Question 1

CH3NH2 + HCl  
CH3NH3+ + Cl-
A conjugate acid-base pair in the reaction shown is ________ and ________.

Accepted Answer

A) CH3NH2 and HCl 
B) CH3NH2 and Cl- 
C) CH3NH3+ and Cl- 
D) HCl and Cl- 
E) HCl and H3O+ 
A) CH3NH2 and HCl 
B) CH3NH2 and Cl- 
C) CH3NH3+ and Cl- 
D) HCl and Cl- 
E) HCl and H3O+ D

Question 2

Which of the following is a diprotic acid?

Accepted Answer

A) acetic acid 
B) hydrochloric acid 
C) phosphoric acid 
D) sulfuric acid 
E) nitric acid 
A) acetic acid 
B) hydrochloric acid 
C) phosphoric acid 
D) sulfuric acid 
E) nitric acid D

Question 3

How many mL of 0.100 M NaOH are needed to neutralize 24.0 mL of 0.150 M HCl?

Accepted Answer

A) 12.0 mL 
B) 18.0 mL 
C) 24.0 mL 
D) 36.0 mL 
E) 48.0 mL 
A) 12.0 mL 
B) 18.0 mL 
C) 24.0 mL 
D) 36.0 mL 
E) 48.0 mL D

Question 4

What is the concentration of an acetic acid solution if a 10.0 mL sample required 26.4 mL of 0.950 M KOH for neutralization?

Accepted Answer

A) 0.379 M 
B) 0.399 M 
C) 0.950 M 
D) 2.51 M 
E) 2.78 M 
A) 0.379 M 
B) 0.399 M 
C) 0.950 M 
D) 2.51 M 
E) 2.78 M

Question 5

Calculate the hydrogen ion concentration in a solution with pH = 6.35.

Accepted Answer

A) 7.65 M 
B) 6.35 M 
C) 4.5 × 10-7 M 
D) 0.80 M 
E) 2.2 × 10-8 M 
A) 7.65 M 
B) 6.35 M 
C) 4.5 × 10-7 M 
D) 0.80 M 
E) 2.2 × 10-8 M

Question 6

Water and HSO4- can either accept protons or donate protons.Such substances are said to be

Accepted Answer

A) amphoteric. 
B) conjugate. 
C) diprotic. 
D) monoprotic. 
E) triprotic. 
A) amphoteric. 
B) conjugate. 
C) diprotic. 
D) monoprotic. 
E) triprotic.

Question 7

The normality of a solution prepared by dissolving 25.0 g of Ca(OH)2 in water to make 250.mL solution is ________ N.

Accepted Answer

A) 2.70 
B) 1.35 
C) 0.675 
D) 3.51 
E) 1.75 
A) 2.70 
B) 1.35 
C) 0.675 
D) 3.51 
E) 1.75

Question 8

In an aqueous solution that is acidic,[H3O+] is ________ than 1.0 × 10-7 and ________ than [OH-].

Accepted Answer

A) greater; less 
B) less; greater 
C) greater; greater 
D) less; less 
E) none of the above 
A) greater; less 
B) less; greater 
C) greater; greater 
D) less; less 
E) none of the above

Question 9

Which example is not basic?

Accepted Answer

A) shampoo 
B) vinegar 
C) window cleaner 
D) limewater 
E) Mg(OH)2,used in remedies for upset stomach 
A) shampoo 
B) vinegar 
C) window cleaner 
D) limewater 
E) Mg(OH)2,used in remedies for upset stomach

Question 10

The base forms a new ________ bond in a Brønsted-Lowry acid-base reaction.

Accepted Answer

A) covalent 
B) aquo 
C) hydrogen 
D) ionic 
E) metallic 
A) covalent 
B) aquo 
C) hydrogen 
D) ionic 
E) metallic

Question 11

What is the concentration of a phosphoric acid solution of a 25.00 mL sample of the acid requires 42.24 mL of 0.135 M NaOH for neutralization?

Accepted Answer

A) 0.228 M 
B) 0.684 M 
C) 0.0760 M 
D) 0.0266 M 
E) 0.0799 M 
A) 0.228 M 
B) 0.684 M 
C) 0.0760 M 
D) 0.0266 M 
E) 0.0799 M

Question 12

What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH for neutralization?

Accepted Answer

A) 0.0300 M 
B) 0.150 M 
C) 0.600 M 
D) 0.750 M 
E) 7.50 M 
A) 0.0300 M 
B) 0.150 M 
C) 0.600 M 
D) 0.750 M 
E) 7.50 M

Question 13

What is the pH of a solution in which [H3O+] = 4.1 × 10-2 M?

Accepted Answer

A) 12.61 
B) 1.39 
C) 1.10 
D) 12.90 
E) 4.10 
A) 12.61 
B) 1.39 
C) 1.10 
D) 12.90 
E) 4.10

Question 14

Which pair of compounds is used in the manufacture of fertilizers?

Accepted Answer

A) HCl and NaOH 
B) HCl and H3PO4 
C) HNO3 and HCl 
D) H2SO4 and H3PO4 
E) HNO3 and NaOH 
A) HCl and NaOH 
B) HCl and H3PO4 
C) HNO3 and HCl 
D) H2SO4 and H3PO4 
E) HNO3 and NaOH

Question 15

In the following equation,which of the following is acting as the Bronsted acid?
HClO4 + H2O --> ClO4- + H3O+

Accepted Answer

A) HClO4 
B) H2O 
C) ClO4- 
D) H3O+ 
A) HClO4 
B) H2O 
C) ClO4- 
D) H3O+

Question 16

How many mL of 0.100 M NaOH are needed to neutralize 50.00 mL of a 0.150 M solution of CH3CO2H,a monoprotic acid?

Accepted Answer

A) 25.00 mL 
B) 37.50 mL 
C) 50.00 mL 
D) 75.00 mL 
E) 100.00 mL 
A) 25.00 mL 
B) 37.50 mL 
C) 50.00 mL 
D) 75.00 mL 
E) 100.00 mL

Question 17

Which of the following pH's corresponds to a strongly basic solution?

Accepted Answer

A) 11.5 
B) 2.7 
C) 6.9 
D) 7.4 
E) 4.3 
A) 11.5 
B) 2.7 
C) 6.9 
D) 7.4 
E) 4.3

Question 18

What is the hydrogen ion concentration in a solution with pH = 2.34?

Accepted Answer

A) 4.57 × 10-3 M 
B) 2.34 × 10-3 M 
C) 2.19 × 10-12 M 
D) 1.17 × 101 M 
E) 4.27 × 10-12 M 
A) 4.57 × 10-3 M 
B) 2.34 × 10-3 M 
C) 2.19 × 10-12 M 
D) 1.17 × 101 M 
E) 4.27 × 10-12 M

Question 19

The H3O+ ion is called the ________ ion.

Accepted Answer

A) hydroxide 
B) hydronium 
C) hydrogen 
D) protium 
E) water 
A) hydroxide 
B) hydronium 
C) hydrogen 
D) protium 
E) water

Question 20

What is the concentration of a weak base solution if a 25.0 mL sample is neutralized by 48.3 mL of 0.105 M H3PO4?

Accepted Answer

A) 0.0543 M 
B) 0.0676 M 
C) 0.163 M 
D) 0.203 M 
E) 0.609 M 
A) 0.0543 M 
B) 0.0676 M 
C) 0.163 M 
D) 0.203 M 
E) 0.609 M

Exam 10: Acids and Bases

CH3NH2 + HCl CH3NH3+ + Cl- A conjugate acid-base pair in the reaction shown is ________ and ________.

Which of the following is a diprotic acid?

How many mL of 0.100 M NaOH are needed to neutralize 24.0 mL of 0.150 M HCl?

What is the concentration of an acetic acid solution if a 10.0 mL sample required 26.4 mL of 0.950 M KOH for neutralization?

Calculate the hydrogen ion concentration in a solution with pH = 6.35.

Water and HSO4- can either accept protons or donate protons.Such substances are said to be

The normality of a solution prepared by dissolving 25.0 g of Ca(OH)2 in water to make 250.mL solution is ________ N.

In an aqueous solution that is acidic,[H3O+] is ________ than 1.0 × 10-7 and ________ than [OH-].

Which example is not basic?

The base forms a new ________ bond in a Brønsted-Lowry acid-base reaction.

What is the concentration of a phosphoric acid solution of a 25.00 mL sample of the acid requires 42.24 mL of 0.135 M NaOH for neutralization?

What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH for neutralization?

What is the pH of a solution in which [H3O+] = 4.1 × 10-2 M?

Which pair of compounds is used in the manufacture of fertilizers?

In the following equation,which of the following is acting as the Bronsted acid? HClO4 + H2O --> ClO4- + H3O+

How many mL of 0.100 M NaOH are needed to neutralize 50.00 mL of a 0.150 M solution of CH3CO2H,a monoprotic acid?

Which of the following pH's corresponds to a strongly basic solution?

What is the hydrogen ion concentration in a solution with pH = 2.34?

The H3O+ ion is called the ________ ion.

What is the concentration of a weak base solution if a 25.0 mL sample is neutralized by 48.3 mL of 0.105 M H3PO4?

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CH₃NH₂ + HCl CH₃NH₃⁺ + Cl^- A conjugate acid-base pair in the reaction shown is and .

Water and HSO₄^- can either accept protons or donate protons.Such substances are said to be

The normality of a solution prepared by dissolving 25.0 g of Ca(OH)₂ in water to make 250.mL solution is ________ N.

In an aqueous solution that is acidic,[H₃O⁺] is than 1.0 × 10^-7 and than [OH^-].

What is the pH of a solution in which [H₃O⁺] = 4.1 × 10^-2 M?

In the following equation,which of the following is acting as the Bronsted acid? HClO₄ + H₂O --> ClO₄^- + H₃O⁺

How many mL of 0.100 M NaOH are needed to neutralize 50.00 mL of a 0.150 M solution of CH₃CO₂H,a monoprotic acid?

The H₃O⁺ ion is called the ________ ion.

What is the concentration of a weak base solution if a 25.0 mL sample is neutralized by 48.3 mL of 0.105 M H₃PO₄?