Question 1

For most reactions of acids with bases, the resulting products are a salt and water.

Accepted Answer

A) True 
 B)False

Question 2

Which of the following is a neutralization reaction?

Accepted Answer

A)  KCl + NaNO₃ → KNO₃ + NaCl 
B)  HNO₃ + KOH → H₂O + KNO₃ 
C)  H₂O + SO₃ → H₂SO₄ 
D)  4Na + O₂ → 2Na2O 
E)  2NO₂ → 2NO + O₂ 
A)  KCl + NaNO₃ → KNO₃ + NaCl 
B)  HNO₃ + KOH → H₂O + KNO₃ 
C)  H₂O + SO₃ → H₂SO₄ 
D)  4Na + O₂ → 2Na2O 
E)  2NO₂ → 2NO + O₂

Question 3

According to the Arrhenius concept, if HNO₃were dissolved in water, it would act as

Accepted Answer

A)  a base. 
B)  an acid. 
C)  a source of hydroxide ions. 
D)  a source of H- ions. 
E)  a proton acceptor. 
A)  a base. 
B)  an acid. 
C)  a source of hydroxide ions. 
D)  a source of H- ions. 
E)  a proton acceptor.

Question 4

25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the NaOH solution is

Accepted Answer

A)  0.212 M 
B)  0.115 M 
C)  0.500 M 
D)  0.390 M 
E)  0.137 M 
A)  0.212 M 
B)  0.115 M 
C)  0.500 M 
D)  0.390 M 
E)  0.137 M

Question 5

Ammonium hydroxide is a weak base because

Accepted Answer

A)  it is a dilute solution. 
B)  it is only slightly soluble in water. 
C)  it cannot hold on to its hydroxide ions. 
D)  it dissociates only slightly in water. 
E)  it is completely ionized in aqueous solution. 
A)  it is a dilute solution. 
B)  it is only slightly soluble in water. 
C)  it cannot hold on to its hydroxide ions. 
D)  it dissociates only slightly in water. 
E)  it is completely ionized in aqueous solution.

Question 6

A 10.0 mL of 0.121 M H₂SO₄ is neutralized by 17.1 mL of KOH solution. The molarity of the KOH solution is

Accepted Answer

A)  0.207 M 
B)  0.4141 M 
C)  0.0708 M 
D)  0.428 M 
E)  0.142 M 
A)  0.207 M 
B)  0.4141 M 
C)  0.0708 M 
D)  0.428 M 
E)  0.142 M

Question 7

If the carbon dioxide level in the blood is too high, more carbonic acid is produced, and this results in the condition termed acidosis.

Accepted Answer

A) True 
 B)False

Question 8

A solution with a pH of 4.0 is basic.

Accepted Answer

A) True 
 B)False

Question 9

The normal blood pH is about

Accepted Answer

A)  6.8. 
B)  7.0. 
C)  7.2. 
D)  7.4. 
E)  7.6. 
A)  6.8. 
B)  7.0. 
C)  7.2. 
D)  7.4. 
E)  7.6.

Question 10

A solution with a pH of 4 is

Accepted Answer

A)  extremely acidic. 
B)  moderately acidic. 
C)  neutral. 
D)  slightly basic. 
E)  extremely basic. 
A)  extremely acidic. 
B)  moderately acidic. 
C)  neutral. 
D)  slightly basic. 
E)  extremely basic.

Question 11

A student had 2.0 L of a sodium hydroxide solution that had a concentration of 0.4000 M. The student needed to make 500 mL of a 0.1000 M solution. How many mL of the concentrated solution was needed?

Accepted Answer

The answer of A student had 2.0 L of a...

Question 12

Which of the following is the strongest acid?

Accepted Answer

A)  HF ( Ka for HF is 7.2 × 10-4) 
B)  HCN (Ka for HCN is 4.9 × 10-10) 
C)  HCNO (Ka for HCNO is 2 × 10-10) 
D)  H3BO₃ (Ka for H3BO₃ is 5.4 × 10-10) 
A)  HF ( Ka for HF is 7.2 × 10-4) 
B)  HCN (Ka for HCN is 4.9 × 10-10) 
C)  HCNO (Ka for HCNO is 2 × 10-10) 
D)  H3BO₃ (Ka for H3BO₃ is 5.4 × 10-10)

Question 13

Identify the Bronsted-Lowry acid in the following reaction. 
H₂O + CO₃2- → HCO₃- + OH-

Accepted Answer

A)  H₂O 
B)  CO₃2- 
C)  HCO₃- 
D)  OH- 
E)  H₂CO₃ 
A)  H₂O 
B)  CO₃2- 
C)  HCO₃- 
D)  OH- 
E)  H₂CO₃

Question 14

How many milliliters of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H3PO₄?

Accepted Answer

A)  7.50 mL 
B)  2.50 mL 
C)  0.833 mL 
D)  5.00 mL 
E)  15.0 mL 
A)  7.50 mL 
B)  2.50 mL 
C)  0.833 mL 
D)  5.00 mL 
E)  15.0 mL

Question 15

The Ka for hydrofluoric acid is 7.2 × 10-4. This means that HF is

Accepted Answer

A)  neutral in water solution. 
B)  able to react with HCl. 
C)  a weak acid. 
D)  a strong acid. 
E)  ionic. 
A)  neutral in water solution. 
B)  able to react with HCl. 
C)  a weak acid. 
D)  a strong acid. 
E)  ionic.

Question 16

For Kw, the product of [H3O+] and [OH-] is

Accepted Answer

A)  1.0 × 10-14. 
B)  1.0 × 10-7. 
C)  1.0 × 10-1. 
D)  1.0. 
E)  1.0 × 1014. 
A)  1.0 × 10-14. 
B)  1.0 × 10-7. 
C)  1.0 × 10-1. 
D)  1.0. 
E)  1.0 × 1014.

Question 17

The pH of 0.001 M HCl is 12.0.

Accepted Answer

A) True 
 B)False

Question 18

HCl is a strong acid.

Accepted Answer

A) True 
 B)False

Question 19

An acid and base react to form a salt and water in a(n) __________ reaction.

Accepted Answer

A)  ionization 
B)  dissociation 
C)  oxidation 
D)  neutralization 
E)  reduction 
A)  ionization 
B)  dissociation 
C)  oxidation 
D)  neutralization 
E)  reduction

Question 20

The conjugate base of HClO₃ is

Accepted Answer

A)  HClO₂. 
B)  ClO₃-. 
C)  Cl(OH)₂. 
D)  ClO₃. 
E)  HClO. 
A)  HClO₂. 
B)  ClO₃-. 
C)  Cl(OH)₂. 
D)  ClO₃. 
E)  HClO.

Exam 10: Acids and Bases

For most reactions of acids with bases, the resulting products are a salt and water.

Which of the following is a neutralization reaction?

According to the Arrhenius concept, if HNO₃were dissolved in water, it would act as

25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the NaOH solution is

Ammonium hydroxide is a weak base because

A 10.0 mL of 0.121 M H₂SO₄ is neutralized by 17.1 mL of KOH solution. The molarity of the KOH solution is

If the carbon dioxide level in the blood is too high, more carbonic acid is produced, and this results in the condition termed acidosis.

A solution with a pH of 4.0 is basic.

The normal blood pH is about

A solution with a pH of 4 is

A student had 2.0 L of a sodium hydroxide solution that had a concentration of 0.4000 M. The student needed to make 500 mL of a 0.1000 M solution. How many mL of the concentrated solution was needed?

Which of the following is the strongest acid?

Identify the Bronsted-Lowry acid in the following reaction. H₂O + CO₃2- → HCO₃- + OH-

How many milliliters of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H3PO₄?

The Ka for hydrofluoric acid is 7.2 × 10-4. This means that HF is

For Kw, the product of [H3O+] and [OH-] is

The pH of 0.001 M HCl is 12.0.

HCl is a strong acid.

An acid and base react to form a salt and water in a(n) __________ reaction.

The conjugate base of HClO₃ is

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Identify the Bronsted-Lowry acid in the following reaction. H₂O + CO₃²- → HCO₃- + OH-

How many milliliters of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H₃PO₄?

The Ka for hydrofluoric acid is 7.2 × 10^-4. This means that HF is

For Kw, the product of [H₃O+] and [OH-] is