Question 1

The number of waters of hydration in the hydrate proton H7O3+ is ________.

Accepted Answer

Question 2

From the following chemical reactions determine the relative Br∅nsted-Lowry acid strengths (strongest to weakest).
HClO4(sol)+ CH3COOH(l)→ CH3C2(OH)2+(sol)+ ClO4-(aq)
H2SO4(sol)+ CH3COOH(l)⇌ CH3C(OH)2+(sol)+ HSO4-(sol)

Accepted Answer

A) HClO4 > H2SO4 > CH3COOH 
B) HClO4 > H2SO4 > CH3C(OH)2+ 
C) HClO4 > CH3COOH > H2SO4 
D) HClO4 > CH3C(OH)2+ > H2SO4 
A) HClO4 > H2SO4 > CH3COOH 
B) HClO4 > H2SO4 > CH3C(OH)2+ 
C) HClO4 > CH3COOH > H2SO4 
D) HClO4 > CH3C(OH)2+ > H2SO4

Question 3

Calculate the pH of a of 0.100 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

Accepted Answer

A) 3)15 
B) 4)85 
C) 9)15 
D) 10.85 
A) 3)15 
B) 4)85 
C) 9)15 
D) 10.85

Question 4

What statement is most consistent for an acid with a pH = 3?

Accepted Answer

A) one one-hundredth as strong as an acid with a pH of 5 
B) half a strong as an acid with a pH = 5 
C) twice as strong as an acid with a pH of 5 
D) one hundred times as strong as an acid with a pH = 5 
A) one one-hundredth as strong as an acid with a pH of 5 
B) half a strong as an acid with a pH = 5 
C) twice as strong as an acid with a pH of 5 
D) one hundred times as strong as an acid with a pH = 5

Question 5

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 6

What is the pH of a 0.020 M HClO4 solution?

Accepted Answer

A) 0)020 
B) 0)040 
C) 1)70 
D) 12.30 
A) 0)020 
B) 0)040 
C) 1)70 
D) 12.30

Question 7

Which one of the following is expected to be the strongest Lewis acid?

Accepted Answer

A) Fe 
B) Fe+ 
C) Fe2+ 
D) Fe3+ 
A) Fe 
B) Fe+ 
C) Fe2+ 
D) Fe3+

Question 8

The following pictures represent aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity.  
-Which acid has the smallest value of Ka?

Accepted Answer

A) HX 
B) HY 
C) HZ 
D) All have the same Ka value. 
A) HX 
B) HY 
C) HZ 
D) All have the same Ka value.

Question 9

A Br∅nsted-Lowry acid is best defined as a substance that can

Accepted Answer

A) accept a hydroxide ion. 
B) donate a hydroxide ion. 
C) accept a proton. 
D) donate a proton. 
A) accept a hydroxide ion. 
B) donate a hydroxide ion. 
C) accept a proton. 
D) donate a proton.

Question 10

What is the equilibrium constant expression (Ka)for the acid dissociation of nitrous acid HNO2? The equation of interest is
HNO2(aq)+ H2O(l)⇌ H3O+(aq)+ NO2-(aq).

Accepted Answer

A) Ka = ([H3O+][NO2-])/([HNO2][H2O]) 
B) Ka = ([H3O+][NO2-])/([HNO2]) 
C) Ka = ([HNO2][H2O])/([H3O+][NO2-]) 
D) Ka = ([HNO2])/([H3O+][NO2-]) 
A) Ka = ([H3O+][NO2-])/([HNO2][H2O]) 
B) Ka = ([H3O+][NO2-])/([HNO2]) 
C) Ka = ([HNO2][H2O])/([H3O+][NO2-]) 
D) Ka = ([HNO2])/([H3O+][NO2-])

Question 11

Vinegar is a 5.0% solution by weight of acetic acid (CH3CO2H)in water.Given that
Ka = 1.8 × 10-5 for acetic acid and assuming the density of vinegar to be 1.00 g/cm3,what is the pH of this vinegar solution?

Accepted Answer

A) 2)00 
B) 2)41 
C) 2)87 
D) 4)74 
A) 2)00 
B) 2)41 
C) 2)87 
D) 4)74

Question 12

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest).
HNO3(aq)+ H2O(l)→ H3O+(aq)+ NO3-(aq)
HF(aq)+ H2O(l)⇌ H3O+(aq)+ F-(aq)

Accepted Answer

A) HNO3 > H3O+ > HF 
B) NO3- > H2O > F- 
C) F- > H2O > NO3- 
D) F- > NO3- > H2O 
A) HNO3 > H3O+ > HF 
B) NO3- > H2O > F- 
C) F- > H2O > NO3- 
D) F- > NO3- > H2O

Question 13

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 14

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest).
2 NaH(s)+ H2O(l)→ 2 NaOH + H2(g)
NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq)

Accepted Answer

A) H- > OH- > NH3 
B) H- > NH3 > OH- 
C) OH-> H- > NH3 
D) OH- > NH3 > H- 
A) H- > OH- > NH3 
B) H- > NH3 > OH- 
C) OH-> H- > NH3 
D) OH- > NH3 > H-

Question 15

If the ionization constant of water,Kw,at 40°C is 2.92 × 10-14,then what is the hydronium ion concentration and pH for an acidic solution?

Accepted Answer

A) [H3O+] > 1.71 × 10-7 M and pH > 6.77 B) [H3O+] > 1.71 × 10-7 M and pH 3O+] -7 M and pH > 6.77 D) [H3O+] -7 M and pH < 6.77 A) [H3O+] > 1.71 × 10-7 M and pH > 6.77 B) [H3O+] > 1.71 × 10-7 M and pH 3O+] -7 M and pH > 6.77 D) [H3O+] -7 M and pH < 6.77

Question 16

What is the pH of a solution prepared by diluting 20.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?

Accepted Answer

A) 1)00 
B) 1)70 
C) 2)00 
D) 3)40 
A) 1)00 
B) 1)70 
C) 2)00 
D) 3)40

Question 17

What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 × 10-4 and Ka2 = 1.0 × 10-11?

Accepted Answer

A) 3)6 × 10-3 M 
B) 1)3 × 10-4 M 
C) 1)3 × 10-5 M 
D) 1)0 × 10-11 M 
A) 3)6 × 10-3 M 
B) 1)3 × 10-4 M 
C) 1)3 × 10-5 M 
D) 1)0 × 10-11 M

Question 18

What is the pH of a 0.200 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is
NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq).

Accepted Answer

A) 2)02 
B) 2)72 
C) 11.98 
D) 11.28 
A) 2)02 
B) 2)72 
C) 11.98 
D) 11.28

Question 19

The pH of a 0.025 M KOH solution is ________.

Accepted Answer

The answer of The pH of a 0.025 M KOH...

Question 20

A 1.25 × 10-4 M solution of the anti-inflammatory drug naproxen has a pH = 4.2.The Ka and pKa of naproxen are ________ and ________.

Accepted Answer

Exam 14: Aqueous Equilibria: Acids and Bases

The number of waters of hydration in the hydrate proton H7O3+ is ________.

From the following chemical reactions determine the relative Br∅nsted-Lowry acid strengths (strongest to weakest). HClO4(sol)+ CH3COOH(l)→ CH3C2(OH)2+(sol)+ ClO4-(aq) H2SO4(sol)+ CH3COOH(l)⇌ CH3C(OH)2+(sol)+ HSO4-(sol)

Calculate the pH of a of 0.100 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

What statement is most consistent for an acid with a pH = 3?

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

What is the pH of a 0.020 M HClO4 solution?

Which one of the following is expected to be the strongest Lewis acid?

The following pictures represent aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity. -Which acid has the smallest value of Ka?

A Br∅nsted-Lowry acid is best defined as a substance that can

What is the equilibrium constant expression (Ka)for the acid dissociation of nitrous acid HNO2? The equation of interest is HNO2(aq)+ H2O(l)⇌ H3O+(aq)+ NO2-(aq).

Vinegar is a 5.0% solution by weight of acetic acid (CH3CO2H)in water.Given that Ka = 1.8 × 10-5 for acetic acid and assuming the density of vinegar to be 1.00 g/cm3,what is the pH of this vinegar solution?

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest). HNO3(aq)+ H2O(l)→ H3O+(aq)+ NO3-(aq) HF(aq)+ H2O(l)⇌ H3O+(aq)+ F-(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?

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest). 2 NaH(s)+ H2O(l)→ 2 NaOH + H2(g) NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq)

If the ionization constant of water,Kw,at 40°C is 2.92 × 10-14,then what is the hydronium ion concentration and pH for an acidic solution?

What is the pH of a solution prepared by diluting 20.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?

What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 × 10-4 and Ka2 = 1.0 × 10-11?

What is the pH of a 0.200 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq).

The pH of a 0.025 M KOH solution is ________.

A 1.25 × 10-4 M solution of the anti-inflammatory drug naproxen has a pH = 4.2.The Ka and pKa of naproxen are ________ and ________.

Chemistry: Matter and Measurement

Atoms, molecules, and Ions

Formulas, equations, and Moles

Reactions in Aqueous Solutions

Periodicity and the Atomic Structure of Atoms

Ionic Bonds and Some Main-Group Chemistry

Covalent Bonds and Molecular Structure

Thermochemistry: Chemical Energy

Gases: Their Properties and Behavior

Liquids,solids,and Phase Changes

Solutions and Their Properties

Chemical Kinetics

Chemical Equilibrium

Applications of Aqueous Equilibria

Thermodynamics: Entropy, free Energy, and Equilibrium

Electrochemistry

Hydrogen, oxygen, and Water

The Main-Group Elements

Transition Elements and Coordination Chemistry

Metals and Solid-State Materials

Nuclear Chemistry

Organic and Biological Chemistry

Filters

The number of waters of hydration in the hydrate proton H₇O₃⁺ is ________.

From the following chemical reactions determine the relative Br∅nsted-Lowry acid strengths (strongest to weakest). HClO₄(sol)+ CH₃COOH(l)→ CH₃C₂(OH)₂⁺(sol)+ ClO₄^-(aq) H₂SO₄(sol)+ CH₃COOH(l)⇌ CH₃C(OH)₂⁺(sol)+ HSO₄^-(sol)

Calculate the pH of a of 0.100 M KBrO solution.K_a for hypobromous acid,HBrO,is 2.0 × 10^-9.

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

What is the pH of a 0.020 M HClO₄ solution?

The following pictures represent aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity. -Which acid has the smallest value of K_a?

What is the equilibrium constant expression (K_a)for the acid dissociation of nitrous acid HNO₂? The equation of interest is HNO₂(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ NO₂^-(aq).

Vinegar is a 5.0% solution by weight of acetic acid (CH₃CO₂H)in water.Given that K_a = 1.8 × 10^-5for acetic acid and assuming the density of vinegar to be 1.00 g/cm³,what is the pH of this vinegar solution?

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest). HNO₃(aq)+ H₂O(l)→ H₃O⁺(aq)+ NO₃^-(aq) HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ F^-(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?

From the following chemical reactions determine the relative Br∅nsted-Lowry base strengths (strongest to weakest). 2 NaH(s)+ H₂O(l)→ 2 NaOH + H₂(g) NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq)

If the ionization constant of water,K_w,at 40°C is 2.92 × 10^-14,then what is the hydronium ion concentration and pH for an acidic solution?

What is the selenide ion concentration [Se^2-] for a 0.100 M H₂Se solution that has the stepwise dissociation constants of K_a1 = 1.3 × 10^-4 and K_a2 = 1.0 × 10^-11?

What is the pH of a 0.200 M NH₃ solution that has K_b = 1.8 × 10^-5? The equation for the dissociation of NH₃ is NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq).

A 1.25 × 10^-4 M solution of the anti-inflammatory drug naproxen has a pH = 4.2.The K_a and pK_a of naproxen are and .