Question 1

Calculate the pH of a 2.0  10-5 M solution of HOC6H5. (Ka = 1.6  10-10)

Accepted Answer

A)   6.94
B)   6.75
C)   7.06
D)   7.25
E)   none of theseF) A) and E)
G) All of the above

Question 2

Calculate [H+] in a 0.012 M solution of HCN, Ka = 6.2  10-10.

Accepted Answer

A)   3.0  10-7 M
B)   3.7  10-9 M
C)   6.2  10-10 M
D)   2.7  10-6 M
E)   2.3  10-4 MF) B) and C)
G) B) and E)

Question 3

Calculate the pOH of a 0.70 M solution of acetic acid (Ka = 1.8  10-5)  at 25°C.

Accepted Answer

A)   2.72
B)   9.26
C)   4.90
D)   11.55
E)   2.45F) B) and C)
G) A) and B)

Question 4

The following three equations represent equilibria that lie far to the right.
HNO3(aq)  + CN-(aq)  3(aq)  + CN-(aq)    HCN(aq)  + NO3-(aq)  HCN(aq)  + OH-(aq)    H2O(l)  + CN-(aq)  H2O(l)  + CH3O-(aq)    CH3OH(aq)  + OH-(aq)  -Identify the strongest base. A)  CH3OH B)  CH3O- C)  H2O D)  NO3- E)  CN- " class="answers-bank-image d-inline" rel="preload" > HCN(aq)  + NO3-(aq) 
HCN(aq)  + OH-(aq)  3(aq)  + CN-(aq)    HCN(aq)  + NO3-(aq)  HCN(aq)  + OH-(aq)    H2O(l)  + CN-(aq)  H2O(l)  + CH3O-(aq)    CH3OH(aq)  + OH-(aq)  -Identify the strongest base. A)  CH3OH B)  CH3O- C)  H2O D)  NO3- E)  CN- " class="answers-bank-image d-inline" rel="preload" > H2O(l)  + CN-(aq) 
H2O(l)  + CH3O-(aq)  3(aq)  + CN-(aq)    HCN(aq)  + NO3-(aq)  HCN(aq)  + OH-(aq)    H2O(l)  + CN-(aq)  H2O(l)  + CH3O-(aq)    CH3OH(aq)  + OH-(aq)  -Identify the strongest base. A)  CH3OH B)  CH3O- C)  H2O D)  NO3- E)  CN- " class="answers-bank-image d-inline" rel="preload" > CH3OH(aq)  + OH-(aq) 
-Identify the strongest base.

Accepted Answer

A)   CH3OH
B)   CH3O-
C)   H2O
D)   NO3-
E)   CN-F) A) and D)
G) B) and D)

Question 5

Calculate the pH of a 0.005 M solution of potassium oxide, K2O.

Accepted Answer

A)   2.3
B)   11.7
C)   7.0
D)   12.0
E)   2.0F) B) and C)
G) A) and D)

Question 6

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (Ka = 1.8  10-5) ? (Assume the volumes are additive.)

Accepted Answer

A)   30 mL
B)   3 L
C)   30 L
D)   300 L
E)   300 mLF) B) and D)
G) All of the above

Question 7

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC2H3O2, C5H5NHCl, KOH, HCN. (Ka for HCN is 6.2  10-10; Ka for HF is 7.2  10-4; Ka for HC2H3O2 is 1.8  10-5; and Kb for C5H5N is 1.7  10-9)

Accepted Answer

A)   C5H5NHCl, HCN, NaF, NaC2H3O2, KOH
B)   NaF, NaC2H3O2, HCN, C5H5NHCl, KOH
C)   KOH, NaC2H3O2, NaF, HCN, C5H5NHCl
D)   HCN, C5H5NHCl, NaF, NaC2H3O2, KOH
E)   none of theseF) B) and E)
G) B) and D)

Question 8

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride  (NH4F)  For NH3, Kb = 1.8  10-5; for HF, Ka = 7.2  10-4.

Accepted Answer

A)   neutral
B)   basic
C)   acidicD) A) and B)
E) A) and C)

Question 9

Which of the following species is not amphoteric?

Accepted Answer

A)   H2PO4-
B)   HPO42-
C)   H2O
D)   HSO4-
E)   All of these are amphoteric.F) A) and B)
G) B) and D)

Question 10

The conjugate base of a weak acid is

Accepted Answer

A)   a strong base.
B)   a strong acid.
C)   a weak base.
D)   a weak acid.
E)   none of theseF) A) and B)
G) B) and C)

Question 11

HOAc Ka = 1.8 10-5 H2CO3 Ka1 = 4.3  10-7, Ka2 = 5.6  10-11
Which of the following 0.01 M solutions has the highest pH?

Accepted Answer

A)   HOAc
B)   NaHCO3
C)   H2CO3
D)   NaOAc
E)   Na2CO3F) D) and E)
G) All of the above

Question 12

The pH of a strong acid solution is always lower than the pH of a weak acid solution. If this is true, explain why and include an example with calculations. If it is false, explain why and include a counterexample with calculations.

Accepted Answer

A) True 
 B)False

Question 13

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate  (NaHCO3)

Accepted Answer

A)   basic
B)   neutral
C)   acidicD) A) and C)
E) All of the above

Question 14

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium cyanide (NaCN)

Accepted Answer

A)   neutral
B)   basic
C)   acidicD) A) and B)
E) A) and C)

Question 15

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO2, a weak acid) , the equilibrium constant expression is

Accepted Answer

A)   2, a weak acid) , the equilibrium constant expression is 
A)     
B)     
C)     
D)   K = [H+][NO2-] 
E)   none of these " class="answers-bank-image d-inline" rel="preload" >
B)   2, a weak acid) , the equilibrium constant expression is 
A)     
B)     
C)     
D)   K = [H+][NO2-] 
E)   none of these " class="answers-bank-image d-inline" rel="preload" >
C)   2, a weak acid) , the equilibrium constant expression is 
A)     
B)     
C)     
D)   K = [H+][NO2-] 
E)   none of these " class="answers-bank-image d-inline" rel="preload" >
D)   K = [H+][NO2-]
E)   none of theseF) C) and D)
G) A) and B)

Question 16

Calculate the pH of a 0.040 M perchloric acid (HClO4)  solution.

Accepted Answer

A)   1.40
B)   2.10
C)   12.60
D)   11.90
E)   none of theseF) B) and C)
G) A) and D)

Question 17

The pH of a solution made of 0.100 mol of a weak monoprotic acid HA in 1.000 L of solution is 1.470. Calculate Ka for this acid.

Accepted Answer

A)   29.5
B)   0
C)   0.100
D)   0.0174
E)   0.0339F) All of the above
G) C) and D)

Question 18

Which of the following reactions is associated with the definition of Ka?

Accepted Answer

A)   [Al(OH2) 6]3+   a? 
A)   [Al(OH2) 6]3+      Al(OH) (OH2) 52+ + H+ 
B)   CN- + H+   HCN 
C)   OCl- + H2O   HOCl + OH- 
D)   Al3+ + 6H2O   Al(OH2) 63+ " class="answers-bank-image d-inline" rel="preload" > Al(OH) (OH2) 52+ + H+
B)   CN- + H+ a? 
A)   [Al(OH2) 6]3+      Al(OH) (OH2) 52+ + H+ 
B)   CN- + H+   HCN 
C)   OCl- + H2O   HOCl + OH- 
D)   Al3+ + 6H2O   Al(OH2) 63+ " class="answers-bank-image d-inline" rel="preload" > HCN
C)   OCl- + H2O a? 
A)   [Al(OH2) 6]3+      Al(OH) (OH2) 52+ + H+ 
B)   CN- + H+   HCN 
C)   OCl- + H2O   HOCl + OH- 
D)   Al3+ + 6H2O   Al(OH2) 63+ " class="answers-bank-image d-inline" rel="preload" > HOCl + OH-
D)   Al3+ + 6H2O a? 
A)   [Al(OH2) 6]3+      Al(OH) (OH2) 52+ + H+ 
B)   CN- + H+   HCN 
C)   OCl- + H2O   HOCl + OH- 
D)   Al3+ + 6H2O   Al(OH2) 63+ " class="answers-bank-image d-inline" rel="preload" > Al(OH2) 63+E) None of the above
F) B) and C)

Question 19

Calculate [H+] in a 1.2  10-5 M solution of NH4Cl. (Kb for NH3 = 1.8  10-5)

Accepted Answer

A)   1.5  10-5 M
B)   8.2  10-8 M
C)   1.3  10-7 M
D)   1.2  10-5 M
E)   7.7  10-8 MF) A) and B)
G) All of the above

Exam 7: Acids and Bases

Calculate the pH of a 0.040 M perchloric acid (HClO₄) solution.

Correct Answer
verified

Calculate [H⁺] in a 1.2  10^-⁵ M solution of NH₄Cl. (K_b for NH₃ = 1.8  10^-⁵)

Correct Answer
verified

Calculate [H⁺] in a 0.012 M solution of HCN, K_a = 6.2  10^-¹⁰.

Correct Answer
verified

Which of the following species is not amphoteric?

Correct Answer
verified

Which of the following reactions is associated with the definition of K_a?

Correct Answer
verified

Calculate the pH of a 0.005 M solution of potassium oxide, K₂O.

Correct Answer
verified

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO₃)

Correct Answer
verified

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC₂H₃O₂, C₅H₅NHCl, KOH, HCN. (K_a for HCN is 6.2  10^-¹⁰; K_a for HF is 7.2  10^-⁴; K_a for HC₂H₃O₂ is 1.8  10^-⁵; and K_b for C₅H₅N is 1.7  10^-⁹)

Correct Answer
verified

The following three equations represent equilibria that lie far to the right. HNO₃(aq) + CN^-(aq) HCN(aq) + NO₃^-(aq) HCN(aq) + OH^-(aq) H₂O(l) + CN^-(aq) H₂O(l) + CH₃O^-(aq) CH₃OH(aq) + OH^-(aq) -Identify the strongest base.

Correct Answer
verified

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (K_a = 1.8  10^-⁵) ? (Assume the volumes are additive.)

Correct Answer
verified

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO₂, a weak acid) , the equilibrium constant expression is

Correct Answer
verified

The pH of a strong acid solution is always lower than the pH of a weak acid solution. If this is true, explain why and include an example with calculations. If it is false, explain why and include a counterexample with calculations.

Correct Answer
verified

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH4F) For NH₃, K_b = 1.8  10^-⁵; for HF, K_a = 7.2  10^-⁴.

Correct Answer
verified

HOAc K_a = 1.8 10^-⁵ H₂CO₃K_a1 = 4.3  10^-⁷,K_a2 = 5.6  10^-¹¹ Which of the following 0.01 M solutions has the highest pH?

Correct Answer
verified

Calculate the pOH of a 0.70 M solution of acetic acid (K_a = 1.8  10^-⁵) at 25°C.

Correct Answer
verified

The conjugate base of a weak acid is

Correct Answer
verified

The pH of a solution made of 0.100 mol of a weak monoprotic acid HA in 1.000 L of solution is 1.470. Calculate K_a for this acid.

Correct Answer
verified

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium cyanide (NaCN)

Correct Answer
verified

Calculate the pH of a 2.0  10^-⁵ M solution of HOC₆H₅. (K_a = 1.6  10^-¹⁰)

Correct Answer
verified

Exam 7: Acids and Bases

Calculate the pH of a 0.040 M perchloric acid (HClO4) solution.

Correct AnswerverifiedShow Answer

Calculate [H+] in a 1.2  10-5 M solution of NH4Cl. (Kb for NH3 = 1.8  10-5)

Correct AnswerverifiedShow Answer

Calculate [H+] in a 0.012 M solution of HCN, Ka = 6.2  10-10.

Correct AnswerverifiedShow Answer

Which of the following species is not amphoteric?

Correct AnswerverifiedShow Answer

Which of the following reactions is associated with the definition of Ka?

Correct AnswerverifiedShow Answer

Calculate the pH of a 0.005 M solution of potassium oxide, K2O.

Correct AnswerverifiedShow Answer

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO3)

Correct AnswerverifiedShow Answer

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC2H3O2, C5H5NHCl, KOH, HCN. (Ka for HCN is 6.2  10-10; Ka for HF is 7.2  10-4; Ka for HC2H3O2 is 1.8  10-5; and Kb for C5H5N is 1.7  10-9)

Correct AnswerverifiedShow Answer

The following three equations represent equilibria that lie far to the right. HNO3(aq) + CN-(aq) HCN(aq) + NO3-(aq) HCN(aq) + OH-(aq) H2O(l) + CN-(aq) H2O(l) + CH3O-(aq) CH3OH(aq) + OH-(aq) -Identify the strongest base.

Correct AnswerverifiedShow Answer

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (Ka = 1.8  10-5) ? (Assume the volumes are additive.)

Correct AnswerverifiedShow Answer

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO2, a weak acid) , the equilibrium constant expression is

Correct AnswerverifiedShow Answer

The pH of a strong acid solution is always lower than the pH of a weak acid solution. If this is true, explain why and include an example with calculations. If it is false, explain why and include a counterexample with calculations.

Correct AnswerverifiedShow Answer

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH4F) For NH3, Kb = 1.8  10-5; for HF, Ka = 7.2  10-4.

Correct AnswerverifiedShow Answer

HOAc Ka = 1.8 10-5 H2CO3 Ka1 = 4.3  10-7, Ka2 = 5.6  10-11 Which of the following 0.01 M solutions has the highest pH?

Correct AnswerverifiedShow Answer

Calculate the pOH of a 0.70 M solution of acetic acid (Ka = 1.8  10-5) at 25°C.

Correct AnswerverifiedShow Answer

The conjugate base of a weak acid is

Correct AnswerverifiedShow Answer

The pH of a solution made of 0.100 mol of a weak monoprotic acid HA in 1.000 L of solution is 1.470. Calculate Ka for this acid.

Correct AnswerverifiedShow Answer

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium cyanide (NaCN)

Correct AnswerverifiedShow Answer

Calculate the pH of a 2.0  10-5 M solution of HOC6H5. (Ka = 1.6  10-10)

Correct AnswerverifiedShow Answer

Calculate the pH of a 0.040 M perchloric acid (HClO₄) solution.

Correct Answer
verified

Calculate [H⁺] in a 1.2  10^-⁵ M solution of NH₄Cl. (K_b for NH₃ = 1.8  10^-⁵)

Correct Answer
verified

Calculate [H⁺] in a 0.012 M solution of HCN, K_a = 6.2  10^-¹⁰.

Correct Answer
verified

Correct Answer
verified

Which of the following reactions is associated with the definition of K_a?

Correct Answer
verified

Calculate the pH of a 0.005 M solution of potassium oxide, K₂O.

Correct Answer
verified

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO₃)

Correct Answer
verified

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC₂H₃O₂, C₅H₅NHCl, KOH, HCN. (K_a for HCN is 6.2  10^-¹⁰; K_a for HF is 7.2  10^-⁴; K_a for HC₂H₃O₂ is 1.8  10^-⁵; and K_b for C₅H₅N is 1.7  10^-⁹)

Correct Answer
verified

The following three equations represent equilibria that lie far to the right. HNO₃(aq) + CN^-(aq) HCN(aq) + NO₃^-(aq) HCN(aq) + OH^-(aq) H₂O(l) + CN^-(aq) H₂O(l) + CH₃O^-(aq) CH₃OH(aq) + OH^-(aq) -Identify the strongest base.

Correct Answer
verified

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (K_a = 1.8  10^-⁵) ? (Assume the volumes are additive.)

Correct Answer
verified

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO₂, a weak acid) , the equilibrium constant expression is

Correct Answer
verified

Correct Answer
verified

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH4F) For NH₃, K_b = 1.8  10^-⁵; for HF, K_a = 7.2  10^-⁴.

Correct Answer
verified

HOAc K_a = 1.8 10^-⁵ H₂CO₃K_a1 = 4.3  10^-⁷,K_a2 = 5.6  10^-¹¹ Which of the following 0.01 M solutions has the highest pH?

Correct Answer
verified

Calculate the pOH of a 0.70 M solution of acetic acid (K_a = 1.8  10^-⁵) at 25°C.

Correct Answer
verified

Correct Answer
verified

The pH of a solution made of 0.100 mol of a weak monoprotic acid HA in 1.000 L of solution is 1.470. Calculate K_a for this acid.

Correct Answer
verified

Correct Answer
verified

Calculate the pH of a 2.0  10^-⁵ M solution of HOC₆H₅. (K_a = 1.6  10^-¹⁰)

Correct Answer
verified