Question 1

What is the strongest monoprotic acid of the following set if all the acids are at 0.100 M concentration?

Accepted Answer

A) hydrofluoric acid with Ka = 3.5 × 10-4 
B) benzoic acid with Ka = 6.5 × 10-5 
C) acetic acid with Ka = 1.8 × 10-5 
D) hypochlorous acid with Ka = 3.5 × 10-8 
A) hydrofluoric acid with Ka = 3.5 × 10-4 
B) benzoic acid with Ka = 6.5 × 10-5 
C) acetic acid with Ka = 1.8 × 10-5 
D) hypochlorous acid with Ka = 3.5 × 10-8

Question 2

Phenobarbital has a pKa = 7.4.Compared to a 1.0 × 10-3 M solution,1.0 × 10-4 M phenobarbital will have a ________ (higher,lower)pH and a ________ (higher,lower)percent ionization.

Accepted Answer

Question 3

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-4 M in hydroxide ion.

Accepted Answer

A) 4.00 × 10-9 M 
B) 4.00 × 10-10 M 
C) 4.00 × 10-11 M 
D) 5.00 × 10-11 M 
A) 4.00 × 10-9 M 
B) 4.00 × 10-10 M 
C) 4.00 × 10-11 M 
D) 5.00 × 10-11 M

Question 4

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A) LiHSO4 
B) NaClO4 
C) KF 
D) CH3NH3I 
A) LiHSO4 
B) NaClO4 
C) KF 
D) CH3NH3I

Question 5

What is the conjugate base of the Br∅nsted-Lowry acid HPO42-?

Accepted Answer

A) H3PO4 
B) H2PO4- 
C) HPO42- 
D) PO43- 
A) H3PO4 
B) H2PO4- 
C) HPO42- 
D) PO43-

Question 6

When dissolved in water,which of the following compounds is an Arrhenius acid?

Accepted Answer

A) HCN 
B) NaOH 
C) NaF 
D) CH3CH2OH 
A) HCN 
B) NaOH 
C) NaF 
D) CH3CH2OH

Question 7

A proton hydrated by ten water molecules has the formula ________.

Accepted Answer

The answer of A proton hydrated by ten water molecules...

Question 8

An Arrhenius acid is best defined as a

Accepted Answer

A) electron pair donor. 
B) proton acceptor. 
C) substance that dissociates in water to produce aqueous hydrogen ions. 
D) substance that dissociates in water to produce aqueous hydroxide ions. 
A) electron pair donor. 
B) proton acceptor. 
C) substance that dissociates in water to produce aqueous hydrogen ions. 
D) substance that dissociates in water to produce aqueous hydroxide ions.

Question 9

Calculate the pH of a 0.800 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

Accepted Answer

A) 2.70 
B) 4.40 
C) 9.60 
D) 11.30 
A) 2.70 
B) 4.40 
C) 9.60 
D) 11.30

Question 10

A solution with a hydrogen ion concentration of 3.25 × 10-5 M is ________ and has a hydroxide ion concentration of ________.

Accepted Answer

A) acidic,3.08 × 10-9 M 
B) acidic,3.08 × 10-10 M 
C) basic,3.08 × 10-9 M 
D) basic,3.08 × 10-10 M 
A) acidic,3.08 × 10-9 M 
B) acidic,3.08 × 10-10 M 
C) basic,3.08 × 10-9 M 
D) basic,3.08 × 10-10 M

Question 11

Write a balanced equation for the dissociation of the Br∅nsted-Lowry acid HSO4- in water.

Accepted Answer

A) HSO4-(aq)+ H2O(l)⇌ H2SO4(aq)+ OH-(aq) 
B) HSO4-(aq)+ H2O(l)⇌ SO42-(aq)+ H3O+(aq) 
C) HSO4-(aq)+ H2O(l)⇌ SO32-(aq)+ OH-(aq) 
D) HSO4-(aq)+ H2O(l)⇌ SO3(g)+ OH-(aq)+ H2O(l) 
A) HSO4-(aq)+ H2O(l)⇌ H2SO4(aq)+ OH-(aq) 
B) HSO4-(aq)+ H2O(l)⇌ SO42-(aq)+ H3O+(aq) 
C) HSO4-(aq)+ H2O(l)⇌ SO32-(aq)+ OH-(aq) 
D) HSO4-(aq)+ H2O(l)⇌ SO3(g)+ OH-(aq)+ H2O(l)

Question 12

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A) KHSO4 
B) RbClO4 
C) BaO 
D) CH3CH3NH3Br 
A) KHSO4 
B) RbClO4 
C) BaO 
D) CH3CH3NH3Br

Question 13

In the following chemical equation indicate the reactant that is a Br∅nsted-Lowry base. HCN(aq)+ H2O(l)⇌ H3O+(aq)+ CN-(aq)

Accepted Answer

A) HCN 
B) H2O 
C) H3O+ 
D) CN- 
A) HCN 
B) H2O 
C) H3O+ 
D) CN-

Question 14

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A) NaI 
B) KBr 
C) RbCl 
D) CsF 
A) NaI 
B) KBr 
C) RbCl 
D) CsF

Question 15

What is the hydronium ion concentration of a 0.300 M acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq)+ H2O(l)⇌ H3O+(aq)+ CH3CO2-(aq).

Accepted Answer

A) 2.3 × 10-2 M 
B) 4.2 × 10-2 M 
C) 2.3 × 10-3 M 
D) 4.2 × 10-3 M 
A) 2.3 × 10-2 M 
B) 4.2 × 10-2 M 
C) 2.3 × 10-3 M 
D) 4.2 × 10-3 M

Question 16

The Br∅nsted-Lowry acids in the chemical equation below are ________ and ________.
HNO2(aq)+ H2O(l)⇌ H3O+(aq)+ NO2-(aq)

Accepted Answer

Question 17

Ammonia NH3,has a base dissociation constant of 1.8 × 10-5.What is the conjugate acid of ammonia and what is its acid dissociation constant?

Accepted Answer

A) NH4+,1.9 × 109 
B) NH4+,1.8 × 10-5 
C) NH4+,5.6 × 10-10 
D) NH2-,5.6 × 10-10 
A) NH4+,1.9 × 109 
B) NH4+,1.8 × 10-5 
C) NH4+,5.6 × 10-10 
D) NH2-,5.6 × 10-10

Question 18

Which one of the following can behave either as a Br∅nsted-Lowry acid or a Br∅nsted-Lowry base in an aqueous solution reaction?

Accepted Answer

A) HSO4- 
B) CH4 
C) HI 
D) H3PO4 
A) HSO4- 
B) CH4 
C) HI 
D) H3PO4

Question 19

What is the pH of a solution prepared by diluting 50.00 mL of 0.020 M Ba(OH)2 with enough water to produce a total volume of 250.00 mL?

Accepted Answer

A) 2.10 
B) 2.40 
C) 11.60 
D) 11.90 
A) 2.10 
B) 2.40 
C) 11.60 
D) 11.90

Question 20

Identify the Lewis acid that acts as a reactant in the following reaction. Fe(H2O)63+(aq)+ 6 CN-(aq)→ Fe(CN)63-(aq)+ 6 H2O(l)

Accepted Answer

A) Fe3+ 
B) H2O 
C) CN- 
D) Fe(H2O)63+ 
A) Fe3+ 
B) H2O 
C) CN- 
D) Fe(H2O)63+

Exam 15: Aqueous Equilibria: Acids and Bases

What is the strongest monoprotic acid of the following set if all the acids are at 0.100 M concentration?

Phenobarbital has a pKa = 7.4.Compared to a 1.0 × 10-3 M solution,1.0 × 10-4 M phenobarbital will have a ________ (higher,lower)pH and a ________ (higher,lower)percent ionization.

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-4 M in hydroxide ion.

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

What is the conjugate base of the Br∅nsted-Lowry acid HPO42-?

When dissolved in water,which of the following compounds is an Arrhenius acid?

A proton hydrated by ten water molecules has the formula ________.

An Arrhenius acid is best defined as a

Calculate the pH of a 0.800 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

A solution with a hydrogen ion concentration of 3.25 × 10-5 M is ________ and has a hydroxide ion concentration of ________.

Write a balanced equation for the dissociation of the Br∅nsted-Lowry acid HSO4- in water.

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

In the following chemical equation indicate the reactant that is a Br∅nsted-Lowry base. HCN(aq)+ H2O(l)⇌ H3O+(aq)+ CN-(aq)

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

What is the hydronium ion concentration of a 0.300 M acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq)+ H2O(l)⇌ H3O+(aq)+ CH3CO2-(aq).

The Br∅nsted-Lowry acids in the chemical equation below are ________ and ________. HNO2(aq)+ H2O(l)⇌ H3O+(aq)+ NO2-(aq)

Ammonia NH3,has a base dissociation constant of 1.8 × 10-5.What is the conjugate acid of ammonia and what is its acid dissociation constant?

Which one of the following can behave either as a Br∅nsted-Lowry acid or a Br∅nsted-Lowry base in an aqueous solution reaction?

What is the pH of a solution prepared by diluting 50.00 mL of 0.020 M Ba(OH)2 with enough water to produce a total volume of 250.00 mL?

Identify the Lewis acid that acts as a reactant in the following reaction. Fe(H2O)63+(aq)+ 6 CN-(aq)→ Fe(CN)63-(aq)+ 6 H2O(l)

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Phenobarbital has a pK_a = 7.4.Compared to a 1.0 × 10^-3 M solution,1.0 × 10^-4 M phenobarbital will have a (higher,lower)pH and a (higher,lower)percent ionization.

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10^-4 M in hydroxide ion.

What is the conjugate base of the Br∅nsted-Lowry acid HPO₄^2-?

Calculate the pH of a 0.800 M KBrO solution.K_a for hypobromous acid,HBrO,is 2.0 × 10^-9.

A solution with a hydrogen ion concentration of 3.25 × 10^-5 M is and has a hydroxide ion concentration of .

Write a balanced equation for the dissociation of the Br∅nsted-Lowry acid HSO₄^- in water.

In the following chemical equation indicate the reactant that is a Br∅nsted-Lowry base. HCN(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ CN^-(aq)

What is the hydronium ion concentration of a 0.300 M acetic acid solution with K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is: CH₃CO₂H(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ CH₃CO₂^-(aq).

The Br∅nsted-Lowry acids in the chemical equation below are and . HNO₂(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ NO₂^-(aq)

Ammonia NH₃,has a base dissociation constant of 1.8 × 10^-5.What is the conjugate acid of ammonia and what is its acid dissociation constant?

What is the pH of a solution prepared by diluting 50.00 mL of 0.020 M Ba(OH)₂ with enough water to produce a total volume of 250.00 mL?

Identify the Lewis acid that acts as a reactant in the following reaction. Fe(H₂O)₆³⁺(aq)+ 6 CN^-(aq)→ Fe(CN)₆^3-(aq)+ 6 H₂O(l)