Question 1

A 25.0 ml sample of 0.105 M HCl was titrated with 31.5 ml of NaOH.What is the concentration of the NaOH?

Accepted Answer

A)  0.0833 M
B)  0.132 M
C)  0.105 M
D)  0.075 M
E)  none of the above A

Question 2

What is the concentration of H+ in solution given the [OH⁻] = 2.54 × 10-4?

Accepted Answer

A)  3.94 × 10-11 M
B)  2.54 × 10-11 M
C)  1.0 × 1014 M
D)  not enough information
E)  none of the above A

Question 3

What is the pH of a solution that has a H⁺ concentration equal to 1.76 × 10-5 M?

Accepted Answer

A)  4.77
B)  5.20
C)  0.22
D)  10.20
E)  none of the above A

Question 4

A 0.10 M solution of an electrolyte has a pH of 4.5.The electrolyte is:

Accepted Answer

A)  a strong acid.
B)  a strong base.
C)  a weak acid.
D)  a weak base.
E)  none of the above

Question 5

Acid rain legislation targeted the release of which compound by industry?

Accepted Answer

A)  CO2
B)  SO2
C)  dioxin
D)  benzene
E)  none of the above

Question 6

Acids turn litmus paper blue.

Accepted Answer

A) True 
 B)False

Question 7

The Bronsted-Lowry definition of a base is:

Accepted Answer

A)  a proton donor.
B)  a proton acceptor.
C)  produces H⁺ in solution.
D)  produces OH⁻ in solution.
E)  none of the above

Question 8

Which combination below will be a buffer solution?

Accepted Answer

A)  HCl and Cl⁻
B)  HNO3 and NaNO3
C)  HC2H3O2 and NaC2H3O2
D)  NaBr and NaOH
E)  All of the above are true.

Question 9

Ammonia (NH3)ionizes in water to form a basic solution.What is the concentration of OH- ions in a
0.75 M NH3 solution?

Accepted Answer

A)  0.75 M
B)  
C)  > 0.75 M
D)  No OH- ions exist in a solution of NH3.
E)  none of the above

Question 10

Exactly 17.0 mL of a H2SO4 solution was required to neutralize 45.0 mL of 0.235 M NaOH.What was the concentration of the H2SO4 solution?
GIVEN: H2SO4 (aq)+ 2NaOH (aq)→ 2H2O (l)+ Na2SO4 (aq)

Accepted Answer

A)  5.63 M
B)  0.622 M
C)  0.00529 M
D)  0.311 M
E)  none of the above

Question 11

What is the concentration of the hydronium ions in a neutral solution?

Accepted Answer

A)  0.0 M
B)  1.0 × 10-7 M
C)  1.0 × 10-14 M
D)  > 1.0× 10-7 M
E)  -7 M

Question 12

A solution that has a pH of 10 would also have a pOH of 4.

Accepted Answer

A) True 
 B)False

Question 13

What is the concentration of H+ in a 0.121 M HCl solution?

Accepted Answer

A)  1.0 × 10-14 M
B)  
C)  0.121 M
D)  not enough information
E)  none of the above

Question 14

A neutralization reaction between an acid and sodium hydroxide formed water and the salt named sodium sulfate.What was the formula of the acid that was neutralized?

Accepted Answer

A)  H2S
B)  H2SO4
C)  HCl
D)  Na2SO4
E)  none of the above

Question 15

Water always acts as an acid in reactions.

Accepted Answer

A) True 
 B)False

Question 16

In a titration,the indicator is used to signal when the endpoint has been reached.

Accepted Answer

A) True 
 B)False

Question 17

The salt that forms due to neutralization of phosphoric acid by calcium hydroxide has the formula Ca3P2.

Accepted Answer

A) True 
 B)False

Question 18

Which solution below has the highest concentration of hydroxide ions?

Accepted Answer

A)  pH = 3.21
B)  pH = 12.49
C)  pH = 7.00
D)  pH = 10.12
E)  pH = 7.93

Question 19

The titration of 25.00 mL a 0.125 M HClO4 solution required 21.37 mL of KOH to reach the endpoint.What is the concentration of the KOH?

Accepted Answer

A)  0.292 M
B)  0.0668 M
C)  0.146 M
D)  0.134 M
E)  none of the above

Question 20

In a solution that has a pH = 7.0,

Accepted Answer

A)  [H3O+] > [OH-]
B)  [H3O+] -]
C)  [H3O+] = [OH-]
D)  [H3O+] + [OH-] = Kw
E)  none of the above

Exam 14: Acids and Bases

A 25.0 ml sample of 0.105 M HCl was titrated with 31.5 ml of NaOH.What is the concentration of the NaOH?

What is the concentration of H⁺ in solution given the [OH⁻] = 2.54 × 10^-⁴?

What is the pH of a solution that has a H⁺ concentration equal to 1.76 × 10^-⁵ M?

A 0.10 M solution of an electrolyte has a pH of 4.5.The electrolyte is:

Acid rain legislation targeted the release of which compound by industry?

Acids turn litmus paper blue.

The Bronsted-Lowry definition of a base is:

Which combination below will be a buffer solution?

Ammonia (NH₃) ionizes in water to form a basic solution.What is the concentration of OH^- ions in a 0.75 M NH₃ solution?

Exactly 17.0 mL of a H₂SO₄ solution was required to neutralize 45.0 mL of 0.235 M NaOH.What was the concentration of the H₂SO₄ solution? GIVEN: H₂SO₄ (aq) + 2NaOH (aq) → 2H₂O (l) + Na₂SO₄ (aq)

What is the concentration of the hydronium ions in a neutral solution?

A solution that has a pH of 10 would also have a pOH of 4.

What is the concentration of H⁺ in a 0.121 M HCl solution?

A neutralization reaction between an acid and sodium hydroxide formed water and the salt named sodium sulfate.What was the formula of the acid that was neutralized?

Water always acts as an acid in reactions.

In a titration,the indicator is used to signal when the endpoint has been reached.

The salt that forms due to neutralization of phosphoric acid by calcium hydroxide has the formula Ca₃P₂.

Which solution below has the highest concentration of hydroxide ions?

The titration of 25.00 mL a 0.125 M HClO₄ solution required 21.37 mL of KOH to reach the endpoint.What is the concentration of the KOH?

In a solution that has a pH = 7.0,

Exam 14: Acids and Bases

A 25.0 ml sample of 0.105 M HCl was titrated with 31.5 ml of NaOH.What is the concentration of the NaOH?

What is the concentration of H+ in solution given the [OH⁻] = 2.54 × 10-4?

What is the pH of a solution that has a H⁺ concentration equal to 1.76 × 10-5 M?

A 0.10 M solution of an electrolyte has a pH of 4.5.The electrolyte is:

Acid rain legislation targeted the release of which compound by industry?

Acids turn litmus paper blue.

The Bronsted-Lowry definition of a base is:

Which combination below will be a buffer solution?

Ammonia (NH3) ionizes in water to form a basic solution.What is the concentration of OH- ions in a 0.75 M NH3 solution?

Exactly 17.0 mL of a H2SO4 solution was required to neutralize 45.0 mL of 0.235 M NaOH.What was the concentration of the H2SO4 solution? GIVEN: H2SO4 (aq) + 2NaOH (aq) → 2H2O (l) + Na2SO4 (aq)

What is the concentration of the hydronium ions in a neutral solution?

A solution that has a pH of 10 would also have a pOH of 4.

What is the concentration of H+ in a 0.121 M HCl solution?

A neutralization reaction between an acid and sodium hydroxide formed water and the salt named sodium sulfate.What was the formula of the acid that was neutralized?

Water always acts as an acid in reactions.

In a titration,the indicator is used to signal when the endpoint has been reached.

The salt that forms due to neutralization of phosphoric acid by calcium hydroxide has the formula Ca3P2.

Which solution below has the highest concentration of hydroxide ions?

The titration of 25.00 mL a 0.125 M HClO4 solution required 21.37 mL of KOH to reach the endpoint.What is the concentration of the KOH?

In a solution that has a pH = 7.0,

What is the concentration of H⁺ in solution given the [OH⁻] = 2.54 × 10^-⁴?

What is the pH of a solution that has a H⁺ concentration equal to 1.76 × 10^-⁵ M?

Ammonia (NH₃) ionizes in water to form a basic solution.What is the concentration of OH^- ions in a 0.75 M NH₃ solution?

Exactly 17.0 mL of a H₂SO₄ solution was required to neutralize 45.0 mL of 0.235 M NaOH.What was the concentration of the H₂SO₄ solution? GIVEN: H₂SO₄ (aq) + 2NaOH (aq) → 2H₂O (l) + Na₂SO₄ (aq)

What is the concentration of H⁺ in a 0.121 M HCl solution?

The salt that forms due to neutralization of phosphoric acid by calcium hydroxide has the formula Ca₃P₂.

The titration of 25.00 mL a 0.125 M HClO₄ solution required 21.37 mL of KOH to reach the endpoint.What is the concentration of the KOH?