (1) What is the hydronium ion concentration in this solution? (2) What is the pH of this solution? (3) What is the pOH of this solution?

1.0×10-10 M 10 4

An aqueous solution has a hydroxide ion concentration of 1.0×10-4 M

1.0×10-10 M basic

An aqueous solution has a hydroxide ion concentration of 1.0×10-2 M (10-2 M) (1) What is the hydronium ion concentration in this solution? (2) What is the pH of this solution? (3) What is the pOH of this solution?

1.0×10-12 M 12 2

An aqueous solution has a hydrogen ion concentration of 1.0×10-2 M (1.0×10-2 M)

1.0×10-12 M acidic

An aqueous solution has a hydroxide ion concentration of 1.0×10-2 M

1.0×10-12 M basic

An aqueous solution has a hydroxide ion concentration of 0.10 M (10-1 M) (1) What is the hydronium ion concentration in this solution? M (2) What is the pH of this solution? (3) What is the pOH of this solution?

1.0×10-13 M 13 1

An aqueous solution has a hydrogen ion concentration of 0.10 M (1.0×10-1 M)

1.0×10-13 M acidic

An aqueous solution has a hydroxide ion concentration of 0.10 M

1.0×10-13 M basic

An aqueous solution has a hydroxide ion concentration of 1.0×10-12 M (10-12 M). (1) What is the hydronium ion concentration in this solution? M (2) What is the pH of this solution? (3) What is the pOH of this solution?

1.0×10-2 M 2 12

An aqueous solution has a hydroxide ion concentration of 1.0×10-12 M

1.0×10-2 M acidic

An aqueous solution has a hydrogen ion concentration of 1.0×10-11 M (1.0×10-11 M)

1.0×10-3 M basic

An aqueous solution has a hydroxide ion concentration of 1.0×10-10 M (10-10 M) (1) What is the hydronium ion concentration in this solution? M (2) What is the pH of this solution? (3) What is the pOH of this solution?

1.0×10-4 M 4 10

An aqueous solution has a hydroxide ion concentration of 1.0×10-10 M

1.0×10-4 M acidic

An aqueous solution has a hydrogen ion concentration of 1.0×10-10 M (1.0×10-10 M)

1.0×10-4 M basic

An aqueous solution has a hydroxide ion concentration of 1.0×10-9 M

1.0×10-5 M acidic

An aqueous solution has a hydroxide ion concentration of 1.0×10-8 M (10-8 M). (1) What is the hydronium ion concentration in this solution? (2) What is the pH of this solution? (3) What is the pOH of this solution?

1.0×10-6 M 6 8

An aqueous solution has a hydroxide ion concentration of 1.0×10-8 M (10-8 M). (1) What is the hydronium ion concentration in this solution? (2) What is the pH of this solution? (3) What is the pOH of this solution?

1.0×10-6 M 6 8

An aqueous solution has a hydroxide ion concentration of 1.0×10-8 M

1.0×10-6 M acidic

An aqueous solution has a hydrogen ion concentration of 1.0×10-8 M (1.0×10-8 M)

1.0×10-6 M basic

An aqueous solution has a hydroxide ion concentration of 1.0×10-7 M

1.0×10-7 M neutral

An aqueous solution has a hydroxide ion concentration of 1.0×10-6 M (10-6 M). (1) What is the hydronium ion concentration in this solution? M (2) What is the pH of this solution? (3) What is the pOH of this solution?

1.0×10-8 M 8 6

1.0×10-6 M (1.0×10-6 M)

1.0×10-8 M acidic

An aqueous solution has a hydroxide ion concentration of 1.0×10-6 M

1.0×10-8 M basic

An aqueous solution has a hydroxide ion concentration of 1.0×10-5 M

1.0×10-9 M basic

What is the pH of 0.49 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 3.6 x 10-13.

1.22

What is the pH of 0.43 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 3.6 x 10-13.

1.25

What is the pH of 0.36 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 3.6 x 10-13.

1.28

The hydroxide ion concentration in an aqueous solution at 25°C is 8.4×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

1.2×10-13 M 12.92 1.08

The hydroxide ion concentration in an aqueous solution at 25°C is 8.5×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

1.2×10-13 M 12.93 1.07

What is the pH of 0.33 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 3.6 x 10-13. 1.41 3.85 2.12 2.61 1.30

1.30

What is the pH of 0.33 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13.

1.30

What is the pH of 0.24 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13.

1.37

What is the pH of 0.23 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13.

1.38

What is the pH of 0.19 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13

1.42

What is the pH of 0.17 M H3PO4? The Ka values for phosphoric acid are Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13.

1.45

What is the Ka of a particular acid if a 3.00×10-2 M aqueous solution of it has a pH of 3.67?

1.52×10-6

Strontium-90 has a half-life of 28.1 years. Starting with 6.40 mg of this isotope, how much would remain after 56.2 years?

1.60 mg

The radioactive isotope carbon-14 is used for radiocarbon dating. The half-life of carbon-14 is 5.730×103 years. A wooden artifact in a museum has a 14C count that is 0.125 times that found in living organisms. Estimate the age of the artifact.

1.72×104 yrs

The hydronium ion concentration in an aqueous solution at 25°C is 5.3×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

1.9×10-13 M 1.28 12.72

An aqueous solution has a pOH of 4 (1) What is the pH of this solution? (2) What is the hydronium ion concentration in this solution? (3) What is the hydroxide ion concentration in this solution?

10 10 -4 M 4

An aqueous solution has a hydrogen ion concentration of 1×10-13 M (10 -13 M) (1) What is the hydroxide ion concentration in this solution? M (2) What is the pOH of this solution? (3) What is the pH of this solution?

10 -1 M 1 13

An aqueous solution has a hydrogen ion concentration of 1×10-13 M (10 -13 M). (1) What is the hydroxide ion concentration in this solution? M (2) What is the pOH of this solution? (3) What is the pH of this solution?

10 -1 M 1 13

An aqueous solution has a hydrogen ion concentration of 1×10-10 M (10 -10 M) (1) What is the hydroxide ion concentration in this solution? (2) What is the pOH of this solution? (3) What is the pH of this solution?

10 -4 M 4 10

An aqueous solution has a hydrogen ion concentration of 1×10-8 M (10 -8 M) (1) What is the hydroxide ion concentration in this solution? (2) What is the pOH of this solution? (3) What is the pH of this solution?

10 -6 M 6 8

An aqueous solution has a hydrogen ion concentration of 1×10-7 M (10 -7 M) (1) What is the hydroxide ion concentration in this solution? M (2) What is the pOH of this solution? (3) What is the pH of this solution?

10 -7 M 7 7

An aqueous solution has a hydrogen ion concentration of 1×10-7 M (10 -7 M) (1) What is the hydroxide ion concentration in this solution? (2) What is the pOH of this solution? (3) What is the pH of this solution?

10 -7 M 7 7

An aqueous solution has a hydrogen ion concentration of 1×10-5 M (10 -5 M). (1) What is the hydroxide ion concentration in this solution? (2) What is the pOH of this solution? (3) What is the pH of this solution?

10 -9 M 9 5

Select the missing product of this nuclear reaction: 235 U + 1 n ? + 3 1 n + 132 Sb 92 0 0 51

101 Nb 41

The liquid 1,4-dibromobutane has a density of 1.82 g/mL at 25 °C. If a 195 gram sample of this compound is needed, what volume of the liquid at 25 °C must be provided?

107.1 ml

Sn-108 undergoes electron capture. The product of this reaction would be

108 In 49

Calculate the pH of a 0.050 M solution of trimethylamine (Kb = 7.4 x 10-5).

11.29

Calculate the pH of a 0.084 M solution of trimethylamine (Kb = 7.4 x 10-5).

11.40

What mass of solid NaCH3CO2 (molar mass = 82.0 g/mol) should be added to 1.00 L of 0.350 M CH3CO2H to make a buffer of pH = 4.36? (Ka for CH3CO2H = 1.8 x 10-5)

12

What mass of solid NaCH3CO2 (molar mass = 82.0 g/mol) should be added to 1.00 L of 0.350 M CH3CO2H to make a buffer of pH = 4.38? (Ka for CH3CO2H = 1.8 x 10-5)

12

An aqueous solution has a pOH of 2 (1) What is the pH of this solution? (2) What is the hydronium ion concentration in this solution? (3) What is the hydroxide ion concentration in this solution?

12 10- 12 M 10 -2 M

The Ka for chlorous acid is 1.2 x 10-2 at 25 °C. What is the pKb for chlorite ion?

12.08

The Ka for sulfurous acid is 1.5 x 10-2 at 25 °C. What is the pKb for sulfite ion?

12.18

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: HClO4 (aq) + P4O10 (s) H3PO4 (aq) + Cl2O7 (l)

12HClO4 (aq) + P4O10 (s) 4H3PO4 (aq) + 6Cl2O7 (l)

Fill in the symbol for the missing particle in the following nuclear equation

131 I 53 -----> 0 e -1 + 131 Xe 54

(1) What is the mass number of an atom that contains 55 protons, 82 neutrons, and 55 electrons? mass number = (2) What is the symbol for the element? element =

137 Cs

When uranium-238 is bombarded with another nucleus, five neutrons and a new isotope with an atomic number of 99.0 and an atomic mass of 247 is produced. Select the bombarding nucleus

14 N 7

Select the missing product of this reaction: 14 N + 1 n 1 H + ? 7 0 1

14 c 6

How many electrons, protons, and neutrons are there in an atom of 29Si?

14 protons 15 neutrons 14 electrons

Complete the following fission reaction: 1 n + 235 U ? + 3 1 n + 92 Kr 0 92 0 36

141 Ba 56

Select the missing product of this nuclear reaction

144 Cs 55

How many orbitals are there in the shell with n = 4 in an atom?

16

Choose the nucleus with which uranium-238 must be bombarded to yield fermium-249 and five neutrons

16 O 8

When plutonium-241 is bombarded with another nucleus, five neutrons and a new isotope with an atomic number of 102 and an atomic mass of 252 is produced. Select the bombarding nucleus

16 O 8

Calculate how long will it take for a sample of a radionuclide with a half-life of 27.0 days decay to 1.0% of its original value

179 days

What is the atomic number for the element that is in group 8A and period 3? 18 What is the atomic number for the element that is in group 1B and period 4? 29 What is the atomic number for the element that is in group 2A and period 2? How many 4f orbitals are there in an atom? What is the maximum number of electrons possible in a set of 4f orbitals?

18 29 4 7 14

Calculate how long will it take for a sample of a radionuclide with a half-life of 29.3 days decay to 1.0% of its original value

195 days

Which of the following reactions is an example of electron capture?

199 Tl + 0 β 199 Hg 81 -1 80

The following Lewis diagram represents the valence electron configuration of a main-group element. X=1

1A cation +1 If X is in period 4 , the ion formed has the same electron configuration as the noble gas: potassium K+

The following Lewis diagram represents the valence electron configuration of a main-group element. X=1

1A cation +1 If X is in period 5 , the ion formed has the same electron configuration as the noble gas: rubidium Rb+

(1) Write the electron configuration for the boron atom (2) Write the electron configuration for the phosphorus atom.

1s2 2s2 2p1 1s2 2s2 2p6 3s2 3p3

(1) What is the complete ground state electron configuration for the gallium atom? (2) What is the complete ground state electron configuration for the scandium atom?

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p1 1s2 2s2 2p6 3s2 3p6 3d1 4s2

What is the complete ground state electron configuration for the lithium atom?

1s22s1

What is the complete ground state electron configuration for the carbon atom? What is the complete ground state electron configuration for the nickel atom?

1s22s22p2 1s22s22p63s23p64s23d8

(1) Write the electron configuration for the carbon atom (2) Write the electron configuration for the chlorine atom.

1s22s22p2 1s22s22p63s23p5

What is the complete ground state electron configuration for the nitrogen atom? What is the complete ground state electron configuration for the iron atom?

1s22s22p3 1s22s22p63s23p64s23d6

Assuming that the octet rule is obeyed, write out the electron configuration for the ion formed by the element fluorine, F.

1s22s22p6 anion charge of -1 same electron configuration as Ne

Assuming that the octet rule is obeyed, write out the electron configuration for the ion formed by the element oxygen, O.

1s22s22p6 anion charge of -2

What is the complete ground state electron configuration for the sodium atom? What is the complete ground state electron configuration for the germanium atom?

1s22s22p63s1 1s22s22p63s23p64s23d104p2

What is the complete ground state electron configuration for the bromine atom? What is the complete ground state electron configuration for the vanadium atom?

1s22s22p63s23p64s23d104p5 1s22s22p63s23p64s23d3

What is the complete ground state electron configuration for the manganese atom?

1s22s22p63s23p64s23d5

How many types of orbitals are there in the shell with n = 2 in an atom?

2

The element selenium would be expected to form

2

The element sulfur would be expected to form

2

What is the maximum number of electrons possible in a set of 4s orbitals?

2

What is the maximum number of electrons possible in the shell with n = 1 in an atom?

2

An aqueous solution has a pOH of 12 (1) What is the pH of this solution? (2) What is the hydronium ion concentration in this solution? (3) What is the hydroxide ion concentration in this solution?

2 10- 2 M 10 -12 M

An aqueous solution has a hydrogen ion concentration of 1×10-12 M (10 -12 M) (1) What is the hydroxide ion concentration in this solution? (2) What is the pOH of this solution? (3) What is the pH of this solution?

2 12 10 -2 M

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of hydrochloric acid and barium hydroxide are combined.

2 HCl ( aq ) + Ba(OH)2 ( aq ) BaCl2 ( aq ) + 2 H2O ( l )

Which of the following statements concerning buffers is/are correct? (1) Buffers are composed of a weak acid diluted with water. (2) The pH of a buffer is normally within ±1 pH unit of the pKa of the weak acid from which it is made. (3) Buffers are resistant to changes in pH when diluted with water.

2 and 3

Which of the following statements concerning buffers is/are correct? (1) Buffers are used as colored indicators for acid-base titrations. (2) The pH of a buffer is normally within ±1 pH unit of the pKa of the weak acid from which it is made. (3) Buffers are resistant to changes in pH when diluted with water.

2 and 3

The element tellurium would be expected to form

2 covalent bonds

In the laboratory, a student dilutes 29.2 mL of a 10.4 M hydrobromic acid solution to a total volume of 150.0 mL. What is the concentration of the diluted solution?

2.02

The hydroxide ion concentration in an aqueous solution at 25°C is 4.7×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

2.1×10-12 12.67 1.33

The hydroxide ion concentration in an aqueous solution at 25°C is 3.9×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

2.6×10-13 M 12.59 1.41

What is the pH of 5.5 × 10-3 M HF? The Ka for hydrofluoric acid is 7.2 × 10-4.

2.78

The hydroxide ion concentration in an aqueous solution at 25°C is 3.7×10-2 M The hydronium ion concentration is The pH of this solution is The pOH is

2.7×10-13 M 12.57 1.43

What is the pH of 4.9 × 10-3 M HF? The Ka for hydrofluoric acid is 7.2 × 10-4.

2.81

What is the pH of 4.4 × 10-3 M HF? The Ka for hydrofluoric acid is 7.2 × 10-4.

2.84

Calculate the pH of a solution prepared by mixing 20.0 mL of 0.010 M HCl with 125.0 mL of 0.10 M HCN. For HCN, Ka = 1.0 × 10-10. Assume that the volumes are additive.

2.86

The pH of a 0.359 M solution of the conjugate base, A-, of a weak acid, HA, is 10.50. What is the Kb for A-?

2.8×10-7

What is the pH of 3.4 × 10-3 M HF? The Ka for hydrofluoric acid is 7.2 × 10-4. A.7.20 B.2.90 C.2.47 D.4.35 E.2.71

2.90

Calculate the pH of a solution prepared by mixing 15.0 mL of 0.010 M HCl with 125.0 mL of 0.10 M HCN. For HCN, Ka = 1.0 × 10-10. Assume that the volumes are additive. 1.00 4.03 1.49 2.00 2.97

2.97

Write the composition of one atom of the 42Ca isotope

20 protons 22 neutrons 20 electrons

Calculate how long will it take for a sample of a radionuclide with a half-life of 30.9 days decay to 1.0% of its original value.

205

Write a balanced nuclear equation for the following: The nuclide thallium-209 undergoes beta emission.

209 TI 81 ---> 0 e -1 + 209 Pb 82

The liquid methanol has a density of 0.791 g/mL at 20 °C. If a sample of this liquid at 20 °C has a volume of 27.0 mL, how many grams of liquid are there in the sample?

21.4 g

Write a balanced nuclear equation for the following: The nuclide bismuth-210 undergoes beta emission

210 Bi 83----> 0 e -1 + 210 Po 84

Bismuth beta decay

214 Bi 83----> 0 e -1 + 214 Po 84

Write a balanced nuclear equation for the following: The nuclide polonium-214 undergoes alpha emission The symbol for polonium-214 = 214 Po 84 The atomic number of the product is 84 - 2 = 82. The element with atomic number 82 is lead. The mass number of the product is 214 - 4 = 210. Therefore the product nuclide is lead-210 =

214 Po 84 ------> 4 He 2 + 210 Pb 82

Calculate how long will it take for a sample of a radionuclide with a half-life of 34.5 days decay to 1.0% of its original value.

229 days

Fill in the nuclide symbol for the missing particle in the following nuclear equation ______ -----> 4 He 2 + 226 Ra 88

230 Th 90

Write a balanced nuclear equation for the following: The nuclide uranium-234 undergoes alpha emission. The atomic number of the product is 92 - 2 = 90. The element with atomic number 90 is thorium. The mass number of the product is 234 - 4 = 230.

230 Th 90

Write a balanced nuclear equation for the following: The nuclide thorium-230 undergoes alpha emission.

230 Th 90 ----> 226 Ra 88 + 4 alpha 2

Write a balanced nuclear equation for the following: The nuclide thorium-234 undergoes beta emission

234 Th 90 ----> 0 e -1 + 234 Pa 91

Select the missing product of this decay reaction

234 pa 91

Which of the following would be the correct symbol for an americium-243 nucleus using the AZX symbolism?

243 am 95

The liquid diethyl ether has a density of 0.714 g/mL at 20 °C. If a sample of this liquid at 20 °C has a volume of 35.2 mL, how many grams of liquid are there in the sample?

25.1 g

Calculate how long will it take for a sample of a radionuclide with a half-life of 38.9 days decay to 1.0% of its original value

259 days

The half-life of the radioactive isotope polonium-210 is 138 days. How long will it take for the mass of a sample of polonium-210 to decay from 70.0 micrograms to 17.5 micrograms?

276 days

Calculate how long will it take for a sample of a radionuclide with a half-life of 42.0 days decay to 1.0% of its original value

279 days

The following Lewis diagram represents the valence electron configuration of a main-group element. This element is in group (it has 2 dots)

2A According to the octet rule, this element would be expected to form a(n) cation, charge of +2 If X is in period 3 , the ion formed has the same electron configuration as the noble gas Ne 1s22s22p6 + 2e-

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: C4H10 (g) + O2 (g) CO2 (g) + H2O (g)

2C4H10 (g) + 13O2 (g) 8CO2 (g) + 10H2O (g)

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: Fe (s) + O2 (g) FeO (s)

2Fe (s) + O2 (g) 2FeO (s)

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: H2O (l) H2 (g) + O2 (g)

2H2O (l) 2H2 (g) + O2 (g)

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: H2S (g) + O2 (g) H2O (l) + SO2 (g)

2H2S (g) + 3O2 (g) 2H2O (l) + 2SO2 (g)

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: HBr (aq) H2 (g) + Br2 (l)

2HBr (aq) H2 (g) + Br2 (l)

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of barium hydroxide and hydrochloric acid are combined.

2HCl + Ba(OH)2BaCl2 + 2H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of barium hydroxide and nitric acid are combined.

2HNO3 + Ba(OH)2Ba(NO3)2 + 2H2O

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: NO (g) + O2 (g) NO2 (g)

2NO (g) + O2 (g) 2NO2 (g)

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: Na (s) + H2O (l) NaOH (aq) + H2 (g)

2Na (s) + 2H2O (l) 2NaOH (aq) + H2 (g)

How many protons can be lost by citric acid, H3C6H5O6?

3

How many types of orbitals are there in the shell with n = 3 in an atom?

3

The element phosphorus would be expected to form

3

How many 4p orbitals are there in an atom? What is the maximum number of electrons possible in a set of 4p orbitals?

3 6

How many 4p orbitals are there in an atom? What is the maximum number of electrons possible in a set of 4p orbitals? (2X3)

3 6

How many 5p orbitals are there in an atom? What is the maximum number of electrons possible in a set of 5p orbitals?

3 6

The element nitrogen would be expected to form

3 covalent bonds

What is the pH of 1.5 x 10-3 M HF? The Ka for hydrofluoric acid is 7.2 x 10-4.

3.13

A buffer solution is made that is 0.434M in HF and 0.434M in KF 1. If Ka for HF is 7.2x10-4, what is the pH of the buffer solution?

3.14

What is the pH of 1.3 x 10-3 M HF? The Ka for hydrofluoric acid is 7.2 x 10-4.

3.17

An aqueous solution of acetone is made by transfering 1.61 mL of liquid acetone to a 50.0 mL volumetric flask, and then adding enough water to fill the flask to the mark. What is the volume/volume percentage of acetone in the solution?

3.22

What is the pH of 4.6 x 10-4 M HF? The Ka for hydrofluoric acid is 7.2 x 10-4.

3.50

What is the pH of 3.9 x 10-4 M HF? The Ka for hydrofluoric acid is 7.2 x 10-4.

3.55

What is the pH of 2.1 x 10-4 M HF? The Ka for hydrofluoric acid is 7.2 x 10-4.

3.77

What is the maximum number of electrons possible in the shell with n = 4 in an atom?

32

Write a balanced nuclear equation for the beta decay of phosphorus-32

32 P 15----> 0 beta -1 + 32 S 16

Write a balanced nuclear equation for the following: The nuclide phosphorus-32 undergoes beta emission.

32 P 15----> 0 e -1 + 32 S 16

Calculate the half-life of a radioisotope if it takes 96 years for a sample to decay to 12.5% of its original activity.

32 yr

The half-life of the radioactive isotope cesium-129 is 32.0 hours. How long will it take for the mass of a sample of cesium-129 to decay from 57.4 micrograms to 28.7 micrograms?

32.0 hours

How many types of orbitals are there in the shell with n = 4 in an atom?

4

The element silicon would be expected to form

4

The balanced chemical equation for the reaction between silicon tetrafluoride and water is: SiF4(s) + 2H2O(l) 4HF(aq) + SiO2(s) We can interpret this to mean: ... 2 moles of water and moles of silicon tetrafluoride React to produce ... moles of hydrofluoric acid and moles of silicon dioxide

4 1 4

Select the basic fusion reaction of the universe

4 1 H 4 He + 2 0 e 1 2 1

When HCl(g) reacts with O2(g) to form H2O(g) and Cl2(g), 6.84 kcal of energy are evolved for each mole of HCl(g) that reacts. Write a balanced equation for the reaction with an energy term in kcal as part of the equation. Use the SMALLEST INTEGER coefficients possible and put the energy term in an appropriate box. If a box is not needed, leave it blank.

4 HCl(g) + O2(g) 2 H2O(g) + 2 Cl2(g) + 27.4 kcal

When HCl(g) reacts with O2(g) to form H2O(g) and Cl2(g), 6.84 kcal of energy are evolved for each mole of HCl(g) that reacts. Write a balanced equation for the reaction with an energy term in kcal as part of the equation

4 HCl(g) + O2(g)---> 2 H2O(g) + 2 Cl2(g) + 27.4 kcal

When 94.871 and 50.40 are multiplied, the answer should have

4 significant figure(s).

How many significant figures are there in each of the following numbers? 40.359: 5 0.806684: 6 336.088: 6 0.031: 2 669.278: 6 0.51: 2 7700: 2 39.233: 5 0.05979: 4 0.403625: 6 877.43: 5 610000: 2 7510: 3 77560.0: 6 67.0: 3 42650.00: 7

42.8: 3 0.015: 2 593.61: 5 0.2137: 4 0.063328: 5 68.737: 5 497.8: 4 0.599260: 6 0.079: 2 49.4 : 3 0.2684: 4 123.338: 6 1990: 3 758000: 3 6500.0: 5 40160.00: 7

If the Kb of a certain amine is 4.50 × 10-4 , what is the approximate ratio of the protonated to the unprotonated amine, respectively, at pH 7.00? Assume the following reaction. RNH2 (aq) + H2O(l) = RNH3+(aq) + OH-(aq)

4500 : 1

How much will it cost to purchase chicken wire for a fence if 65 feet are needed and the fencing costs $2.20 / yard?

47.7

Calculate the half-life of a radioisotope if it takes 144 years for a sample to decay to 12.5% of its original activity

48 years

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: Fe (s) + O2 (g) Fe2O3 (s)

4Fe (s) + 3O2 (g) 2Fe2O3 (s)

How many 5d orbitals are there in an atom? What is the maximum number of electrons possible in a set of 5d orbitals?

5 10

An aqueous solution has a pOH of 9 (1) What is the pH of this solution? (2) What is the hydronium ion concentration in this solution? (3) What is the hydroxide ion concentration in this solution?

5 10- 5 M 10 -9 M

A student determines that the value of pKa for HCN = 9.29 What is the value of Ka?

5.13 x10x^-10

The Ka for hypobromous acid is 2.0 x 10-9 at 25 °C. What is the pKb for hypobromite ion?

5.30

Chromium-51 is a radioisotope that is used to assess the lifetime of red blood cells The half-life of chromium-51 is 27.7 days. How many milligrams of a 70.0 milligram sample of chromium-51 will be lost by radioactive decay during 55.4 days?

52.5 mg

Write a balanced nuclear equation for the following: The nuclide chromium-56 undergoes beta emission.

56 Cr---> 0 e -1 + 56 Mn 25

Calculate how long it will take for a sample of 234Th with a half-life of 24.1 days to decay to 20% of its original value

56 days

Calculate the half-life of a radioisotope if it takes 168 years for a sample to decay to 12.5% of its original activity

56 yr

Fill in the symbol for the missing particle in the following nuclear equation.

59 Fe 26 ---> 0 e -1 + 59 Co 27

An aqueous solution has a pOH of 8 1) What is the pH of this solution? (2) What is the hydronium ion concentration in this solution? (3) What is the hydroxide ion concentration in this solution?

6 10- 6 M 10 -8 M

What is the Ka of a particular acid if a 2.00×10-2 M aqueous solution of it has a pH of 5.44?

6.59×10-10

A certain element consists of two stable isotopes. The first has an atomic mass of 7.0160 amu and a percent natural abundance of 92.58 %. The second has an atomic mass of 6.0150 amu and a percent natural abundance of 7.42 %.

6.94 amu

A certain element consists of two stable isotopes. The first has an atomic mass of 62.9298 amu and a percent natural abundance of 69.09 %. The second has an atomic mass of 64.9278 amu and a percent natural abundance of 30.91 %. Fraction = percent/100

63.55 amu

How many 5f orbitals are there in an atom? What is the maximum number of electrons possible in a set of 5f orbitals?

7 14

What is the Ka of a particular acid if a 2.80×10-2 M aqueous solution of it has a pH of 3.84?

7.46×10-7

Sodium-24 has a half-life of 15 hours. Calculate the number of mg of an initial 40-mg sample that remains after one day and 12 hours

7.6

Calculate the pH of a 2.83E-2 M NaF solution (Kb = 1.4 x 10-11).

7.8

Sodium-24 has a half-life of 15 hours. Calculate the number of mg of an initial 47-mg sample that remains after one day and 15 hours

7.8 mg

The radioactive isotope decays by beta emission. If the mass of a sample of gallium-74 decays from 98.1 micrograms to 49.1 micrograms in 7.90 minutes, what is the half-life of gallium-74?

7.90 minutes

Calculate the pH of a 4.96E-2 M NaF solution (Kb = 1.4 x 10-11).

7.92

The following Lewis diagram represents the valence electron configuration of a main-group element. X=7 dots

7A Anion -1 If X is in period 2 , the ion formed has the same electron configuration as the noble gas: fluorine F-

The following Lewis diagram represents the valence electron configuration of a main-group element. X=7 dots

7A anion charge of -1 If X is in period 3 , the ion formed has the same electron configuration as the noble gas: chlorine Cl-

The following Lewis diagram represents the valence electron configuration of a main-group element. X=7 dots

7a anion -1 If X is in period 4 , the ion formed has the same electron configuration as the noble gas: bromine Br-

What is the maximum number of electrons possible in the shell with n = 2 in an atom?

8

Calculate the pH of a 7.94E-2 M NaF solution (Kb = 1.4 x 10-11).

8.02

If the Kb of a certain aromatic amine is 2.24 × 10-9 , what is the pKb?

8.65

What is the Ka of a particular acid if a 2.10×10-2 M aqueous solution of it has a pH of 4.87?

8.67×10-9

What is the Ka of a particular acid if a 3.30×10-2 M aqueous solution of it has a pH of 3.27?

8.74×10-6

The half-life of the radioactive isotope chromium-51 is 27.7 days. How long will it take for the mass of a sample of chromium-51 to decay from 56.0 micrograms to 7.00 micrograms?

83.1 days

How many orbitals are there in the shell with n = 3 in an atom?

9

What is the pH of the buffer that results when 6.50 g of NH3 and 6.83 g of NH4Cl are diluted with water to a volume of 300 mL? (Ka for NH4+ = 5.6 x 10-10.)

9.73

What is the pH of the buffer that results when 5.92 g of NH3 and 5.80 g of NH4Cl are diluted with water to a volume of 300 mL? (Ka for NH4+ = 5.6 x 10-10.)

9.76

What is the pH of the buffer that results when 7.48 g of NH3 and 6.53 g of NH4Cl are diluted with water to a volume of 500 mL? (Ka for NH4+ = 5.6 x 10-10.)

9.81

Fill in the symbol for the missing particle in the following nuclear equation

90 Sr 38----> 0 e -1 + 90 Y 39

Write a balanced nuclear equation for the following: The nuclide strontium-90 undergoes beta emission.

90 Sr 38---> 0 e -1 + 90 Y 39

Calculate how long it will take for a sample of 234Th with a half-life of 24.1 days to decay to 7.0% of its original value

92 days

Complete the following nuclear bombardment equation by filling in the nuclear symbol for the missing species. 235 U 92 + 1 n 0--->_________ + 139 xe 54 + 3 1 n 0

94 Sr 38

Write the composition of one atom of the 244Pu isotope

94 protons 150 neutrons 94 electrons

Complete the following fission reaction: 1 n + 235 U ? + 2 1 n + 137 Te 0 92 0 52

97 Zr 40

The stronger acid is A. H2SO3 1.7×10-2 B. H3PO4 7.5×10-3

A

The stronger acid is A. HF 7.2×10-4 B. HNO2 4.5×10-4

A

Which one of the following is a strong acid? A. perchloric acid, HClO4 B. hypobromous acid, HOBr C. nitrous acid, HNO2 D. bromic acid, HBrO3 E. phosphoric acid, H3PO4

A

Which of the following occurs when the weak base ammonia, NH 3 , is dissolved in water?

A very small number of ammonia molecules take an H + from the water.

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HCN (aq) + CO32- CN- + HCO3-

Acid base base acid CN- HCO3-

Write a formula for the compound formed between each of the pairs of ions given in the table: Ag+ & O2- Fe3+ & S2- Cu+ & Cl- K+& CH3COO- Ba2+ & NO3- Na+ & OH- Ca2+ & PO43- Ni2+ & F- NH4+ & I- Ag+ & Br- Fe3+ & I- Cr3+ & S2- Al3+& NO3- Ca2+ & CO32- Mg2+ & CrO42- Cu+ & Br- NH4+ & HCO3- Cu2+ & F- Fe2+ & Cl- Pb2+ & O2- Ag+ & F- Al3+ & CrO42- K+ & HCO3- Mg2+ & NO3- Al3+ & OH- Cu2+ & SO42- Cu+ & CO32- Co2+ & I- Pb2+ & S2- Cu+ & Cl- Ca2+ & SO32- Al3+ & CN- Mg2+ & CH3COO- NH4+ & CrO42- K+ & SO32- Pb2+ & F- Cu+ & S2- Cu2+ & I- Ni2+ & Cl- Al3+ & CO32- Ca2+ & NO2- Zn2+ & CrO42- Mg2+ & S2- Ag+ & I- Cu+ & O2- Na+ & CN- Ba2+ & PO43- Cu+ & CH3COO- K+ & F- Pb2+ & SO42- Zn2+ & O2- Pb2+ & Cl- Mn2+ & S2- Ba2+ & SO32- Na+ and SO32- Ag+ and CN- Co3+ and CH3COO- Cr2+ and F- Mn2+ and Br- Zn2+ and I- Na+ HCO3- Mg2+ SO32- Al3+ NO3- Co2+ and OH- Fe3+ and S2- Co3+ and CH3COO- Co2+ and Cl- Ni2+ and Br- Fe2+ and S2- Al3+ CH3COO- Ba2+ CO32- Ca2+ CN- Fe2+ and SO32- Co2+ and SO42- Cu2+ and O2- Mn2+ and I- Zn2+ and S2 NH4+ and F- Ca2+ CO32- Al3+ SO42- Na+ SO32- Co3+ and NO3- Fe2+ and Br- Fe2+ and CrO42- Cr3+ SO42- Na+ and S2-

Ag2O Fe2S3 CuCl KCH3COO Ba(NO3)2 NaOH Ca3(PO4)2 NiF2 NH4I AgBr FeI3 Cr2S3 Al(NO3)3 CaCO3 MgCrO4 CuBr NH4HCO3 CuF2 FeCl2 PbO AgF Al2(CrO4)3 KHCO3 Mg(NO3)2 Al(OH)3 CuSO4 Cu2CO3 CoI2 PbS CuCl CaSO3 Al(CN)3 Mg(CH3COO)2 (NH4)2CrO4 K2SO3 PbF2 Cu2S CuI2 NiCl2 Al2(CO3)3 Ca(NO2)2 ZnCrO4 MgS AgI Cu2O NaCN Ba3(PO4)2 CuCH3COO KF PbSO4 ZnO PbCl2 MnS BaSO3 Na2SO3 AgCN Co3+ and CH3COO- CrF2 MnBr2 ZnI2 NaHCO3 MgSO3 Al(NO3)3 Co(OH)2 Fe2S3 Co(CH3COO)3 CoCl2 NiBr2 FeS Al(CH3COO)3 BaCO3 Ca(CN)2 FeSO3 CoSO4 CuO MnI2 ZnS NH4F CaCO3 Al2(SO4)3 Na2SO3 Co(NO3)3 FeBr2 FeCrO4 Cr2(SO4)3 Na2

What is the formula of the compound in which the atom combining ratios are: aluminum : oxygen = 2 : 3

Al203

What is the formula of the compound in which the atom combining ratios are: aluminum : oxygen = 2 : 3

Al2O3

What is the formula of the compound in which the atom combining ratios are: aluminum : fluorine = 1 : 3

AlF3

Write a net ionic equation to show that hydrochloric acid, HCl, behaves as an acid in water.

An acid forms the hydronium ion in water. In this case, HCl donates a proton to H2O to form Cl- and H3O+ *HCL donates H+ to H2O HCl (aq) +H2O (l)-----> Cl- (aq)+H3O+ (aq)

Write a net ionic equation to show that perchloric acid, HClO4, behaves as an acid in water.

An acid forms the hydronium ion in water. In this case, HClO4 donates a proton to H2O to form ClO4- and H3O+. HClO4 (aq) + H2O (l) ------> ClO4- (aq) + H3O+ (aq) The single arrow to the right in the equation indicates that the reaction goes essentially to completion.

Write a net ionic equation to show that nitrous acid , HNO2 , behaves as an acid in water.

An acid forms the hydronium ion in water. In this case, HNO2 donates a proton to H2O to form NO2- and H3O+. HNO2(aq)+H2O (l) ____>-----> NO2-(aq)+H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion.

Alpha decay:

An alpha particle is a helium-4 nucleus which has a mass number of 4 and an atomic number of 2. When alpha decay occurs, the mass number decreases by four and the atomic number decreases by two. Therefore the reactant nuclide will have a mass number that is four larger and an atomic number that is two larger

What is the formula of the compound in which the atom combining ratios are: boron : fluorine = 1 : 3

BF3

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of barium hydroxide and sulfuric acid are combined.

Ba(OH)2 ( aq ) + H2SO4 ( aq ) BaSO4 ( s ) + 2 H2O ( l )

A reaction occurs when aqueous solutions of barium hydroxide and sulfuric acid are combined.

Ba(OH)2 ( aq ) + H2SO4 ( aq ) BaSO4 ( s ) + H2O ( l ) not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation: Ba(OH)2 ( aq ) + H2SO4 ( aq ) BaSO4 ( s ) + 2 H2O ( l )

Write a net ionic equation to show why solid barium hydroxide, Ba(OH)2 (s), forms a basic solution when it dissolves in water.

Ba(OH)2 (s)---->Ba2+ (aq) + 2 OH- (aq)

What is the formula of the compound in which the atom combining ratios are: barium : chlorine = 1 : 2

BaCl2

In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base 1. C2H5NH2(aq) + H2O(l) C2H5NH3+(aq)(aq) + OH-(aq) The formula of the reactant that acts as a proton donor is: H2O The formula of the reactant that acts as a proton acceptor is C2H5NH2 2. HNO2(aq) + H2O(l) NO2-(aq) + H3O+(aq) The formula of the reactant that acts as a proton donor is HNO2 The formula of the reactant that acts as a proton acceptor is h2o 3. (CH3)2NH(aq) + H2O(l) (CH3)2NH2+(aq) + OH-(aq) The formula of the reactant that acts as a proton donor is H2O The formula of the reactant that acts as a proton acceptor is (CH3)2NH 4. C6H5NH2(aq) + H2O(l) C6H5NH3+(aq) + OH-(aq) The formula of the reactant that acts as a proton donor is H2O The formula of the reactant that acts as a proton acceptor is C6H5NH2 5. HC9H7O4(aq) + H2O(l) C9H7O4-(aq) + H3O+(aq) The formula of the reactant that acts as a proton donor is HC9H7O4 The formula of the reactant that acts as a proton acceptor is h2o 6. C9H7N(aq) + H2O(l) C9H7NH+(aq) + OH-(aq) The formula of the reactant that acts as a proton donor is H2O The formula of the reactant that acts as a proton acceptor is C9H7N 7. HCOOH(aq) + H2O(l) HCOO-(aq) + H3O+(aq) The formula of the reactant that acts as a proton donor is HCOOH The formula of the reactant that acts as a proton acceptor is h2o 8. (C2H5)3N(aq) + H2O(l) (C2H5)3NH+(aq) + OH-(aq) The formula of the reactant that acts as a proton donor is H2O The formula of the reactant that acts as a proton acceptor is (C2H5)3N 9. C6H15O3N(aq) + H2O(l) C6H15O3NH+(aq) + OH-(aq) The formula of the reactant that acts as a proton donor is h2o The formula of the reactant that acts as a proton acceptor is C6H15O3N 10. HCN(aq) + H2O(l) CN-(aq) + H3O+(aq) The formula of the reactant that acts as a proton donor is HCN The formula of the reactant that acts as a proton acceptor is h2o 11. C18H21O3N(aq) + H2O(l) C18H21O3NH+(aq) + OH-(aq) The formula of the reactant that acts as a proton donor is h2o The formula of the reactant that acts as a proton acceptor is C18H21O3N 12. (CH3)3N(aq) + H2O(l) H(CH3)3N+(aq) + OH-(aq) The formula of the reactant that acts as a proton donor is h2o The formula of the reactant that acts as a proton acceptor is (CH3)3N 13. HClO(aq) + H2O(l) ClO-(aq) + H3O+(aq) The formula of the reactant that acts as a proton donor is HCLO The formula of the reactant that acts as a proton acceptor is h2o 14. C17H19O3N(aq) + H2O(l) C17H19O3NH+(aq) + OH-(aq) The formula of the reactant that acts as a proton donor is h2o The formula of the reactant that acts as a proton acceptor is C17H19O3N 15. HNO2(aq) + H2O(l) NO2-(aq) + H3O+(aq) HNO2 donates H2O accepts 16. (C2H5)2NH(aq) + H2O(l) (C2H5)2NH2+(aq) + OH-(aq) H2O donates 17. C6H5COOH(aq) + H2O(l) C6H5COO-(aq) + H3O+(aq) C6H5COOH donates 18. C5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq) H2O donates 19. CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq) CH3COOH donates 20. NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) H2O donates

Base, acid. acid, base. base, acid base, acid acid, base base, acid acid, base base, acid base, acid acid, base base, acid base, acid acid, base base, acid acid, base base, acid acid, base base, acid acid, base base, acid

Which of the following is a physical measurement of radioactivity?

Becquerel

Which of the following elements are nonmetals? (Z = atomic number) Choose all that apply.

Br (Z = 35) Fe (Z = 26) Cl (Z = 17)

Which of the following species is not amphiprotic? A. HC4H4O4- B. HC3H2O4- C. C2H3O2- D. None, all of them are amphiprotic.

C

Classify the underlined property as chemical or physical: The colorless liquid ethanol burns in air. The purple crystalline solid potassium permanganate forms a purple solution when dissolved in water. When aluminum foil is placed into liquid bromine a white solid forms.

C P C

Classify each of the following changes as chemical or physical: digesting food removing nail polish freezing ice cream

C P P

The substance morphine is a weak nitrogenous base like ammonia. Write a net ionic equation to show how morphine, C17H19O3N, behaves as a base in water.

C17H19O3N (aq) + H2O (l)---->____> C17H19O3NH+ (aq) + OH- (aq)

The substance codeine is a weak nitrogenous base like ammonia. Write a net ionic equation to show how codeine, C18H21O3N, behaves as a base in water.

C18H21O3N (aq) + H2O (l)---->___>C18H21O3NH+ (aq) + OH- (aq)

What is the formula of the compound in which the atom combining ratios are: carbon : hydrogen : oxygen = 3 : 8 : 3

C3H8O3

The substance pyridine is a weak nitrogenous base like ammonia. Write a net ionic equation to show how pyridine, C5H5N, behaves as a base in water.

C5H5N (aq) + H2O (l)--->___> C5H5NH+ (aq) + OH- (aq)

What is the formula of the compound in which the atom combining ratios are: carbon : chlorine = 1 : 4

CCl4

Write the net ionic equation for the reaction that occurs when 0.108 mol HCl is added to 1.00 L of the buffer solution. Use H3O+ instead of H+

CH3COO- + H3O+ CH3COOH + H2O

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CH3COO- + H2PO4- CH3COOH + HPO42- The formula for the conjugate CH3COO- The formula for the conjugate H2PO4- CH3COO- is a base H2PO4- is an acid CH3COOH is an acid HPO42- is a base

CH3COOH HPO42-

Write the net ionic equation for the reaction that occurs when 0.098 mol KOH is added to 1.00 L of the buffer solution

CH3COOH + OH-CH3COO- + H2O

Write the net ionic equation for the reaction that occurs when 0.110 mol NaOH is added to 1.00 L of the buffer solution

CH3COOH + OH-CH3COO- + H2O

Write a net ionic equation to show that acetic acid , CH3COOH , behaves as an acid in water.

CH3COOH is not an bronsted-lowrey acid, but is a lewis acid. In this case, CH3COOH donates a proton to H2O to form CH3COO- and H3O+ CH3COOH(aq) + H2O (l)--->____> CH3COO-(aq)+H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion.

The substance methylamine is a weak nitrogenous base like ammonia. Write a net ionic equation to show how methylamine, CH3NH2, behaves as a base in water.

CH3NH2 (aq) + H2O (l)--___>---> CH3NH3+ (aq) + OH- (aq)

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: CH4 (g) + CCl4 (g) CH2Cl2 (g)

CH4 (g) + CCl4 (g) 2CH2Cl2 (g)

Write the net ionic equation for the reaction that occurs when 0.083 mol HCl is added to 1.00 L of the buffer solution

CN- + H3O+ HCN + H2O

Write the net ionic equation for the equilibrium that is established when barium cyanide is dissolved in water

CN-(aq) + H2O HCN(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when calcium cyanide is dissolved in water

CN-(aq) + H2O HCN(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when potassium cyanide is dissolved in water

CN-(aq) + H2O HCN(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when potassium cyanide is dissolved in water.

CN-(aq) + H2O HCN(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when sodium cyanide is dissolved in water

CN-(aq) + H2O HCN(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when sodium cyanide is dissolved in water.

CN-(aq) + H2O HCN(aq) + OH -(aq) basic

Choose the reaction that is responsible for the natural acidity of rain.

CO2(g) + 2 H2O(l) → H3O+(aq) + HCO3-(aq)

The reaction between carbon monoxide and water is given below: CO(g) + H2O(l) CO2(g) + H2(g) We therefore know that which of the following reactions can also occur?

CO2(g) + H2(g) CO(g) + H2O(l)

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of calcium hydroxide and hydrochloric acid are combined.

Ca(OH)2 ( aq ) + 2 HCl ( aq ) CaCl2 ( aq ) + 2 H2O ( l )

A reaction occurs when aqueous solutions of calcium hydroxide and hydrochloric acid are combined.

Ca(OH)2 ( aq ) + HCl ( aq ) CaCl2 ( aq ) + H2O ( l ) not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation: Ca(OH)2 ( aq ) + 2 HCl ( aq ) CaCl2 ( aq ) + 2 H2O ( l )

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: CaCO3 (s) CaO (s) + CO2 (g)

CaCO3 (s) CaO (s) + CO2 (g)

What is the formula of the compound in which the atom combining ratios are: calcium : oxygen = 1 : 1

CaO

Nuclear power plants have control rods that absorb neutrons to control the reaction. What is the composition of the control rods?

Carbon

The acid with the smallest [H3O+] in a 0.10 M aqueous solution is:

Carbonic 4.2x10-7

The acid with the smallest pOH in a 0.10 M aqueous solution is:

Carbonic 4.2x10-7

Click on a lanthanide element

Ce

Click on an element within the halogen group

Cl

Write the net ionic equation for the equilibrium that is established when calcium hypochlorite is dissolved in water

ClO-(aq) + H2O HClO(aq) + OH -(aq basic

Write the net ionic equation for the equilibrium that is established when barium hypochlorite is dissolved in water.

ClO-(aq) + H2O HClO(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when potassium hypochlorite is dissolved in water

ClO-(aq) + H2O HClO(aq) + OH -(aq) basic

What is the formula of the compound in which the atom combining ratios are: chlorine : oxygen : fluorine = 1 : 3 : 1

ClO3F

Select the isotope used for food irradiation

Cobalt-60

Gamma emissions can be stopped with the use of an electromagnetic field because of their dense charge and their mass.

FALSE

Click on a transition element

Fe

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: Fe (s) + HCl (aq) FeCl2 (aq) + H2 (g)

Fe (s) + 2HCl (aq) FeCl2 (aq) + H2 (g)

A reaction occurs when aqueous solutions of sulfuric acid and calcium hydroxide are combined.

First translate the sentence into a chemical equation: H2SO4 ( aq ) + Ca(OH)2 ( s ) CaSO4 ( s ) + H2O ( l ) not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation: H2SO4 ( aq ) + Ca(OH)2 ( s ) CaSO4 ( s ) + 2 H2O ( l )

X with 2 dots

Group 2 A

Which of the following occurs when hydrogen chloride gas is dissolved in water to form hydrochloric acid?

H + is transferred from HCl to water.

In the Brønsted theory, both acids and bases are defined in terms of how substances lose or gain

H+

Which of these equations shows the net neutralization reaction between hydrobromic acid and sodium hydroxide ?

H+(aq) + OH-(aq) yields H2O(l)

Write a net ionic equation to show that oxalic acid, H2C2O4, behaves as an acid in water. Consider only its first ionization.

H2C2O4 (aq) + H2O (l) = HC2O4- (aq) + H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion. H2C2O4 is a diprotic acid because it has 2 ionizable protons. This is indicated by the two H atoms at the beginning of its formula .

Write the net ionic equation for the reaction that occurs when 0.115 mol NaOH is added to 1.00 L of the buffer solution

H2C2O4 + OH-HC2O4- + H2O

Write a net ionic equation to show that ascorbic acid, H2C6H6O6, behaves as an acid in water. Consider only its first ionization.

H2C6H6O6 donates a proton to H2O to form HC6H6O6- and H3O+. H2C6H6O6 (aq) + H2O (l) = HC6H6O6- (aq) + H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion. H2C6H6O6 is a diprotic acid because it has 2 ionizable protons. This is indicated by the two H atoms at the beginning of its formula .

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HCO3-+ HCN (aq) H2CO3 (aq) + CN- The formula for the conjugate HCO3- The formula for the conjugate HCN HCO3- is a base HCN is an acid H2CO3 acid CN- base

H2CO3 CN-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HCO3- + H3PO4 (aq) H2CO3 (aq + H2PO4- The formula for the conjugate of HCO3- is The formula for the conjugate of H3PO4 is HCO3- is a base H3PO4 is an acid H2CO3 is an acid H2PO4 is a base

H2CO3 H2PO4-

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of carbonic acid and sodium hydroxide are combined. Assume excess base

H2CO3 + 2NaOH Na2CO3 + 2H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of sodium hydroxide and carbonic acid are combined. Assume excess base.

H2CO3 + 2NaOH Na2CO3 + 2H2O

A reaction occurs when aqueous solutions of sodium hydroxide and carbonic acid are combined. Assume excess base.

H2CO3 + NaOH Na2CO3 + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. H2CO3 + 2NaOH Na2CO3 + 2H2O

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. H3PO4 (aq) + HS- H2PO4- + H2S (aq) the conjugate of H3PO4 the conjugate of HS- H3PO4 (aq) is a acid HS- is a base H2PO4- is a base H2S is an acid

H2PO4- H2S

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of hydrosulfuric acid and potassium hydroxide are combined. Assume excess base.

H2S + 2KOH K2S + 2H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of hydrosulfuric acid and sodium hydroxide are combined. Assume excess base.

H2S + 2NaOH Na2S + 2H2O

A reaction occurs when aqueous solutions of hydrosulfuric acid and potassium hydroxide are combined. Assume excess

H2S + KOH K2S + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. H2S + 2KOH K2S + 2H2O

A reaction occurs when aqueous solutions of hydrosulfuric acid and potassium hydroxide are combined. Assume excess base.

H2S + KOH K2S + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. H2S + 2KOH K2S + 2H2O

A reaction occurs when aqueous solutions of hydrosulfuric acid and sodium hydroxide are combined. Assume excess base.

H2S + NaOH Na2S + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. H2S + 2NaOH Na2S + 2H2O

Write the net ionic equation for the reaction that occurs when 0.064 mol NaOH is added to 1.00 L of the buffer solution.

H2SO3 + OH-HSO3- + H2O

Write the net ionic equation for the reaction that occurs when 0.098 mol KOH is added to 1.00 L of the buffer solution.

H2SO3 + OH-HSO3- + H2O

A reaction occurs when aqueous solutions of sulfuric acid and calcium hydroxide are combined.

H2SO4 ( aq ) + Ca(OH)2 ( s ) CaSO4 ( s ) + 2 H2O ( l )

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of sulfuric acid and calcium hydroxide are combined

H2SO4 ( aq ) + Ca(OH)2 ( s ) CaSO4 ( s ) + 2 H2O ( l )

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of sulfuric acid and calcium hydroxide are combined.

H2SO4 ( aq ) + Ca(OH)2 ( s ) CaSO4 ( s ) + 2 H2O ( l )

A reaction occurs when aqueous solutions of sulfuric acid and calcium hydroxide are combined.

H2SO4 ( aq ) + Ca(OH)2 ( s ) CaSO4 ( s ) + H2O ( l ) not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation: H2SO4 ( aq ) + Ca(OH)2 ( s ) CaSO4 ( s ) + 2 H2O ( l )

A reaction occurs when aqueous solutions of sulfuric acid and zinc hydroxide are combined.

H2SO4 ( aq ) + Zn(OH)2 ( s ) ZnSO4 ( aq ) + 2 H2O ( l )

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of sulfuric acid and zinc hydroxide are combined

H2SO4 ( aq ) + Zn(OH)2 ( s ) ZnSO4 ( aq ) + 2 H2O ( l )

According to Arrhenius which species is associated with all acids?

H3O+

Which of the following chemical equations is a net ionic equation for the reaction between aqueous HCl and a weak base?

H3O+(aq) + CN-(aq) → HCN(aq) + H2O(l)

Which of the following chemical equations is a net ionic equation for the reaction between aqueous HCl and a weak base?

H3O+(aq) + F-(aq) HF(aq) + H2O(l)

Which of the following chemical equations is a net ionic equation for the reaction between aqueous HCl and a weak base?

H3O+(aq) + NO2-(aq) HNO2(aq) + H2O(l)

Which of the following chemical equations is a net ionic equation for the reaction between aqueous HCl and a weak base?

H3O+(aq) + NO2-(aq) → HNO2(aq) + H2O(l)

A reaction occurs when aqueous solutions of potassium hydroxide and phosphoric acid are combined. Assume excess base.

H3PO4 + 3KOH K3PO4 + 3H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of potassium hydroxide and phosphoric acid are combined. Assume excess base

H3PO4 + 3KOH K3PO4 + 3H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of potassium hydroxide and phosphoric acid are combined. Assume excess base.

H3PO4 + 3KOH K3PO4 + 3H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of sodium hydroxide and phosphoric acid are combined. Assume excess base

H3PO4 + 3NaOH Na3PO4 + 3H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of sodium hydroxide and phosphoric acid are combined. Assume excess base.

H3PO4 + 3NaOH Na3PO4 + 3H2O

A reaction occurs when aqueous solutions of sodium hydroxide and phosphoric acid are combined. Assume excess base

H3PO4 + NaOH Na3PO4 + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. H3PO4 + 3NaOH Na3PO4 + 3H2O

A reaction occurs when aqueous solutions of sodium hydroxide and phosphoric acid are combined. Assume excess base.

H3PO4 + NaOH Na3PO4 + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. H3PO4 + 3NaOH Na3PO4 + 3H2O

What is the formula of the compound in which the atom combining ratios are: hydrogen : phosphorous : oxygen = 4 : 2 : 7

H4P2O7

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of potassium hydroxide and hydrobromic acid are combined.

HBr + KOHKBr + H2O

Write a net ionic equation to show that hydrobromic acid, HBr, behaves as an acid in water.

HBr donates a proton to H2O to form Br- and H3O+ HBr (aq) + H2O (l) -->Br- (aq) + H3O+ (aq) The single arrow to the right in the equation indicates that the reaction goes essentially to completion.

In a buffer solution made up of equal concentrations of acetic acid and sodium acetate, NaC2H3O2, which component is used to buffer against added OH−?

HC2H3O2

The monoprotic acids are an acid that yield one proton per molecule when dissolved. these acids are-

HCL, HNO3, HCLO4, HBr, HI, HClO3

The formula for the conjugate acid of CN- is

HCN

The weaker acid is: HCN HF

HCN

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CN-+HF (aq) HCN (aq) +F- The formula for the conjugate CN- The formula for the conjugate HF

HCN F-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CN- + HSO3- HCN (aq) + SO32- The formula for the conjugate CN- The formula for the conjugate HSO3- CN- is a base HSO3- is an acid HCN is an acid SO3 2- is a base

HCN SO3 2-

Write the net ionic equation for the reaction that occurs when 0.105 mol NaOH is added to 1.00 L of the buffer solution.

HCN + OH-CN- + H2O

A buffer solution that is 0.436M in HCN and 0.436M in KCN has a pH of 9.40. Addition of which of the following would increase the capacity of the buffer for added OH- ?

HCN and KCN

Write a net ionic equation to show that hydrocyanic acid , HCN , behaves as an acid in water.

HCN(aq)+H2O (l) = CN-(aq) + H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion.

A reaction occurs when aqueous solutions of hydrochloric acid and barium hydroxide are combined.

HCl ( aq ) + Ba(OH)2 ( aq ) BaCl2 ( aq ) + H2O ( l ) not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation: 2 HCl ( aq ) + Ba(OH)2 ( aq ) BaCl2 ( aq ) + 2 H2O ( l )

Write a net ionic equation to show that hydrochloric acid, HCl, behaves as an acid in water.

HCl (aq) + H2O (l)-->Cl- (aq) + H3O+ (aq) The single arrow to the right in the equation indicates that the reaction goes essentially to completion.

A reaction occurs when aqueous solutions of barium hydroxide and hydrochloric acid are combined

HCl + Ba(OH)2BaCl2 + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. 2HCl + Ba(OH)2BaCl2 + 2H2O

Which one of the following chemical equations illustrate the ionization of hydrochloric acid , HCl , when it dissolves in water?

HCl + H2O H3O+ + Cl-

A reaction occurs when aqueous solutions of potassium hydroxide and hydrochloric acid are combined.

HCl + KOHKCl + H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of potassium hydroxide and hydrochloric acid are combined.

HCl + KOHKCl + H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of sodium hydroxide and hydrochloric acid are combined.

HCl + NaOHNaCl + H2O

A reaction occurs when aqueous solutions of sodium hydroxide and hydrochloric acid are combined.

HCl + NaOHNaCl + H2O Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. In this case the equation is already balanced with all coefficients equal to unity. HCl + NaOHNaCl + H2O

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. ClO- + HNO2 (aq) HClO + NO2- The formula for the conjugate CLO- The formula for the conjugate HNO2 CLO- is a base HNO2 is an acid HCLO is an acid NO2- is a base

HClO NO 2-

Write a net ionic equation to show that hypochlorous acid , HClO , behaves as an acid in water.

HClO donates a proton to H2O to form ClO- and H3O+. HClO(aq)+H2O (l) = ClO-(aq)+H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion.

Write a net ionic equation to show that perchloric acid, HClO4, behaves as an acid in water.

HClO4 (aq) + H2O (l) ClO4- (aq) + H3O+ (aq) The single arrow to the right in the equation indicates that the reaction goes essentially to completion.

Which one of the following chemical equations illustrate the ionization of perchloric acid , HClO4 , when it dissolves in water?

HClO4 + H2O H3O+ + ClO4-

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of perchloric acid and potassium hydroxide are combined.

HClO4 + KOHKClO4 + H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of potassium hydroxide and perchloric acid are combined.

HClO4 + KOHKClO4 + H2O

A reaction occurs when aqueous solutions of potassium hydroxide and perchloric acid are combined.

HClO4 + KOHKClO4 + H2O Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. In this case the equation is already balanced with all coefficients equal to unity. HClO4 + KOHKClO4 + H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of potassium hydroxide and hydroiodic acid are combined.

HI + KOHKI + H2O

A reaction occurs when aqueous solutions of potassium hydroxide and hydroiodic acid are combined.

HI + KOHKI + H2O Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. In this case the equation is already balanced with all coefficients equal to unity. HI + KOHKI + H2O

Write a balanced equation for the double-replacement neutralization reaction described, using the smallest possible integer coefficients. A reaction occurs when aqueous solutions of sodium hydroxide and hydroiodic acid are combined.

HI + NaOHNaI + H2O

A reaction occurs when aqueous solutions of sodium hydroxide and hydroiodic acid are combined.

HI + NaOHNaI + H2O Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. In this case the equation is already balanced with all coefficients equal to unity. HI + NaOHNaI + H2O

Identify the Brønsted acid(s) in the reaction. HIO3(aq) + H2O (l) H3O+ (aq) + IO3- (aq)

HIO3 and H3O+

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. NO2- + CH3COOH HNO2 (aq) + CH3COO- The formula for the conjugat NO2- The formula for the conjugat CH3COOH NO2- base CH3COOH acid HNO2 acid CH3COO- base

HNO2 CH3COO-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. NO2- + HS- HNO2 (aq) + S-2 The formula for the conjugate of NO2- is The formula for the conjugate of HS- is NO2- is a base HS- is an acid HNO2 is a acid S2- is a base

HNO2 S2-

A buffer solution that is 0.307 M in HNO2 and 0.307 M in KNO2 has a pH of 3.35. Addition of which of the following would increase the capacity of the buffer for added OH-?

HNO2 both HNO2 and KNO2

A reaction occurs when aqueous solutions of barium hydroxide and nitric acid are combined

HNO3 + Ba(OH)2Ba(NO3)2 + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. 2HNO3 + Ba(OH)2Ba(NO3)2 + 2H2O

A reaction occurs when aqueous solutions of barium hydroxide and nitric acid are combined.

HNO3 + Ba(OH)2Ba(NO3)2 + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. 2HNO3 + Ba(OH)2Ba(NO3)2 + 2H2O

Which one of the following chemical equations illustrate the ionization of nitric acid , HNO3 , when it dissolves in water?

HNO3 + H2O H3O+ + NO3-

Which one of the following combinations cannot produce a buffer solution? All of these will produce a buffer solution. HF and KF HNO3 and NaNO3 NH3 and NH4Cl HNO2 and NaNO2

HNO3 and NaNO3

Write a net ionic equation to show that carbonic acid, H2CO3, behaves as an acid in water. Consider only its first ionization.

In this case, H2CO3 donates a proton to H2O to form HCO3- and H3O+. H2CO3 (aq) + H2O (l)___>----->HCO3- (aq) + H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion. H2CO3 is a diprotic acid because it has 2 ionizable protons. This is indicated by the two H atoms at the beginning of its formula .

Write a net ionic equation to show that sulfurous acid, H2SO3, behaves as an acid in water. Consider only its first ionization.

In this case, H2SO3 donates a proton to H2O to form HSO3- and H3O+. H2SO3 (aq) + H2O (l) = HSO3- (aq) + H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion. H2SO3 is a diprotic acid because it has 2 ionizable protons. This is indicated by the two H atoms at the beginning of its formula .

Write a net ionic equation to show that hydrofluoric acid , HF , behaves as an acid in water.

In this case, HF donates a proton to H2O to form F- and H3O+. HF(aq)+H2O (l) ___>----> F-(aq) + H3O+ (aq) The double arrow in the equation indicates that the reaction does not go to completion.

Write a net ionic equation to show that hydroiodic acid, HI, behaves as an acid in water.

In this case, HI donates a proton to H2O to form I- and H3O+. HI (aq) + H2O (l)----> I- (aq) + H3O+ (aq) The single arrow to the right in the equation indicates that the reaction goes essentially to completion.

The substance trimethylamine is a weak nitrogenous base like ammonia. Complete the following equation that shows how trimethylamine reacts when dissolved in water.

In this case, trimethylamine acts as a Bronsted-Lowry base . The nitrogen atom accepts a proton from H2O to form the trimethylammonium ion and OH-. H2O + OH

What is the formula of the compound in which the atom combining ratios are: potassium : oxygen = 2 : 1

K2O

A buffer solution that is 0.410 M in HF and 0.410 M in KF has a pH of 3.14. Addition of which of the following would increase the capacity of the buffer for added H3O+?

KF both HF and KF

Which of the following substances could behave as an Arrhenius base? Na2CO3 Na3PO4 K2S KOH

KOH

Write a net ionic equation to show why solid potassium hydroxide, KOH (s), forms a basic solution when it dissolves in water.

KOH (s)----->K+ (aq) + OH- (aq) The single arrow in the equation indicates that the reaction goes essentially to completion.

The compound potassium hydroxide, KOH is soluble in water. Write the net ionic equation for the dissociation reaction that occurs when solid potassium hydroxide dissolves in water:

KOH(s)----->K+(aq) + OH-(aq)

Write the correct acid ionization constant expression for aqueous hypochlorous acid.

Ka = [H3O+] [ClO-] [H2O] [HClO]

Write the correct acid ionization constant expression for aqueous hypochlorous acid.

Ka = [H3O+] [ClO-] [HClO]

The expression for the Ka of the weak acid HF would be which of the following?

Ka= [F-][H+]/[HF]

Write the equilibrium constant expression for NaCN acting as a base.

Kb = [OH- ] [HCN] [CN- ]

Write the equilibrium constant expression, Kc, for the following reaction: If either the numerator or denominator is blank, please enter 1 2SO2(g) + O2(g) 2SO3(g)

Kc = [SO3]2 [SO2]2 [O2]

Write the correct acid ionization constant expression for aqueous acetic acid.

Kp = [H3O+] [C2H3O2-] [H3O+] [C2H3O2-]

In pure water at 25 °C, [H3O+] = [OH-] = 1.0 10-7M and the following relationship is true:

Kw = [H3O+][OH-] = 1.0 x 10^-14; where Kw is called the ionization constant for the water equilibrium.

Click on an element within the alkali metal group

Li

Write a net ionic equation to show why solid lithium hydroxide, LiOH (s), forms a basic solution when it dissolves in water.

LiOH (s)-------> Li+ (aq) + OH- (aq)

Which technique of medical investigation presents no ionizing radiation risk to the patient?

MRI

What is the formula of the compound in which the atom combining ratios are: magnesium : bromine = 1 : 2

MgBr2

What is the formula of the compound in which the atom combining ratios are: magnesium : sulfur = 1 : 1

MgS

Classify each of the following as either a pure substance or a mixture: salad dressing ethyl alcohol vodka

Mix pure pure

Which of the following consists of a stream of charged particles? Alpha rays Gamma rays Beta rays More than one response is correct.

More than one response is correct.

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: N2 (g) + O2 (g) NO (g)

N2 (g) + O2 (g) 2NO (g)

Write a net ionic equation to show how ammonia behaves as a base in water.

NH3 (aq) + H2O (l)---->___> NH4+ (aq) + OH- (aq) double arrow

Write a net ionic equation to show how ammonia behaves as a base in water.

NH3(aq) + H2O(l) (double arrows) NH4+ + OH-

Write the net ionic equation for the equilibrium that is established when ammonium bromide is dissolved in water.

NH4+(aq) + H2O H3O+(aq) + NH3(aq) will be acidic

Write the net ionic equation for the equilibrium that is established when ammonium bromide is dissolved in water

NH4+(aq) + H2O H3O+(aq) + NH3(aq) acidic

Write the net ionic equation for the equilibrium that is established when ammonium chloride is dissolved in water

NH4+(aq) + H2O H3O+(aq) + NH3(aq) acidic

Write the net ionic equation for the equilibrium that is established when ammonium chloride is dissolved in water.

NH4+(aq) + H2O H3O+(aq) + NH3(aq) acidic

Write the net ionic equation for the equilibrium that is established when ammonium iodide is dissolved in water

NH4+(aq) + H2O H3O+(aq) + NH3(aq) acidic

Write the net ionic equation for the equilibrium that is established when ammonium iodide is dissolved in water.

NH4+(aq) + H2O H3O+(aq) + NH3(aq) acidic

Write the net ionic equation for the equilibrium that is established when ammonium nitrate is dissolved in water.

NH4+(aq) + H2O H3O+(aq) + NH3(aq) acidic

Write the net ionic equation for the equilibrium that is established when ammonium perchlorate is dissolved in water

NH4+(aq) + H2O H3O+(aq) + NH3(aq) acidic

Write the net ionic equation for the equilibrium that is established when ammonium perchlorate is dissolved in water.

NH4+(aq) + H2O H3O+(aq) + NH3(aq) acidic

write the net ionic equation for the equilibrium that is established when ammonium bromide is dissolved in water

NH4+(aq) + H2O H3O+(aq) + NH3(aq) acidic

The compound ammonium bromide, NH4Br is soluble in water. Write the net ionic equation for the dissociation reaction that occurs when solid ammonium bromide dissolves in water: Use the pull-down boxes to specify states such as (aq) or (s).

NH4Br(s)NH4+(aq) + Br-(aq)

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: NH4NO2 (aq) N2 (g) + H2O (l)

NH4NO2 (aq) N2 (g) + 2H2O (l)

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: NH4NO3 (aq) N2O (g) + H2O (l)

NH4NO3 (aq) N2O (g) + 2H2O (l)

Buffer solutions:

NH4NO3 + NH3 HNO2 + NaNO2 CH3COOH + 0.10 M CH3COO NH4NO3 + 0.35 M NH3 HCN + 0.17 M KCN CH3COOH + 0.29 M CH3COOK HNO2 + 0.20 M KNO2 NH4NO3 + 0.33 M NH3 HF + 0.22 M KF HNO2 + 0.14 M KNO2 NH4NO3 + 0.38 M NH3 HCN + 0.23 M NaCN HF + 0.18 M KF HCN + 0.28 M NaCN CH3COOH + 0.19 M CH3COO NH4Br + 0.35 M NH3 NH4Br + 0.38 M NH3 HClO + 0.26 M KClO HCN + 0.11 M NaCN CH3COOH + 0.22 M CH3COOK NH4Br + 0.33 M NH3 0.15 M HClO + 0.15 M NaClO 0.29 M NH4Br + 0.37 M NH3 0.36 M HClO + 0.26 M NaClO 0.11 M HNO2 + 0.10 M KNO2 0.11 M HCN + 0.20 M NaCN 0.30 M HClO + 0.22 M KClO 0.27 M NH4NO3 + 0.40 M NH3 0.13 M HClO + 0.17 M KClO 0.28 M NH4Br + 0.36 M NH3 0.21 M HClO + 0.13 M KClO 0.40 M CH3COOH + 0.23 M CH3COOK 0.35 M NH4Br + 0.34 M NH3 0.40 M HCN + 0.26 M KCN 0.21 M HClO + 0.13 M NaClO 0.31 M CH3COOH + 0.29 M CH3COONa HCN + 0.12 M KCN HNO2 + KNO2 HClO + 0.23 M NaClO HF + 0.22 M NaF NH4Br + 0.32 M NH3 HCN + 0.18 M NaCN HF + 0.24 M KF

What is the formula of the compound in which the atom combining ratios are: nitrogen : oxygen = 1 : 2

NO2

Write the net ionic equation for the equilibrium that is established when sodium nitrite is dissolved in water.

NO2-(aq) + H2O HNO2(aq) + OH -(aq) BASIC

Write the net ionic equation for the equilibrium that is established when calcium nitrite is dissolved in water

NO2-(aq) + H2O HNO2(aq) + OH -(aq) basic

Write the net ionic equation for the equilibrium that is established when sodium nitrite is dissolved in water

NO2-(aq) + H2O HNO2(aq) + OH -(aq) basic

Which of the following salts will produce a basic solution when it is dissolved in water?

NaCN

When solid sodium hydroxide is dissolved in water which of the following species is NOT present in the solution?

NaOH

Write a net ionic equation to show why solid sodium hydroxide, NaOH (s), forms a basic solution when it dissolves in water.

NaOH (s)----->Na+ (aq) + OH- (aq)

Which of the following occurs when NaOH is dissolved in water to form a basic solution?

NaOH breaks up to form Na + (aq) and OH - (aq)

Write a net ionic equation to show why solid sodium hydroxide, NaOH (s), forms a basic solution when it dissolves in water.

NaOH is a strong base. When the solid dissolves, it dissociates completely into the hydrated ions Na+ (aq) and OH- (aq). NaOH (s)----->Na+ (aq) + OH- (aq) The single arrow in the equation indicates that the reaction goes essentially to completion.

Classify each of the following properties as chemical or physical: conductivity of a metal flammability acidity

P C C

Classify each of the following changes as chemical or physical: melting wax adding antifreeze to a car radiator baking bread flammability conductivity of a metal resistance to corrosion

P P C C P P

What is the formula of the compound in which the atom combining ratios are: phosphorus : nitrogen : fluorine = 1 : 1 : 2

PNF2

What is the formula of the compound in which the atom combining ratios are: phosphorus : nitrogen : iodine = 1 : 1 : 2

PNI2

Select the major source of radiation absorbed by most people

Radon emission

Consider the following system at equilibrium at 298 K: 2NO(g) N2(g) + O2(g) If the PRESSURE of the equilibrium system is suddenly increased at constant temperature:

Remain the same. Already at equilibrium Remain the same

Which of the following are transuranium elements?

Rf Pu Hs Cm Lr Sg Bk Bh Es Fm Am Md Mt

Consider the following system at equilibrium at 298 K: 2NO(g) double arrow N2(g) + O2(g) + 43.2 kcal If the TEMPERATURE on the equilibrium system is suddenly decreased:

Run in the forward direction to restablish equilibrium increase

Consider the following system at equilibrium at 1150 K: 2SO3(g) 2SO2(g) + O2(g) When some SO2(g) is added to the equilibrium system at constant temperature:

Run in the reverse direction to restablish equilibrium DECREASE

What is the formula of the compound in which the atom combining ratios are: sulfur : chlorine = 1 : 2

SCl2

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: SO2 (g) + H2O (l) H2SO3 (g)

SO2 (g) + H2O (l) H2SO3 (g)

What is the formula of the compound in which the atom combining ratios are: sulfur : oxygen = 1 : 3

SO3

The formula for the conjugate base of HSO3- is

SO3 2-

What is the formula of the compound in which the atom combining ratios are: sulfur : oxygen : chlorine = 1 : 1 : 2

SOCl2

What is the formula of the compound in which the atom combining ratios are: silicon : bromine : iodine = 1 : 2 : 2

SiBr2I2

What is the formula of the compound in which the atom combining ratios are: silicon : chlorine : bromine = 1 : 2 : 2

SiCl2Br2

What is the formula of the compound in which the atom combining ratios are: silicon : oxygen = 1 : 2

SiO2

What is the formula of the compound in which the atom combining ratios are: silicon : oxygen = 1 : 2 Enter elements in the order given:

SiO2

Write formulas for the major species in the water solution of each compound. HI

Strong electrolyte, H3O+, I-

Write formulas for the major species in the water solution of each compound. HNO3

Strong electrolyte, H3O, NO-

Based on your calculations, indicate whether each statement is True (T) or False (F): 1. Each experiment started with a different initial concentration of N2O4. 2. The ratio ([NO2] / [N2O4]) is equal to a constant value. 3. The ratio (2 [NO2] / [N2O4]) is equal to a constant value. 4. The ratio ([NO2]2 / [N2O4]) is equal to a constant value. 5. Each experiment reached a different set of equilibrium concentrations.

T F F T T

According to the Brønsted Theory, a conjugate pair is composed of a Brønsted acid and a Brønsted base.

TRU

According to the Brønsted Theory, a conjugate pair is composed of a Brønsted acid and a Brønsted base. True False

TRU

Ionizing radiation produced fee radicals in living tissue

TRU

The salt of a strong acid and a weak base will give an acidic solution.

TRU

What radionuclide is used extensively in medical diagnosis?

Technetium-99m

Select the isotope used for medical diagnosis

Thallium-201

The following Lewis diagram represents the valence electron configuration of a main-group element. If this element is in period 2, its valence electron configuration is * the lewis diagram has 8 dots

The Lewis diagram shows 8 valence electrons, and represents a valence electron configuration of the type ns2np6. In period 2, n = 2 and the valence electron configuration is 2s22p6

For the following equilibrium system, K = 7.50×104 at 298K. H3PO4(aq) + HS-(aq)H2PO4-(aq) + H2S(aq) Assuming that you start with equal concentrations of H3PO4 and HS-, and that no H2PO4- or H2S is initially present, which of the following best describes the equilibrium system?

The forward reaction is favored at equilibrium

Uranium-235, under the proper circumstances, will undergo nuclear decay releasing 3 high speed neutrons in the process

The neutrons released can cause a chain reaction with other U-235 atoms

barium chloride

The pH will be approximately equal to 7

calcium iodide

The pH will be approximately equal to 7

calcium chloride

The pH will be approximately equal to 7.

calcium perchlorate

The pH will be approximately equal to 7.

potassium bromide

The pH will be approximately equal to 7.

potassium perchlorate

The pH will be approximately equal to 7.

sodium bromide

The pH will be approximately equal to 7.

barium fluoride

The pH will be greater than 7.

calcium cyanide

The pH will be greater than 7.

calcium fluoride

The pH will be greater than 7.

potassium nitrite

The pH will be greater than 7.

sodium hypochlorite

The pH will be greater than 7.

ammonium bromide

The pH will be less than 7.

ammonium iodide

The pH will be less than 7.

ammonium nitrate

The pH will be less than 7.

ammonium perchlorate

The pH will be less than 7.

Which of the following is characteristic of a buffer?

The pH will go down very slightly when H3O+ is added to a buffer.

Which of the following is characteristic of a buffer?

The pH will go up very slightly when OH- is added to the buffer.

A reaction occurs when aqueous solutions of carbonic acid and sodium hydroxide are combined. Assume excess base.

Translate the sentence into a chemical equation: H2CO3 + NaOH Na2CO3 + H2O not balanced Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. H2CO3 + 2NaOH Na2CO3 + 2H2O

A reaction occurs when aqueous solutions of potassium hydroxide and hydrobromic acid are combined.

Translate the sentence into a chemical equation: HBr + KOHKBr + H2O Then place a coefficient in front of one or more of the formulas, as necessary, to balance the equation. In this case the equation is already balanced with all coefficients equal to unity. HBr + KOHKBr + H2O

Click on an actinide element

U

Choose the best definition of the equivalence point of a titration.

When the stoichiometric amount of titrant has been added

Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N2O4 is colorless. This reaction is: A. Exothermic

When the temperature is increased the equilibrium constant K decreases When the temperature is increased the equilibrium concentration of N2O4 decreases

(NH2)2CO (s) (NH2)2CO (aq)

Would not cause the bulb to light.

C3H7OH (l) C3H7OH (aq)

Would not cause the bulb to light.

C4H9OH (l) C4H9OH (aq)

Would not cause the bulb to light.

C6H12O6 (s) C6H12O6 (aq)

Would not cause the bulb to light.

CH3OH (l) CH3OH (aq)

Would not cause the bulb to light.

Ca(ClO4)2 (s) Ca2+(aq) + 2ClO4-(aq)

Would produce a bright light.

HBr (g) + H2O (l) H3O+(aq) + Br-(aq)

Would produce a bright light.

The behaviors of four different solutes when dissolved in water are indicated by the four equations below. Match each of the resulting solutions to its expected behavior in a conductance apparatus like the one shown to the left, if the solute is present at a concentration of 0.2 M. HClO4 (l) + H2O (l) H3O+(aq) + ClO4-(aq)

Would produce a bright light.

HCOOH (aq) + H2O (l) H3O+(aq) + HCOO-(aq)

Would produce a dim light.

HClO (aq) + H2O (l) H3O+(aq) + ClO-(aq)

Would produce a dim light.

The behaviors of four different solutes when dissolved in water are indicated by the four equations below. Match each of the resulting solutions to its expected behavior in a conductance apparatus like the one shown to the left, if the solute is present at a concentration of 0.2 M. C6H5COOH (aq) + H2O (l) H3O+(aq) + C6H5COO-(aq)

Would produce a dim light.

1s22s1

X with 1 dot

The following Lewis diagram represents the valence electron configuration of a main-group element

X with 2 dots 2A cation +2 If X is in period 3 , the ion formed has the same electron configuration as the noble gas

1s22s22p63s23p1

X with 3 dots

1s22s22p63s23p64s23d104p1

X with 3 dots

1s22s22p63s23p6

X with 8 dots

Write a balanced chemical equation for the reaction of zinc carbonate with nitric acid.

ZnCO3(s) + 2 HNO3(aq) → Zn(NO3)2(aq) + H2O(l) + CO2(g)

The compound dimethylamine, (CH3)2NH, is a weak base when dissolved in water. Write the Kb expression for the weak base equilibrium that occurs in an aqueous solution of dimethylamine:

[(CH3)2NH2+] [OH-]/[(CH3)2NH]

The compound trimethylamine, (CH3)3N, is a weak base when dissolved in water. Write the Kb expression for the weak base equilibrium that occurs in an aqueous solution of trimethylamine:

[(CH3)3NH+] [OH-]/[(CH3)3N]

The compound methylamine, CH3NH2, is a weak base when dissolved in water. Write the Kb expression for the weak base equilibrium that occurs in an aqueous solution of methylamine:

[CH3NH3+] [OH-]/[CH3NH2]

Write the correct acid ionization constant expression for aqueous chlorous acid.

[H3O+] [ClO2-] Ka = [HClO2]

write the correct acid ionization constant expression for aqueous nitrous acid.

[H3O+] [NO2-] Ka = [HNO2]

Write the Ka expression for an aqueous solution of acetic acid:

[H3O+][C2H3O2-]/[CH3COOH]

The compound ammonia, NH3, is a weak base when dissolved in water. Write the Kb expression for the weak base equilibrium that occurs in an aqueous solution of ammonia:

[NH4+] [OH-]/[NH3]

Write the Ka expression for an aqueous solution of hydrocyanic acid:

[h3o+][[cn-]/[hcn]

Write the Ka expression for an aqueous solution of hypochlorous acid:

[h3o+][clo-]/[hclo]

Write the Ka expression for an aqueous solution of nitrous acid:

[h3o+][no2-]/[hno2]

Choose the conjugate acid-base pair that would yield a good buffer at pH 3.35. Acid K a HNO2 4.5×10-4 HF 7.2×10-4 HClO 3.5×10-8 NH4+ 5.6×10-10 a. HNO2 / NO2- b. NH4+ / NH3 c. HClO- / ClO- d. HF / F-

a

Choose the pair that constitutes a conjugate acid-base pair. C3H7OH / C3H7O- H2NCH2CH2CO2H / H3NCH2CH2CO2 CH3CH2CH2Cl / CH3CH2CH2- CH3NH2 / CH3CH2NH2

a

Listed below are four weak acids and their ionization constants.Which acid has the greatest acid strength (the strongest acid)? A.cyanic acid, HOCN, Ka = 3.5 x 10-4 B.lactic acid, HC3H5O3, Ka = 1.4 x 10-4 C.hydrocyanic, HCN, Ka = 6.2 x 10-10 D.acetic acid, CH3COOH, Ka = 1.8 x 10-5

a

Which of the following IS the conjugate acid of HPO42- A. H2PO4- B. PO43- C. H3O+ D. H3PO4

a

Choose the pair that constitutes a conjugate acid-base pair. HClO2 / ClO2- HNO3 / H3O+ C2H6 / C2H5OH H2O / NH3

a. HClO2 / ClO2-

Which of the following salts will produce a basic solution when it is dissolved in water? a. KNO2 b. NaNO3 c. NaCl d. KI e. KClO4

a. KNO2

Which of the following correctly arranges 1.00 M solutions of the strong electrolytes in order of increasing boiling point (lowest to highest)? a. NaNO3 < Mg(NO3)2 < Al(NO3)3 b. Al(NO3)3 < Mg(NO3)2 < NaNO3 c. Mg(NO3)2 < Al(NO3)3 < NaNO3 d. All have the same boiling point.

a. NaNO3 < Mg(NO3)2 < Al(NO3)3

The hydroxide concentration in an aqueous solution is 3.5x10-2 M.

a. The hydronium ion concentration is: 2.86x10^-13M b. The pH of this solution is: 12.54 c. The pOH is: 1.46

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CH3COOH + S2- CH3COO- + HS-

acid base base acid CH3COO- HS-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CH3COOH + HPO42- CH3COO- + H2PO4-

acid base base acid CH3COO- H2PO4-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HCN (aq) + S2- CN- + HS-

acid base base acid CN- HS-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HF (aq) + HPO42- F- + H2PO4-

acid base base acid F- H2PO4-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. H2CO3 (aq) + NO2- HCO3- + HNO2 (aq)

acid base base acid HCO3- HNO2

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. H2S (aq) + H2PO4- HS- + H3PO4 (aq)

acid base base acid HS- H3PO4

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. H2S (aq) + ClO- HS- + HClO

acid base base acid HS- HClO

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HNO2 (aq) + H2PO4- NO2- + H3PO4 (aq)

acid base base acid NO2- H3PO4

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HNO2 (aq) + CO32- NO2- + HCO3-

acid base base acid NO2- HCO3-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HNO2 (aq) + SO32- NO2- + HSO3-

acid base base acid NO2- HSO3-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CH3COOH + SO32- CH3COO- + HSO3-

acid, base base acid The formula for the conjugate of CH3COOH is CH3COO- The formula for the conjugate of SO32- is HSO3-

What are some of the symptoms of radiation sickness? Hemorrhage Anemia Nausea All

all

What type(s) of intermolecular forces are expected between CH3CH2CH2CH2CH2OH molecules?

all

Transmutation is caused by which of the following radioactive processes?

alpha

Arrange the following elements in order of increasing electronegativity: silicon, phosphorus, aluminum, sulfur

aluminum silicon phosphorus sulfur

Complete the following for the compound aluminum carbonate. formula = Al2(CO3)3

aluminum 2 carbon 3 oxygen 9

Complete the following for the compound aluminum sulfite. formula = Al2(SO3)3

aluminum: 2 sulfur: 3 oxygen: 9

Complete the following for the compound aluminum chromate. formula = Al2(CrO4)3

aluminum: 2 chromium: 3 oxygen: 12

Arrange the following elements in order of increasing electronegativity: iodine, bromine, astatine, chlorine

astatine iodine bromine chlorine

How many meq are contained in 25.00 mL of a 0.225 M solution of CaCl2? a. 1.12 × 10-2 meq b. 1.12 × 101 meq c. 2.81 meq d. 5.62 × 10-3 meq

b

In a buffer solution made up of equal concentrations of acetic acid and sodium acetate, NaC2H3O2, which component is used to buffer against added OH−? a. OH− b. HC2H3O2 c. Na+ d. C2H3O2

b

Which of the following mixtures would represent a buffer? Sodium sulfate/Sulfuric acid Sodium formate/Formic acid Sodium chloride/Hydrochloric acid

b

Which of the following reaction is a Bronsted-Lowry acid-base reaction? 2 HNO3(aq) + Zn(s) Zn(NO3)2(aq) + H2(g) NH4+(aq) + H2O(l) NH3(aq) + H3O+(aq) Cu2+(aq) + 4 F-(aq) CuF42-(aq) 2 Cu+(aq) Cu(s) + Cu2+(aq) NaCl(s) Na+(aq) + Cl-(aq)

b

Which of the following is a diprotic acid? a. HCl b. H2SO4 c. H3PO4 d. HNO3

b. H2SO4

Identify the Brønsted acid(s) in the reaction. HIO3(aq) + H2O (l) H3O+ (aq) + IO3- (aq) HIO3 HIO3 and H3O+ H2O H2O and HIO3

b. HIO3 and H3O+

Listed below are four weak acids and their ionization constants in alphabetical order. Which acid has the greatest acid strength (the strongest acid)? a. hydrocyanic acid, HCN, Ka = 6.2 x 10-10 b. hydrofluoric acid, HF, Ka = 7.2 x 10-4 c. lactic acid, HC3H5O3, Ka = 1.4 x 10-4 d. benzoic acid, C6H5COOH, Ka = 6.3 x 10-5

b. hydrofluoric acid, HF, Ka = 7.2 x 10-4

Listed below are four weak acids and their ionization constants. Which acid has the greatest acid strength (the strongest acid)? a. hydrocyanic, HCN, Ka = 6.2 x 10-10 b. hydrofluoric acid, HF, Ka = 7.2 x 10-4 c. lactic acid, HC3H5O3, Ka = 1.4 x 10-4 d. benzoic acid, C6H5COOH, Ka = 6.3 x 10-5

b. hydrofluoric acid, HF, Ka = 7.2 x 10-4

When the nuclide cesium-137 undergoes beta decay:

barium 137 Ba 56

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CH3COO- + H2SO3 (aq) CH3COOH + HSO3-

base acid acid base CH3COOH HSO3-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CH3COO- + HSO3- CH3COOH + SO32-

base acid acid base CH3COOH SO32-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HS- + H2CO3 (aq) H2S (aq) + HCO3-

base acid acid base H2S HCO3-.

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HSO3- + H2CO3 (aq) H2SO3 (aq) + HCO3-

base acid acid base H2SO3 HCO3-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HSO3- + H2S (aq) H2SO3 (aq) + HS-

base acid acid base H2SO3 HS-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CN- + H2PO4- HCN (aq) + HPO42-

base acid acid base HCN HPO42-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CN- + HCO3- HCN (aq) + CO32-

base acid acid base HCN CO32-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. NO2- + HS- HNO2 (aq) + S2-

base acid acid base HNO2 S2-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. NO2- + H2PO4- HNO2 (aq) + HPO42-

base acid acid base HNO2 HPO42-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base F-+HCO3- --->HF (aq)+CO32- The formula for the conjugate of F- is The formula for the conjugate of HCO3- is

base, acid acid, base HF CO32-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HS + HCN ---> H2S (aq)+CN- The formula for the conjugate HS is The formula for the conjugate HCN is

base, acid, acid, base H2S CN-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. CN+ HS---> HCN + S2 The formula for the conjugate of CN is The formula for the conjugate of HS is

base, acid, acid, base HCN S2-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. ClO-+HSO3- ----> HClO+SO32- The formula for the conjugate of ClO- is The formula for the conjugate of HSO3- is

base, acid, acid, base HClO SO32-

In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. NO2- + H2S (aq) HNO2 (aq) +HS- The formula for the conjugate of NO2- is The formula for the conjugate of H2S is

base, acid, acid, base HNO2 HS-

Arrange the following elements in order of increasing electronegativity: beryllium, nitrogen, carbon, boron

beryllium boron carbon nitrogen

Manganese can undergo several types of radioactive emission. In which type of decay does the following reaction occur?

beta

Which of the following radioactive processes does not result in transmutation?

beta

When the nuclide lead-214 undergoes beta decay:

bismuth 214 Bi 83

Arrange the following elements in order of increasing electronegativity: boron, oxygen, nitrogen, carbon

boron carbon nitrogen oxygen

Arrange the following elements in order of increasing electronegativity: carbon, nitrogen, boron, oxygen

boron carbon nitrogen oxygen

A buffer solution that is 0.472 M in CH3COOH and 0.472 M in CH3COO has a pH of 4.74. Addition of which of the following would increase the capacity of the buffer for added H3O+?

both CH3COOH and CH3COO CH3COO

A buffer solution that is 0.398 M in CH3COOH and 0.398 M in CH3COO has a pH of 4.74. Addition of which of the following would increase the capacity of the buffer for added OH-?

both CH3COOH and CH3COO CH3COOH

A buffer solution that is 0.377 M in HCN and 0.377 M in KCN has a pH of 9.40. Addition of which of the following would increase the capacity of the buffer for added OH-?

both HCN and KCN HCN

A buffer solution that is 0.354 M in HClO and 0.354 M in KClO has a pH of 7.46. Addition of which of the following would increase the capacity of the buffer for added OH-?

both HClO and KClO HClO

A buffer solution that is 0.437 M in HClO and 0.437 M in NaClO has a pH of 7.46. Addition of which of the following would increase the capacity of the buffer for added H3O+?

both HClO and NaClO NaClO

A buffer solution that is 0.351 M in HNO2 and 0.351 M in NaNO2 has a pH of 3.35. Addition of which of the following would increase the capacity of the buffer for added OH-?

both HNO2 and NaNO2 HNO2

A buffer solution that is 0.357 M in HNO2 and 0.357 M in NaNO2 has a pH of 3.35. Addition of which of the following would increase the capacity of the buffer for added OH-?

both HNO2 and NaNO2 HNO2

A buffer solution that is 0.458 M in HNO2 and 0.458 M in NaNO2 has a pH of 3.35. Addition of which of the following would increase the capacity of the buffer for added H3O+?

both HNO2 and NaNO2 NaNO2

HCN (AQ)

bronsten lowry acid

HF (AQ)

bronsten lowry acid

CN-

bronsten lowry base

F-

bronsten lowry base

Choose the pair that does not constitute a conjugate acid-base pair. A.HSO3- / SO32- B.OH- / H2O C.H2SO4 / SO42- D.CH3CO2H / CH3CO2-

c

For the titration of a weak acid, select the point in the titration at which the pH of the solution equals the pKa of the acid. A. When the indicator changes color B. When the pH of the solution no longer changes when additional base or acid has been added C. When half of the stoichiometric amount of titrant has been added D. When the stoichiometric amount of titrant has been added

c

In a buffer solution made up of equal concentrations of acetic acid and sodium acetate, NaC2H3O2, which component is used to buffer against added OH−? Na+ C2H3O2 HC2H3O2 OH−

c

The pH of a 0.336 M solution of the conjugate base, A-, of a weak acid, HA, is 11.30. What is the Kb for A-? A.7.5×10-23 B.6.7×10-4 C.1.2×10-5 D.5.0×10-12 E.1.5×10-1

c

Which of the following is the conjugate acid of HPO42- A. PO43- B. H3O+ C. H2PO4- D. H3PO4

c

Which of the following molecules or ions is amphiprotic? A.NH4+ B.HBr C.H2PO4- D.CO32- E.H3PO4

c

Which of the following molecules or ions is amphiprotic? CH3CO2- SO42- HC2O4- H3O+ H3PO4

c

Which of the following reaction is a Bronsted-Lowry acid-base reaction? NaCl(s) Na+(aq) + Cl-(aq) 2 HNO3(aq) + Zn(s) Zn(NO3)2(aq) + H2(g) F-(aq) + H2O(l) HF(aq) + OH-(aq) 2 NO2(g) N2O4(g) 2 Cu+(aq) Cu(s) + Cu2+(aq)

c

Which of the following species is not amphiprotic? A. HC3H2O4- B. HC4H4O4- C. C2H3O2-

c

Classify each of the following properties as chemical or physical: combustibility resistance to corrosion souring of milk burning charcoal in a grill grilling a steak basicity viscosity

c c c c c c p

Classify the underlined property as chemical or physical: A child gets a sunburn from staying too long in the sun. Plants use carbon dioxide from the air to produce oxygen. The purple crystalline solid potassium permanganate forms a purple solution when dissolved in water. The colorless liquid ethanol burns in air. The purple crystalline solid potassium permanganate forms a purple solution when dissolved in water. When aluminum foil is placed into liquid bromine a white solid forms. Silver is a shiny metal that has a density of 10.5 g/mL. The colorless liquid ethanol burns in air. Ether is a colorless liquid that boils at 35 °C. The colorless gas methane burns in air.

c c p c p c p c p c

Classify each of the following changes as chemical or physical: ripening of bananas salting highways lighting a candle

c p c

Which of the following mixtures would represent a buffer? a. Sodium sulfate/Sulfuric acid b. Sodium chloride/Hydrochloric acid c. Sodium formate/Formic acid d. none

c. Sodium formate/Formic acid

Arrange the following elements in order of increasing electronegativity: nitrogen, oxygen, carbon, fluorine

carbon nitrogen oxygen fluorine

Arrange the following elements in order of increasing electronegativity: carbon, fluorine, oxygen, nitrogen

carbon nitrogen oxygen fluorine

Arrange the following elements in order of increasing electronegativity: barium, thallium, cesium, lead

cesium barium thallium lead

Complete the following for the compound cobalt(III) sulfate. formula = Co2(SO4)3

cobalt 2 sulfur 3 oxygen 12

Complete the following for the compound cobalt(III) nitrate. formula = Co(NO3)3

cobalt: 1 nitrogen: 3 oxygen: 9

Complete the following for the compound copper(I) carbonate. formula = Cu2CO3

copper 2 carbon 1 oxygen 3

Complete the following for the compound copper(I) sulfate. formula = Cu2SO4

copper 2 sulfur 1 oxygen 4

Complete the following for the compound copper(I) sulfite. formula = Cu2SO3

copper: 2 sulfur:1 oxygen: 3

Which of the following buffers will have the lowest pH? A. a solution containing 0.10 M HC2H3O2 and 0.10 M NaC2H3O2 B. a solution containing 0.30 M HC2H3O2 and 0.30 M NaC2H3O2 C. a solution containing 0.20 M HC2H3O2 and 0.20 M NaC2H3O2 D. They all have the same pH.

d

Which of the following would you expect to be a weak electrolyte? Sodium acetate Water Acetic acid More than one answer is correct.

d

Which one of the following is a strong acid? A. nitrous acid, HNO2 B. hydrocyanic acid, HCN C. hypobromous acid, HOBr D. sulfuric acid, H2SO4 E. benzoic acid, HC7H5O2

d

Which one of these can serve as a Lewis base? A. NH4+ B. C2H6 C. CH4 D. H2O

d. H2O

Which one of the following combinations CANNOT produce a buffer solution? a. HF and KF b. NH3 and (NH4)2SO4 c. HC2H3O2 and NaC2H3O2 d. HNO3 and NaNO3 e. all

d. HNO3 and NaNO3

Which of the following species can be characterized as amphiprotic? A. HPO42- B. HCO3- C. H2O D. all of them

d. all

Which of the following species can be characterized as amphiprotic? a. HCO3- b. H2O c. HPO42- d. all

d. all

Which of the following would you expect to be a weak electrolyte? a. Sodium acetate b. Acetic acid c. Water d. More than one answer is correct.

d. more than one answer is correct

A buffer solution that is 0.375 M in HClO and 0.375 M in KClO has a pH of 7.46. (1) The addition of 0.01 mol of H3O+ to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added H3O+ could be increased by the addition of 0.114 mol

decrease slightly salt

A buffer solution that is 0.463 M in HNO2 and 0.463 M in KNO2 has a pH of 3.35. (1) The addition of 0.01 mol of H3O+ to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added H3O+ could be increased by the addition of 0.173 mol

decrease slightly salt

A buffer solution that is 0.370 M in HClO and 0.370 M in KClO has a pH of 7.46. (1) The addition of 0.01 mol of H3O+ to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added OH- could be increased by the addition of 0.141 mol

decrease slightly weak acid

A buffer solution that is 0.386 M in HNO2 and 0.386 M in NaNO2 has a pH of 3.35. (1) The addition of 0.01 mol of H3O+ to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added H3O+ could be increased by the addition of 0.126 mol

decreases slightly salt

Which of the following molecules or ions is amphiprotic? a. H3O+ b. SO42- c. H3PO4 d. CH3CO2- e. H2PO4-

e. H2PO4-

Choose the pair that does NOT constitute a conjugate acid-base pair. a. H3O+ / H2O b. CH3CO2H / CH3CO2- c. HCO3- / CO32- d. H2SO4 / SO42- e. they all constitute as a conjugate blah blah blah

e. all

Which of the following would be expected to be the most soluble in water? ethanol pentane hexanol

ethanol

Which of the following would be expected to be the most soluble in water? pentanol butane ethanol

ethanol

Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N2O4 is colorless. If we represent the equilibrium as:...N2O4(g) 2 NO2(g) We can conclude that:

exothermic When the temperature is decreased the equilibrium constant, K: decreases When the temperature is decreased the equilibrium concentration of NO2: decrease

The curie, becquerel and roentgen are all physical units of radiation

false

Consider the following system at equilibrium at 800 K: 2H2S(g) + 69.3 kcal2H2(g) + S2(g) If the TEMPERATURE on the equilibrium system is suddenly increased:

forward increase

Arrange the following elements in order of increasing electronegativity: germanium, arsenic, gallium, selenium

gallium germanium arsenic selenium

What is the most penetrating type of radiation?

gamma

The sample has no definite shape or volume.

gas

X with 3 dots

group 3A

X with 6 dots

group 6A

The substance N-cyclohexylaniline is a weak nitrogenous base like ammonia. Complete the following equation that shows how N-cyclohexylaniline reacts when dissolved in water.

h20 + oh-

The substance ethanamine is a weak nitrogenous base like ammonia. Complete the following equation that shows how ethanamine reacts when dissolved in water.

h20 + oh-

The substance piperidine is a weak nitrogenous base like ammonia. Complete the following equation that shows how piperidine reacts when dissolved in water.

h2o + oh-

1s22s22p63s23p4

has the X with 6 dots

1s22s22p63s23p64s23d104p65s24d105p4

has the X with 6 dots

1s22s22p63s23p64s23d104p65s24d105p6

has the X with 8 dots

When hydrogen chloride gas is dissolved in water which of the following species is not present in the solution?

hcl

One mole of the nonelectrolyte C6H12O6 dissolved in 1000 g H2O

highest freezing point

Classify each of the following mixtures as either homogeneous or heterogeneous: pewter gin mud

homo homo hetero

The species H + can be called which of the following?

hydrogen ion, or proton

What ion is produced when any hydrogen halide is dissolved in water?

hydronium ion, H3O+

The osmolarity of physiological saline solution is 0.30 osmol/L. Assuming that the cell membrane is not permeable to its ions, is a 2.99 % w/v solution of potassium phosphate, K3PO4, hypertonic, hypotonic or isotonic to red blood cells?

hypertonic

Physiological saline solution has an osmolarity of 0.30 osmol/L. An aqueous solution of ammonium chloride is made by dissoving 26.8 g NH4Cl in enough water to make a liter of solution. Assuming that the cell membrane is not permeable to its ions, is this NH4Cl solution hypertonic, hypotonic or isotonic to red blood cells? hypertonic- net flow of H2O out of cell crenation isotonic-no net flow of H2O no effect hypotonic- net flow of H2O into cell swelling and eventual hemolysis

hypertonic crenation

A buffer solution that is 0.344 M in HF and 0.344 M in NaF has a pH of 3.14. (1) The addition of 0.01 mol of OH- to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added H3O+ could be increased by the addition of 0.110 mol

increase slightly of the salt

A buffer solution that is 0.486 M in CH3COOH and 0.486 M in CH3COO has a pH of 4.74. (1) The addition of 0.01 mol of OH- to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added H3O+ could be increased by the addition of 0.163 mol

increase slightly of the salt

A buffer solution that is 0.475 M in HF and 0.475 M in KF has a pH of 3.14. (1) The addition of 0.01 mol of OH- to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added OH- could be increased by the addition of 0.189 mol

increase slightly of the weak acid

A buffer solution that is 0.388 M in HCN and 0.388 M in KCN has a pH of 9.40. (1) The addition of 0.01 mol of OH- to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added OH- could be increased by the addition of 0.122 mol .

increase slightly of weak acid

A buffer solution that is 0.388 M in HCN and 0.388 M in NaCN has a pH of 9.40. (1) The addition of 0.01 mol of OH- to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added H3O+ could be increased by the addition of 0.128 mol

increase slighty of the salt

A buffer solution that is 0.384 M in HClO and 0.384 M in KClO has a pH of 7.46. (1) The addition of 0.01 mol of OH- to 1.0 L of this buffer would cause the pH to . (2) The capacity of this buffer for added OH- could be increased by the addition of 0.129 mol

increased weak acid

Arrange the following elements in order of increasing electronegativity: gallium, aluminum, indium, boron

indium gallium aluminum boron

Which one of the following types of radiation is not an ionizing radiation?

infrared

One mole of the ionic compound CrSO4 dissolved in 1000 g H2O

intermediate freezing point

Arrange the following elements in order of increasing electronegativity: bromine, chlorine, iodine, fluorine

iodine bromine chlorine fluorine

Complete the following for the compound iron(III) sulfite. formula = Fe2(SO3)3

iron: 2 sulfur: 3 oxygen: 9

Which of the following characterizes a gamma ray?

is a product of natural radioactive decay is very-high-energy similar to X-rays is more penetrating than an alpha ray

Which of the following characterizes a beta ray?

is attracted to the positively charged plate in an electric field is composed of electrons is a product of natural radioactive decay carries a negative charge is composed of particles

When the nuclide thallium-209 undergoes beta decay:

lead 209 Pb 82

Arrange the following elements in order of increasing electronegativity: lead, astatine, polonium, bismuth (smallest to largest)

lead bismuth polonium astatine

Arrange the following elements in order of increasing electronegativity: bismuth, polonium, lead, astatine

lead bismuth polonium astatine

The sample is only slightly compressible.

liquid

One mole of the ionic compound CaBr2 dissolved in 1000 g H2O

lowest freezing point

Arrange the following elements in order of increasing electronegativity: magnesium, phosphorus, silicon, aluminum

magnesium aluminum silicon phosphorus

Complete the following for the compound magnesium phosphate. formula = Mg3(PO4)2

magnesium: 3 phosphorus: 2 oxygen: 8

(1) What is the element with an electron configuration of 1s22s22p63s23p64s23d5? (2) What is the element with an electron configuration of 1s22s22p63s23p64s23d104p6?

manganese krypton

When the nuclide chromium-56 undergoes beta decay

manganese 56 Mn 25

Complete the following for the compound manganese(II) phosphate. formula = Mn3(PO4)2

manganese: 3 phosphorus: 2 oxygen: 8

Converting between metric units is necessary to solve many chemistry problems. For practice, complete the following table.

millimeters meters centimeters 90 9.02x10^-2 9.02 1.16×104 11.6 1.16×103 cm 507 mm 0.507 m 50.7

When the nuclide carbon-14 undergoes beta decay:

nitrogen 14 N 7

Complete the following for the compound ammonium carbonate. formula = (NH4)2CO3

nitrogen: 2 hydrogen: 8 carbon: 1 oxygen: 3

Complete the following for the compound ammonium chromate. formula = (NH4)2CrO4

nitrogen: 2 hydrogen: 8 chromium: 1 oxygen: 4

Complete the following for the compound ammonium sulfite. formula = (NH4)2SO3

nitrogen: 2 hydrogen: 8 sulfur: 1 oxygen: 3

Complete the following for the compound ammonium phosphate. formula = (NH4)3PO4

nitrogen: 3 hydrogen: 12 phosphorus: 1 oxygen: 4

The pKa value for CH3COOH is 4.74. (1) Would a buffer prepared from CH3COOH and CH3COONa with a pH of 2.74 be considered to be an effective buffer? (2) A buffer in which the mole ratio of CH3COONa to CH3COOH is 1.9 has a pH of 5.03. [CH3COO-] = 1.9 [CH3COOH] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

no OH-

The pKa value for HCN is 9.40. (1) Would a buffer prepared from HCN and NaCN with a pH of 11.2 be considered to be an effective buffer? (2) A buffer in which the mole ratio of NaCN to HCN is 2.0 has a pH of 9.70. [CN-] = 2.0 [HCN] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

no added acid

The pKa value for HCN is 9.40. (1) Would a buffer prepared from HCN and NaCN with a pH of 7.40 be considered to be an effective buffer? (2) A buffer in which the mole ratio of NaCN to HCN is 2.1 has a pH of 9.73. [CN-] = 2.1 [HCN] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

no added acid

The pKa value for CH3COOH is 4.74. (1) Would a buffer prepared from CH3COOH and CH3COOK with a pH of 6.74 be considered to be an effective buffer? (2) A buffer in which the mole ratio of CH3COOK to CH3COOH is 0.41 has a pH of 4.35. [CH3COO-] = 0.41 [CH3COOH] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

no added base

The pKa value for CH3COOH is 4.74. (1) Would a buffer prepared from CH3COOH and CH3COOK with a pH of 2.94 be considered to be an effective buffer? (2) A buffer in which the mole ratio of CH3COOK to CH3COOH is 0.45 has a pH of 4.39. [CH3COO-] = 0.45 [CH3COOH] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

no base

What is the emission that is used to obtain an MRI? Alpha X-ray Beta None

none

Which of our senses can we use to detect nuclear radiation?

none nig watch out

C3H5(OH)3 (l) C3H5(OH)3(aq)

nonelectrolyte

C4H9OH (l) C4H9OH(aq)

nonelectrolyte

C6H12O6 (s) C6H12O6(aq)

nonelectrolyte

Write formulas for the major species in the water solution of each compound. (NH2)2CO (s) (NH2)2CO(aq)

nonelectrolyte

HOCH2CH2OH

nonelectrolyte HOCH2CH2OH (aq)

(NH2)2CO

nonelectrolyte, (NH2)2CO (aq)

Write formulas for the major species in the water solution of each compound. C3H7OH

nonelectrolyte, C3H7OH

Write formulas for the major species in the water solution of each compound. c3h7oh

nonelectrolyte, C3H7OH

C3H7OH

nonelectrolyte, C3H7OH (aq)

C6H12O6

nonelectrolyte, C6H12O6 (aq)

Which of the following would be expected to be the most soluble in water? propane propanol butane

not butanol

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: KHSO4 (aq) + KOH (aq) K2SO4 (aq) + H2O (l)

nothing changes

Nuclear power plants produce electricity by carefully controlling the process of

nuclear fission

In nuclear reactions, the principle change occurs in the

nucleus

Use the VSEPR model to predict the bond angles about each numbered atom.

number of regions 4 3 2 predicted angle 109.5° 120° 180°

To predict bond angles about an atom, count the regions For atom C1, the number of regions is 4 and the predicted angle is 109.5 degrees. For atom C2, the number of regions is 4 and the predicted angle is 109.5 degrees. For atom O3, the number of regions is 4 and the predicted angle is 109.5 degrees.

of electron density about it. Each unshared pair of electrons and each bonded atom counts as a region of electron density. number of regions predicted angle Region 4: 109.5° Region 3: 120° Region 2: 180°

Classify each of the following properties as chemical or physical: malleablilty stability conductivity of a metal flammability acidity

p c p c c

When the nuclide radon-222 undergoes alpha decay:

polonium 218 PO 84

Arrange the following elements in order of increasing electronegativity: tellurium, selenium, polonium, sulfur (smallest to largest)

polonium tellurium selenium sulfur

Arrange the following elements in order of increasing electronegativity: tellurium, selenium, polonium, sulfur

polonium tellurium selenium sulfur

Complete the following for the compound potassium carbonate. formula = K2CO3

potassium 2 carbon 1 oxygen 3

Complete the following for the compound potassium sulfate. formula = K2SO4

potassium: 2 sulfur: 1 oxygen: 4

The greatest threat posed by a nuclear (fission) power plant is:

release of radioactive isotopes when the molten core reaches the water table

Which of the following units quantifies the amount of biological damage caused by the absorption of radiation?

rem

Consider the following system at equilibrium at 600 K: COCl2(g) CO(g) + Cl2(g) When some CO(g) is added to the equilibrium system at constant temperature:

reverse The concentration of Cl2 will: decrease

Consider the following system at equilibrium at 698 K: 2HI(g) + 2.49 kcalH2(g) + I2(g) If the TEMPERATURE on the equilibrium system is suddenly decreased:

reverse decrease

Arrange the following elements in order of increasing electronegativity: strontium, indium, rubidium, tin

rubidium strontium indium tin

Arrange the following elements in order of increasing electronegativity: rubidium, tin, indium, strontium

rubidium strontium indium tin

Consider the following system at equilibrium at 600 K: COCl2(g) + 25.9 kcalCO(g) + Cl2(g) If the TEMPERATURE on the equilibrium system is suddenly increased:

run forward increase

At room temperature and pressure, classify each of the following macroscopic samples as solid, liquid or gas aluminum foil oil carbon dioxide

s l g

What is a desired characteristic of a diagnostic tracer?

short half life

Arrange the following elements in order of increasing electronegativity: silicon, chlorine, sulfur, phosphorus

silicon phosphorus sulfur chlorine

Complete the following for the compound silver sulfite. formula = Ag2SO3

silver 2 sulfur 1 oxygen 3

Complete the following for the compound silver carbonate. formula = Ag2CO3

silver: 2 carbon: 1 oxygen: 3

Complete the following for the compound silver chromate. formula = Ag2CrO4

silver: 2 chromium: 1 oxygen: 4

Arrange the following elements in order of increasing electronegativity: sodium, silicon, aluminum, magnesium

sodium magnesium aluminum silicon

Complete the following for the compound sodium carbonate. formula = Na2CO3

sodium 2 carbon 1 oxygen 3

Complete the following for the compound sodium phosphate. formula = Na3PO4

sodium 3 phosphorus 1 oxygen 4

Complete the following for the compound sodium sulfite. formula = Na2SO3

sodium: 2 sulfur: 1 oxygen: 3

Complete the following for the compound sodium sulfate. formula = Na2SO4

sodium: 2 sulfur: 1 oxygen: 4

The substance has a definite shape and a definite volume.

solid

HNO3 (l) + H2O(l) H3O+(aq) + NO3-(aq)

strong

HClO4

strong ACID

HBr

strong acid

HCL is a

strong acid

HClO4

strong acid

HI

strong acid

Ba(OH)2

strong base

KOH is a

strong base

LiOH

strong base

NaOH is a

strong base

Ca(OH)2 (s) Ca2+(aq) + 2OH-(aq)

strong electrolyte

HCl (g) + H2O(l) H3O+(aq) + Cl-(aq)

strong electrolyte

NaBr (s) Na+(aq) + Br-(aq)

strong electrolyte

BaCl2

strong electrolyte Ba2+(aq),Cl-(aq)

Ba(OH)2

strong electrolyte, Ba2+(aq),OH-(aq)

Write formulas for the major species in the water solution of each compound. bA(no3)2

strong electrolyte, Ba2+, NO3-

CaBr2

strong electrolyte, Ca2+(aq),Br-(aq)

HBr

strong electrolyte, H3O+(aq),Br-(aq)

HCl

strong electrolyte, H3O+(aq),Cl-(aq)

HClO4 HClO2 C3H7OH Ba(OH)2

strong electrolyte, H3O+(aq),ClO4-(aq) weak electrolyte, HClO2 (aq) nonelectrolyte, C3H7OH (aq) strong electrolyte, Ba2+(aq),OH-(aq)

NaNO3

strong electrolyte, Na+(aq),NO3-(aq)

Write formulas for the major species in the water solution of each compound. NaOH

strong electrolyte, Na+, oh-

Arrange the following elements in order of increasing electronegativity: strontium, antimony, tin, indium

strontium indium tin antimony

When the nuclide phosphorus-32 undergoes beta decay

sulfur 32 S 16

Arrange the following elements in order of increasing electronegativity: selenium, sulfur, tellurium, oxygen

tellurium selenium sulfur oxygen

The electron-pair geometry around the P atom in PO43- is

tetra 4 unshared pairs PO43- molecule is tetra

Use the following Lewis diagram for methyl acetate to answer the questions

tetra trigonal planar bent

The electron-pair geometry around the S atom in SCl2 is

tetrahedral 2 unshared pairs SCl2 molecule is bent

Arrange the following elements in order of increasing electronegativity: lead, bismuth, thallium, polonium

thallium lead bismuth polonium

If a nucleus decays by successive α, β, α, β emissions

the atomic number will decrease by two, and the mass number will decrease by eight

If a nucleus decays by successive α, β, β, α emissions

the atomic number will decrease by two, and the mass number will decrease by eight

If a nucleus decays by successive β, α, β emissions

the atomic number will not change, and the mass number will decrease by four

As given in the text, which of the following appears in the denominator of the fractional term of the Henderson-Hasselbalch equation?

the concentration of weak acid

The classification of an acid or base as weak or strong is based upon

the extent of dissociation of the acid or base.

When the nuclide thorium-230 undergoes alpha decay thorium-230= 230 Th 90

the product nuclide is radium-226= 226 Ra 88

Free radicals are dangerous because

they are substances that are missing some electrons and are extremely active chemically

When the nuclide uranium-234 undergoes alpha decay: The name of the product nuclide is The symbol for the product nuclide is

thorium 230 Th 90

Moderators are used

to slow down high-energy neutrons in chain reactions

The radioisotope radon-222 is a gas that is a health hazard because it can make its way into the house from the soil in which it is produced, be inhaled, and cause lung cancer.

true

A change in which of the following conditions would change the value of the half-life?

using a different isotope

Citric acid, a natural food preservative, accounts for the tartness of citrus fruits. It is shown below. About 730 g of this material can be dissolved in water, making a liter of solution. However, only about 1.5% of it dissociates. As such, it would be considered a _____. pseudoelectrolyte weak electrolyte strong electrolyte nonelectrolyte

weak

HC9H7O4(aq) + H2O(l) H3O+(aq) + C9H7O4-(aq)

weak

CH3COOH

weak acid

HCOOH

weak acid

HCOOH is a

weak acid

HClO is a

weak acid

HF is a

weak acid

HNO2

weak acid

(CH3)3N

weak base

C2H5NH2

weak base

C5H11N is a

weak base

C5H5N

weak base

C6H5NH2 is a

weak base

C9H7N

weak base

NH2OH is a

weak base

CH3COOH(aq) + H2O(l) H3O+(aq) + CH3COO-(aq)

weak electrolyte

HNO2(aq) + H2O(l) H3O+(aq) + NO2-(aq)

weak electrolyte

HCN

weak electrolyte HCN (aq)

Write formulas for the major species in the water solution of each compound. CH3COOH

weak electrolyte, CH3COOH

CH3COOH

weak electrolyte, CH3COOH (aq)

Write formulas for the major species in the water solution of each compound. HClO2

weak electrolyte, HCLO2

HClO

weak electrolyte, HClO (aq)

HNO2

weak electrolyte, HNO2 (aq)

The pKa value for CH3COOH is 4.74. (1) Would a buffer prepared from CH3COOH and CH3COONa with a pH of 4.24 be considered to be an effective buffer? (2) A buffer in which the mole ratio of CH3COONa to CH3COOH is 1.5 has a pH of 4.92. [CH3COO-] = 1.5 [CH3COOH] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

yes acid

The pKa value for HCN is 9.40. (1) Would a buffer prepared from HCN and NaCN with a pH of 8.90 be considered to be an effective buffer? (2) A buffer in which the mole ratio of NaCN to HCN is 1.8 has a pH of 9.65. [CN-] = 1.8 [HCN] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

yes acid

The pKa value for HClO is 7.46. (1) Would a buffer prepared from HClO and NaClO with a pH of 6.96 be considered to be an effective buffer? (2) A buffer in which the mole ratio of NaClO to HClO is 2.0 has a pH of 7.77. [ClO-] = 2.0 [HClO] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

yes added acid

The pKa value for HCN is 9.40. (1) Would a buffer prepared from HCN and NaCN with a pH of 8.90 be considered to be an effective buffer? (2) A buffer in which the mole ratio of NaCN to HCN is 0.62 has a pH of 9.19. [CN-] = 0.62 [HCN] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

yes added base

The pKa value for HCN is 9.40. (1) Would a buffer prepared from HCN and KCN with a pH of 8.90 be considered to be an effective buffer? (2) A buffer in which the mole ratio of KCN to HCN is 2.0 has a pH of 9.70. [CN-] = 2.0 [HCN] Would this buffer solution have a greater capacity for added acid (H3O+) or added base (OH-)?

yes acid