Question 1

Calculate the hydrogen ion concentration in a solution having a pH of 4.60.

Accepted Answer

A) 4.0 × 10-3 M 
B) 4.0 × 10-9 M 
C) 4.0 × 10-10 M 
D) 2.5 × 10-5 M 
E) 2.5 × 10-4 M 
A) 4.0 × 10-3 M 
B) 4.0 × 10-9 M 
C) 4.0 × 10-10 M 
D) 2.5 × 10-5 M 
E) 2.5 × 10-4 M

Question 2

The oxides CO2 and SO3 will form the following acids in water, respectively.

Accepted Answer

A) H2CO3(aq)and H2SO3(aq) 
B) H2CO3(aq)and H2SO4(aq) 
C) H2CO2(aq)and H2SO3(aq) 
D) H2CO2(aq)and H2SO4(aq) 
E) HCOO-(aq)and H2SO3(aq) 
A) H2CO3(aq)and H2SO3(aq) 
B) H2CO3(aq)and H2SO4(aq) 
C) H2CO2(aq)and H2SO3(aq) 
D) H2CO2(aq)and H2SO4(aq) 
E) HCOO-(aq)and H2SO3(aq)

Question 3

For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13.An aqueous solution of Na3PO4 therefore would be

Accepted Answer

A) neutral 
B) basic 
C) acidic 
A) neutral 
B) basic 
C) acidic

Question 4

What is the pH of a 0.15 M solution of the weak base aniline (C6H5NH2; Kb = 3.8 x 10-10)

Accepted Answer

A) 5.12 
B) 8.88 
C) 13.18 
D) 9.42 
E) 10.24 
A) 5.12 
B) 8.88 
C) 13.18 
D) 9.42 
E) 10.24

Question 5

The equilibrium expression for the ionization of a weak monoprotic acid, HA, in water is:

Accepted Answer

A) Ka = [HA]/[OH-][H3O+] 
B) Ka = [OH-][H3O+]/[HA] 
C) Ka = [H3O+][HA]/[A-] 
D) Ka = [H3O+][A-]/[HA] 
E) Ka = [HA]/[H3O+][A-] 
A) Ka = [HA]/[OH-][H3O+] 
B) Ka = [OH-][H3O+]/[HA] 
C) Ka = [H3O+][HA]/[A-] 
D) Ka = [H3O+][A-]/[HA] 
E) Ka = [HA]/[H3O+][A-]

Question 6

Write the formula for the conjugate acid of H2PO4-.

Accepted Answer

Question 7

Calculate the pH of a 3.5 × 10-3 M HNO3 solution.

Accepted Answer

A) -2.46 
B) 0.54 
C) 2.46 
D) 3.00 
E) 3.46 
A) -2.46 
B) 0.54 
C) 2.46 
D) 3.00 
E) 3.46

Question 8

Calculate the pH of a 0.20 M solution of NH4NO3 (Kb(NH3)= 1.8 x 10-5)

Accepted Answer

A) 0.69 
B) 4.74 
C) 2.72 
D) 4.98 
E) 9.02 
A) 0.69 
B) 4.74 
C) 2.72 
D) 4.98 
E) 9.02

Question 9

What is the pH of a 0.023 M solution of HCN (Ka = 4.9 x 10-10)?

Accepted Answer

A) 1.64 
B) 10.95 
C) 3.05 
D) 5.47 
E) 4.97 
A) 1.64 
B) 10.95 
C) 3.05 
D) 5.47 
E) 4.97

Question 10

Lime is used in farming to reduce the acidity of the soil.The chemical name for lime is calcium oxide.When water in the soil reacts with lime, what base is formed?

Accepted Answer

The answer of Lime is used in farming to reduce...

Question 11

Hydrosulfuric acid is a diprotic acid, for which Ka1 = 5.7 × 10-8 and Ka2 = 1 × 10-19.Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Accepted Answer

A) 0.10 M 
B) 7.5 × 10-5 M 
C) 5.7 × 10-9 M 
D) 1 × 10-19 M 
E) 1 × 10-20 M 
A) 0.10 M 
B) 7.5 × 10-5 M 
C) 5.7 × 10-9 M 
D) 1 × 10-19 M 
E) 1 × 10-20 M

Question 12

The hydrolysis of NH4NO2 will result in which of the following types of solutions given: (Ka(NH4+)= 5.6 x 10-10, Kb(NO2-)= 2.2 x 10-11)

Accepted Answer

A) acidic, pH  7 
C) neutral, pH = 7 
A) acidic, pH  7 
C) neutral, pH = 7

Question 13

What mass of sodium cyanide must be added to 250.mL of water in order to obtain a solution having a pH of 10.50? [Ka(HCN)= 4.9 × 10-10]

Accepted Answer

A) 240 g 
B) 0.032 g 
C) 0.059 g 
D) 0.94 g 
E) 0.24 g 
A) 240 g 
B) 0.032 g 
C) 0.059 g 
D) 0.94 g 
E) 0.24 g

Question 14

Calculate the hydrogen ion concentration in a solution of fruit juice having a pH of 4.25.

Accepted Answer

A) 1.0 × 10-14 M 
B) 5.6 × 10-5 M 
C) 4.0 × 10-25 M 
D) 2.5 × 10-4 M 
E) 5.6 × 10-4 M 
A) 1.0 × 10-14 M 
B) 5.6 × 10-5 M 
C) 4.0 × 10-25 M 
D) 2.5 × 10-4 M 
E) 5.6 × 10-4 M

Question 15

Calculate the pH of a 0.055 M solution of CH3COONa (Ka(CH3COOH)= 1.8 x 10-5)

Accepted Answer

A) 12.74 
B) 4.74 
C) 8.74 
D) 9.26 
E) 5.26 
A) 12.74 
B) 4.74 
C) 8.74 
D) 9.26 
E) 5.26

Question 16

A 1.5 L sample of a 0.44 M HBr solution is mixed with 2.2 L of a 0.080 M HClO4 solution.What is the pH of the mixture?

Accepted Answer

A) 0.28 
B) 0.36 
C) 1.45 
D) 0.73 
E) 0.65 
A) 0.28 
B) 0.36 
C) 1.45 
D) 0.73 
E) 0.65

Question 17

For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13.An aqueous solution of NaH2PO4 therefore would be

Accepted Answer

A) neutral 
B) basic 
C) acidic 
A) neutral 
B) basic 
C) acidic

Question 18

What mass of sodium nitrite must be added to 350.mL of water to give a solution with pH = 8.40? [Ka(HNO2)= 5.6 × 10-4]

Accepted Answer

A) 68 g 
B) 1.7 × 10-4 g 
C) 0.039 g 
D) 8.3 g 
E) 24 g 
A) 68 g 
B) 1.7 × 10-4 g 
C) 0.039 g 
D) 8.3 g 
E) 24 g

Question 19

In the reaction Ag+(aq)+ Cl-(aq) $\rarr$ AgCl(s), Ag+ acts as a Lewis acid.

Accepted Answer

A) True 
 B)False

Question 20

The equilibrium expression for the hydrolysis of a weak base, A-, in water is:

Accepted Answer

A) Kb = [A-]/[OH-][H3O+] 
B) Kb = [OH-][H3O+]/[A-] 
C) Kb = [OH-][HA]/[A-] 
D) Kb = [OH-][A-]/[HA] 
E) Kb = [OH-][HA]/[A-][H3O+] 
A) Kb = [A-]/[OH-][H3O+] 
B) Kb = [OH-][H3O+]/[A-] 
C) Kb = [OH-][HA]/[A-] 
D) Kb = [OH-][A-]/[HA] 
E) Kb = [OH-][HA]/[A-][H3O+]

Exam 15: Acids and Bases

Calculate the hydrogen ion concentration in a solution having a pH of 4.60.

The oxides CO2 and SO3 will form the following acids in water, respectively.

For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13.An aqueous solution of Na3PO4 therefore would be

What is the pH of a 0.15 M solution of the weak base aniline (C6H5NH2; Kb = 3.8 x 10-10)

The equilibrium expression for the ionization of a weak monoprotic acid, HA, in water is:

Write the formula for the conjugate acid of H2PO4-.

Calculate the pH of a 3.5 × 10-3 M HNO3 solution.

Calculate the pH of a 0.20 M solution of NH4NO3 (Kb(NH3)= 1.8 x 10-5)

What is the pH of a 0.023 M solution of HCN (Ka = 4.9 x 10-10)?

Lime is used in farming to reduce the acidity of the soil.The chemical name for lime is calcium oxide.When water in the soil reacts with lime, what base is formed?

Hydrosulfuric acid is a diprotic acid, for which Ka1 = 5.7 × 10-8 and Ka2 = 1 × 10-19.Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

The hydrolysis of NH4NO2 will result in which of the following types of solutions given: (Ka(NH4+)= 5.6 x 10-10, Kb(NO2-)= 2.2 x 10-11)

What mass of sodium cyanide must be added to 250.mL of water in order to obtain a solution having a pH of 10.50? [Ka(HCN)= 4.9 × 10-10]

Calculate the hydrogen ion concentration in a solution of fruit juice having a pH of 4.25.

Calculate the pH of a 0.055 M solution of CH3COONa (Ka(CH3COOH)= 1.8 x 10-5)

A 1.5 L sample of a 0.44 M HBr solution is mixed with 2.2 L of a 0.080 M HClO4 solution.What is the pH of the mixture?

For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13.An aqueous solution of NaH2PO4 therefore would be

What mass of sodium nitrite must be added to 350.mL of water to give a solution with pH = 8.40? [Ka(HNO2)= 5.6 × 10-4]

In the reaction Ag+(aq)+ Cl-(aq) →\rarr→ AgCl(s), Ag+ acts as a Lewis acid.

The equilibrium expression for the hydrolysis of a weak base, A-, in water is:

Chemistry: the Study of Change

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Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

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Filters

The oxides CO₂ and SO₃ will form the following acids in water, respectively.

For H₃PO₄, K_a1 = 7.3 × 10^-3, K_a2 = 6.2 × 10^-6, and K_a3 = 4.8 × 10^-13.An aqueous solution of Na₃PO₄ therefore would be

What is the pH of a 0.15 M solution of the weak base aniline (C₆H₅NH₂; K_b = 3.8 x 10^-10)

Write the formula for the conjugate acid of H₂PO₄^-.

Calculate the pH of a 3.5 × 10^-3 M HNO₃ solution.

Calculate the pH of a 0.20 M solution of NH₄NO₃(K_b(NH₃)= 1.8 x 10^-5)

What is the pH of a 0.023 M solution of HCN (K_a = 4.9 x 10^-10)?

Hydrosulfuric acid is a diprotic acid, for which K_a1 = 5.7 × 10^-8 andK_a2 = 1 × 10^-19.Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

The hydrolysis of NH₄NO₂ will result in which of the following types of solutions given: (K_a(NH₄⁺)= 5.6 x 10^-10, K_b(NO₂^-)= 2.2 x 10^-11)

What mass of sodium cyanide must be added to 250.mL of water in order to obtain a solution having a pH of 10.50? [K_a(HCN)= 4.9 × 10^-10]

Calculate the pH of a 0.055 M solution of CH₃COONa (K_a(CH₃COOH)= 1.8 x 10^-5)

A 1.5 L sample of a 0.44 M HBr solution is mixed with 2.2 L of a 0.080 M HClO₄ solution.What is the pH of the mixture?

For H₃PO₄, K_a1 = 7.3 × 10^-3, K_a2 = 6.2 × 10^-6, and K_a3 = 4.8 × 10^-13.An aqueous solution of NaH₂PO₄ therefore would be

What mass of sodium nitrite must be added to 350.mL of water to give a solution with pH = 8.40? [K_a(HNO₂)= 5.6 × 10^-4]

In the reaction Ag⁺(aq)+ Cl^-(aq) $\rarr$ AgCl(s), Ag⁺ acts as a Lewis acid.

The equilibrium expression for the hydrolysis of a weak base, A^-, in water is: