Question 1

In the reaction CaO(s)+ SO2(g)     CaSO3(s),

Accepted Answer

A) O2- acts as a Lewis base, and SO2 acts as a Lewis acid. 
B) Ca2+ acts as a Lewis base, and SO42- acts as a Lewis acid. 
C) SO42- acts as a Lewis base, and SO2 acts as a Lewis acid. 
D) SO2 acts as a Lewis base, and O2- acts as a Lewis acid. 
E) SO2 acts as a Lewis base, and Ca2+ acts as a Lewis acid. 
A) O2- acts as a Lewis base, and SO2 acts as a Lewis acid. 
B) Ca2+ acts as a Lewis base, and SO42- acts as a Lewis acid. 
C) SO42- acts as a Lewis base, and SO2 acts as a Lewis acid. 
D) SO2 acts as a Lewis base, and O2- acts as a Lewis acid. 
E) SO2 acts as a Lewis base, and Ca2+ acts as a Lewis acid.

Question 2

Calculate the pH of a 0.20 M solution of the weak base pyridine (C5H5N; Kb = 1.7 x 10-9)

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

A 2.1 L sample of a 0.23 M NaOH solution is mixed with 1.9 L of a 0.021 M KOH solution.What is the pH of the mixture?

Accepted Answer

A) 13.40 
B) 13.12 
C) 11.68 
D) 12.84 
E) 13.04 
A) 13.40 
B) 13.12 
C) 11.68 
D) 12.84 
E) 13.04

Question 5

Which of the following is both a Lewis Acid and Brønsted Acid?

Accepted Answer

A) BF3 
B) NH3 
C) CO2 
D) HNO2 
E) PCl3 
A) BF3 
B) NH3 
C) CO2 
D) HNO2 
E) PCl3

Question 6

The oxides SO2 and N2O5 will form the following acids in water, respectively.

Accepted Answer

A) H2SO4(aq)and HNO3(aq) 
B) H2SO3(aq)and HNO3(aq) 
C) H2SO4(aq)and HNO2(aq) 
D) H2SO3(aq)and HNO2(aq) 
E) H2S(aq)and HNO3(aq) 
A) H2SO4(aq)and HNO3(aq) 
B) H2SO3(aq)and HNO3(aq) 
C) H2SO4(aq)and HNO2(aq) 
D) H2SO3(aq)and HNO2(aq) 
E) H2S(aq)and HNO3(aq)

Question 7

Which one of these salts will form a basic solution upon dissolving in water?

Accepted Answer

A) NaCl 
B) NaNO2 
C) NH4NO3 
D) KBr 
E) AlCl3 
A) NaCl 
B) NaNO2 
C) NH4NO3 
D) KBr 
E) AlCl3

Question 8

The salt hydrolysis reaction for CH3COONa that represents the acidic or basic nature of the solution is:

Accepted Answer

A) Na+(aq)+ H2O(l)     NaH(s)+ OH-(aq) 
B) CH3COO-(aq)+ H2O(l)     CH2COO2-(aq)+ H3O+(aq) 
C) CH3COO-(aq)+ H2O(l)     CH3COOH(aq)+ OH-(aq) 
D) Na2O(s)+ H2O(l)     2NaOH(aq) 
E) CH3COO-(aq)+ Na+(aq)     CH3COONa 
A) Na+(aq)+ H2O(l)     NaH(s)+ OH-(aq) 
B) CH3COO-(aq)+ H2O(l)     CH2COO2-(aq)+ H3O+(aq) 
C) CH3COO-(aq)+ H2O(l)     CH3COOH(aq)+ OH-(aq) 
D) Na2O(s)+ H2O(l)     2NaOH(aq) 
E) CH3COO-(aq)+ Na+(aq)     CH3COONa

Question 9

Predict the direction in which the equilibrium will lie for the reaction H3PO4(aq)+ HSO4-(aq)    
H2PO4-(aq) + H2SO4(aq).
Ka1(H3PO4)= 7.5 × 10-3; Ka(H2SO4)= very large

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 10

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 11

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 12

Write the chemical formula for the acid formed when Cl2O5 is dissolved in water.

Accepted Answer

Question 13

What is the pH of a 0.001 M Ca(OH)2 solution?

Accepted Answer

A) 3.0 
B) 11.0 
C) 2.7 
D) 17.0 
E) 11.3 
A) 3.0 
B) 11.0 
C) 2.7 
D) 17.0 
E) 11.3

Question 14

Which of the following solutions is acidic?

Accepted Answer

A) [OH-] = 1.0 x 10-7 M 
B) [OH-] > 1.0 x 10-7 M 
C) [OH-] = 1.0 x 10-10 M 
D) [H3O+] = 1.0 x 10-10 M 
E) [H3O+] -7 M 
A) [OH-] = 1.0 x 10-7 M 
B) [OH-] > 1.0 x 10-7 M 
C) [OH-] = 1.0 x 10-10 M 
D) [H3O+] = 1.0 x 10-10 M 
E) [H3O+] -7 M

Question 15

Which solution will have the lowest pH?

Accepted Answer

A) 0.25 M HClO 
B) 0.25 M HClO2 
C) 0.25 M HClO3 
D) 0.25 M HClO4 
E) 0.25 M NaClO4 
A) 0.25 M HClO 
B) 0.25 M HClO2 
C) 0.25 M HClO3 
D) 0.25 M HClO4 
E) 0.25 M NaClO4

Question 16

Which of the following does not fit the definition of a Brønsted Acid?

Accepted Answer

A) H3PO4 
B) H2PO4- 
C) H2O 
D) NH4+ 
E) CO2 
A) H3PO4 
B) H2PO4- 
C) H2O 
D) NH4+ 
E) CO2

Question 17

In the reaction HNO3 + NH3    
NH4+ + NO3-, NH4+ and NH3 are a conjugate acid-base pair.

Accepted Answer

A) True 
 B)False

Question 18

Calculate the H+ ion concentration in a 8.8 × 10-4 M Ca(OH)2 solution.

Accepted Answer

A) 8.8 × 10-4 M 
B) 1.8 × 10-3 M 
C) 2.2 × 10-11 M 
D) 1.1 × 10-11 M 
E) 5.7 × 10-12 M 
A) 8.8 × 10-4 M 
B) 1.8 × 10-3 M 
C) 2.2 × 10-11 M 
D) 1.1 × 10-11 M 
E) 5.7 × 10-12 M

Question 19

Arrange the acids HOCl, HClO3, and HClO2 in order of increasing acid strength.

Accepted Answer

A) HOCl 3 2 
B) HOCl 2 3 
C) HClO2 3 
D) HClO3 2 
E) HClO3 2 < HOCl 
A) HOCl 3 2 
B) HOCl 2 3 
C) HClO2 3 
D) HClO3 2 
E) HClO3 2 < HOCl

Question 20

In the reaction: 2H2O(l)     H3O+(aq)+ OH- (aq)the conjugate acid-base pairs are

Accepted Answer

A) pair 1: H2O and H2O; pair 2: H3O+ and OH- 
B) pair 1: H3O+ and OH-; pair 2: H3O+ and H2O 
C) pair 1: H3O+ and OH-; pair 2: OH- and H2O 
D) pair 1: H2O and OH-; pair 2: H2O and H3O+ 
E) pair 1: H3O+ and HO-: pair 2: OH- and H3O+ 
A) pair 1: H2O and H2O; pair 2: H3O+ and OH- 
B) pair 1: H3O+ and OH-; pair 2: H3O+ and H2O 
C) pair 1: H3O+ and OH-; pair 2: OH- and H2O 
D) pair 1: H2O and OH-; pair 2: H2O and H3O+ 
E) pair 1: H3O+ and HO-: pair 2: OH- and H3O+

Exam 15: Acids and Bases

In the reaction CaO(s)+ SO2(g) CaSO3(s),

Calculate the pH of a 0.20 M solution of the weak base pyridine (C5H5N; Kb = 1.7 x 10-9)

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

A 2.1 L sample of a 0.23 M NaOH solution is mixed with 1.9 L of a 0.021 M KOH solution.What is the pH of the mixture?

Which of the following is both a Lewis Acid and Brønsted Acid?

The oxides SO2 and N2O5 will form the following acids in water, respectively.

Which one of these salts will form a basic solution upon dissolving in water?

The salt hydrolysis reaction for CH3COONa that represents the acidic or basic nature of the solution is:

Predict the direction in which the equilibrium will lie for the reaction H3PO4(aq)+ HSO4-(aq) H2PO4-(aq) + H2SO4(aq). Ka1(H3PO4)= 7.5 × 10-3; Ka(H2SO4)= very large

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

Calculate the pH of 2.6 × 10-2 M KOH.

Write the chemical formula for the acid formed when Cl2O5 is dissolved in water.

What is the pH of a 0.001 M Ca(OH)2 solution?

Which of the following solutions is acidic?

Which solution will have the lowest pH?

Which of the following does not fit the definition of a Brønsted Acid?

In the reaction HNO3 + NH3 NH4+ + NO3-, NH4+ and NH3 are a conjugate acid-base pair.

Calculate the H+ ion concentration in a 8.8 × 10-4 M Ca(OH)2 solution.

Arrange the acids HOCl, HClO3, and HClO2 in order of increasing acid strength.

In the reaction: 2H2O(l) H3O+(aq)+ OH- (aq)the conjugate acid-base pairs are

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In the reaction CaO(s)+ SO₂(g) CaSO₃(s),

Calculate the pH of a 0.20 M solution of the weak base pyridine (C₅H₅N; K_b = 1.7 x 10^-9)

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

The oxides SO₂ and N₂O₅ will form the following acids in water, respectively.

The salt hydrolysis reaction for CH₃COONa that represents the acidic or basic nature of the solution is:

Predict the direction in which the equilibrium will lie for the reaction H₃PO₄(aq)+ HSO₄^-(aq) H₂PO₄^-(aq)+ H₂SO₄(aq). K_a1(H₃PO₄)= 7.5 × 10^-3; K_a(H₂SO₄)= very large

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

Write the chemical formula for the acid formed when Cl₂O₅ is dissolved in water.

What is the pH of a 0.001 M Ca(OH)₂ solution?

In the reaction HNO₃ + NH₃ NH₄⁺ + NO₃^-, NH₄⁺ and NH₃ are a conjugate acid-base pair.

Calculate the H⁺ ion concentration in a 8.8 × 10^-4 M Ca(OH)₂ solution.

Arrange the acids HOCl, HClO₃, and HClO₂ in order of increasing acid strength.

In the reaction: 2H₂O(l) H₃O⁺(aq)+ OH^- (aq)the conjugate acid-base pairs are