Question 1

Which of the following is a strong base?

Accepted Answer

A) Cl- 
B) NH3 
C) CH3OH 
D) NO3⁻ 
E) KOH 
A) Cl- 
B) NH3 
C) CH3OH 
D) NO3⁻ 
E) KOH

Question 2

List the major source of energy in North America.

Accepted Answer

The answer of List the major source of energy in...

Question 3

Determine the Ka of an acid whose 0.294 mol L-1 solution has a pH of 2.80.

Accepted Answer

A) 1.2 × 10-5 
B) 8.5 × 10-6 
C) 2.7 
D) 4.9 × 10-7 
E) 5.4 × 10-3 
A) 1.2 × 10-5 
B) 8.5 × 10-6 
C) 2.7 
D) 4.9 × 10-7 
E) 5.4 × 10-3

Question 4

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10-2 mol L-1?

Accepted Answer

A) 6.67 × 10-12 mol L-1, 2.82 
B) 6.67 × 10-12 mol L-1, 11.18 
C) 6.67 × 10-13 mol L-1, 1.82 
D) 6.67 × 10-13 mol L-1, 12.17 
A) 6.67 × 10-12 mol L-1, 2.82 
B) 6.67 × 10-12 mol L-1, 11.18 
C) 6.67 × 10-13 mol L-1, 1.82 
D) 6.67 × 10-13 mol L-1, 12.17

Question 5

Which of the following is the correct Arrhenius definition of acids?

Accepted Answer

A) An acid is a substance that produces H+ ions in aqueous solutions. 
B) An acid is a substance that reacts with H+ ions in aqueous solutions. 
C) An acid is a substance that produces OH- ions in aqueous solutions. 
D) An acid is a substance that decreases the amount of H+ ions in aqueous solutions. 
E) An acid is a substance that does not alter the amount of H+ ions in aqueous solutions. 
A) An acid is a substance that produces H+ ions in aqueous solutions. 
B) An acid is a substance that reacts with H+ ions in aqueous solutions. 
C) An acid is a substance that produces OH- ions in aqueous solutions. 
D) An acid is a substance that decreases the amount of H+ ions in aqueous solutions. 
E) An acid is a substance that does not alter the amount of H+ ions in aqueous solutions.

Question 6

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-6 mol L-1 in hydroxide ion.

Accepted Answer

A) 4.00 × 10-7 mol L-1 
B) 4.00 × 10-8 mol L-1 
C) 4.00 × 10-9 mol L-1 
D) 5.00 × 10-9 mol L-1 
A) 4.00 × 10-7 mol L-1 
B) 4.00 × 10-8 mol L-1 
C) 4.00 × 10-9 mol L-1 
D) 5.00 × 10-9 mol L-1

Question 7

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5)is below:

Accepted Answer

A) 3.0 mol L-1 
B) 0.056 mol L-1 
C) 1.8 × 10-2 mol L-1 
D) 1.0 × 10-3 mol L-1 
A) 3.0 mol L-1 
B) 0.056 mol L-1 
C) 1.8 × 10-2 mol L-1 
D) 1.0 × 10-3 mol L-1

Question 8

Which of the following is a general property of a base?

Accepted Answer

A) Bases have sour taste. 
B) Bases turn blue litmus paper red. 
C) Bases leave red litmus paper unchanged. 
D) Bases turn red litmus paper blue. 
E) Bases easily dissolve many metallic elements. 
A) Bases have sour taste. 
B) Bases turn blue litmus paper red. 
C) Bases leave red litmus paper unchanged. 
D) Bases turn red litmus paper blue. 
E) Bases easily dissolve many metallic elements.

Question 9

Determine the pH of a 0.023 mol L-1 HNO3 solution.

Accepted Answer

A) 12.36 
B) 3.68 
C) 1.64 
D) 2.30 
E) 2.49 
A) 12.36 
B) 3.68 
C) 1.64 
D) 2.30 
E) 2.49

Question 10

Which of the following is a strong acid?

Accepted Answer

A) C6H5CO2H 
B) HCN 
C) HClO4 
D) NH4+ 
E) H2O 
A) C6H5CO2H 
B) HCN 
C) HClO4 
D) NH4+ 
E) H2O

Question 11

Determine the pH of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

Accepted Answer

A) 8.62 
B) 13.06 
C) 13.37 
D) 0.63 
E) 12.56 
A) 8.62 
B) 13.06 
C) 13.37 
D) 0.63 
E) 12.56

Question 12

Which of the following is an Arrhenius base?

Accepted Answer

A) CH3CO2H 
B) NaOH 
C) CH3OH 
D) LiCl 
E) H2CO3 
A) CH3CO2H 
B) NaOH 
C) CH3OH 
D) LiCl 
E) H2CO3

Question 13

Determine the pH of a 0.741 mol L-1 KOH solution at 25 °C.

Accepted Answer

A) 0.13 
B) 13.87 
C) 0.17 
D) 12.65 
E) 11.88 
A) 0.13 
B) 13.87 
C) 0.17 
D) 12.65 
E) 11.88

Question 14

Determine the [H3O⁺] in a 0.265 mol L-1 HClO solution. The Ka of HClO is 2.9 × 10-8.

Accepted Answer

A) 1.1 × 10-10 mol L-1 
B) 7.7 × 10-9 mol L-1 
C) 1.3 × 10-6 mol L-1 
D) 4.9 × 10-4 mol L-1 
E) 8.8 × 10-5 mol L-1 
A) 1.1 × 10-10 mol L-1 
B) 7.7 × 10-9 mol L-1 
C) 1.3 × 10-6 mol L-1 
D) 4.9 × 10-4 mol L-1 
E) 8.8 × 10-5 mol L-1

Question 15

What is the concentration of hydroxide ions in pure water at 30.0 ∘C if Kw at this temperature is 1.47 × 10-14?

Accepted Answer

A) 1.00 × 10-7 mol L-1 
B) 1.30 × 10-7 mol L-1 
C) 1.47 × 10-7 mol L-1 
D) 8.93 × 10-8 mol L-1 
E) 1.21 × 10-7 mol L-1 
A) 1.00 × 10-7 mol L-1 
B) 1.30 × 10-7 mol L-1 
C) 1.47 × 10-7 mol L-1 
D) 8.93 × 10-8 mol L-1 
E) 1.21 × 10-7 mol L-1

Question 16

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25 °C.

Accepted Answer

A) 7.1 × 10-5 mol L-1 
B) 4.2 × 10-10 mol L-1 
C) 8.7 × 10-10 mol L-1 
D) 6.5 × 10-5 mol L-1 
E) 1.4 × 10-10 mol L-1 
A) 7.1 × 10-5 mol L-1 
B) 4.2 × 10-10 mol L-1 
C) 8.7 × 10-10 mol L-1 
D) 6.5 × 10-5 mol L-1 
E) 1.4 × 10-10 mol L-1

Question 17

Identify the strongest acid.

Accepted Answer

A) H2O 
B) H2S 
C) H2Se 
D) H2Te 
E) CaH2 
A) H2O 
B) H2S 
C) H2Se 
D) H2Te 
E) CaH2

Question 18

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of 2.25 × 10-2 mol L-1?

Accepted Answer

A) 4.44 × 10-12 mol L-1 and 2.65 
B) 4.44 × 10-12 mol L-1 and 11.35 
C) 4.44 × 10-13 mol L-1 and 1.65 
D) 4.44 × 10-13 mol L-1 and 12.35 
A) 4.44 × 10-12 mol L-1 and 2.65 
B) 4.44 × 10-12 mol L-1 and 11.35 
C) 4.44 × 10-13 mol L-1 and 1.65 
D) 4.44 × 10-13 mol L-1 and 12.35

Question 19

Which of the following is the correct Arrhenius definition of bases?

Accepted Answer

A) A base is a substance that produces H+ ions in aqueous solutions. 
B) A base is a substance that reacts with OH- ions in aqueous solutions. 
C) A base is a substance that decreases the amount of OH- ions in aqueous solutions. 
D) A base is a substance that produces OH- ions in aqueous solutions. 
E) A base is a substance that does not change the concentration of OH- ions in aqueous solutions. 
A) A base is a substance that produces H+ ions in aqueous solutions. 
B) A base is a substance that reacts with OH- ions in aqueous solutions. 
C) A base is a substance that decreases the amount of OH- ions in aqueous solutions. 
D) A base is a substance that produces OH- ions in aqueous solutions. 
E) A base is a substance that does not change the concentration of OH- ions in aqueous solutions.

Question 20

Determine the pH of a 0.18 mol L-1 H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A) 11.00 
B) 10.44 
C) 5.50 
D) 4.31 
E) 3.56 
A) 11.00 
B) 10.44 
C) 5.50 
D) 4.31 
E) 3.56

Exam 15: Acids and Bases

Which of the following is a strong base?

List the major source of energy in North America.

Determine the Ka of an acid whose 0.294 mol L-1 solution has a pH of 2.80.

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10-2 mol L-1?

Which of the following is the correct Arrhenius definition of acids?

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-6 mol L-1 in hydroxide ion.

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5)is below:

Which of the following is a general property of a base?

Determine the pH of a 0.023 mol L-1 HNO3 solution.

Which of the following is a strong acid?

Determine the pH of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

Which of the following is an Arrhenius base?

Determine the pH of a 0.741 mol L-1 KOH solution at 25 °C.

Determine the [H3O⁺] in a 0.265 mol L-1 HClO solution. The Ka of HClO is 2.9 × 10-8.

What is the concentration of hydroxide ions in pure water at 30.0 ∘C if Kw at this temperature is 1.47 × 10-14?

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25 °C.

Identify the strongest acid.

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of 2.25 × 10-2 mol L-1?

Which of the following is the correct Arrhenius definition of bases?

Determine the pH of a 0.18 mol L-1 H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

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Filters

Determine the K_a of an acid whose 0.294 mol L^-1 solution has a pH of 2.80.

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10^-2 mol L^-1?

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10^-6 mol L^-1in hydroxide ion.

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00. The equation for the dissociation of NH₃ (K_b= 1.8 × 10^-5)is below:

Determine the pH of a 0.023 mol L^-1 HNO₃ solution.

Determine the pH of a 0.116 mol L^-1 Ba(OH)₂ solution at 25 °C.

Determine the pH of a 0.741 mol L^-1 KOH solution at 25 °C.

Determine the [H₃O⁺] in a 0.265 mol L^-1 HClO solution. The K_a of HClO is 2.9 × 10^-8.

What is the concentration of hydroxide ions in pure water at 30.0 ^∘C if K_w at this temperature is 1.47 × 10^-14?

What is the hydronium ion concentration and the pH for an aqueous solution of NH₃ that has a hydroxide ion concentration of 2.25 × 10^-2 mol L^-1?

Determine the pH of a 0.18 mol L^-1 H₂CO₃ solution. Carbonic acid is a diprotic acid whose K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.