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 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 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
The element fluorine would be expected to form
1 covalent bond
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
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 0.033 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
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
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)
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
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
What is the pH of 7.7 × 10-3 M HF? The Ka for hydrofluoric acid is 7.2 × 10-4.
2.69
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)
The element phosphorus would be expected to form
3
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
The acid with the smallest pKa:
Acetic 1.8x10-5
What is the formula of the compound in which the atom combining ratios are: boron : fluorine = 1 : 3
BF3
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
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)
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
Click on a transition element
Fe
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+
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 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)
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
The weaker acid is: HCN HF
HCN
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
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.
Which one of the following chemical equations illustrate the ionization of hydrochloric acid , HCl , when it dissolves in water?
HCl + H2O H3O+ + Cl-
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 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
Identify the Brønsted acid(s) in the reaction. HIO3(aq) + H2O (l) H3O+ (aq) + IO3- (aq)
HIO3 and H3O+
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 the correct acid ionization constant expression for aqueous hypochlorous acid.
Ka = [H3O+] [ClO-] [H2O] [HClO]
The expression for the Ka of the weak acid HF would be which of the following?
Ka= [F-][H+]/[HF]
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.
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
Classify each of the following as either a pure substance or a mixture: salad dressing ethyl alcohol vodka
Mix pure pure
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 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
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 is characteristic of a buffer?
The pH will go up very slightly when OH- is added to the buffer.
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
1s22s1
X with 1 dot
1s22s22p63s23p1
X with 3 dots
Which of the following IS the conjugate acid of HPO42- A. H2PO4- B. PO43- C. H3O+ D. H3PO4
a
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
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
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
Which of the following species is not amphiprotic? A. HC3H2O4- B. HC4H4O4- C. C2H3O2-
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 species can be characterized as amphiprotic? A. HPO42- B. HCO3- C. H2O D. all of them
d. all
Complete the following for the compound potassium carbonate. formula = K2CO3
potassium 2 carbon 1 oxygen 3
Complete the following for the compound silver chromate. formula = Ag2CrO4
silver: 2 chromium: 1 oxygen: 4
HBr
strong electrolyte, H3O+(aq),Br-(aq)
HClO
weak electrolyte, HClO (aq)
An ion from a given element has 55 protons and 54 electrons
+1 cesium
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 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
What is the pH of 3.8 × 10-4 M HF? The Ka for hydrofluoric acid is 7.2 × 10-4.
...3.56
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 4s orbitals are there 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
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
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
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
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 0.24 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
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 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
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 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
Select the missing product of this reaction: 14 N + 1 n 1 H + ? 7 0 1
14 c 6
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
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
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+
(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
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
How many types of orbitals are there in the shell with n = 2 in an atom?
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
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 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
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 thorium-234 undergoes beta emission
234 Th 90 ----> 0 e -1 + 234 Pa 91
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)
How many protons can be lost by citric acid, H3C6H5O6?
3
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
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
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
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
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
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
Select the basic fusion reaction of the universe
4 1 H 4 He + 2 0 e 1 2 1
When 94.871 and 50.40 are multiplied, the answer should have
4 significant figure(s).
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
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
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
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
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
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
Calculate the pH of a 2.83E-2 M NaF solution (Kb = 1.4 x 10-11).
7.8
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
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
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
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
Choose the species that can act as a Lewis acid. a. Fe3+ b. CCl4 c. NH3 d. CH3CH2NH2
A. Fe3+
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-
Which salt shifts the pH when dissolved in water?
Al(NO3)3
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 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.
The stronger acid is AH2CO3 4.2×10-7 BH3PO4 7.5×10-3
B
What is the formula of the compound in which the atom combining ratios are: boron : hydrogen : chlorine = 4 : 9 : 1
B4H9Cl
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 )
What is the formula of the compound in which the atom combining ratios are: barium : chlorine = 1 : 2
BaCl2
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)
Classify each of the following changes as chemical or physical: digesting food removing nail polish freezing ice cream
C P P
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)
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)
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)
What is the formula of the compound in which the atom combining ratios are: carbon : hydrogen : oxygen = 3 : 8 : 3
C3H8O3
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 0.110 mol NaOH is added to 1.00 L of the buffer solution
CH3COOH + OH-CH3COO- + H2O
Choose the reaction that is responsible for the natural acidity of rain.
CO2(g) + 2 H2O(l) → H3O+(aq) + HCO3-(aq)
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 )
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
Click on a lanthanide element
Ce
Click on an element within the halogen group
Cl
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
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)
Which of these equations shows the net neutralization reaction between hydrobromic acid and sodium hydroxide ?
H+(aq) + OH-(aq) yields H2O(l)
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 )
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)
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
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.
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
Click on an element within the alkali metal group
Li
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
What is the formula of the compound in which the atom combining ratios are: nitrogen : oxygen = 1 : 2
NO2
When solid sodium hydroxide is dissolved in water which of the following species is NOT present in the solution?
NaOH
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
Select the major source of radiation absorbed by most people
Radon emission
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
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.
Click on an actinide element
U
(NH2)2CO (s) (NH2)2CO (aq)
Would not cause the bulb to light.
C3H7OH (l) C3H7OH (aq)
Would not cause the bulb to light.
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]
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
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
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-
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
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
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-
When the nuclide lead-214 undergoes beta decay:
bismuth 214 Bi 83
CN-
bronsten lowry base
F-
bronsten lowry base
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
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
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 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
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
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
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
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
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
When the nuclide thallium-209 undergoes beta decay:
lead 209 Pb 82
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
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
CH3OH (l) CH3OH(aq)
non
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
When the nuclide radon-222 undergoes alpha decay:
polonium 218 PO 84
Which of the following is not a nuclear reaction?
redox
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
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 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
HNO3 (l) + H2O(l) H3O+(aq) + NO3-(aq)
strong
HClO4
strong ACID
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
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
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
A change in which of the following conditions would change the value of the half-life?
using a different isotope
HC9H7O4(aq) + H2O(l) H3O+(aq) + C9H7O4-(aq)
weak
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 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 38 protons and 36 electrons
+2 strontium
An ion from a given element has 30 protons and 28 electrons
+2 zinc
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 ion from a given element has 26 protons and 23 electrons
+3 iron
An ion from a given element has 53 protons and 54 electrons
-1 iodine
An ion from a given element has 15 protons and 18 electrons
-3 phosphorus
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
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 orbitals are there in the shell with n = 1 in an atom?
1
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
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 0.66 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 0.49 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
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
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
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 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
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? (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
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 0.050 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
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
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
How many electrons, protons, and neutrons are there in an atom of 29Si?
14 protons 15 neutrons 14 electrons
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 25.3 days decay to 1.0% of its original value.
168 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 5 , the ion formed has the same electron configuration as the noble gas: rubidium Rb+
(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
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 sulfur atom? What is the complete ground state electron configuration for the zinc atom?
1s22s22p63s23p4 1s22s22p63s23p64s23d10
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
The element oxygen would be expected to form
2
The element selenium would be expected to form
2
The element sulfur would be expected to form
2
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 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
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
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
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 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
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
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
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
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-
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+
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 types of orbitals are there in the shell with n = 3 in an atom?
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
The element nitrogen would be expected to form
3 covalent bonds
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
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
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
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
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
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
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
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
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
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
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
Fill in the symbol for the missing particle in the following nuclear equation.
56 Cr 24 ----> 0 e -1 + 56 Mn 25
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
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
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 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
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
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 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
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
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
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
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.
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
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.
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)
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
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 = 5 : 8 : 1
B5H8Cl
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)
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 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
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)
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)
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 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
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)
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)
The acid with the smallest pOH in a 0.10 M aqueous solution is:
Carbonic 4.2x10-7
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
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 reaction is a Bronsted-Lowry acid-base reaction?
F-(aq) + H2O(l) HF(aq) + OH-(aq)
Gamma emissions can be stopped with the use of an electromagnetic field because of their dense charge and their mass.
FALSE
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
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 )
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 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
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 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 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
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 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 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
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
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 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
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-] [HClO]
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]
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
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.
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 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
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
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
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.
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
What is the formula of the compound in which the atom combining ratios are: phosphorus : nitrogen : iodine = 1 : 1 : 2
PNI2
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
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
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.
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
Choose the best definition of the equivalence point of a titration.
When the stoichiometric amount of titrant has been added
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.
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
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]
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
The decay of Pb to Bi occurs through the emission of
a positron
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 + 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-
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
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- + 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
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
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
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
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
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
Complete the following for the compound copper(I) sulfite. formula = Cu2SO3
copper: 2 sulfur:1 oxygen: 3
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
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
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
Arrange the following elements in order of increasing electronegativity: germanium, arsenic, gallium, selenium
gallium germanium arsenic selenium
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
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
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
HCN
is a weak acid
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
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
(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
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
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
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 sulfate. formula = K2SO4
potassium: 2 sulfur: 1 oxygen: 4
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
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
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
The substance has a definite shape and a definite volume.
solid
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)
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
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
The classification of an acid or base as weak or strong is based upon
the extent of dissociation of the acid or base.
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
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
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
HNO2
weak electrolyte, HNO2 (aq)
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