Question 1

Explain why we cannot directly compare Ksp values in comparing solubilities of ionic solids with different numbers of ions.

Accepted Answer

See Sectio

Question 2

A 200-mL solution contains 0.018 mol each of I-, Br-, and Cl-. When the solution is mixed with 200 mL of 0.24 M AgNO3, how much AgCl(s) precipitates out?

Accepted Answer

A)  2.6 g 
B)  0.0 g 
C)  3.3 g 
D)  5.0 g 
E)  1.7 g 
A)  2.6 g 
B)  0.0 g 
C)  3.3 g 
D)  5.0 g 
E)  1.7 g

Question 3

After adding 25.0 mL of 0.100 M NaOH to 100.0 mL of 0.100 M weak acid (HA), the pH is found to be 5.90. Determine the value of Ka for the acid HA.

Accepted Answer

A)  4.2 F1F1F1S1F1F1F10 10-7 
B)  3.5 F1F1F1S1F1F1F10 10-9 
C)  1.6 F1F1F1S1F1F1F10 10-11 
D)  2.1 F1F1F1S1F1F1F10 10-5 
E)  none of these 
A)  4.2 F1F1F1S1F1F1F10 10-7 
B)  3.5 F1F1F1S1F1F1F10 10-9 
C)  1.6 F1F1F1S1F1F1F10 10-11 
D)  2.1 F1F1F1S1F1F1F10 10-5 
E)  none of these

Question 4

Equal volumes of 0.1 M HCl and 0.1 M HC2H3O2 are titrated with 0.1 M NaOH. Which of the following would be equal for both titrations?

Accepted Answer

A)  the pH at the equivalence point 
B)  the volume of NaOH added to reach the equivalence point 
C)  the initial pH 
D)  the pH at the halfway point 
E)  two of the above 
A)  the pH at the equivalence point 
B)  the volume of NaOH added to reach the equivalence point 
C)  the initial pH 
D)  the pH at the halfway point 
E)  two of the above

Question 5

Consider the titration of 200.0 mL of a 0.100 M solution of the weak acid H2A with 0.200 M NaOH. The first equivalence point is reached after 100.0 mL of 0.200 M NaOH has been added, and the pH is 6.27. The pH after 65.0 mL of 0.200 M NaOH has been added, the pH is 4.95. Calculate the value of Ka1 for H2A.

Accepted Answer

A)  2.10 F1F1F1S1F1F1F10 10-5 
B)  5.37 F1F1F1S1F1F1F10 10-7 
C)  1.40 F1F1F1S1F1F1F10 10-8 
D)  1.12 F1F1F1S1F1F1F10 10-5 
E)  none of these 
A)  2.10 F1F1F1S1F1F1F10 10-5 
B)  5.37 F1F1F1S1F1F1F10 10-7 
C)  1.40 F1F1F1S1F1F1F10 10-8 
D)  1.12 F1F1F1S1F1F1F10 10-5 
E)  none of these

Question 6

Which of the following solutions will be the best buffer at a pH of 9.26? (Ka for HC2H3O2 is 1.8 F1F1F1S1F1F1F10 10-5; Kb for NH3 is 1.8 F1F1F1S1F1F1F10 10-5.)

Accepted Answer

A)  0.20 M NH3 and 0.20 M NH4Cl 
B)  3.0 M HC2H3O2 and 3.0 M NH4Cl 
C)  0.20 M HC2H3O2 and 0.20 M NaC2H3O2 
D)  3.0 M NH3 and 3.0 M NH4Cl 
E)  3.0 M HC2H3O2 and 3.0 M NH3 
A)  0.20 M NH3 and 0.20 M NH4Cl 
B)  3.0 M HC2H3O2 and 3.0 M NH4Cl 
C)  0.20 M HC2H3O2 and 0.20 M NaC2H3O2 
D)  3.0 M NH3 and 3.0 M NH4Cl 
E)  3.0 M HC2H3O2 and 3.0 M NH3

Question 7

You have a solution of 0.10 M Cl- and   . You add 0.10 M silver nitrate dropwise into the solution. Ksp for Ag2CrO4 is 9.0 F1F1F1S1F1F1F10 10-12 and for AgCl is1.6 F1F1F1S1F1F1F10 10-10. Which of the following will precipitate first?

Accepted Answer

A)  silver nitrate 
B)  silver chromate 
C)  cannot be determined from the information given 
D)  silver chloride 
E)  none of these 
A)  silver nitrate 
B)  silver chromate 
C)  cannot be determined from the information given 
D)  silver chloride 
E)  none of these

Question 8

Explain how the solubility of an ionic solid at a constant temperature for a given ionic solid can vary.

Accepted Answer

See Sectio

Question 9

11.8 mL of 0.30 M HCl is added to a 122.0-mL sample of 0.210 M HNO2 (Ka for HNO2 = 4.0 F1F1F1S1F1F1F10 10-4). What is the equilibrium concentration of NO2- ions?

Accepted Answer

A)  2.9 F1F1F1S1F1F1F10 10-3 M 
B)  2.6 F1F1F1S1F1F1F10 10-2 M 
C)  4.2F1F1F1S1F1F1F10F1F1F1S1F1F1F10 10-3 M 
D)  5.5 F1F1F1S1F1F1F10 10-4 M 
E)  9.2 F1F1F1S1F1F1F10 10-3 M 
A)  2.9 F1F1F1S1F1F1F10 10-3 M 
B)  2.6 F1F1F1S1F1F1F10 10-2 M 
C)  4.2F1F1F1S1F1F1F10F1F1F1S1F1F1F10 10-3 M 
D)  5.5 F1F1F1S1F1F1F10 10-4 M 
E)  9.2 F1F1F1S1F1F1F10 10-3 M

Question 10

What is the solubility of Mg(OH)2 (Ksp = 8.9 F1F1F1S1F1F1F10 10-12) in 1.0 L of a solution buffered (with large capacity) at pH 10.0?

Accepted Answer

A)  8.9 F1F1F1S1F1F1F10 10-1 mol 
B)  8.9 F1F1F1S1F1F1F10 10-4 mol 
C)  8.9 F1F1F1S1F1F1F10 109 mol 
D)  8.9 F1F1F1S1F1F1F10 10-7 mol 
E)  none of these 
A)  8.9 F1F1F1S1F1F1F10 10-1 mol 
B)  8.9 F1F1F1S1F1F1F10 10-4 mol 
C)  8.9 F1F1F1S1F1F1F10 109 mol 
D)  8.9 F1F1F1S1F1F1F10 10-7 mol 
E)  none of these

Question 11

Silver acetate (AgC2H3O2) is a sparingly soluble salt with Ksp = 1.9 F1F1F1S1F1F1F10 10-3. Consider a saturated solution in equilibrium with the solid salt. Compare the effects on the solubility of adding to the solution either the acid HNO3 or the base NH3.

Accepted Answer

A)  NH3 would increase the solubility, but HNO3 would decrease it. 
B)  NH3 would decrease the solubility, but HNO3 would increase it. 
C)  NH3 would increase the solubility, but HNO3 would have virtually no effect. 
D)  Either substance would decrease the solubility. 
E)  Either substance would increase the solubility. 
A)  NH3 would increase the solubility, but HNO3 would decrease it. 
B)  NH3 would decrease the solubility, but HNO3 would increase it. 
C)  NH3 would increase the solubility, but HNO3 would have virtually no effect. 
D)  Either substance would decrease the solubility. 
E)  Either substance would increase the solubility.

Question 12

The two salts AgX and AgY have very similar solubilities in water. The salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY?

Accepted Answer

A)  HY is stronger than HX. 
B)  Nothing can be said about their relative strengths. 
C)  HX is stronger than HY. 
D)  The acids have equal strengths. 
A)  HY is stronger than HX. 
B)  Nothing can be said about their relative strengths. 
C)  HX is stronger than HY. 
D)  The acids have equal strengths.

Question 13

Calculate the pH of a solution prepared by mixing 50 mL of a 0.10 M solution of HF with 25 mL of a 0.20 M solution of NaF. pKa of HF is 3.14.

Accepted Answer

A)  5.83 
B)  12.00 
C)  3.14 
D)  7.35 
E)  10.80 
A)  5.83 
B)  12.00 
C)  3.14 
D)  7.35 
E)  10.80

Question 14

The value of Ksp for AgI is 1.5 F1F1F1S1F1F1F10 10-16. Calculate the solubility, in moles per liter, of AgI in a 0.36 M NaI solution.

Accepted Answer

A)  1.2 F1F1F1S1F1F1F10 10-8 mol/L 
B)  4.2 F1F1F1S1F1F1F10 10-16 mol/L 
C)  2.4 F1F1F1S1F1F1F10 10-9 mol/L 
D)  5.4 F1F1F1S1F1F1F10 10-17 mol/L 
E)  2.0 F1F1F1S1F1F1F10 10-8 mol/L 
A)  1.2 F1F1F1S1F1F1F10 10-8 mol/L 
B)  4.2 F1F1F1S1F1F1F10 10-16 mol/L 
C)  2.4 F1F1F1S1F1F1F10 10-9 mol/L 
D)  5.4 F1F1F1S1F1F1F10 10-17 mol/L 
E)  2.0 F1F1F1S1F1F1F10 10-8 mol/L

Question 15

You have 0.20 M HNO2 (Ka = 4.0 *10-4) and 0.20 M KNO2. You need 1.00 L of a buffered solution at a pH of 3.00. What volumes of each solution do you add together to make this buffered solution?

Accepted Answer

714 mL of 0.20 M HNO

Question 16

You are given a solution of the weak base Novocain, Nvc. Its pH is 11.00. You add to the solution a small amount of a salt containing the conjugate acid of Novocain, NvcH+. Which statement is true?

Accepted Answer

A)  The pH and the pOH remain unchanged. 
B)  The pH and the pOH both decrease. 
C)  The pH and the pOH both increase. 
D)  The pH increases and pOH decreases. 
E)  The pH decreases and the pOH increases. 
A)  The pH and the pOH remain unchanged. 
B)  The pH and the pOH both decrease. 
C)  The pH and the pOH both increase. 
D)  The pH increases and pOH decreases. 
E)  The pH decreases and the pOH increases.

Question 17

Calculate the pH when 200.0 mL of a 1.00 M solution of HS1U1B12S1U1B0A (KS1U1B1a1S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P16S1S1P0, KS1U1B1a2S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P110S1S1P0) is titrated with the following volumes of 1.00 M NaOH.
-0 mL of 1.00 M NaOH

Accepted Answer

A)  3.00 
B)  6.00 
C)  0 
D)  3.35 
E)  None of these 
A)  3.00 
B)  6.00 
C)  0 
D)  3.35 
E)  None of these

Question 18

Calculate the pH when 200.0 mL of a 1.00 M solution of HS1U1B12S1U1B0A (KS1U1B1a1S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P16S1S1P0, KS1U1B1a2S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P110S1S1P0) is titrated with the following volumes of 1.00 M NaOH.
-150.0 mL of 1.00 M NaOH

Accepted Answer

A)  6.00 
B)  6.48 
C)  8.00 
D)  8.50 
E)  None of these 
A)  6.00 
B)  6.48 
C)  8.00 
D)  8.50 
E)  None of these

Question 19

Given the following values of equilibrium constants:   What is the value of the equilibrium constant for the following reaction? Cu(OH)2(s) + 4NH3(aq)   Cu(NH3)42+(aq) + 2OH-(aq)

Accepted Answer

A)  1.6 F1F1F1S1F1F1F10 10-19 
B)  1.6 F1F1F1S1F1F1F10 10-6 
C)  6.2 F1F1F1S1F1F1F10 1031 
D)  1.0 F1F1F1S1F1F1F10 1013 
E)  1.6 F1F1F1S1F1F1F10 10-32 
A)  1.6 F1F1F1S1F1F1F10 10-19 
B)  1.6 F1F1F1S1F1F1F10 10-6 
C)  6.2 F1F1F1S1F1F1F10 1031 
D)  1.0 F1F1F1S1F1F1F10 1013 
E)  1.6 F1F1F1S1F1F1F10 10-32

Question 20

Solubility Products (Ksp) 
BaSO4 1.5 F1F1F1S1F1F1F10 10-9 
CoS 5.0 F1F1F1S1F1F1F10 10-22 
PbSO4  1.3 F1F1F1S1F1F1F10 10-8 
AgBr 5.0 F1F1F1S1F1F1F10 10-13
BaCO3 1.6 F1F1F1S1F1F1F10 10-9
Which of the following compounds is the most soluble (in moles per liter)?

Accepted Answer

A)  PbSO4 
B)  BaSO4 
C)  CoS 
D)  AgBr 
E)  BaCO3 
A)  PbSO4 
B)  BaSO4 
C)  CoS 
D)  AgBr 
E)  BaCO3

Explain why we cannot directly compare K_sp values in comparing solubilities of ionic solids with different numbers of ions.

A 200-mL solution contains 0.018 mol each of I^-, Br^-, and Cl^-. When the solution is mixed with 200 mL of 0.24 M AgNO₃, how much AgCl(s) precipitates out?

After adding 25.0 mL of 0.100 M NaOH to 100.0 mL of 0.100 M weak acid (HA), the pH is found to be 5.90. Determine the value of K_a for the acid HA.

Equal volumes of 0.1 M HCl and 0.1 M HC₂H₃O₂ are titrated with 0.1 M NaOH. Which of the following would be equal for both titrations?

Which of the following solutions will be the best buffer at a pH of 9.26? (K_a for HC₂H₃O₂ is 1.8  10^-⁵; K_b for NH₃ is 1.8  10^-⁵.)

You have a solution of 0.10 M Cl^- and . You add 0.10 M silver nitrate dropwise into the solution. K_sp for Ag₂CrO₄ is 9.0  10^-¹² and for AgCl is1.6  10^-¹⁰. Which of the following will precipitate first?

Explain how the solubility of an ionic solid at a constant temperature for a given ionic solid can vary.

11.8 mL of 0.30 M HCl is added to a 122.0-mL sample of 0.210 M HNO₂ (K_a for HNO₂ = 4.0  10^-⁴). What is the equilibrium concentration of NO₂^- ions?

What is the solubility of Mg(OH)₂ (K_sp = 8.9  10^-¹²) in 1.0 L of a solution buffered (with large capacity) at pH 10.0?

Silver acetate (AgC₂H₃O₂) is a sparingly soluble salt with K_sp = 1.9  10^-³. Consider a saturated solution in equilibrium with the solid salt. Compare the effects on the solubility of adding to the solution either the acid HNO₃ or the base NH₃.

The two salts AgX and AgY have very similar solubilities in water. The salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY?

Calculate the pH of a solution prepared by mixing 50 mL of a 0.10 M solution of HF with 25 mL of a 0.20 M solution of NaF. pK_a of HF is 3.14.

The value of K_sp for AgI is 1.5  10^-¹⁶. Calculate the solubility, in moles per liter, of AgI in a 0.36 M NaI solution.

You have 0.20 M HNO₂ (K_a = 4.0 *10^-⁴) and 0.20 M KNO₂. You need 1.00 L of a buffered solution at a pH of 3.00. What volumes of each solution do you add together to make this buffered solution?

You are given a solution of the weak base Novocain, Nvc. Its pH is 11.00. You add to the solution a small amount of a salt containing the conjugate acid of Novocain, NvcH⁺. Which statement is true?

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -0 mL of 1.00 M NaOH

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -150.0 mL of 1.00 M NaOH

Given the following values of equilibrium constants: What is the value of the equilibrium constant for the following reaction? Cu(OH)₂(s) + 4NH₃(aq) Cu(NH₃)₄²⁺(aq) + 2OH^-(aq)

Solubility Products (K_sp) BaSO₄ 1.5  10^-⁹ CoS 5.0  10^-²² PbSO₄ 1.3  10^-⁸ AgBr 5.0  10^-¹³ BaCO₃ 1.6  10^-⁹ Which of the following compounds is the most soluble (in moles per liter)?

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Chemical Equilibrium

Acids and Bases

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

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Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

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The Nucleus: a Chemists View

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Exam 8: Applications of Aqueous Equilibria

Explain why we cannot directly compare Ksp values in comparing solubilities of ionic solids with different numbers of ions.

A 200-mL solution contains 0.018 mol each of I-, Br-, and Cl-. When the solution is mixed with 200 mL of 0.24 M AgNO3, how much AgCl(s) precipitates out?

After adding 25.0 mL of 0.100 M NaOH to 100.0 mL of 0.100 M weak acid (HA), the pH is found to be 5.90. Determine the value of Ka for the acid HA.

Equal volumes of 0.1 M HCl and 0.1 M HC2H3O2 are titrated with 0.1 M NaOH. Which of the following would be equal for both titrations?

Which of the following solutions will be the best buffer at a pH of 9.26? (Ka for HC2H3O2 is 1.8  10-5; Kb for NH3 is 1.8  10-5.)

You have a solution of 0.10 M Cl- and . You add 0.10 M silver nitrate dropwise into the solution. Ksp for Ag2CrO4 is 9.0  10-12 and for AgCl is1.6  10-10. Which of the following will precipitate first?

Explain how the solubility of an ionic solid at a constant temperature for a given ionic solid can vary.

11.8 mL of 0.30 M HCl is added to a 122.0-mL sample of 0.210 M HNO2 (Ka for HNO2 = 4.0  10-4). What is the equilibrium concentration of NO2- ions?

What is the solubility of Mg(OH)2 (Ksp = 8.9  10-12) in 1.0 L of a solution buffered (with large capacity) at pH 10.0?

Silver acetate (AgC2H3O2) is a sparingly soluble salt with Ksp = 1.9  10-3. Consider a saturated solution in equilibrium with the solid salt. Compare the effects on the solubility of adding to the solution either the acid HNO3 or the base NH3.

The two salts AgX and AgY have very similar solubilities in water. The salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY?

Calculate the pH of a solution prepared by mixing 50 mL of a 0.10 M solution of HF with 25 mL of a 0.20 M solution of NaF. pKa of HF is 3.14.

The value of Ksp for AgI is 1.5  10-16. Calculate the solubility, in moles per liter, of AgI in a 0.36 M NaI solution.

You have 0.20 M HNO2 (Ka = 4.0 *10-4) and 0.20 M KNO2. You need 1.00 L of a buffered solution at a pH of 3.00. What volumes of each solution do you add together to make this buffered solution?

You are given a solution of the weak base Novocain, Nvc. Its pH is 11.00. You add to the solution a small amount of a salt containing the conjugate acid of Novocain, NvcH+. Which statement is true?

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0  10-6, Ka2 = 1.0  10-10) is titrated with the following volumes of 1.00 M NaOH. -0 mL of 1.00 M NaOH

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0  10-6, Ka2 = 1.0  10-10) is titrated with the following volumes of 1.00 M NaOH. -150.0 mL of 1.00 M NaOH

Given the following values of equilibrium constants: What is the value of the equilibrium constant for the following reaction? Cu(OH)2(s) + 4NH3(aq) Cu(NH3)42+(aq) + 2OH-(aq)

Solubility Products (Ksp) BaSO4 1.5  10-9 CoS 5.0  10-22 PbSO4 1.3  10-8 AgBr 5.0  10-13 BaCO3 1.6  10-9 Which of the following compounds is the most soluble (in moles per liter)?

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Explain why we cannot directly compare K_sp values in comparing solubilities of ionic solids with different numbers of ions.

A 200-mL solution contains 0.018 mol each of I^-, Br^-, and Cl^-. When the solution is mixed with 200 mL of 0.24 M AgNO₃, how much AgCl(s) precipitates out?

After adding 25.0 mL of 0.100 M NaOH to 100.0 mL of 0.100 M weak acid (HA), the pH is found to be 5.90. Determine the value of K_a for the acid HA.

Equal volumes of 0.1 M HCl and 0.1 M HC₂H₃O₂ are titrated with 0.1 M NaOH. Which of the following would be equal for both titrations?

Which of the following solutions will be the best buffer at a pH of 9.26? (K_a for HC₂H₃O₂ is 1.8  10^-⁵; K_b for NH₃ is 1.8  10^-⁵.)

You have a solution of 0.10 M Cl^- and . You add 0.10 M silver nitrate dropwise into the solution. K_sp for Ag₂CrO₄ is 9.0  10^-¹² and for AgCl is1.6  10^-¹⁰. Which of the following will precipitate first?

11.8 mL of 0.30 M HCl is added to a 122.0-mL sample of 0.210 M HNO₂ (K_a for HNO₂ = 4.0  10^-⁴). What is the equilibrium concentration of NO₂^- ions?

What is the solubility of Mg(OH)₂ (K_sp = 8.9  10^-¹²) in 1.0 L of a solution buffered (with large capacity) at pH 10.0?

Silver acetate (AgC₂H₃O₂) is a sparingly soluble salt with K_sp = 1.9  10^-³. Consider a saturated solution in equilibrium with the solid salt. Compare the effects on the solubility of adding to the solution either the acid HNO₃ or the base NH₃.

Calculate the pH of a solution prepared by mixing 50 mL of a 0.10 M solution of HF with 25 mL of a 0.20 M solution of NaF. pK_a of HF is 3.14.

The value of K_sp for AgI is 1.5  10^-¹⁶. Calculate the solubility, in moles per liter, of AgI in a 0.36 M NaI solution.

You have 0.20 M HNO₂ (K_a = 4.0 *10^-⁴) and 0.20 M KNO₂. You need 1.00 L of a buffered solution at a pH of 3.00. What volumes of each solution do you add together to make this buffered solution?

You are given a solution of the weak base Novocain, Nvc. Its pH is 11.00. You add to the solution a small amount of a salt containing the conjugate acid of Novocain, NvcH⁺. Which statement is true?

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -0 mL of 1.00 M NaOH

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -150.0 mL of 1.00 M NaOH

Given the following values of equilibrium constants: What is the value of the equilibrium constant for the following reaction? Cu(OH)₂(s) + 4NH₃(aq) Cu(NH₃)₄²⁺(aq) + 2OH^-(aq)

Solubility Products (K_sp) BaSO₄ 1.5  10^-⁹ CoS 5.0  10^-²² PbSO₄ 1.3  10^-⁸ AgBr 5.0  10^-¹³ BaCO₃ 1.6  10^-⁹ Which of the following compounds is the most soluble (in moles per liter)?