Question 1

Will a 0.1 M solution of NaH2PO4(aq)be acidic, basic, or neutral?

Accepted Answer

Question 2

The pH of a certain solution is 3.0. How many H+(aq)ions are there in 1.0 L of the solution?

Accepted Answer

A) 0.001 ions 
B) 1,000 ions 
C) 6.* 1020 ions 
D) 3 ions 
E) 6.* 1026 ions 
A) 0.001 ions 
B) 1,000 ions 
C) 6.* 1020 ions 
D) 3 ions 
E) 6.* 1026 ions

Question 3

In the reaction Ag+(aq)+ Cl-(aq)$\rarr$ AgCl(s), Ag+ acts as a Lewis acid.

Accepted Answer

A) True 
 B)False

Question 4

When 2.0 * 10-2 mole of nicotinic acid (a monoprotic acid)is dissolved in 350.mL of water, the pH is 3.05.What is the Ka of nicotinic acid?

Accepted Answer

1.4 * 10<s

Question 5

Which response gives the products of hydrolysis of KF?

Accepted Answer

A) KOH + HF 
B) OH- + HF 
C) KOH + H+ + F- 
D) KH + F- + OH- 
E) No hydrolysis occurs. 
A) KOH + HF 
B) OH- + HF 
C) KOH + H+ + F- 
D) KH + F- + OH- 
E) No hydrolysis occurs.

Question 6

Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized.

Accepted Answer

A) 1.00 
B) 0.00070 
C) 3.15 
D) 5.15 
E) 7.00 
A) 1.00 
B) 0.00070 
C) 3.15 
D) 5.15 
E) 7.00

Question 7

What is the pH of an aqueous solution that contains 2.7 *1020 H3O+ ions per liter of solution?

Accepted Answer

A) 2.70 
B) 3.35 
C) 6.02 
D) 10.65 
E) 11.30 
A) 2.70 
B) 3.35 
C) 6.02 
D) 10.65 
E) 11.30

Question 8

What is the concentration of H+ in a 2.5 M HCl solution?

Accepted Answer

A) 0 
B) 1.3 M 
C) 2.5 M 
D) 5.0 M 
E) 10.M 
A) 0 
B) 1.3 M 
C) 2.5 M 
D) 5.0 M 
E) 10.M

Question 9

Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.00 * 102 mL of solution.

Accepted Answer

A) 1.35 
B) 2.35 
C) 7.00 
D) 11.65 
E) 12.65 
A) 1.35 
B) 2.35 
C) 7.00 
D) 11.65 
E) 12.65

Question 10

If the pH of an acid rain storm is approximately 3.0, how many times greater is the [H+] in the rain than in a cup of coffee having a pH of 5.0?

Accepted Answer

A) 1000 
B) 100 
C) 20 
D) 1.7 
E) 0.60 
A) 1000 
B) 100 
C) 20 
D) 1.7 
E) 0.60

Question 11

In 0.10 M KCN, the chemical species with the highest concentration (except H2O)is

Accepted Answer

A) Na+ 
B) CN- 
C) H3O+ (or H+) 
D) OH- 
E) K+ 
A) Na+ 
B) CN- 
C) H3O+ (or H+) 
D) OH- 
E) K+

Question 12

Calculate the pH of a 3.5 * 10-3 M HNO3 solution.

Accepted Answer

A) -2.46 
B) 0.54 
C) 2.46 
D) 3.00 
E) 3.46 
A) -2.46 
B) 0.54 
C) 2.46 
D) 3.00 
E) 3.46

Question 13

Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0 * 106 L of water. If the pH of this pond is found to be 9.81, what volume of liquid ammonia found its way into the pond? [Given: Kb(NH3)= 1.8 * 10-5; the density of liquid ammonia is 0.771 g/cm3]

Accepted Answer

A) 15 L 
B) 25 L 
C) 11 L 
D) 19 L 
E) 320 L 
A) 15 L 
B) 25 L 
C) 11 L 
D) 19 L 
E) 320 L

Question 14

For H3PO4, Ka1 = 7.3 * 10-3, Ka2 = 6.2 *10-6, and Ka3 = 4.8 *10-13. An aqueous solution of Na3PO4 therefore would be

Accepted Answer

A) neutral 
B) basic 
C) acidic 
A) neutral 
B) basic 
C) acidic

Question 15

Which one of these net ionic equations represents the reaction of a strong acid with a weak base?

Accepted Answer

A) H+(aq)+ OH-(aq)$\rarr$H2O(aq) 
B) H+(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq) 
C) OH-(aq)+ HCN(aq)$\rarr$H2O(aq)+ CN-(aq) 
D) HCN(aq)+ CH3NH2(aq)$\rarr$CH3NH3+  (aq)+ CN-(aq) 
A) H+(aq)+ OH-(aq)$\rarr$H2O(aq) 
B) H+(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq) 
C) OH-(aq)+ HCN(aq)$\rarr$H2O(aq)+ CN-(aq) 
D) HCN(aq)+ CH3NH2(aq)$\rarr$CH3NH3+  (aq)+ CN-(aq)

Question 16

Write the chemical formula for hydrochloric acid.

Accepted Answer

The answer of Write the chemical formula for hydrochloric acid....

Question 17

Rain collected on a remote island in the Pacific assumed to be unaffected by human pollution.The pH of the rainwater on this island was not 7.Do you expect the pH to be greater than 7 or less than 7? Explain your reasoning.

Accepted Answer

The pH is expected to be less

Question 18

Which one of these equations represents the reaction of a weak acid with a strong base?

Accepted Answer

A) H+(aq)+ OH-(aq)$\rarr$H2O(aq) 
B) H+(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq) 
C) OH-(aq)+ HCN(aq)$\rarr$H2O(aq)+ CN-(aq) 
D) HCN(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq)+ CN-(aq) 
A) H+(aq)+ OH-(aq)$\rarr$H2O(aq) 
B) H+(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq) 
C) OH-(aq)+ HCN(aq)$\rarr$H2O(aq)+ CN-(aq) 
D) HCN(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq)+ CN-(aq)

Question 19

Predict the direction in which the equilibrium will lie for the reaction H2SO3(aq)+ HCO3- (aq)   HSO3-(aq)+ H2CO3(aq).
Ka1(H2SO3)= 1 * 10-2; Ka1(H2CO3)= 4.2 * 10-7

Accepted Answer

A) to the right 
B) to the left 
C) in the middle 
A) to the right 
B) to the left 
C) in the middle

Question 20

Arrange the acids HBr, H2Se, and H3As in order of increasing acid strength.

Accepted Answer

A) HBr 2Se 3As 
B) HBr 3As 2Se 
C) H2Se 3As 3As 2Se 3As 2Se 
A) HBr 2Se 3As 
B) HBr 3As 2Se 
C) H2Se 3As 3As 2Se 3As 2Se

Exam 15: Acids and Bases

Will a 0.1 M solution of NaH2PO4(aq)be acidic, basic, or neutral?

The pH of a certain solution is 3.0. How many H+(aq)ions are there in 1.0 L of the solution?

In the reaction Ag+(aq)+ Cl-(aq) →\rarr→ AgCl(s), Ag+ acts as a Lewis acid.

When 2.0 * 10-2 mole of nicotinic acid (a monoprotic acid)is dissolved in 350.mL of water, the pH is 3.05.What is the Ka of nicotinic acid?

Which response gives the products of hydrolysis of KF?

Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized.

What is the pH of an aqueous solution that contains 2.7 *1020 H3O+ ions per liter of solution?

What is the concentration of H+ in a 2.5 M HCl solution?

Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.00 * 102 mL of solution.

If the pH of an acid rain storm is approximately 3.0, how many times greater is the [H+] in the rain than in a cup of coffee having a pH of 5.0?

In 0.10 M KCN, the chemical species with the highest concentration (except H2O)is

Calculate the pH of a 3.5 * 10-3 M HNO3 solution.

Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0 * 106 L of water. If the pH of this pond is found to be 9.81, what volume of liquid ammonia found its way into the pond? [Given: Kb(NH3)= 1.8 * 10-5; the density of liquid ammonia is 0.771 g/cm3]

For H3PO4, Ka1 = 7.3 * 10-3, Ka2 = 6.2 *10-6, and Ka3 = 4.8 *10-13. An aqueous solution of Na3PO4 therefore would be

Which one of these net ionic equations represents the reaction of a strong acid with a weak base?

Write the chemical formula for hydrochloric acid.

Rain collected on a remote island in the Pacific assumed to be unaffected by human pollution.The pH of the rainwater on this island was not 7.Do you expect the pH to be greater than 7 or less than 7? Explain your reasoning.

Which one of these equations represents the reaction of a weak acid with a strong base?

Predict the direction in which the equilibrium will lie for the reaction H2SO3(aq)+ HCO3- (aq) HSO3-(aq)+ H2CO3(aq). Ka1(H2SO3)= 1 * 10-2; Ka1(H2CO3)= 4.2 * 10-7

Arrange the acids HBr, H2Se, and H3As in order of increasing acid strength.

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

Acid-Base Equilibria and Solubility Equilibria

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

Filters

Will a 0.1 M solution of NaH₂PO₄(aq)be acidic, basic, or neutral?

The pH of a certain solution is 3.0. How many H⁺(aq)ions are there in 1.0 L of the solution?

In the reaction Ag⁺(aq)+ Cl^-(aq) $\rarr$ AgCl(s), Ag⁺ acts as a Lewis acid.

When 2.0 * 10^-2 mole of nicotinic acid (a monoprotic acid)is dissolved in 350.mL of water, the pH is 3.05.What is the K_a of nicotinic acid?

What is the pH of an aqueous solution that contains 2.7 *10²⁰ H₃O⁺ ions per liter of solution?

What is the concentration of H⁺ in a 2.5 M HCl solution?

Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.00 * 10² mL of solution.

If the pH of an acid rain storm is approximately 3.0, how many times greater is the [H⁺] in the rain than in a cup of coffee having a pH of 5.0?

In 0.10 M KCN, the chemical species with the highest concentration (except H₂O)is

Calculate the pH of a 3.5 * 10^-3 M HNO₃ solution.

For H₃PO₄, K_a1 = 7.3 * 10^-3, K_a2 = 6.2 10^-6, and K_a3 = 4.8 10^-13. An aqueous solution of Na₃PO₄ therefore would be

Predict the direction in which the equilibrium will lie for the reaction H₂SO₃(aq)+ HCO₃^-(aq) HSO₃^-(aq)+ H₂CO₃(aq). K_a1(H₂SO₃)= 1 * 10^-2; K_a1(H₂CO₃)= 4.2 * 10^-7

Arrange the acids HBr, H₂Se, and H₃As in order of increasing acid strength.