Question 1

The Ksp for silver(I)phosphate is 1.8 * 10-18. Calculate the molar solubility of silver(I)phosphate.

Accepted Answer

A) 1.6 * 10-5 M 
B) 2.1 * 10-5 M 
C) 3.7 * 10-5 M 
D) 7.2 * 10-1 M 
E) 1.8 * 10-1 M 
A) 1.6 * 10-5 M 
B) 2.1 * 10-5 M 
C) 3.7 * 10-5 M 
D) 7.2 * 10-1 M 
E) 1.8 * 10-1 M

Question 2

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 3

Which of the following would decrease the Ksp for PbI2?

Accepted Answer

A) Lowering the pH of the solution 
B) Adding a solution of Pb(NO3)2 
C) Adding a solution of KI 
D) None of the above-the Ksp of a compound is constant at constant temperature. 
A) Lowering the pH of the solution 
B) Adding a solution of Pb(NO3)2 
C) Adding a solution of KI 
D) None of the above-the Ksp of a compound is constant at constant temperature.

Question 4

Will a precipitate of magnesium fluoride form when 200.mL of 1.9 * 10-3 M MgCl2 are added to 300.mL of 1.4 * 10-2 M NaF? [Ksp (MgF2)= 6.9 * 10-9]

Accepted Answer

A) Yes, Q > Ksp 
B) No, Q sp 
C) No, Q = Ksp 
D) Yes, Q sp 
A) Yes, Q > Ksp 
B) No, Q sp 
C) No, Q = Ksp 
D) Yes, Q sp

Question 5

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 6

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 7

Write an equation showing the net reaction that occurs when a strong base is added to a CO32-/HCO3- buffer solution (for carbonic acid, Ka1 = 4.2 * 10-7, Ka2 = 2.4 * 10-8):

Accepted Answer

HCO<sub>3</sub><sup>

Question 8

The solubility of a salt increases as its Ksp increases.

Accepted Answer

A) True 
 B)False

Question 9

The Ksp for silver(I)phosphate is 1.8 * 10-18. Determine the silver ion concentration in a saturated solution of silver(I)phosphate.

Accepted Answer

A) 1.6 * 10-5 M 
B) 2.1 * 10-5 M 
C) 3.7 * 10-5 M 
D) 1.1 * 10-13 M 
E) 4.8 * 10-5 M 
A) 1.6 * 10-5 M 
B) 2.1 * 10-5 M 
C) 3.7 * 10-5 M 
D) 1.1 * 10-13 M 
E) 4.8 * 10-5 M

Question 10

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 pH of the lake?

Accepted Answer

The answer of An environmental chemist obtained a 200.mL sample...

The K_sp for silver(I)phosphate is 1.8 * 10^-18. Calculate the molar solubility of silver(I)phosphate.

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

Which of the following would decrease the K_sp for PbI₂?

Will a precipitate of magnesium fluoride form when 200.mL of 1.9 * 10^-3 M MgCl₂ are added to 300.mL of 1.4 * 10^-2 M NaF? [K_sp (MgF₂)= 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]

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?

Write an equation showing the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 * 10^-7, K_a2 = 2.4 * 10^-8):

The solubility of a salt increases as its K_sp increases.

The K_sp for silver(I)phosphate is 1.8 * 10^-18. Determine the silver ion concentration in a saturated solution of silver(I)phosphate.

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 pH of the lake?

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

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 Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Nuclear Chemistry

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Synthetic and Natural Organic Polymers

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Exam 16: Acid-Base Equilibria and Solubility Equilibria

The Ksp for silver(I)phosphate is 1.8 * 10-18. Calculate the molar solubility of silver(I)phosphate.

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

Which of the following would decrease the Ksp for PbI2?

Will a precipitate of magnesium fluoride form when 200.mL of 1.9 * 10-3 M MgCl2 are added to 300.mL of 1.4 * 10-2 M NaF? [Ksp (MgF2)= 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]

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?

Write an equation showing the net reaction that occurs when a strong base is added to a CO32-/HCO3- buffer solution (for carbonic acid, Ka1 = 4.2 * 10-7, Ka2 = 2.4 * 10-8):

The solubility of a salt increases as its Ksp increases.

The Ksp for silver(I)phosphate is 1.8 * 10-18. Determine the silver ion concentration in a saturated solution of silver(I)phosphate.

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 pH of the lake?

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

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 Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Nuclear Chemistry

Organic Chemistry

Synthetic and Natural Organic Polymers

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The K_sp for silver(I)phosphate is 1.8 * 10^-18. Calculate the molar solubility of silver(I)phosphate.

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

Which of the following would decrease the K_sp for PbI₂?

Will a precipitate of magnesium fluoride form when 200.mL of 1.9 * 10^-3 M MgCl₂ are added to 300.mL of 1.4 * 10^-2 M NaF? [K_sp (MgF₂)= 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]

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?

Write an equation showing the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 * 10^-7, K_a2 = 2.4 * 10^-8):

The solubility of a salt increases as its K_sp increases.

The K_sp for silver(I)phosphate is 1.8 * 10^-18. Determine the silver ion concentration in a saturated solution of silver(I)phosphate.