Question 1

All of the following compounds are acids containing chlorine.Which compound is the weakest acid?

Accepted Answer

A)  HCl 
B)  HClO 
C)  HClO2 
D)  HClO3 
E)  HClO4 
A)  HCl 
B)  HClO 
C)  HClO2 
D)  HClO3 
E)  HClO4 B

Question 2

What is the hydronium-ion concentration in a solution formed by combining 750 mL of 0.10 M NaOH with 250 mL of 0.30 M HCl?
NaOH(aq)+ HCl(aq)$\to$ NaCl(aq)+ H2O(l)

Accepted Answer

A)  0.075 M 
B)  1.7 $\times$ 10-13 M 
C)  1.0 $\times$ 10-7 M 
D)  0.30 M 
E)  0.10 M 
A)  0.075 M 
B)  1.7 $\times$ 10-13 M 
C)  1.0 $\times$ 10-7 M 
D)  0.30 M 
E)  0.10 M C

Question 3

Rank H3PO4,H2PO4-,and HPO42- in order of increasing acid strength.

Accepted Answer

A)  HPO42- 2PO4- 3PO4 
B)  H2PO4- 42- 3PO4 
C)  H2PO4- 3PO4 42- 
D)  HPO42- 3PO4 2PO4- 
E)  H3PO4 2PO4- 42- 
A)  HPO42- 2PO4- 3PO4 
B)  H2PO4- 42- 3PO4 
C)  H2PO4- 3PO4 42- 
D)  HPO42- 3PO4 2PO4- 
E)  H3PO4 2PO4- 42- A

Question 4

Which of the following statements is INCORRECT?

Accepted Answer

A)  H3PO4 is a stronger acid than H2PO4-. 
B)  HClO3 is a stronger acid than HClO2. 
C)  HNO3 is a stronger acid than HNO2. 
D)  [Fe(H2O)6]2+ is a stronger acid than [Fe(H2O)6]3+. 
E)  HOCl is stronger acid than HOBr. 
A)  H3PO4 is a stronger acid than H2PO4-. 
B)  HClO3 is a stronger acid than HClO2. 
C)  HNO3 is a stronger acid than HNO2. 
D)  [Fe(H2O)6]2+ is a stronger acid than [Fe(H2O)6]3+. 
E)  HOCl is stronger acid than HOBr.

Question 5

When a Lewis acid and a Lewis base combine,the product may be referred to as an acid-base ________.

Accepted Answer

The answer of When a Lewis acid and a Lewis...

Question 6

What is the equilibrium hydronium ion concentration of an initially 5.4 M solution of hypochlorous acid,HOCl,at 25°C (Ka =   )?

Accepted Answer

A)    M 
B)    M 
C)    M 
D)    M 
E)    M 
A)    M 
B)    M 
C)    M 
D)    M 
E)    M

Question 7

What is the pH of a 0.11 M solution of methylamine (CH3NH2,Kb = 4.4 $\times$ 10-4)at 25oC? (Kw = 1.01 $\times$ 10-14)

Accepted Answer

A)  5.80 
B)  0.96 
C)  11.83 
D)  13.04 
E)  2.17 
A)  5.80 
B)  0.96 
C)  11.83 
D)  13.04 
E)  2.17

Question 8

In the reaction
CuO(s)+ CO2(g)$\to$CuCO3(s),

Accepted Answer

A)  O2- acts as a Lewis base and CO2 acts as a Lewis acid. 
B)  O2- acts as a Lewis base and Cu2+ acts as a Lewis acid. 
C)  CuO is the Lewis acid and CuCO3 is its conjugate base. 
D)  CO2 is the Lewis acid and CuCO3 is its conjugate base. 
E)  Cu2+ acts as a Lewis acid and CO32- acts as a Lewis base. 
A)  O2- acts as a Lewis base and CO2 acts as a Lewis acid. 
B)  O2- acts as a Lewis base and Cu2+ acts as a Lewis acid. 
C)  CuO is the Lewis acid and CuCO3 is its conjugate base. 
D)  CO2 is the Lewis acid and CuCO3 is its conjugate base. 
E)  Cu2+ acts as a Lewis acid and CO32- acts as a Lewis base.

Question 9

What is the OH- concentration of an aqueous solution with a pH of 9.83? (Kw = 1.01 $\times$ 10-14)

Accepted Answer

A)  1.3 $\times$ 10-10 M 
B)  6.8 $\times$ 10-5 M 
C)  6.8 $\times$ 10-1 M 
D)  1.5 $\times$ 10-2 M 
E)  7.4 $\times$ 109 M 
A)  1.3 $\times$ 10-10 M 
B)  6.8 $\times$ 10-5 M 
C)  6.8 $\times$ 10-1 M 
D)  1.5 $\times$ 10-2 M 
E)  7.4 $\times$ 109 M

Question 10

What is the pH of a solution prepared by dissolving 0.923 g of NaOH(s)in 5.50 L of water? (Kw = 1.01 $\times$ 10-14)

Accepted Answer

A)  1.637 
B)  12.363 
C)  7.000 
D)  11.623 
E)  2.377 
A)  1.637 
B)  12.363 
C)  7.000 
D)  11.623 
E)  2.377

Question 11

What is the equilibrium pH of an initially 0.64 M solution of the monoprotic acid benzoic acid at 25°C (Ka =   )?

Accepted Answer

A)  2.20 
B)  7.00 
C)  1.90 
D)  12.10 
E)  5.10 
A)  2.20 
B)  7.00 
C)  1.90 
D)  12.10 
E)  5.10

Question 12

Calculate the pH of the following aqueous solution:
0)29 M H2S (pKa1 = 7.00; pKa2 = 12.89)

Accepted Answer

A)  10.23 
B)  6.46 
C)  3.77 
D)  7.54 
E)  7.00 
A)  10.23 
B)  6.46 
C)  3.77 
D)  7.54 
E)  7.00

Question 13

The pH of a solution of 2.2 M H2A (Ka1 = 1.0 $\times$ 10-6 and Ka2 is 1.0 $\times$ 10-10)is:

Accepted Answer

A)  10.00 
B)  2.83 
C)  11.17 
D)  5.66 
E)  7.00 
A)  10.00 
B)  2.83 
C)  11.17 
D)  5.66 
E)  7.00

Question 14

Which equation depicts aqueous hydrogen sulfide behaving as a Brønsted-Lowry acid in water?

Accepted Answer

A)  H2S(aq)+ 2 OH-(aq)   SO2(aq)+ 2 H2(g) 
B)  H2S(aq)+ H3O+(aq)   H3S+(aq)+ H2O(   ) 
C)  H2S(aq)+ H2O(   )   HS-(aq)+ H3O+(aq) 
D)  HS-(aq)+ H3O+(aq)   H2S(aq)+ H2O(   ) 
E)  H2S(aq)+ H2O(   )   H3S++(aq)+ OH-(aq) 
A)  H2S(aq)+ 2 OH-(aq)   SO2(aq)+ 2 H2(g) 
B)  H2S(aq)+ H3O+(aq)   H3S+(aq)+ H2O(   ) 
C)  H2S(aq)+ H2O(   )   HS-(aq)+ H3O+(aq) 
D)  HS-(aq)+ H3O+(aq)   H2S(aq)+ H2O(   ) 
E)  H2S(aq)+ H2O(   )   H3S++(aq)+ OH-(aq)

Question 15

What is the H3O+ concentration in 0.0047 M NaOH(aq)at 25 S1U1P1$\circ$S1S1P0C? (Kw = 1.01 $\times$ 10-14)

Accepted Answer

A)  2.1 $\times$ 10-12 M 
B)  4.7 $\times$ 10-3 M 
C)  1.0 $\times$ 10-14 M 
D)  1.0 $\times$ 10-7 M 
E)  4.7 $\times$ 10-17 M 
A)  2.1 $\times$ 10-12 M 
B)  4.7 $\times$ 10-3 M 
C)  1.0 $\times$ 10-14 M 
D)  1.0 $\times$ 10-7 M 
E)  4.7 $\times$ 10-17 M

Question 16

Carbonic acid is a diprotic acid,H2CO3,with Ka1 = 4.2 $\times$ 10-7 and Ka2 = 4.8 $\times$ 10-11 at 25°C.The ion product for water is Kw = 1.0 $\times$ 10-14 at 25°C.What is the OH- concentration of a solution that is 0.18 M in Na2CO3?

Accepted Answer

A)  6.1 $\times$ 10-3 M 
B)  2.1 $\times$ 10-4 M 
C)  6.5 $\times$ 10-5 M 
D)  2.9 $\times$ 10-6 M 
E)  2.7 $\times$ 10-4 M 
A)  6.1 $\times$ 10-3 M 
B)  2.1 $\times$ 10-4 M 
C)  6.5 $\times$ 10-5 M 
D)  2.9 $\times$ 10-6 M 
E)  2.7 $\times$ 10-4 M

Question 17

The concentration of H3O+ in a solution is 7 $\times$ 10-4 M at 25°C.What is its hydroxide-ion concentration? (Kw = 1.01 $\times$ 10-14)

Accepted Answer

A)  7 $\times$ 10-4 M 
B)  1 $\times$ 10-10 M 
C)  2 $\times$ 10-10 M 
D)  3 $\times$ 10-10 M 
E)  1 $\times$ 10-11 M 
A)  7 $\times$ 10-4 M 
B)  1 $\times$ 10-10 M 
C)  2 $\times$ 10-10 M 
D)  3 $\times$ 10-10 M 
E)  1 $\times$ 10-11 M

Question 18

An aqueous solution with a pH of 10.60 is diluted from 1.0 L to 2.0 L.What is the pH of the diluted solution?

Accepted Answer

A)  5.30 
B)  9.60 
C)  10.30 
D)  10.60 
E)  10.90 
A)  5.30 
B)  9.60 
C)  10.30 
D)  10.60 
E)  10.90

Question 19

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 4.6 $\times$ 10-4 M.What is the acid-ionization constant,Ka,for this acid?

Accepted Answer

A)  2.1 $\times$ 10-2 
B)  3.2 $\times$ 10-3 
C)  4.6 $\times$ 10-4 
D)  2.1 $\times$ 10-6 
E)  5.5 $\times$ 10-5 
A)  2.1 $\times$ 10-2 
B)  3.2 $\times$ 10-3 
C)  4.6 $\times$ 10-4 
D)  2.1 $\times$ 10-6 
E)  5.5 $\times$ 10-5

Question 20

Which of the following is the correct equation for the reaction of ammonia in water?

Accepted Answer

A)  NH3(aq)+ H2O(l)   NH4+(aq)+ OH-(aq) 
B)  NH3(aq)+ H2O(l)   NH2-(aq)+ H3O+(aq) 
C)  NH3(aq)+ H3O+(aq)   NH4+(aq)+ H2O(l) 
D)  NH3(aq)+ OH-(aq)   NH2-(aq)+ H2O(l) 
E)  NH3(aq)+ H2O(l)   NH2-(aq)+ H3O+(aq) 
A)  NH3(aq)+ H2O(l)   NH4+(aq)+ OH-(aq) 
B)  NH3(aq)+ H2O(l)   NH2-(aq)+ H3O+(aq) 
C)  NH3(aq)+ H3O+(aq)   NH4+(aq)+ H2O(l) 
D)  NH3(aq)+ OH-(aq)   NH2-(aq)+ H2O(l) 
E)  NH3(aq)+ H2O(l)   NH2-(aq)+ H3O+(aq)

Exam 17: The Chemistry of Acids and Bases

All of the following compounds are acids containing chlorine.Which compound is the weakest acid?

What is the hydronium-ion concentration in a solution formed by combining 750 mL of 0.10 M NaOH with 250 mL of 0.30 M HCl? NaOH(aq)+ HCl(aq) →\to→ NaCl(aq)+ H2O(l)

Rank H3PO4,H2PO4-,and HPO42- in order of increasing acid strength.

Which of the following statements is INCORRECT?

When a Lewis acid and a Lewis base combine,the product may be referred to as an acid-base ________.

What is the equilibrium hydronium ion concentration of an initially 5.4 M solution of hypochlorous acid,HOCl,at 25°C (Ka = )?

What is the pH of a 0.11 M solution of methylamine (CH3NH2,Kb = 4.4 ×\times× 10-4)at 25oC? (Kw = 1.01 ×\times× 10-14)

In the reaction CuO(s)+ CO2(g) →\to→ CuCO3(s),

What is the OH- concentration of an aqueous solution with a pH of 9.83? (Kw = 1.01 ×\times× 10-14)

What is the pH of a solution prepared by dissolving 0.923 g of NaOH(s)in 5.50 L of water? (Kw = 1.01 ×\times× 10-14)

What is the equilibrium pH of an initially 0.64 M solution of the monoprotic acid benzoic acid at 25°C (Ka = )?

Calculate the pH of the following aqueous solution: 0)29 M H2S (pKa1 = 7.00; pKa2 = 12.89)

The pH of a solution of 2.2 M H2A (Ka1 = 1.0 ×\times× 10-6 and Ka2 is 1.0 ×\times× 10-10)is:

Which equation depicts aqueous hydrogen sulfide behaving as a Brønsted-Lowry acid in water?

What is the H3O+ concentration in 0.0047 M NaOH(aq)at 25 ∘\circ∘ C? (Kw = 1.01 ×\times× 10-14)

Carbonic acid is a diprotic acid,H2CO3,with Ka1 = 4.2 ×\times× 10-7 and Ka2 = 4.8 ×\times× 10-11 at 25°C.The ion product for water is Kw = 1.0 ×\times× 10-14 at 25°C.What is the OH- concentration of a solution that is 0.18 M in Na2CO3?

The concentration of H3O+ in a solution is 7 ×\times× 10-4 M at 25°C.What is its hydroxide-ion concentration? (Kw = 1.01 ×\times× 10-14)

An aqueous solution with a pH of 10.60 is diluted from 1.0 L to 2.0 L.What is the pH of the diluted solution?

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 4.6 ×\times× 10-4 M.What is the acid-ionization constant,Ka,for this acid?

Which of the following is the correct equation for the reaction of ammonia in water?

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What is the hydronium-ion concentration in a solution formed by combining 750 mL of 0.10 M NaOH with 250 mL of 0.30 M HCl? NaOH(aq)+ HCl(aq) $\to$ NaCl(aq)+ H₂O(l)

Rank H₃PO₄,H₂PO₄^-,and HPO₄^2- in order of increasing acid strength.

What is the equilibrium hydronium ion concentration of an initially 5.4 M solution of hypochlorous acid,HOCl,at 25°C (K_a = )?

What is the pH of a 0.11 M solution of methylamine (CH₃NH₂,K_b = 4.4 $\times$ 10^-4)at 25^oC? (K_w = 1.01 $\times$ 10^-14)

In the reaction CuO(s)+ CO₂(g) $\to$ CuCO₃(s),

What is the OH^- concentration of an aqueous solution with a pH of 9.83? (K_w = 1.01 $\times$ 10^-14)

What is the pH of a solution prepared by dissolving 0.923 g of NaOH(s)in 5.50 L of water? (K_w = 1.01 $\times$ 10^-14)

What is the equilibrium pH of an initially 0.64 M solution of the monoprotic acid benzoic acid at 25°C (K_a = )?

Calculate the pH of the following aqueous solution: 0)29 M H₂S (pK_a1 = 7.00; pK_a2 = 12.89)

The pH of a solution of 2.2 M H₂A (K_a1= 1.0 $\times$ 10^-6 and K_a2is 1.0 $\times$ 10^-10)is:

What is the H₃O⁺ concentration in 0.0047 M NaOH(aq)at 25 ^$\circ$C? (K_w = 1.01 $\times$ 10^-14)

Carbonic acid is a diprotic acid,H₂CO₃,with K_a1 = 4.2 $\times$ 10^-7 and K_a2 = 4.8 $\times$ 10^-11 at 25°C.The ion product for water is K_w = 1.0 $\times$ 10^-14 at 25°C.What is the OH^- concentration of a solution that is 0.18 M in Na₂CO₃?

The concentration of H₃O⁺ in a solution is 7 $\times$ 10^-4 M at 25°C.What is its hydroxide-ion concentration? (K_w = 1.01 $\times$ 10^-14)

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 4.6 $\times$ 10^-4 M.What is the acid-ionization constant,K_a,for this acid?