Question 1

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 2

Calculate the equilibrium constant Kc for the net reaction shown below.
AgI(s)+ 2NH3(aq) $\rarr$ Ag(NH3)2+(aq)+ I-(aq)
For AgI, Ksp = 8.3 * 10-17; for Ag(NH3)2+, Kf = 1.5 * 107.

Accepted Answer

1.2 * 10<s

Question 3

The solubility product for barium sulfate is 1.1 * 10-10. Calculate the molar solubility of barium sulfate.

Accepted Answer

A) 5.5 * 10-11 mol/L 
B) 1.1 * 10-5 mol/L 
C) 2.1 * 10-5 mol/L 
D) 1.1  * 10-10 mol/L 
E) 2.2 * 10-10 mol/L 
A) 5.5 * 10-11 mol/L 
B) 1.1 * 10-5 mol/L 
C) 2.1 * 10-5 mol/L 
D) 1.1  * 10-10 mol/L 
E) 2.2 * 10-10 mol/L

Question 4

A sample of rainwater collected near a lead smelter is analyzed for acid content. Experiments show that a 100. mL sample of the rainwater is neutralized by 22.4 milliters of 0.0122 M NaOH. Assuming that the acid present is sulfurous acid, which resulted from the reaction of SO2 with water, what is the molarity of acid in the rainwater?

Accepted Answer

1.37 * 10<

Question 5

Find the concentration of Pb2+ ions in a solution made by adding 5.00 g of lead(II)iodide to 500. mL of 0.150 M KI. [For PbI2, Ksp = 1.39 * 10-8.]

Accepted Answer

A) 3.04 * 10-4 M 
B) 1.54 * 10-7 M 
C) 6.18 * 10-7 M 
D) 1.52 * 10-4 M 
E) 9.27 * 10-8 M 
A) 3.04 * 10-4 M 
B) 1.54 * 10-7 M 
C) 6.18 * 10-7 M 
D) 1.52 * 10-4 M 
E) 9.27 * 10-8 M

Question 6

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF2 , Ksp = 6.9 * 10-9.)

Accepted Answer

A) 1.4 * 107 M 
B) 6.9 * 10-9 M 
C) 6.9 * 10-8 M 
D) 1.7 * 10-7 M 
E) 6.9 * 10-7 M 
A) 1.4 * 107 M 
B) 6.9 * 10-9 M 
C) 6.9 * 10-8 M 
D) 1.7 * 10-7 M 
E) 6.9 * 10-7 M

Question 7

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH)and 0.20 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka = 1.8 * 10-5]

Accepted Answer

A) 4.65 
B) 4.71 
C) 4.56 
D) 4.84 
E) 5.07 
A) 4.65 
B) 4.71 
C) 4.56 
D) 4.84 
E) 5.07

Question 8

Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO2/HNO2 buffer.

Accepted Answer

H+ + NO<s

Question 9

The molar solubility of manganese(II)carbonate is 4.2 * 10-6 M. What is Ksp for this compound?

Accepted Answer

A) 4.2 * 10-6 
B) 8.4 * 10-6 
C) 3.0 * 10-16 
D) 1.8 * 10-11 
E) 2.0 * 10-3 
A) 4.2 * 10-6 
B) 8.4 * 10-6 
C) 3.0 * 10-16 
D) 1.8 * 10-11 
E) 2.0 * 10-3

Question 10

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO2/HNO2 buffer.

Accepted Answer

OH- + HNO

Question 11

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 12

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

The answer of Calculate the pH at the equivalence point...

Question 13

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20? [Ka(C6H5COOH)= 6.5 * 10-5]

Accepted Answer

The answer of What molar ratio of benzoate ion to...

Question 14

An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H+ in the lake?

Accepted Answer

1.8 * 10<s

Question 15

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 16

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide solution is added to a buffer solution containing NH4Cl and NH3.

Accepted Answer

OH- + NH<

Question 17

Will a precipitate (ppt)form when 20.0 mL of 1.1 * 10-3 M Ba(NO3)2 are added to 80.0 mL of 8.4 * 10-4 M Na2CO3?

Accepted Answer

A) Yes, the ppt is Ba(NO3)2. 
B) Yes, the ppt is NaNO3. 
C) Yes, the ppt is BaCO3. 
D) Yes, the ppt is Na2CO3. 
E) No, a precipitate will not form. 
A) Yes, the ppt is Ba(NO3)2. 
B) Yes, the ppt is NaNO3. 
C) Yes, the ppt is BaCO3. 
D) Yes, the ppt is Na2CO3. 
E) No, a precipitate will not form.

Question 18

Which one of the following is a buffer solution?

Accepted Answer

A) 0.40 M HCN and 0.10 KCN 
B) 0.20 M CH3COOH 
C) 1.0 M HNO3 and 1.0 M NaNO3 
D) 0.10 M KCN 
E) 0.50 M HCl and 0.10 NaCl 
A) 0.40 M HCN and 0.10 KCN 
B) 0.20 M CH3COOH 
C) 1.0 M HNO3 and 1.0 M NaNO3 
D) 0.10 M KCN 
E) 0.50 M HCl and 0.10 NaCl

Question 19

What volume of 0.200 M potassium hydroxide should be added to 300. mL of 0.150 M propanoic acid (C2H5COOH)to obtain a solution with a pH of 5.25? [Ka(C2H5COOH)= 1.34 * 10-5]

Accepted Answer

A) 32 mL 
B) 210 mL 
C) 160 mL 
D) 65 mL 
E) 13 mL 
A) 32 mL 
B) 210 mL 
C) 160 mL 
D) 65 mL 
E) 13 mL

Question 20

Calculate the pH at the equivalence point for the titration of 0.25 M CH3COOH with 0.25 M NaOH. (For CH3COOH, Ka= 1.8 * 10-5)

Accepted Answer

The answer of Calculate the pH at the equivalence point...

Exam 17: Acid-Base Equilibria and Solubility Equilibria

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

Calculate the equilibrium constant Kc for the net reaction shown below. AgI(s)+ 2NH3(aq) →\rarr→ Ag(NH3)2+(aq)+ I-(aq) For AgI, Ksp = 8.3 * 10-17; for Ag(NH3)2+, Kf = 1.5 * 107.

The solubility product for barium sulfate is 1.1 * 10-10. Calculate the molar solubility of barium sulfate.

Find the concentration of Pb2+ ions in a solution made by adding 5.00 g of lead(II)iodide to 500. mL of 0.150 M KI. [For PbI2, Ksp = 1.39 * 10-8.]

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF2 , Ksp = 6.9 * 10-9.)

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH)and 0.20 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka = 1.8 * 10-5]

Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO2/HNO2 buffer.

The molar solubility of manganese(II)carbonate is 4.2 * 10-6 M. What is Ksp for this compound?

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO2/HNO2 buffer.

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

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)

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20? [Ka(C6H5COOH)= 6.5 * 10-5]

An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H+ in the lake?

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

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide solution is added to a buffer solution containing NH4Cl and NH3.

Will a precipitate (ppt)form when 20.0 mL of 1.1 * 10-3 M Ba(NO3)2 are added to 80.0 mL of 8.4 * 10-4 M Na2CO3?

Which one of the following is a buffer solution?

What volume of 0.200 M potassium hydroxide should be added to 300. mL of 0.150 M propanoic acid (C2H5COOH)to obtain a solution with a pH of 5.25? [Ka(C2H5COOH)= 1.34 * 10-5]

Calculate the pH at the equivalence point for the titration of 0.25 M CH3COOH with 0.25 M NaOH. (For CH3COOH, Ka= 1.8 * 10-5)

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

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

Calculate the equilibrium constant K_c for the net reaction shown below. AgI(s)+ 2NH₃(aq) $\rarr$ Ag(NH₃)₂⁺(aq)+ I^-(aq) For AgI, K_sp = 8.3 * 10^-17; for Ag(NH₃)₂⁺, K_f = 1.5 * 10⁷.

The solubility product for barium sulfate is 1.1 * 10^-10. Calculate the molar solubility of barium sulfate.

Find the concentration of Pb²⁺ ions in a solution made by adding 5.00 g of lead(II)iodide to 500. mL of 0.150 M KI. [For PbI₂, K_sp = 1.39 * 10^-8.]

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF₂ , K_sp = 6.9 * 10^-9.)

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH₃COOH)and 0.20 M sodium acetate (CH₃COONa). What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [K_a = 1.8 * 10^-5]

Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO₂/HNO₂ buffer.

The molar solubility of manganese(II)carbonate is 4.2 * 10^-6 M. What is K_sp for this compound?

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO₂/HNO₂ buffer.

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 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)

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20? [K_a(C₆H₅COOH)= 6.5 * 10^-5]

An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H⁺ in the lake?

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide solution is added to a buffer solution containing NH₄Cl and NH₃.

Will a precipitate (ppt)form when 20.0 mL of 1.1 * 10^-3 M Ba(NO₃)₂ are added to 80.0 mL of 8.4 * 10^-4 M Na₂CO₃?

What volume of 0.200 M potassium hydroxide should be added to 300. mL of 0.150 M propanoic acid (C₂H₅COOH)to obtain a solution with a pH of 5.25? [K_a(C₂H₅COOH)= 1.34 * 10^-5]

Calculate the pH at the equivalence point for the titration of 0.25 M CH₃COOH with 0.25 M NaOH. (For CH₃COOH, K_a= 1.8 * 10^-5)