Question 1

Consider the Ksp values for two compounds: MZ,Ksp = 1.5 × 10-20 and MZ2,Ksp = 1.5 × 10-20.Why don't these compounds have the same molar solubility?

Accepted Answer

These two compounds have the same solubility product constant,but that does not mean they have the same molar solubilities.Since the first compound contains 2 ions and the second compound contains 3 ions,their solubility product expressions differ and therefore their molar solubilities must differ.Compound MZ₂ will have a higher molar solubility.

Question 2

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 M HCl to reach the equivalence point?

Accepted Answer

A) 0.300 M 
B) 0.312 M 
C) 0.800 M 
D) 1.30 M 
A) 0.300 M 
B) 0.312 M 
C) 0.800 M 
D) 1.30 M C

Question 3

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 50.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A) 8.26 
B) 9.26 
C) 11.13 
D) 12.40 
A) 8.26 
B) 9.26 
C) 11.13 
D) 12.40 D

Question 4

The molar solubility of ZnS is 1.6 × 10-12 M in pure water.Calculate the Ksp for ZnS.

Accepted Answer

A) 8.0 × 10-13 
B) 3.2 × 10-12 
C) 1.6 × 10-35 
D) 2.6 × 10-24 
E) 6.80 × 10-5 
A) 8.0 × 10-13 
B) 3.2 × 10-12 
C) 1.6 × 10-35 
D) 2.6 × 10-24 
E) 6.80 × 10-5

Question 5

Copper(II)chloride is highly soluble in water.This compound has ________.

Accepted Answer

A) high solubility product 
B) low solubility product 
C) high equilibrium constant 
D) high dissociation constant 
A) high solubility product 
B) low solubility product 
C) high equilibrium constant 
D) high dissociation constant

Question 6

When titrating a weak monoprotic acid with NaOH at 25°C,the

Accepted Answer

A) pH will be less than 7 at the equivalence point. 
B) pH will be equal to 7 at the equivalence point. 
C) pH will be greater than 7 at the equivalence point. 
D) titration will require more moles of base than acid to reach the equivalence point. 
E) titration will require more moles of acid than base to reach the equivalence point. 
A) pH will be less than 7 at the equivalence point. 
B) pH will be equal to 7 at the equivalence point. 
C) pH will be greater than 7 at the equivalence point. 
D) titration will require more moles of base than acid to reach the equivalence point. 
E) titration will require more moles of acid than base to reach the equivalence point.

Question 7

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 66.67 mL of LiOH.(This is the equivalence point. )

Accepted Answer

A) 0.97 
B) 13.03 
C) 2.76 
D) 11.24 
E) 7.00 
A) 0.97 
B) 13.03 
C) 2.76 
D) 11.24 
E) 7.00

Question 8

You wish to prepare an HC2H3O2 buffer with a pH of 5.44.If the pKa of is 4.74,what ratio of
C2H3O2-/HC2H3O2 must you use?

Accepted Answer

A) 0.70 
B) 0.20 
C) 1.4 
D) 5.0 
E) 1.1 
A) 0.70 
B) 0.20 
C) 1.4 
D) 5.0 
E) 1.1

Question 9

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89,which of the following is true?

Accepted Answer

A) [HCHO2] 2] 
B) [HCHO2] = [NaCHO2] 
C) [HCHO2] > [NaCHO2] 
D) [HCHO2] >> [NaCHO2] 
E) It is not possible to make a buffer of this pH from HCHO2 and NaCHO2. 
A) [HCHO2] 2] 
B) [HCHO2] = [NaCHO2] 
C) [HCHO2] > [NaCHO2] 
D) [HCHO2] >> [NaCHO2] 
E) It is not possible to make a buffer of this pH from HCHO2 and NaCHO2.

Question 10

A 100.0 mL sample of 0.180 M HClO4 is titrated with 0.270 M LiOH.Determine the pH of the solution after the addition of 75.0 mL of LiOH.

Accepted Answer

A) 12.1 
B) 2.65 
C) 11.35 
D) 1.89 
E) 13.06 
A) 12.1 
B) 2.65 
C) 11.35 
D) 1.89 
E) 13.06

Question 11

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH before any base is added? 
The Ka of butanoic acid is 1.5 × 10-5.

Accepted Answer

A) 2.83 
B) 1.5 × 10-3 
C) 4.82 
D) 4.00 
E) 1.0 × 104  
A) 2.83 
B) 1.5 × 10-3 
C) 4.82 
D) 4.00 
E) 1.0 × 104

Question 12

Give the expression for the solubility product constant for Ca3(PO4)2.

Accepted Answer

A)    
B)    
C)    
D) [Ca2+]2[PO43-]3 
E) [Ca2+]3[PO43-]2 
A)    
B)    
C)    
D) [Ca2+]2[PO43-]3 
E) [Ca2+]3[PO43-]2

Question 13

A solution contains 0.021 M Cl⁻ and 0.017 M I⁻.A solution containing copper (I)ions is added to selectively precipitate one of the ions.At what concentration of copper (I)ion will a precipitate begin to form? What is the identity of the precipitate? Ksp (CuCl)= 1.0 × 10-6,Ksp (CuI)= 5.1 × 10-12.

Accepted Answer

A) 3.0 × 10-10 M,CuI 
B) 3.0 × 10-10 M,CuCl 
C) 4.8 × 10-5 M,CuCl 
D) 4.8 × 10-5 M,CuI 
E) No precipitate will form at any concentration of copper (I). 
A) 3.0 × 10-10 M,CuI 
B) 3.0 × 10-10 M,CuCl 
C) 4.8 × 10-5 M,CuCl 
D) 4.8 × 10-5 M,CuI 
E) No precipitate will form at any concentration of copper (I).

Question 14

The highest pH for an effective buffer occurs when the base is how many times as concentrated as the acid?

Accepted Answer

A) 2 
B) 5 
C) 10 
D) 20 
E) 15 
A) 2 
B) 5 
C) 10 
D) 20 
E) 15

Question 15

Give the expression for the solubility product constant for BaF2.

Accepted Answer

A)    
B)    
C) [Ba2+]2[F⁻] 
D) [Ba2+][F⁻]2 
E) [Ba2+][F⁻] 
A)    
B)    
C) [Ba2+]2[F⁻] 
D) [Ba2+][F⁻]2 
E) [Ba2+][F⁻]

Question 16

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.

Accepted Answer

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 
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

Question 17

Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO2)and 0.290 M in potassium nitrite (KNO2).The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Accepted Answer

A) 3.487 
B) 3.210 
C) 13.86 
D) 10.51 
E) 4.562 
A) 3.487 
B) 3.210 
C) 13.86 
D) 10.51 
E) 4.562

Question 18

Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO.The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A) 7.54 
B) 6.67 
C) 3.77 
D) 6.46 
E) 7.33 
A) 7.54 
B) 6.67 
C) 3.77 
D) 6.46 
E) 7.33

Question 19

Identify the indicator that can be used at the lowest pH.

Accepted Answer

A) Alizarin 
B) Thymol blue 
C) Crystal violet 
D) Phenolphthalein 
E) Alizarin yellow R 
A) Alizarin 
B) Thymol blue 
C) Crystal violet 
D) Phenolphthalein 
E) Alizarin yellow R

Question 20

A ligand is a molecule or ion that acts as a ________.

Accepted Answer

A) Lewis acid 
B) Br∅nsted-Lowry acid 
C) Br∅nsted-Lowry base 
D) Lewis base 
E) None of the above 
A) Lewis acid 
B) Br∅nsted-Lowry acid 
C) Br∅nsted-Lowry base 
D) Lewis base 
E) None of the above

Consider the K_sp values for two compounds: MZ,K_sp = 1.5 × 10^-20 and MZ₂,K_sp = 1.5 × 10^-20.Why don't these compounds have the same molar solubility?

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 M HCl to reach the equivalence point?

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 50.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H.

The molar solubility of ZnS is 1.6 × 10^-12 M in pure water.Calculate the K_sp for ZnS.

Copper(II)chloride is highly soluble in water.This compound has ________.

When titrating a weak monoprotic acid with NaOH at 25°C,the

A 100.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 66.67 mL of LiOH.(This is the equivalence point. )

You wish to prepare an HC₂H₃O₂ buffer with a pH of 5.44.If the pK_a of is 4.74,what ratio of C₂H₃O₂^-/HC₂H₃O₂ must you use?

If the pK_a of HCHO₂ is 3.74 and the pH of an HCHO₂/NaCHO₂solution is 3.89,which of the following is true?

A 100.0 mL sample of 0.180 M HClO₄ is titrated with 0.270 M LiOH.Determine the pH of the solution after the addition of 75.0 mL of LiOH.

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH before any base is added? The K_a of butanoic acid is 1.5 × 10^-5.

Give the expression for the solubility product constant for Ca₃(PO₄)₂.

The highest pH for an effective buffer occurs when the base is how many times as concentrated as the acid?

Give the expression for the solubility product constant for BaF₂.

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,K_sp= 1.7 × 10^-6.

Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO₂)and 0.290 M in potassium nitrite (KNO₂).The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO.The K_a for HClO is 2.9 × 10^-8.

Identify the indicator that can be used at the lowest pH.

A ligand is a molecule or ion that acts as a ________.

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Exam 16: Aqueous Ionic Equilibrium

Consider the Ksp values for two compounds: MZ,Ksp = 1.5 × 10-20 and MZ2,Ksp = 1.5 × 10-20.Why don't these compounds have the same molar solubility?

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 M HCl to reach the equivalence point?

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 50.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3CO2H.

The molar solubility of ZnS is 1.6 × 10-12 M in pure water.Calculate the Ksp for ZnS.

Copper(II)chloride is highly soluble in water.This compound has ________.

When titrating a weak monoprotic acid with NaOH at 25°C,the

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 66.67 mL of LiOH.(This is the equivalence point. )

You wish to prepare an HC2H3O2 buffer with a pH of 5.44.If the pKa of is 4.74,what ratio of C2H3O2-/HC2H3O2 must you use?

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89,which of the following is true?

A 100.0 mL sample of 0.180 M HClO4 is titrated with 0.270 M LiOH.Determine the pH of the solution after the addition of 75.0 mL of LiOH.

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10-5.

Give the expression for the solubility product constant for Ca3(PO4)2.

The highest pH for an effective buffer occurs when the base is how many times as concentrated as the acid?

Give the expression for the solubility product constant for BaF2.

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.

Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO2)and 0.290 M in potassium nitrite (KNO2).The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO.The Ka for HClO is 2.9 × 10-8.

Identify the indicator that can be used at the lowest pH.

A ligand is a molecule or ion that acts as a ________.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Free Energy and Thermodynamics

Electrochemistry

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Consider the K_sp values for two compounds: MZ,K_sp = 1.5 × 10^-20 and MZ₂,K_sp = 1.5 × 10^-20.Why don't these compounds have the same molar solubility?

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 50.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H.

The molar solubility of ZnS is 1.6 × 10^-12 M in pure water.Calculate the K_sp for ZnS.

A 100.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 66.67 mL of LiOH.(This is the equivalence point. )

You wish to prepare an HC₂H₃O₂ buffer with a pH of 5.44.If the pK_a of is 4.74,what ratio of C₂H₃O₂^-/HC₂H₃O₂ must you use?

If the pK_a of HCHO₂ is 3.74 and the pH of an HCHO₂/NaCHO₂solution is 3.89,which of the following is true?

A 100.0 mL sample of 0.180 M HClO₄ is titrated with 0.270 M LiOH.Determine the pH of the solution after the addition of 75.0 mL of LiOH.

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH before any base is added? The K_a of butanoic acid is 1.5 × 10^-5.

Give the expression for the solubility product constant for Ca₃(PO₄)₂.

Give the expression for the solubility product constant for BaF₂.

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,K_sp= 1.7 × 10^-6.

Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO₂)and 0.290 M in potassium nitrite (KNO₂).The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO.The K_a for HClO is 2.9 × 10^-8.