Question 1

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?

Accepted Answer

A) 4.9 × 10 −2 
B) 1.7 × 10 −5 
C) 8.5 × 10 −6 
D) 4.2 × 10 −6 
E) −6 
A) 4.9 × 10 −2 
B) 1.7 × 10 −5 
C) 8.5 × 10 −6 
D) 4.2 × 10 −6 
E) −6

Question 2

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 × 10−4

Accepted Answer

A) 1.1 × 10 −4  M 
B) 2.6 × 10 −4  M 
C) 4.3 × 10 −4 M 
D) 6.7 × 10 −5 M 
E) None of these choices are correct. 
A) 1.1 × 10 −4  M 
B) 2.6 × 10 −4  M 
C) 4.3 × 10 −4 M 
D) 6.7 × 10 −5 M 
E) None of these choices are correct.

Question 3

The salts X(NO3)2 and Y(NO3)2 (where X+ and Y+ are metal ions) are dissolved in water to give a solution which is 0.1 M in each of them. Using the Ksp values listed below, decide which aqueous reagent, if any, will definitely precipitate X+ before precipitating Y+ from solution. Given Ksp values:XCl2, 1 × 10−5 YCl2, 1 × 10−10 X(OH)2, 1 × 10−10 Y(OH)2, 1 × 10−5

Accepted Answer

A) 1 M NaNO 3 
B) 1 M HCl 
C) 1 M HNO 3 
D) 1 M NaCl 
E) None of these choices are correct. 
A) 1 M NaNO 3 
B) 1 M HCl 
C) 1 M HNO 3 
D) 1 M NaCl 
E) None of these choices are correct.

Question 4

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, Ka = 7.2 × 10−4.

Accepted Answer

A) [base]/[acid] = 0.14 
B) [base]/[acid] = 0.42 
C) [base]/[acid] = 2.36 
D) [base]/[acid] = 7.20 
E) None of these choices are correct. 
A) [base]/[acid] = 0.14 
B) [base]/[acid] = 0.42 
C) [base]/[acid] = 2.36 
D) [base]/[acid] = 7.20 
E) None of these choices are correct.

Question 5

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

Accepted Answer

A) 0.85 
B) 0.75 
C) 0.66 
D) 0.49 
E) 3.8 
A) 0.85 
B) 0.75 
C) 0.66 
D) 0.49 
E) 3.8

Question 6

When a weak acid is titrated with a weak base, the pH at the equivalence point

Accepted Answer

A) is greater than 7.0. 
B) is equal to 7.0. 
C) is less than 7.0. 
D) is determined by the sizes of K a and K b. 
E) is no longer affected by addition of base. 
A) is greater than 7.0. 
B) is equal to 7.0. 
C) is less than 7.0. 
D) is determined by the sizes of K a and K b. 
E) is no longer affected by addition of base.

Question 7

A sample of a monoprotic acid (HA) weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

Accepted Answer

A) 37.0 g/mol 
B) 81.0 g/mol 
C) 128 g/mol 
D) 20.3 g/mol 
E) 211 g/mol 
A) 37.0 g/mol 
B) 81.0 g/mol 
C) 128 g/mol 
D) 20.3 g/mol 
E) 211 g/mol

Question 8

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3)2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10−5 for calcium sulfate.

Accepted Answer

A) 1.2 × 10 −2 mol 
B) 4.9 × 10 −3 mol 
C) 3.5 × 10 −3 mol 
D) 1.2 × 10 −5 mol 
E) 4.8 × 10 −8 mol 
A) 1.2 × 10 −2 mol 
B) 4.9 × 10 −3 mol 
C) 3.5 × 10 −3 mol 
D) 1.2 × 10 −5 mol 
E) 4.8 × 10 −8 mol

Question 9

The salts X(NO3)2 and Y(NO3)2 (where X+ and Y+ are metal ions) are dissolved in water to give a solution which is 0.1 M in each of them. Using the Ksp values listed below, decide which aqueous reagent, if any, will definitely precipitate X+ before precipitating Y+ from solution. Given Ksp values:XCl2, 1 × 10−5 YCl2, 1 × 10−10 X(OH)2, 1 × 10−10 Y(OH)2, 1 × 10−5

Accepted Answer

A) 1 M NaCl 
B) 1 M HCl 
C) 1 M HNO 3 
D) 1 M NaOH 
E) None of these choices are correct. 
A) 1 M NaCl 
B) 1 M HCl 
C) 1 M HNO 3 
D) 1 M NaOH 
E) None of these choices are correct.

Question 10

Write the ion product expression for magnesium fluoride, MgF2.

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 11

What is the [H3O+] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? Ka = 3.5 × 10−8

Accepted Answer

A) 7.8 × 10 −9  M 
B) 1.8 × 10 −8  M 
C) 6.7 × 10 −8  M 
D) 1.6 × 10 −7  M 
E) None of these choices are correct. 
A) 7.8 × 10 −9  M 
B) 1.8 × 10 −8  M 
C) 6.7 × 10 −8  M 
D) 1.6 × 10 −7  M 
E) None of these choices are correct.

Question 12

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak diprotic acid H2A (0.10 mol L−1) with a strong base of the same concentration?

Accepted Answer

A) A 
B) B 
C) C 
D) D 
E) E 
A) A 
B) B 
C) C 
D) D 
E) E

Question 13

The salts X(NO3)2 and Y(NO3)2 (where X+ and Y+ are metal ions) are dissolved in water to give a solution which is 0.1 M in each of them. Using the Ksp values listed below, decide which aqueous reagent, if any, will definitely precipitate X+ before precipitating Y+ from solution. Given Ksp values:XCl2, 1 × 10−5 YCl2, 1 × 10−10 X(OH)2, 1 × 10−10 Y(OH)2, 1 × 10−5

Accepted Answer

A) 1 M NH 3 
B) 1 M HCl 
C) 1 M HNO 3 
D) 1 M NaCl 
E) None of these choices are correct. 
A) 1 M NH 3 
B) 1 M HCl 
C) 1 M HNO 3 
D) 1 M NaCl 
E) None of these choices are correct.

Question 14

A popular buffer solution consists of carbonate (CO32−) and hydrogen carbonate (HCO3−) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Accepted Answer

A) 1 L of 0.9 M CO 3 2− and 0.1 M HCO 3 − 
B) 1 L of 0.1 M CO 3 2− and 0.9 M HCO 3 − 
C) 1 L of 0.5 M CO 3 2− and 0.5 M HCO 3 − 
D) 1 L of 0.1 M CO32− and 0.1 M HCO3− 
E) They can all neutralize the same amount of hydrochloric acid. 
A) 1 L of 0.9 M CO 3 2− and 0.1 M HCO 3 − 
B) 1 L of 0.1 M CO 3 2− and 0.9 M HCO 3 − 
C) 1 L of 0.5 M CO 3 2− and 0.5 M HCO 3 − 
D) 1 L of 0.1 M CO32− and 0.1 M HCO3− 
E) They can all neutralize the same amount of hydrochloric acid.

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the K_sp of PbCl₂?

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 × 10⁻⁴

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, K_a = 7.2 × 10⁻⁴.

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

When a weak acid is titrated with a weak base, the pH at the equivalence point

A sample of a monoprotic acid (HA) weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃)₂before precipitation of calcium sulfate begins? K_sp = 2.4 × 10⁻⁵ for calcium sulfate.

Write the ion product expression for magnesium fluoride, MgF₂.

What is the [H₃O⁺] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? K_a = 3.5 × 10⁻⁸

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak diprotic acid H₂A (0.10 mol L⁻¹) with a strong base of the same concentration?

A popular buffer solution consists of carbonate (CO₃²⁻) and hydrogen carbonate (HCO₃⁻) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Thermodynamics: Entropy, Free Energy, and Reaction Direction

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 19: Ionic Equilibria in Aqueous Systems

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 × 10−4

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, Ka = 7.2 × 10−4.

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

When a weak acid is titrated with a weak base, the pH at the equivalence point

A sample of a monoprotic acid (HA) weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3)2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10−5 for calcium sulfate.

Write the ion product expression for magnesium fluoride, MgF2.

What is the [H3O+] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? Ka = 3.5 × 10−8

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak diprotic acid H2A (0.10 mol L−1) with a strong base of the same concentration?

A popular buffer solution consists of carbonate (CO32−) and hydrogen carbonate (HCO3−) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Thermodynamics: Entropy, Free Energy, and Reaction Direction

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the K_sp of PbCl₂?

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 × 10⁻⁴

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, K_a = 7.2 × 10⁻⁴.

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃)₂before precipitation of calcium sulfate begins? K_sp = 2.4 × 10⁻⁵ for calcium sulfate.

Write the ion product expression for magnesium fluoride, MgF₂.

What is the [H₃O⁺] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? K_a = 3.5 × 10⁻⁸

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak diprotic acid H₂A (0.10 mol L⁻¹) with a strong base of the same concentration?

A popular buffer solution consists of carbonate (CO₃²⁻) and hydrogen carbonate (HCO₃⁻) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?