Question 1

The molar solubility of lead(II) iodate in water is 4.0 * 10-5 mol/L. Calculate Ksp for lead(II) iodate.

Accepted Answer

A)  1.6 * 10-9 
B)  6.4 * 10-14 
C)  2.6 * 10-13 
D)  4.0 * 10-5 
E)  4.0 * 10-15 
A)  1.6 * 10-9 
B)  6.4 * 10-14 
C)  2.6 * 10-13 
D)  4.0 * 10-5 
E)  4.0 * 10-15

Question 2

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed

Accepted Answer

A)  0.10M H2CO3 and 0.050M HCl 
B)  0.10M H2CO3 and 0.10M KOH 
C)  0.10M H2CO3 and 0.10M HCl 
D)  0.10M H2CO3 and 0.050M KOH 
E)  0.10M K2CO3 and 0.050M KOH 
A)  0.10M H2CO3 and 0.050M HCl 
B)  0.10M H2CO3 and 0.10M KOH 
C)  0.10M H2CO3 and 0.10M HCl 
D)  0.10M H2CO3 and 0.050M KOH 
E)  0.10M K2CO3 and 0.050M KOH

Question 3

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed

Accepted Answer

A)  0.10M HCl and 0.10 M NaCl 
B)  0.15 M HNO3 and 0.15 M NaNO3 
C)  0.10M HF and 0.10M NaF 
D)  0.10M HClO4 and 0.10 NaClO4 
E)  0.15M HBr and 0.15M NaBr 
A)  0.10M HCl and 0.10 M NaCl 
B)  0.15 M HNO3 and 0.15 M NaNO3 
C)  0.10M HF and 0.10M NaF 
D)  0.10M HClO4 and 0.10 NaClO4 
E)  0.15M HBr and 0.15M NaBr

Question 4

Calculate the silver ion concentration in a saturated solution of silver(I) sulfate (Ksp = 1.4 * 10-5).

Accepted Answer

A)  1.5 * 10-2 M 
B)  2.4 * 10-2 M 
C)  3.0 * 10-2 M 
D)  1.4 * 10-5 M 
E)  None of the above. 
A)  1.5 * 10-2 M 
B)  2.4 * 10-2 M 
C)  3.0 * 10-2 M 
D)  1.4 * 10-5 M 
E)  None of the above.

Question 5

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH. (Ka = 4.9 * 10-10 for HCN)

Accepted Answer

A)  10.58 
B)  10.78 
C)  10.98 
D)  11.18 
E)  None of the above 
A)  10.58 
B)  10.78 
C)  10.98 
D)  11.18 
E)  None of the above

Question 6

Acid dissociation constants for phosphoric acid are given below. $\begin{array}{|l|l|l|l|}
\hline & \mathrm{K}_{\mathrm{a} 1} & \mathrm{~K}_{\mathrm{a} 2} & \mathrm{~K}_{\mathrm{a} 3} \
\hline \mathrm{H}_{3} \mathrm{PO}_{4} & 7.5 \times 10^{-3} & 6.2 \times 10^{-8} & 4.8 \times 10^{-13} \
\hline
\end{array}$ A buffer with a pH = 7.4 can best be made by using

Accepted Answer

A)  H3PO4 and NaH2PO4. 
B)  NaH2PO4 and Na2HPO4. 
C)  Na2HPO4 and Na3PO4. 
D)  only NaH2PO4. 
E)  only Na2HPO4. 
A)  H3PO4 and NaH2PO4. 
B)  NaH2PO4 and Na2HPO4. 
C)  Na2HPO4 and Na3PO4. 
D)  only NaH2PO4. 
E)  only Na2HPO4.

Question 7

The molar solubility of magnesium carbonate is 1.8 * 10-4 mol/L. What is Ksp for this compound

Accepted Answer

A)  1.8 * 10-4 
B)  3.6 * 10-4 
C)  1.3 * 10-7 
D)  3.2 * 10-8 
E)  2.8 * 10-14 
A)  1.8 * 10-4 
B)  3.6 * 10-4 
C)  1.3 * 10-7 
D)  3.2 * 10-8 
E)  2.8 * 10-14

Question 8

Which of the following compounds is more soluble in acidic solution than in pure neutral water

Accepted Answer

A)  PbI2 
B)  CuBr 
C)  KClO4 
D)  FeS 
E)  NaNO3 
A)  PbI2 
B)  CuBr 
C)  KClO4 
D)  FeS 
E)  NaNO3

Question 9

The molar solubility of tin(II) iodide is 1.28 * 10-2 mol/L. What is Ksp for this compound

Accepted Answer

A)  8.4 * 10-6 
B)  1.28 * 10-2 
C)  4.2 * 10-6 
D)  1.6 * 10-4 
E)  2.1 * 10-6 
A)  8.4 * 10-6 
B)  1.28 * 10-2 
C)  4.2 * 10-6 
D)  1.6 * 10-4 
E)  2.1 * 10-6

Question 10

Calculate the pH of a buffer solution prepared by dissolving 0.2 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 1.0 liter of solution. [Ka(HCNO) = 2.0 * 10-4]

Accepted Answer

A)  0 
B)  3.0 
C)  3.7 
D)  4.4 
E)  5.0 
A)  0 
B)  3.0 
C)  3.7 
D)  4.4 
E)  5.0

Question 11

The concentration of Mg2+ in seawater is 5.0 * 10-2 M. What hydroxide concentration is needed to remove 90% of the Mg2+ by precipitation (For Mg(OH)2, Ksp = 1.2 * 10-11.)

Accepted Answer

A)  5.1 * 10-5 M 
B)  4.9 * 10-5 M 
C)  4.7 * 10-5 M 
D)  4.5 * 10-5 M 
E)  None of the above 
A)  5.1 * 10-5 M 
B)  4.9 * 10-5 M 
C)  4.7 * 10-5 M 
D)  4.5 * 10-5 M 
E)  None of the above

Question 12

Which one of the following combinations cannot function as a buffer solution

Accepted Answer

A)  HCN and KCN 
B)  NH3 and (NH4)2SO4 
C)  HNO3 and NaNO3 
D)  HF and NaF 
E)  HNO2 and NaNO2 
A)  HCN and KCN 
B)  NH3 and (NH4)2SO4 
C)  HNO3 and NaNO3 
D)  HF and NaF 
E)  HNO2 and NaNO2

Question 13

For which type of titration will the pH be neutral at the equivalence point

Accepted Answer

A)  Strong acid vs. strong base. 
B)  Strong acid vs. weak base. 
C)  Weak acid vs. strong base. 
D)  All of the above. 
E)  None of the above. 
A)  Strong acid vs. strong base. 
B)  Strong acid vs. weak base. 
C)  Weak acid vs. strong base. 
D)  All of the above. 
E)  None of the above.

Question 14

What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution

Accepted Answer

A) H+ + H2O $\rarr$H3O+ 
B) H+ + OCl- $\rarr$ HOCl 
C) HOCl $\rarr$ H+ + OCl- 
D) H+ + HOCl $\rarr$ H2OCl+ 
E) HCl + HOCl $\rarr$ H2O + Cl2 
A) H+ + H2O $\rarr$H3O+ 
B) H+ + OCl- $\rarr$ HOCl 
C) HOCl $\rarr$ H+ + OCl- 
D) H+ + HOCl $\rarr$ H2OCl+ 
E) HCl + HOCl $\rarr$ H2O + Cl2

Question 15

At 25 $\circ$C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the hydroxide ion concentration in a 0.150 M solution of ammonia at 25 $\circ$C.

Accepted Answer

A)  1.6 * 10-2 M 
B)  3.2 * 10-2 M 
C)  1.6 * 10-3 M 
D)  3.2 * 10-3M 
E)  None of the above 
A)  1.6 * 10-2 M 
B)  3.2 * 10-2 M 
C)  1.6 * 10-3 M 
D)  3.2 * 10-3M 
E)  None of the above

Question 16

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (Ka = 4.9 * 10-10) with 0.10 M NaOH

Accepted Answer

A)  3.0 
B)  6.0 
C)  7.0 
D)  11.0 
E)  12.0 
A)  3.0 
B)  6.0 
C)  7.0 
D)  11.0 
E)  12.0

Question 17

The Ksp of CaF2 is 4 * 10-11. What is the maximum concentration of Ca2+ possible in a 0.10 M NaF solution

Accepted Answer

A)  4 * 10-7 M 
B)  4 * 10- 8 M 
C)  4 * 10-9 M 
D)  4 * 10-10 M 
E)  None of the above 
A)  4 * 10-7 M 
B)  4 * 10- 8 M 
C)  4 * 10-9 M 
D)  4 * 10-10 M 
E)  None of the above

Question 18

Within what pH range is a HOCl - NaOCl buffer effective

Accepted Answer

A)  pH 2.0 - pH 4.0 
B)  pH 7.5 - pH 9.5 
C)  pH 6.5 - pH 8.5 
D)  pH 6.5 - pH 9.5 
E)  pH 1.0 - pH 14.0 
A)  pH 2.0 - pH 4.0 
B)  pH 7.5 - pH 9.5 
C)  pH 6.5 - pH 8.5 
D)  pH 6.5 - pH 9.5 
E)  pH 1.0 - pH 14.0

Question 19

At 25 $\circ$C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100. mL of 0.150 M ammonia.

Accepted Answer

A)  3.47 
B)  8.73 
C)  10.4 
D)  12.3 
E)  None of the above 
A)  3.47 
B)  8.73 
C)  10.4 
D)  12.3 
E)  None of the above

Question 20

Calculate the percent ionization of cyanic acid, Ka = 2.0 * 10-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO.

Accepted Answer

A)  0.02% 
B)  0.10% 
C)  0.20% 
D)  2.0% 
E)  20% 
A)  0.02% 
B)  0.10% 
C)  0.20% 
D)  2.0% 
E)  20%

Exam 16: Acid-Base Equilibria and Solubility Equilibria

The molar solubility of lead(II) iodate in water is 4.0 * 10-5 mol/L. Calculate Ksp for lead(II) iodate.

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed

Calculate the silver ion concentration in a saturated solution of silver(I) sulfate (Ksp = 1.4 * 10-5).

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH. (Ka = 4.9 * 10-10 for HCN)

Acid dissociation constants for phosphoric acid are given below. 7.5\times1 6.2\times1 4.8\times1 A buffer with a pH = 7.4 can best be made by using

The molar solubility of magnesium carbonate is 1.8 * 10-4 mol/L. What is Ksp for this compound

Which of the following compounds is more soluble in acidic solution than in pure neutral water

The molar solubility of tin(II) iodide is 1.28 * 10-2 mol/L. What is Ksp for this compound

Calculate the pH of a buffer solution prepared by dissolving 0.2 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 1.0 liter of solution. [Ka(HCNO) = 2.0 * 10-4]

The concentration of Mg2+ in seawater is 5.0 * 10-2 M. What hydroxide concentration is needed to remove 90% of the Mg2+ by precipitation (For Mg(OH)2, Ksp = 1.2 * 10-11.)

Which one of the following combinations cannot function as a buffer solution

For which type of titration will the pH be neutral at the equivalence point

What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution

At 25 ∘\circ∘ C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the hydroxide ion concentration in a 0.150 M solution of ammonia at 25 ∘\circ∘ C.

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (Ka = 4.9 * 10-10) with 0.10 M NaOH

The Ksp of CaF2 is 4 * 10-11. What is the maximum concentration of Ca2+ possible in a 0.10 M NaF solution

Within what pH range is a HOCl - NaOCl buffer effective

At 25 ∘\circ∘ C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100. mL of 0.150 M ammonia.

Calculate the percent ionization of cyanic acid, Ka = 2.0 * 10-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO.

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

The molar solubility of lead(II) iodate in water is 4.0 * 10^-5 mol/L. Calculate K_sp for lead(II) iodate.

Calculate the silver ion concentration in a saturated solution of silver(I) sulfate (K_sp = 1.4 * 10^-5).

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH. (K_a = 4.9 * 10^-10 for HCN)

The molar solubility of magnesium carbonate is 1.8 * 10^-4 mol/L. What is K_sp for this compound

The molar solubility of tin(II) iodide is 1.28 * 10^-2 mol/L. What is K_sp for this compound

Calculate the pH of a buffer solution prepared by dissolving 0.2 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 1.0 liter of solution. [K_a(HCNO) = 2.0 * 10^-4]

The concentration of Mg²⁺ in seawater is 5.0 * 10^-2 M. What hydroxide concentration is needed to remove 90% of the Mg²⁺ by precipitation (For Mg(OH)₂, K_sp = 1.2 * 10^-11.)

At 25 ^$\circ$C, the base ionization constant for NH₃ is 1.8 * 10^-5. Determine the hydroxide ion concentration in a 0.150 M solution of ammonia at 25 ^$\circ$C.

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (K_a = 4.9 * 10^-10) with 0.10 M NaOH

The K_sp of CaF₂ is 4 * 10^-11. What is the maximum concentration of Ca²⁺ possible in a 0.10 M NaF solution

At 25 ^$\circ$C, the base ionization constant for NH₃ is 1.8 * 10^-5. Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100. mL of 0.150 M ammonia.

Calculate the percent ionization of cyanic acid, K_a = 2.0 * 10^-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO.