Question 1

Which of the following is the acid found in our stomachs?

Accepted Answer

A) H2SO4 
B) HI 
C) HCl 
D) HF 
E) HBr 
A) H2SO4 
B) HI 
C) HCl 
D) HF 
E) HBr

Question 2

Which of the following solutions would have the highest pH? Assume that they are all 0.10 mol L-1 in acid at 25 °C? The acid is followed by its Ka value.

Accepted Answer

A) HF,3.5 × 10-4 
B) HCN,4.9 × 10-10 
C) HNO2,4.6 × 10-4 
D) HCHO2,1.8 × 10-4 
E) HClO2,1.1 × 10-2 
A) HF,3.5 × 10-4 
B) HCN,4.9 × 10-10 
C) HNO2,4.6 × 10-4 
D) HCHO2,1.8 × 10-4 
E) HClO2,1.1 × 10-2

Question 3

Determine the pH in a 0.235 mol L-1 NaOH solution.

Accepted Answer

A) 13.76 
B) 0.24 
C) 13.37 
D) 0.63 
E) 12 
A) 13.76 
B) 0.24 
C) 13.37 
D) 0.63 
E) 12

Question 4

Which of the following is a Bronsted-Lowry base?

Accepted Answer

A) CH4 
B) HCN 
C) NH3 
D) Cl2 
E) B2H6 
A) CH4 
B) HCN 
C) NH3 
D) Cl2 
E) B2H6

Question 5

Identify the weakest acid.

Accepted Answer

A) HF 
B) HCl 
C) HBr 
D) HI 
E) All of the above are weak acids. 
A) HF 
B) HCl 
C) HBr 
D) HI 
E) All of the above are weak acids.

Question 6

Determine the Kb for CN- at 25 °C.The Ka for HCN is 4.9 × 10-10.

Accepted Answer

A) 4.9 × 10-14 
B) 2.3 × 10-9 
C) 1.4 × 10-5 
D) 2.0 × 10-5 
E) 3.7 × 10-7 
A) 4.9 × 10-14 
B) 2.3 × 10-9 
C) 1.4 × 10-5 
D) 2.0 × 10-5 
E) 3.7 × 10-7

Question 7

Identify the weak diprotic acid.

Accepted Answer

A) HNO3 
B) H3PO4 
C) H2SO3 
D) HClO4 
E) H2SO4 
A) HNO3 
B) H3PO4 
C) H2SO3 
D) HClO4 
E) H2SO4

Question 8

Calculate the concentration of OH- in a solution that contains 3.9 × 10-4 mol L-1 H3O+ at 25 °C.Also identify the solution as acidic,basic,or neutral.

Accepted Answer

A) 2.6 × 10-11 mol L-1,acidic 
B) 2.6 × 10-11 mol L-1,basic 
C) 3.9 × 10-4 mol L-1,neutral 
D) 2.7 × 10-2 mol L-1,basic 
E) 2.7 × 10-2 mol L-1,acidic 
A) 2.6 × 10-11 mol L-1,acidic 
B) 2.6 × 10-11 mol L-1,basic 
C) 3.9 × 10-4 mol L-1,neutral 
D) 2.7 × 10-2 mol L-1,basic 
E) 2.7 × 10-2 mol L-1,acidic

Question 9

Determine the pH of a 0.22 mol L-1 NaF solution at 25 °C.The Ka of HF is 3.5 × 10-5.

Accepted Answer

A) 10.20 
B) 5.10 
C) 8.90 
D) 11.44 
E) 2.56 
A) 10.20 
B) 5.10 
C) 8.90 
D) 11.44 
E) 2.56

Question 10

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of $2.25 \times 10 ^ { - 2 } \mathrm {~mol} \mathrm {~L} ^ { - 1 } ?$

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 11

Calculate the pH for an aqueous solution of acetic acid that contains $2.15 \times 10 - 3 \mathrm {~mol} \mathrm {~L} ^ { - 1 }$ hydronium ion.

Accepted Answer

A) 4.65 × 10-12  
B) 2.15 × 10-3  
C) 2.67 
D) 11.33 
A) 4.65 × 10-12  
B) 2.15 × 10-3  
C) 2.67 
D) 11.33

Question 12

Which of the following bases is the strongest? The base is followed by its Kb.

Accepted Answer

A) (CH3CH2)2NH,8.6 × 10-4 
B) CH3NH2,4.4 × 10-4 
C) C6H5NH2,4.0 × 10-10 
D) NH3,1.76 × 10-5 
E) C5H5N,1.7 × 10-9 
A) (CH3CH2)2NH,8.6 × 10-4 
B) CH3NH2,4.4 × 10-4 
C) C6H5NH2,4.0 × 10-10 
D) NH3,1.76 × 10-5 
E) C5H5N,1.7 × 10-9

Question 13

Calculate the pH of a 0.400 mol L-1 solution of formic acid,Ka = 1.8 × 10-4.

Accepted Answer

A) 3.71 
B) 3.44 
C) 2.29 
D) 4.00 
E) 2.07 
A) 3.71 
B) 3.44 
C) 2.29 
D) 4.00 
E) 2.07

Question 14

What is the hydronium ion concentration of a 0.150 mol L-1 hypochlorous acid solution with $K _ { \mathrm { a } } = 3.5 \times 10 - 8 ?$ The equation for the dissociation of hypochlorous acid is below: $$\mathrm { HOCl } ( a q ) + \mathrm { H } _ { 2 } \mathrm { O } ( l ) \rightleftharpoons \mathrm { H } _ { 3 } \mathrm { O }^ + ( a q ) + \mathrm { OCl } ^ { - } ( a q )$$

Accepted Answer

A) 1.9 × 10-4 mol L-1 
B) 7.2 × 10-4 mol L-1 
C) 2.8 × 10-5 mol L-1 
D) 7.2 × 10-5 mol L-1 
A) 1.9 × 10-4 mol L-1 
B) 7.2 × 10-4 mol L-1 
C) 2.8 × 10-5 mol L-1 
D) 7.2 × 10-5 mol L-1

Question 15

What is the hydronium ion concentration of a 0.500 mol L-1 acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is below: $$\mathrm { CH } _ { 3 } \mathrm { CO } _ { 2 } \mathrm { H } ( a q ) + \mathrm { H } _ { 2 } \mathrm { O } ( l ) \rightleftharpoons \mathrm { H } _ { 3 } \mathrm { O } ^+ ( a q ) + \mathrm { CH } _ { 3 } \mathrm { CO } _ { 2 }^ - ( a q )$$

Accepted Answer

A) 3.0 × 10-2 mol L-1 
B) 4.2 × 10-2 mol L-1 
C) 3.0 × 10-3 mol L-1 
D) 4.2 × 10-3 mol L-1 
A) 3.0 × 10-2 mol L-1 
B) 4.2 × 10-2 mol L-1 
C) 3.0 × 10-3 mol L-1 
D) 4.2 × 10-3 mol L-1

Question 16

Which of the following is an acid-base neutral ion?

Accepted Answer

A) Al3+ 
B) CN- 
C) CO32- 
D) Cl- 
E) NH4+ 
A) Al3+ 
B) CN- 
C) CO32- 
D) Cl- 
E) NH4+

Question 17

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: $$\mathrm { NH } _ { 3 } ( a q ) + \mathrm { H } _ { 2 } \mathrm { O } ( l ) \rightleftharpoons \mathrm { NH } _ { 4 } ^+ ( a q ) + \mathrm { OH } ^- ( a q )$$

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 18

Calculate the pH of a 0.080 mol L-1 carbonic acid solution,H2CO3(aq),that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A) 1.10 
B) 3.73 
C) 6.37 
D) 10.25 
A) 1.10 
B) 3.73 
C) 6.37 
D) 10.25

Question 19

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 20

Determine the pH of a 0.00598 mol L-1 HClO4 solution.

Accepted Answer

A) 1.777 
B) 6.434 
C) 7.566 
D) 2.223 
E) 3.558 
A) 1.777 
B) 6.434 
C) 7.566 
D) 2.223 
E) 3.558

Exam 15: Acids and Bases

Which of the following is the acid found in our stomachs?

Which of the following solutions would have the highest pH? Assume that they are all 0.10 mol L-1 in acid at 25 °C? The acid is followed by its Ka value.

Determine the pH in a 0.235 mol L-1 NaOH solution.

Which of the following is a Bronsted-Lowry base?

Identify the weakest acid.

Determine the Kb for CN- at 25 °C.The Ka for HCN is 4.9 × 10-10.

Identify the weak diprotic acid.

Calculate the concentration of OH- in a solution that contains 3.9 × 10-4 mol L-1 H3O+ at 25 °C.Also identify the solution as acidic,basic,or neutral.

Determine the pH of a 0.22 mol L-1 NaF solution at 25 °C.The Ka of HF is 3.5 × 10-5.

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?2.25 \times 10 ^ { - 2 } \mathrm {~mol} \mathrm {~L} ^ { - 1 } ?2.25×10−2 mol L−1?

Calculate the pH for an aqueous solution of acetic acid that contains 2.15×10−3 mol L−12.15 \times 10 - 3 \mathrm {~mol} \mathrm {~L} ^ { - 1 }2.15×10−3 mol L−1 hydronium ion.

Which of the following bases is the strongest? The base is followed by its Kb.

Calculate the pH of a 0.400 mol L-1 solution of formic acid,Ka = 1.8 × 10-4.

Which of the following is an acid-base neutral ion?

Calculate the pH of a 0.080 mol L-1 carbonic acid solution,H2CO3(aq),that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

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

Determine the pH of a 0.00598 mol L-1 HClO4 solution.

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Filters

Which of the following solutions would have the highest pH? Assume that they are all 0.10 mol L^-1in acid at 25 °C? The acid is followed by its K_a value.

Determine the pH in a 0.235 mol L^-1 NaOH solution.

Determine the K_b for CN^- at 25 °C.The K_a for HCN is 4.9 × 10^-10.

Calculate the concentration of OH^- in a solution that contains 3.9 × 10^-4 mol L^-1 H₃O⁺ at 25 °C.Also identify the solution as acidic,basic,or neutral.

Determine the pH of a 0.22 mol L^-1 NaF solution at 25 °C.The K_a of HF is 3.5 × 10^-5.

What is the hydronium ion concentration and the pH for an aqueous solution of NH₃ that has a hydroxide ion concentration of $2.25 \times 10 ^ { - 2 } \mathrm {~mol} \mathrm {~L} ^ { - 1 } ?$

Calculate the pH for an aqueous solution of acetic acid that contains $2.15 \times 10 - 3 \mathrm {~mol} \mathrm {~L} ^ { - 1 }$ hydronium ion.

Which of the following bases is the strongest? The base is followed by its K_b.

Calculate the pH of a 0.400 mol L^-1 solution of formic acid,K_a = 1.8 × 10^-4.

Calculate the pH of a 0.080 mol L^-1 carbonic acid solution,H₂CO₃₍_aq_),that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Determine the pH of a 0.00598 mol L^-1 HClO₄ solution.