CHEM 1010 Final

Group I Cations; precipitated as _____; precipitating agent is _____.

-Ag+, Pb2+, Hg22+ (mercury (I) or mercurous) -Precipitated as chlorides (Cl-) -Precipitating agent: dil HCl

Group III Cations; Precipitated as and precipitating agent; Other group precipitated as and precipitating agent?

-Al3+, Fe2+, Fe3+, Cr3+, Co2+, Ni2+, Zn2+, Mn2+ -Al3+, Fe2+, Fe3+, Cr3+ are precipitated as hydroxides (OH-) •Precipitating agent of this subgroup: NH4Cl + NH4OH -Co2+, Ni2+, Zn2+, Mn2+ are precipitated as sulfides (S2-) •Precipitating agent of this subgroup: NH4Cl + NH4OH + (NH4)2S

Group IV Cations, precipitated as ___, Precipitating agent_____?

-Ba2+, Ca2+, Mg2+, Na+, K+, NH4+ -Ba2+, Ca2+, Mg2+ are precipitated as carbonates (CO32-) •Precipitating agent: NH4Cl + NH4OH + (NH4)2CO3

Group II Cations; Precipitated as ____; Precipitating agent is ____.

-Cu2+, Bi3+, Cd2+, Hg2+, Sb3+, Sn2+, Sn4+ -Precipitated as sulfides (S2-) -Precipitating agent: dil HCl + H2S

what is needed to drive an exchange (metathesis) reaction?

-formation of ppt -generation of gas -production of weak electrolyte -production of nonelectrolyte

What are the four factors affecting solubility?

1.The Common-Ion Effect 2.pH 3.The presence of a complexing agent 4.The temperature

Calculate the concentration of sulfide (S2-) ions in a saturated solution of bismuth(III) sulfide. The solubility product constant of Bi2S3 is 1.82 × 10-79. Show your work.

2.1 x 10-16 M

What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO3)2 (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant (Kf) for water is 1.86 °C/m. A) -3.34 B) -1.11 C) 3.34 D) 1.11 E) 0.00

A) -3.34

Calculate the maximum concentration (in M) of silver ions (Ag+) in a solution that contains 0.025 M of CO32-. The Ksp of Ag2CO3 is 8.1 × 10-12. A) 1.8 × 10-5 B) 1.4 × 10-6 C) 2.8 × 10-6 D) 3.2 × 10-10 E) 8.1 × 10-12

A) 1.8 × 10-5

When the following equation is completed and balanced, the products, showing the correct phases, are ______________. ____ Hg2(NO3)2(aq) + __2__ HCl(aq) ® A) Hg2Cl2(s) + 2HNO3(aq) B) 2HgCl(s) + 2HNO3(aq) C) Hg2Cl2(s) + H(NO3)2(aq) D) HgCl2(s) + H2NO3(aq) E) Hg2Cl(s) + 2HClNO3(aq)

A) Hg2Cl2(s) + 2HNO3(aq)

Which is the correct Ksp expression for PbCl2(s) dissolving in water? A) Ksp = [Pb2+].[Cl-]2 B) Ksp = [Pb2+].[Cl-] C) Ksp = [Pb2+]2.[Cl-] D) Ksp = [PbCl+] [Cl-] E) Ksp = [Pb+].[Cl-]2

A) Ksp = [Pb2+].[Cl-]2

What precautions are needed with long hair and beards? A) Keep long hair tied back, and keep hair away from flames B) Must be shampooed C) No long hair and/or beards allowed in the lab D) Get your hair cut before the beginning of each lab E) No precautions are necessary

A. Keep long hair tied back, and keep hair away from flames

Describe the procedure for smelling a chemical. A) Stick your nose close to the vessel and breathe deeply B) Point vessel away from face while gently fanning vapors toward nose C) Point the test tube towards your partner's nose. D) Never smell a chemical E) Smell a chemical as you would anything else

B Point vessel away from face while gently fanning vapors towards nose

Match the following descriptions of titration curves with the diagrams. The curve for a strong acid added to a strong base is ___________ while the curve for a strong base added to a polyprotic acid is _________. A) (i), (iv) B) (ii), (iv) C) (i), (iii) D) (ii), (iii) E) (i), (ii)

B) (ii), (iv)

4)Determine the Ksp for magnesium hydroxide (Mg(OH)2) where the solubility of Mg(OH)2 is 1.4 × 10-4 M. A) 2.7 × 10-12 B) 1.1 × 10-11 C) 2.0 × 10-8 D) 3.9 × 10-8 E) 1.4 × 10-4

B) 1.1 × 10-11

Determine the Ksp for magnesium hydroxide (Mg(OH)2) where the solubility of Mg(OH)2 is 1.4 × 10-4 M. A) 2.7 × 10-12 B) 1.1 × 10-11 C) 2.0 × 10-8 D) 3.9 × 10-8 E) 1.4 × 10-4

B) 1.1 × 10-11

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds _________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10-6. A) 5.9 × 10-5 B) 1.1 × 10-2 C) 2.4 × 10-8 D) 2.7 × 10-3 E) 1.2 × 10-4

B) 1.1 × 10-2

1)The concentration of iodide ions in a saturated solution of lead(II) iodide is __________ M. The solubility product constant of PbI2 is 1.4 x 10-8. A) 3.8 × 10-4 B) 3.0 × 10-3 C) 1.5 × 10-3 D) 3.5 × 10-9 E) 1.4 × 10-8

B) 3.0 × 10-3

The concentration of iodide ions in a saturated solution of lead (II) iodide is __________ M. The solubility product constant of PbI2 is 1.4 x 10-8. A) 3.8 × 10-4 B) 3.0 × 10-3 C) 1.5 × 10-3 D) 3.5 × 10-9 E) 1.4 × 10-8

B) 3.0 × 10-3

What is the concentration of Cl- ion (in M) in PbCl2 solution in water? The Ksp of PbCl2 is 1.6 × 10-5. A) 2.0 × 10-3 B) 3.2 × 10-2 C) 1.6 × 10-14 D) 2.5 × 10-2 E) 1.6 × 10-2

B) 3.2 × 10-2

Calculate the molality of a 17.5% (by mass) aqueous solution of nitric acid (MM = 63.01 g/mol). A) 0.274 m B) 3.37 m C) 3.04 m D) 4.33 m E) The density of the solution is needed to solve the problem.

B) 3.37 m

The concentration of copper ion of an unknown Cu sample (mass of the sample = 0.870 g dissolved in 400.0 mL solution) was spectrophotometrically determined. 8.00 mL of the sample were diluted to 10.00 mL and measured. The concentration was found to be 0.575 mg/mL. Calculate the % of copper in the unknown copper sample. A) 26.4% B) 33.0 % C) 66.1% D) 21.1% E) 264%

B) 33.0 %

The solubility of manganese (II) hydroxide (Mn(OH)2) is 2.2 × 10-5 M. What is the Ksp of Mn(OH)2? A) 1.1 × 10-14 B) 4.3 × 10-14 C) 2.1 × 10-14 D) 4.8 × 10-10 E) 2.2 × 10-5

B) 4.3 × 10-14

The solubility of manganese(II) hydroxide (Mn(OH)2) is 2.2 × 10-5 M. What is the Ksp of Mn(OH)2? A) 1.1 × 10-14 B) 4.3 × 10-14 C) 2.1 × 10-14 D) 4.8 × 10-10 E) 2.2 × 10-5

B) 4.3 × 10-14

Of the following, a 0.10 M aqueous solution of ________ will have the lowest freezing point. A) NaCl B) Al(NO3)3 C) K2CrO4 D) Na2SO4 E) C12H22O11

B) Al(NO3)3

When the following equation is completed and balanced, the products, showing the correct phases, are ______________. ___BaCl2(aq) + ___NaBO2(aq) ® A) Ba2(BO2)2(s) + 2NaCl(aq) B) Ba(BO2)2(s) + 2NaCl(aq) C) Ba(BO2(s) + Na2Cl(aq) D) Ba2BO2(s) + NaCl(aq) E) BaBO2(s) + NaCl(aq)

B) Ba(BO2)2(s) + 2NaCl(aq)

When the following equation is completed and balanced, the products, showing the correct phases, are ______________. ___CaC2O4(s) + __ HCl(aq) --> A) CaCl2(s) + 2HClO4(aq) B) CaCl2(aq) + H2C2O4(aq) C) CaCl(s) + H2CO3(aq) D) CaCl2(s) + HClO3(aq) + CO2(g) E) CaCl2(s) + 2HCO2(aq)

B) CaCl2(aq) + H2C2O4(aq)

The energy of a photon of light is __________ proportional to its frequency and __________ proportional to its wavelength. A) inversely, not, respectively B) directly, inversely, respectively C) directly, directly, respectively D) inversely, inversely, respectively E) inversely, directly, respectively

B) directly, inversely, respectively

Consider the following aqueous reaction: Cu(H2O)42+(aq) + 4CN-(aq) ⇌ Cu(CN)42-(aq) + 4H2O(l), DH = −348 kJ/mol light blue dark blue If the Cu(CN)42- concentration is increased, the equilibrium will _____________ and the absorbance (A) will _________. A) shift right, decrease B) shift left, decrease C) shift left, increase D) shift right, increase E) shift right, not change

B) shift left, decrease

Consider the following aqueous reaction: Cu(H2O)42+(aq) + 4CN-(aq) ⇌ Cu(CN)42-(aq) + 4H2O(l), DH = −348 kJ/mol light blue dark blue If the solution is heated, the equilibrium will _____________ and the absorbance (A) will _________. A) shift right, decrease B) shift left, decrease C) shift left, increase D) shift right, increase E) shift right, not change

B) shift left, decrease

At equilibrium, ________. A) all chemical reactions have ceased B) the rates of the forward and reverse reactions are equal C) the rate constants of the forward and reverse reactions are equal D) the value of the equilibrium constant is 1 E) the limiting reagent has been consumed

B) the rates of the forward and reverse reactions are equal

When the following equation is completed and balanced, the products, showing the correct phases, are ______________. ____ BaCl2(aq) + ____ Na2SO4(aq) ® A) BaSO2(s) + NaCl(aq) + NaO(s) B) Ba2SO4(s) + Na2Cl(aq) C) BaSO4(s) + 2NaCl(aq) D) Ba(SO4)2(s) + 2NaCl(aq) E) BaSO4(aq) + NaCl(s)

C) BaSO4(s) + 2NaCl(aq)

Which of the following equilibria would NOT be affected by increasing the overall pressure based on Le Châtelier's principle? A) N2(g) + 3H2(g) ⇌ 2NH3(g) B) N2O4(g) ⇌ 2NO2(g) C) N2(g) + O2(g) ⇌ 2NO(g) D) CO(g) + H2O(l) ⇌ CO2(g) + H2(g) E) CaCO3(s) ⇌ CaO(s) + CO2(g)

C) N2(g) + O2(g) ⇌ 2NO(g)

When the following equation is completed and balanced, the products, showing the correct phases, are ______________. ____NH4NO3(aq) + ____NaOH(aq) + Heat ® A) NH4OH(aq) + NaNO3(s) B) NH4OH(s) + Na(NO3)2(aq) C) NH3(g) + H2O(l) + NaNO3(aq) D) NNH4OH(s) + NaNO3(aq) E) NH4+(g) + HNO2(aq) + NaNO3(aq)

C) NH3(g) + H2O(l) + NaNO3(aq)

_____chemical analysis is the determination of what is present in a sample, while _____ chemical analysis is the measurement of how much of a chemical substance is present. A) Quantitative; qualitative B) Stoichiometric; qualitative C) Qualitative; quantitative D) Stoichiometric; identification E) Quantitative; identification

C) Qualitative; quantitative

When a solute is added to a solvent, how does the freezing point of the newly created solution change relative to the pure solvent? A) No change is observed. B) The freezing point of the solution is higher. C) The freezing point of the solution is lower. D) The freezing point will remain the same. E) It is not possible to determine.

C) The freezing point of the solution is lower.

Consider the following absorbance (A)-wavelength (l) spectrum for a certain dye solution: What color would you expect this solution to appear? A) Red B) Green C) Yellow D) Orange E) Violet

C) Yellow

An unsaturated solution is one that ________. A) has no double bonds B) contains the maximum concentration of solute possible, and is in equilibrium with undissolved solute C) has a solute concentration lower than the solubility D) contains more dissolved solute than the solubility allows E) contains no solute

C) has a solute concentration lower than the solubility

Consider the following aqueous reaction: Cu(H2O)42+(aq) + 4CN-(aq) ⇌ Cu(CN)42-(aq) + 4H2O(l), DH = −348 kJ/mol light blue dark blue If CN- ion is removed, the equilibrium will _____________ and the absorbance (A) will _________. A) shift right, decrease B) shift left, increase C) shift left, decrease D) shift right, increase E) not change, not change

C) shift left, decrease

Eating and drinking are not permitted in the lab because____________. A) there would not be enough time to finish the experiment B) the stockroom serves terrible appetizers C) you could be poisoned D) the lab would become quite messy with this type of activity E) your partner may ask you to share the drink or the food

C. You could be poisoned.

Group I cations are precipitated as ___________ using _________, respectively. A) chlorides, BaCl2 B) sulfides, H2S C) chlorides, HCl D) sulfates, H2SO4 E) hydroxides, NaOH

C. chlorides, HCl

Complete and balance the following equation. Show all phases. ______KI(aq) + ______Pb(NO3)2(aq) →PbI2(s) + 2KNO3(aq)

Complete and balance the following equation. Show all phases. ___2___KI(aq) + ______Pb(NO3)2(aq) →PbI2(s) + 2KNO3(aq)

Which of the following is a colligative property? (i) Osmotic pressure (ii) Density (iii) Vapor pressure lowering (iv) Freezing point (v) Boiling point A) (i), (iii), (iv), and (v) B) (iv) and (v) only C) (iii), (iv), and (v) D) (i) and (iii) only E) All are colligative properties

D) (i) and (iii) only

The solubility of lead (II) chloride (PbCl2) is 1.6 × 10-2 M. What is the Ksp of PbCl2 A) 5.0 × 10-4 B) 4.1 × 10-6 C) 3.1 × 10-7 D) 1.6 × 10-5 E) 1.6 × 10-2

D) 1.6 × 10-5

The solubility of lead (II) chloride (PbCl2) is 1.6 × 10-2 M. What is the Ksp of PbCl2 A) 5.0 × 10-4 B) 4.1 × 10-6 C) 3.1 × 10-7 The solubility of lead (II) chloride (PbCl2) is 1.6 × 10-2 M. What is the Ksp of PbCl2 A) 5.0 × 10-4 B) 4.1 × 10-6 C) 3.1 × 10-7 D) 1.6 × 10-5 E) 1.6 × 10-2

D) 1.6 × 10-5

What volume (mL) of a concentrated solution of copper(II) nitrate (9.00 mg/mL) must be diluted to 350. mL to make a 2.75 mg/mL solution of copper(II) nitrate? A) 1145 B) 50.0 C) 45.0 D) 107 E) 350

D) 107

Consider the following absorbance (A)-wavelength (l) spectrum for a certain dye solution: Determine the percent Transmittance (%T) at 450 nm. A) 60.0% B) 0.600% C) 1.40% D) 25.1% E) 3.98%

D) 25.1%

When the following equation is completed and balanced, the products, showing the correct phases, are ______________. ____HCl(aq) + ____ Na2CO3(aq) ® A) 2NaCl(aq) + H2CO3(aq) B) NaHCO3Cl(aq) + HCO2(aq) + H2O(l) C) Na2Cl(s) + CO2(g) + H2O(l) D) 2NaCl(aq) + CO2(g) + H2O(l) E) Na2Cl2(s) + CO2(g) + H2O(l)

D) 2NaCl(aq) + CO2(g) + H2O(l)

A sample of Cu(NH3)42+ had an absorbance of 0.170 at 610 nm in a cuvette with a 2.0-cm path length. Use Beer's law to calculate the concentration of Cu(NH3)42+ in mol/L. The molar absorptivity is 201 M-1.cm-1. A) 2.36 × 103 M B) 2.58 × 10-1 C) 1.52 M D) 4.23 × 10-4 M E) 8.46 × 10-4 M

D) 4.23 × 10-4 M

What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 × 10-5. A) 2.0 × 10-3 B) 1.1 × 10-4 C) 1.8 × 10-4 D) 7.1 × 10-4 E) 1.6 × 10-5

D) 7.1 × 10-4

What is the molar solubility of barium fluoride (BaF2) in water? The solubility-product constant for BaF2 is 1.7 × 10-6 at 25°C. A) 6.5 × 10-4 B) 1.2 × 10-2 C) 1.8 × 10-3 D) 7.5 × 10-3 E) 5.7 × 10-7

D) 7.5 × 10-3

Group IV cations include which of the following: A) C4+, Si4+, Sn2+, Ge4+, and Pb2+ B) Ca2+, Ba2+, and NH32+ C) Pb2+, Ag+, and Hg22+ D) Ca2+, Ba2+, and NH4+ E) Ti3+, Zr4+, Hf3+, Rf2+

D) Ca2+, Ba2+, and NH4+

When the following equation is completed and balanced, the products, showing the correct phases, are ______________. ___ CaCl2(aq) + ____ (NH4)2C2O4(aq) ® A) CaCO3(s) + CO2(g) + 2NH4Cl(aq) B) Ca(NO3)2(aq) + HCl(aq) + NH3(g) C) Ca2C2O4(aq) + NH4Cl2(aq) D) CaC2O4(s) + 2NH4Cl(aq) E) CaCO4(s) + NH3Cl(aq)

D) CaC2O4(s) + 2NH4Cl(aq)

Which of the following is not a part of a spectrophotometer? A) Light source B) Monochromator C) Sample holder D) Furnace E) Detector

D) Furnace

When the following equation is completed and balanced, the products, showing the correct phases, are __________________________. ____ Pb(NO3)2(aq) + ____ K2CrO4(aq) ® A) PbCrO4(s) + K2(NO3)2(aq) B) PbCrO4(s) + K(NO3)2(aq) C) PbK2(s) + NO3CrO4(aq) D) PbCrO4(s) + 2KNO3(aq) E) Pb(CrO4)2(s) + 2KNO3(aq

D) PbCrO4(s) + 2KNO3(aq)

The effect of a catalyst on an equilibrium is to __________. A) increase the rate of the forward reaction only B) increase the equilibrium constant so that products are favored C) slow the reverse reaction only D) increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture E) shift the equilibrium to the right

D) increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture

Consider the following aqueous reaction: Cu(H2O)42+(aq) + 4CN-(aq) ⇌ Cu(CN)42-(aq) + 4H2O(l), DH = −348 kJ/mol light blue dark blue If H2O(l) is removed, the equilibrium will _____________ and the absorbance (A) will _________. A) shift right, decrease B) shift left, decrease C) shift left, increase D) shift right, increase E) not change, not change

D) shift right, increase

What is the absorbance value (A) of a dye solution that has %T of 32%. A) 2.49 B) 1.68 C) 3.51 D) 1.51 E) 0.495

E) 0.495

What is the molar solubility of magnesium carbonate (MgCO3) in water? The solubility-product constant for MgCO3 is 3.5 × 10-8 at 25°C. A) 1.8 × 10-8 B) 7.0 × 10-8 C) 7.46 D) 2.6 × 10-4 E) 1.9 × 10-4

E) 1.9 × 10-4

What is the frequency of light (s-1) that has a wavelength of 1.23 × 10-6 cm? Speed of light = 3.00 × 108 m/s. A) 2.44 × 1016 s-1 B) 1.04 × 10-13 s-1 C) 4.10 × 10-17 s-1 D) 9.62 × 1012 s-1 E) 2.44 × 1014 s-1

E) 2.44 × 1014 s-1

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about ________ M. A) 0.0828 B) 0.160 C) 0.0821 D) 0.224 E) 2.88

E) 2.88

What is the % of Cu (MM = 63.550 g/mol) in Cu3(PO4)2 (MM = 380.58 g/mol)? A) 5.989% B) 16.698% C) 25.047% D) 33.396% E) 50.091%

E) 50.091%

Which of the following aqueous solutions has the highest [OH-]? A) A solution with a pH of 3.0 B) A 1 × 10-4 M solution of HNO3 C) A solution with a pOH of 12.0 D) Pure water E) A solution with a pH of 13.0

E) A solution with a pH of 13.0

When the following equation is completed and balanced, the products, showing the correct phases, are ______________. ____ AgNO3(aq) + ____ NaCl(aq) ® A) AgCl(aq) + NaNO3(s) B) AgCl2(aq) + NaNO3(aq) C) Ag2Cl(s) + NaNO2(aq)l) D) AgCl(s) + NaNO2(aq) E) AgCl(s) + NaNO3(aq)

E) AgCl(s) + NaNO3(aq)

When the following equation is completed and balanced, the products, showing the correct phases, are ______________. ____BaCl2(aq) + ____(NH4)2SO4(aq) ® A) Ba(SO4)2(s) + NH4Cl(aq) B) Ba2SO4(s) + NH3(g) + H2O(l) C) BaSO4(aq) + 2NH4Cl(s) D) BaSO3(s) + NH3Cl(aq) E) BaSO4(s) + 2NH4Cl(aq)

E) BaSO4(s) + 2NH4Cl(aq)

The correct symbols for the carbonate, borate, sulfate, and nitrate ions are: A) CO32-, BO-, SO22-, NO3-, respectively B) CO32-, BO2-, SO42-, NO2- , respectively C) CO32-, BO3-, SO32-, NO3-, respectively D) CO32-, BO22-, SO42-, NO3-, respectively E) CO32-, BO2-, SO42-, NO3-, respectively

E) CO32-, BO2-, SO42-, NO3-, respectively

Which one of the following solutes has a limiting van't Hoff factor (i) of 3 when dissolved in water? A) KNO3 B) CH3OH C) CBr4 D) C6H12O6 E) K2SO4

E) K2SO4

Molality (m) is defined as the ________. A) moles solute/moles solvent B) moles solute/liters solution C) moles solute/kg solution D) moles solute/moles solution E) moles solute/kg solvent

E) moles solute/kg solvent

Consider the following aqueous reaction: Cu(H2O)42+(aq) + 4CN-(aq) ⇌ Cu(CN)42-(aq) + 4H2O(l), DH = −348 kJ/mol light blue dark blue If the volume of the reaction vessel is increased, the equilibrium will _____________ and the absorbance (A) will _________. A) shift right, decrease B) shift left, decrease C) shift left, increase D) shift right, increase E) not change, not change

E) not change, not change

Which of the following safety items is located in the laboratory? A) Fire extinguisher B) Fire blanket C) Emergency shower D) Eye wash station E) All of the above

E. All of the above

Accidents often result from ____________. A) failure to use common sense B) failure to follow instructions C) making mistakes D) an indifferent attitude E) All of the above

E. All of the above.

General guidelines for preventing accidents include ______________. A) never play tricks or indulge in horseplay in the chemical laboratory B) know where the safety equipment is C) become familiar with the hazards of the chemicals to be used D) follow all safety instructions carefully E) all of the above

E. All of the above.

safety equipment

Eye wash station Emergency shower Fire extinguisher Fire blanket Landline phone Spill kit First aid kit

TRUE OR FALSE: The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

FALSE

TRUE OR FALSE: The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction. The solubility of a slightly soluble salt is decreased by the presence of a second solute that provides a common ion to the system. The solubility of slightly soluble salts containing basic anions is proportional to the pH of the solution.

FALSE TRUE FALSE

True/False A cooling curve is a graph that relates the temperature of the solution (y axis) vs. the amount of solute (x axis).

False

True/False A pH titration curve is a plot of pH vs. the volume of the analyte solution.

False

True/False A spectrophotometer that uses UV light is called a colorimeter.

False

True/False Ba2+ ion is precipitated as phosphates.

False

True/False NH3(aq) is also known as ammonium hydroxide, has a pH < 7, and turns blue litmus paper red.

False

True/False Potentiometric acid-base titrations require the use of an acid-base indicator for the detection of the end point.

False

True/False Potentiometric measurements involve the measurement of the current difference between a reference electrode and an indicator electrode.

False

True/False The absorbance of Cu(NH3)42+ is measured at 610 nm because the complex shows minimum absorption at that wavelength.

False

True/False The absorption of a monochromatic EMR beam decreases with increasing the width of the cuvette.

False

True/False The color of light that is absorbed is the same as the visible color of the solution.

False

True/False The difference in the sizes of particles are used to separate cations in mixtures.

False

True/False The equation: A = abc shows that, for all concentration, the absorbance is directly related to the concentration of the absorbing species.

False

True/False The freezing point of an aqueous solution containing 25 g of KCl is higher than that of a solution containing 10. g of KCl.

False

True/False The pH of 0.100 M HCl is higher than that of 0.100 M CH3COOH.

False

True/False Upon addition of conc. H2SO4 to a solid sulfate salt, brown fumes of NO2 gas form.

False

True/False Upon the addition of AgNO3 to a nitrate salt, a white precipitate of AgCl forms.

False

True/False Upon the addition of concentrated H2SO4(aq) to a solid NaCl, CO2 gas evolves.

False

What group are the following in? Ca2+, Ba2+, and NH4+; What color are they?

Group 4 cations. colorless

pH

If a substance has a basic anion, it will be more soluble in an acidic solution. Substances with acidic cations are more soluble in basic solutions.

The Common-Ion Effect

If one of the ions in a solution equilibrium is already dissolved in the solution, the equilibrium will shift to the left and the solubility of the salt will decrease.

Temperature

Increasing the temperature can cause either an increase or decrease in the solubility of a given salt

The solubility of PbCl2 in a saturated solution of lead(II) chloride is 1.6 × 10-2 M. Calculate the solubility product constant of PbCl2. Show your work.

Ksp=1.64 x 10-5

A solutions was prepared by adding 1.00 × 10-3 M Pb(NO3)2(aq), 2.00 × 10-3 M KI(aq), and deionized water together in a test tube. The Ksp of PbI2 is 9.8 × 10-9. Complete the following table. Express each answer in scientific notation. Show your work under the table.

Look at question

Complexing Agents

Metal ions can act as Lewis acids and form complex ions with Lewis bases in the solvent. The formation of these complex ions increases the solubility of these salts. AgCl(s) + 2 NH3(aq) ⇌ [Ag(NH3)2]Cl(aq)

All Cl-, Br-, and I- are soluble in water except those of ___, ___, and ___.

Pb2+, Hg22+, and Ag+

____ dissolves in hot water while ___ dissolves in ammonia solution, NH3(aq)

PbCl2; AgCl

True/False A calibration curve is general method used to predict the unknown concentration of an analyte of interest based on the response of the instrument to known standards for the same analyte.

True

True/False A pH electrode is an ion selective electrode that responds only to changes in the [H+].

True

True/False All of the Group IV ions are colorless in their solution.

True

True/False All types of EMR travel through vacuum at the speed of light.

True

True/False An X-ray radiation has a higher energy than a visible radiation.

True

True/False At 50% neutralization of a weak acid, the pH of the solution equals pKa for the weak acid.

True

True/False Barium salts give a green flame while calcium salts give red flame.

True

True/False Beer's law states that at low concentration, the absorption of a monochromatic EMR beam increases with increasing the concentration of the absorbing species.

True

True/False For a basic solution, the [OH-] is > 1.0 × 10-7 M and the pH is greater than 7.

True

True/False In an endothermic equilibrium reaction in the forward direction, increasing the reaction temperature favors the formation of the products.

True

True/False Le Châtelier's principle states that if a system at equilibrium is disturbed, the equilibrium Position will shift to minimize these disturbances.

True

True/False Lead(II) chloride is soluble in hot water while silver chloride is soluble in aqueous ammonia.

True

True/False NH4+ salt solutions form ammonia gas when heated with NaOH(aq).

True

True/False The brown-ring test is used to test for the presence of the nitrate ion.

True

True/False The freezing point of an aqueous solution containing 0.500 m NaBr(aq) is the same as that of a solution containing 0.500 m LiF(aq).

True

True/False The objective of the lab was to determine the % of Cu in a given unknown Cu salt.

True

True/False Upon the addition of concentrated H2SO4 and methanol to a borate sample and heating, a green flame forms.

True

Wash chemicals out of eyes or report incident to instructor?

Wash then report

All _____, _____, _____ are insoluble in water except those of Na+, K+, and NH4+

arsenates (AsO32-), borates (B4O72-), carbonates (CO32-)

Examples of personal protective equipment do not include __________________. A) goggles and long pants B) lab coats C) long-sleeve shirts D) contact lenses E) covered shoes

contact lenses

endothermic dissolution

heat is absorbed. Increasing temp will increase dissolution (solubility

exothermic dissolution

heat is released. increasing temp will decrease solubility (dissolution)

All _____ are insoluble except those of Na+, K+, and NH4+

hydroxides

All sulfides (S2-) are _____ except Na+, K+, and NH4+

insoluble

Material to be disposed of in the laboratory __________________. A) can be disposed in the sink B) must always be diluted copiously with water first C) must always be neutralized first before being disposed in the sink D) can be disposed in the bathroom E) must always be handled in accordance with safety guidelines specific to that class of compound as directed by the instructor

must always be handled in accordance with safety guidelines specific to that class of compound as directed by the instructor

What should be worn in a laboratory at all times to decrease the likelihood of eye injury? A) Corrective lenses B) Safety glasses C) A mask D) An apron E) An Apple watch

safety glasses

Ksp will be a "true" measure of the solubilities of different salts ONLY if the dissociation of ALL of the salts produce the what?

same number of ions

All acetates (CH3COO-) and nitrates (NO3-) are _____ in water.

soluble

All salts of Na+, K+, and NH4+ are _____ in water.

soluble

Barium is precipitated as _____. What color? Calcium is precipitated as ____. What color?

sulfate, apple green oxalate, brick red

All ____ are soluble except those of Ba2+, Pb2+, and Hg22+

sulfates

Eating, drinking, chewing gum, and smoking are not allowed true or false?

true

What should be the very last function performed in the lab before you leave? A) Bid the instructor farewell B) Make sure that your locker is secure C) Wash your hands D) Arrange a time with your lab partner for lunch E) Clean your work area

wash your hands

lab rules

•Eye protection must be worn at all times. •It is strongly recommended that contact lenses not be worn. •Laboratory work should be quiet and thoughtful. -NO horseplay. -You will be directed to leave if you do not comply.