Question 1

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 2

Write the formula for the conjugate base of H2PO4-.

Accepted Answer

Question 3

Arrange the acids HOBr, HBrO3, and HBrO2 in order of increasing acid strength.

Accepted Answer

A) HOBr 3 2 
B) HOBr 2 3 
C) HBrO2 3 
D) HBrO3 2 
E) HBrO3 2 < HOBr 
A) HOBr 3 2 
B) HOBr 2 3 
C) HBrO2 3 
D) HBrO3 2 
E) HBrO3 2 < HOBr

Question 4

Acid strength decreases in the series: strongest HSO4- > HF > HCN. Which of these species is the weakest base?

Accepted Answer

A) HF 
B) SO42- 
C) F- 
D) CN- 
A) HF 
B) SO42- 
C) F- 
D) CN-

Question 5

Calculate the pH of a solution containing 0.20 g of NaOH in 2,000. mL of solution.

Accepted Answer

The answer of Calculate the pH of a solution containing...

Question 6

Predict the direction in which the equilibrium will lie for the reaction H2SO3(aq)+ HCO3- (aq)$\rarr$ 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 7

Which one of the following statements is true for a 0.1 M solution of a weak acid HA?

Accepted Answer

A) The concentration of H+ is slightly greater than the concentration of A-. 
B) The pH equals 1.0. 
C) The concentration of H+ is exactly equal to the concentration of A-. 
D) The pH is less than 1.0. 
E) The concentration of H+ is slightly less than the concentration of A-. 
A) The concentration of H+ is slightly greater than the concentration of A-. 
B) The pH equals 1.0. 
C) The concentration of H+ is exactly equal to the concentration of A-. 
D) The pH is less than 1.0. 
E) The concentration of H+ is slightly less than the concentration of A-.

Question 8

What is the pH of 10.0 mL of 0.0020 M HCl?

Accepted Answer

A) 0.70 
B) 2.70 
C) 3.70 
D) 5.70 
E) 10.0 
A) 0.70 
B) 2.70 
C) 3.70 
D) 5.70 
E) 10.0

Question 9

The pOH of a solution is 10.40. Calculate the hydrogen ion concentration in the solution.

Accepted Answer

A) 4.0* 10-11 M 
B) 3.6 M 
C) 4.0 * 10-10 M 
D) 2.5 * 10-4 M 
E) 1.8 * 10-4 M 
A) 4.0* 10-11 M 
B) 3.6 M 
C) 4.0 * 10-10 M 
D) 2.5 * 10-4 M 
E) 1.8 * 10-4 M

Question 10

Which of these acids is stronger, H2SO4 or HSO4-?

Accepted Answer

Question 11

Which one of these salts will form a neutral solution on dissolving in water?

Accepted Answer

A) NaCl 
B) KNO2 
C) NaCN 
D) NH4NO3 
E) FeCl3 
A) NaCl 
B) KNO2 
C) NaCN 
D) NH4NO3 
E) FeCl3

Question 12

Calculate the pH of 2.6 * 10-2 M KOH.

Accepted Answer

A) 12.41 
B) 15.59 
C) 2.06 
D) 7.00 
E) 1.59 
A) 12.41 
B) 15.59 
C) 2.06 
D) 7.00 
E) 1.59

Question 13

Acid strength decreases in the series HI > HSO4- > HF > HCN. Which of these anions is the weakest base?

Accepted Answer

A) I- 
B) SO42- 
C) F- 
D) CN- 
A) I- 
B) SO42- 
C) F- 
D) CN-

Question 14

Calculate the pOH of a solution containing 0.25 g of HCl in 800. mL of solution.

Accepted Answer

The answer of Calculate the pOH of a solution containing...

Question 15

Acid strength decreases in the series: HCl > HSO4- > HCN. Which of these species is the strongest base?

Accepted Answer

A) CN- 
B) SO42- 
C) HCN 
D) Cl- 
A) CN- 
B) SO42- 
C) HCN 
D) Cl-

Question 16

Identify the conjugate acid of HCO3- in the reaction HCO3- + HPO42- $\rarr$ H2CO3 + PO43-

Accepted Answer

A) H2O 
B) HCO3- 
C) H2CO3 
D) PO43- 
E) HPO42- 
A) H2O 
B) HCO3- 
C) H2CO3 
D) PO43- 
E) HPO42-

Question 17

The pH of a 0.6 M solution of a weak acid is 4.0. What percent of the acid has ionized?

Accepted Answer

The answer of The pH of a 0.6 M solution...

Question 18

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 19

Identify the conjugate acid of SO42- in the reaction CO32- + HSO4- $\rarr$ HCO3- + SO42-

Accepted Answer

A) CO32- 
B) HSO4- 
C) OH- 
D) H3O+ 
E) SO42- 
A) CO32- 
B) HSO4- 
C) OH- 
D) H3O+ 
E) SO42-

Question 20

The pH of a 0.02 M solution of an unknown weak base is 8.1. What is the pKb of the unknown base?

Accepted Answer

Exam 16: Acids and Bases

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.

Write the formula for the conjugate base of H2PO4-.

Arrange the acids HOBr, HBrO3, and HBrO2 in order of increasing acid strength.

Acid strength decreases in the series: strongest HSO4- > HF > HCN. Which of these species is the weakest base?

Calculate the pH of a solution containing 0.20 g of NaOH in 2,000. mL of solution.

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

Which one of the following statements is true for a 0.1 M solution of a weak acid HA?

What is the pH of 10.0 mL of 0.0020 M HCl?

The pOH of a solution is 10.40. Calculate the hydrogen ion concentration in the solution.

Which of these acids is stronger, H2SO4 or HSO4-?

Which one of these salts will form a neutral solution on dissolving in water?

Calculate the pH of 2.6 * 10-2 M KOH.

Acid strength decreases in the series HI > HSO4- > HF > HCN. Which of these anions is the weakest base?

Calculate the pOH of a solution containing 0.25 g of HCl in 800. mL of solution.

Acid strength decreases in the series: HCl > HSO4- > HCN. Which of these species is the strongest base?

Identify the conjugate acid of HCO3- in the reaction HCO3- + HPO42- →\rarr→ H2CO3 + PO43-

The pH of a 0.6 M solution of a weak acid is 4.0. What percent of the acid has ionized?

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

Identify the conjugate acid of SO42- in the reaction CO32- + HSO4- →\rarr→ HCO3- + SO42-

The pH of a 0.02 M solution of an unknown weak base is 8.1. What is the pKb of the unknown base?

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

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

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.

Write the formula for the conjugate base of H₂PO₄^-.

Arrange the acids HOBr, HBrO₃, and HBrO₂ in order of increasing acid strength.

Acid strength decreases in the series: strongest HSO₄^- > HF > HCN. Which of these species is the weakest base?

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

Which of these acids is stronger, H₂SO₄ or HSO₄^-?

Calculate the pH of 2.6 * 10^-2 M KOH.

Acid strength decreases in the series HI > HSO₄^- > HF > HCN. Which of these anions is the weakest base?

Acid strength decreases in the series: HCl > HSO₄^- > HCN. Which of these species is the strongest base?

Identify the conjugate acid of HCO₃^- in the reaction HCO₃^- + HPO₄^2- $\rarr$ H₂CO₃ + PO₄^3-

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

Identify the conjugate acid of SO₄^2- in the reaction CO₃^2- + HSO₄^- $\rarr$ HCO₃^- + SO₄^2-

The pH of a 0.02 M solution of an unknown weak base is 8.1. What is the pK_b of the unknown base?