Question 1

What concentration of potassium hydroxide will result from the reaction of 0.170 g of potassium with 100.mL of water?

Accepted Answer

4.35 * 10^-2 M

Question 2

Identify the conjugate acid of HCO3- in the reaction HCO3- + HPO42-   H2CO3 + PO43-

Accepted Answer

A) H2O 
B) HCO3- 
C) H2CO3 
D) PO43- 
E) HPO42- 
A) H2O 
B) HCO3- 
C) H2CO3 
D) PO43- 
E) HPO42- C

Question 3

What is the H+ ion concentration in a 4.8 * 10-2 M KOH solution?

Accepted Answer

A) 4.8 * 10-2 M 
B) 1.0 * 10-7 M 
C) 4.8 * 10-11 M 
D) 4.8 * 10-12 M 
E) 2.1 * 10-13 M 
A) 4.8 * 10-2 M 
B) 1.0 * 10-7 M 
C) 4.8 * 10-11 M 
D) 4.8 * 10-12 M 
E) 2.1 * 10-13 M E

Question 4

Acid strength decreases in the series: HCl > HSO4- > HCN. Which of these species is the strongest base?

Accepted Answer

A) CN- 
B) SO42- 
C) HCN 
D) Cl- 
A) CN- 
B) SO42- 
C) HCN 
D) Cl-

Question 5

Calculate the concentration of chromate ion (CrO42-)in a 0.450 M solution of chromic acid (H2CrO4).[For chromic acid, Ka1 = 0.18, Ka2 = 3.2 * 10-7.]

Accepted Answer

A) 3.2 * 10-7 M 
B) 1.5 * 10-6 M 
C) 0.081 M 
D) 1.1 * 10-6 M 
E) 0.21 M 
A) 3.2 * 10-7 M 
B) 1.5 * 10-6 M 
C) 0.081 M 
D) 1.1 * 10-6 M 
E) 0.21 M

Question 6

The pH of a Ba(OH)2 solution is 10.00. What is the H+ ion concentration of this solution?

Accepted Answer

A) 4.0 * 10-11 M 
B) 1.6 * 10-10 M 
C) 1.3 * 10-5 M 
D) 1.0 * 10-10 M 
E) 10.M 
A) 4.0 * 10-11 M 
B) 1.6 * 10-10 M 
C) 1.3 * 10-5 M 
D) 1.0 * 10-10 M 
E) 10.M

Question 7

The pH of a 0.6 M solution of a weak acid is 4.0.What percent of the acid has ionized?

Accepted Answer

The answer of The pH of a 0.6 M solution...

Question 8

Predict the direction in which the equilibrium will lie for the reaction H3PO4 + NO3-   H2PO4- + HNO3 Ka(H3PO4)= 7.5 * 10-3

Accepted Answer

A) to the right 
B) to the left 
C) in the middle 
A) to the right 
B) to the left 
C) in the middle

Question 9

Arrange the acids HOBr, HBrO3, and HBrO2 in order of increasing acid strength.

Accepted Answer

A) HOBr 3 2 
B) HOBr 2 3 
C) HBrO2 3 
D) HBrO3 2 
E) HBrO3 2 < HOBr 
A) HOBr 3 2 
B) HOBr 2 3 
C) HBrO2 3 
D) HBrO3 2 
E) HBrO3 2 < HOBr

Question 10

Write the chemical formula for perchloric acid.

Accepted Answer

The answer of Write the chemical formula for perchloric acid....

Question 11

When comparing acid strength of binary acids HX, as X varies within a particular group of the periodic table, which one of these factors dominates in affecting the acid strength?

Accepted Answer

A) bond strength 
B) electron withdrawing effects 
C) percent ionic character of the H-X bond 
D) solubility 
E) Le Châtelier's principle 
A) bond strength 
B) electron withdrawing effects 
C) percent ionic character of the H-X bond 
D) solubility 
E) Le Châtelier's principle

Question 12

The equilibrium constant for the reaction C7H15COOH(aq)+ HCOO-(aq)   C7H15COO-(aq)+ HCOOH(aq)
Is 7.23 * 10-2 at 25°C. If Ka for formic acid (HCOOH)is 1.77 * 10-4, what is the acid dissociation constant for C7H15COOH?

Accepted Answer

A) 2.45 * 10-3 
B) 4.08 * 10-2 
C) 7.81 * 10-4 
D) 1.00 * 10-4 
E) 1.28 * 10-5 
A) 2.45 * 10-3 
B) 4.08 * 10-2 
C) 7.81 * 10-4 
D) 1.00 * 10-4 
E) 1.28 * 10-5

Question 13

In the reaction HNO3 + NH3   NH4+ + NO3-, NH4+ and NH3 are a conjugate acid-base pair.

Accepted Answer

A) True 
 B)False

Question 14

Predict the direction in which the equilibrium will lie for the reaction H3PO4(aq)+ HSO4-(aq)    H2PO4-(aq) + H2SO4(aq).
Ka1(H3PO4)= 7.5 * 10-3; Ka(H2SO4)= very large

Accepted Answer

A) to the right 
B) to the left 
C) in the middle 
A) to the right 
B) to the left 
C) in the middle

Question 15

An unknown substance was added to a solution and the pH decreases. What type of substance was added?

Accepted Answer

The answer of An unknown substance was added to a...

Question 16

The OH- concentration in a 2.5 * 10-3 M Ba(OH)2 solution is

Accepted Answer

A) 4.0 * 10-12 M. 
B) 2.5 * 10-3 M. 
C) 5.0 * 10-3 M. 
D) 1.2 * 10-2 M. 
E) 0.025 M. 
A) 4.0 * 10-12 M. 
B) 2.5 * 10-3 M. 
C) 5.0 * 10-3 M. 
D) 1.2 * 10-2 M. 
E) 0.025 M.

Question 17

Calculate the concentration of malonate ion (C3H2O42-)in a 0.200 M solution of malonic acid (C3H4O4).[For malonic acid, Ka1 = 1.4 * 10-3, Ka2 = 2.0 * 10-6.]

Accepted Answer

A) 2.8 * 10-4 M 
B) 0.016 M 
C) 1.8 * 10-4 M 
D) 1.4 * 10-3 M 
E) 2.0 * 10-6 M 
A) 2.8 * 10-4 M 
B) 0.016 M 
C) 1.8 * 10-4 M 
D) 1.4 * 10-3 M 
E) 2.0 * 10-6 M

Question 18

If the pH of seawater is 8.0, what is the hydroxide ion concentration in seawater?

Accepted Answer

1 * 10<sup

Question 19

Which one of these equations represents the reaction of a weak acid with a weak base?

Accepted Answer

A) H+(aq)+ OH-(aq)$\rarr$H2O(aq) 
B) H+(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq) 
C) OH-(aq)+ HCN(aq)$\rarr$H2O(aq)+ CN-(aq) 
D) HCN(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq)+ CN-(aq) 
A) H+(aq)+ OH-(aq)$\rarr$H2O(aq) 
B) H+(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq) 
C) OH-(aq)+ HCN(aq)$\rarr$H2O(aq)+ CN-(aq) 
D) HCN(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq)+ CN-(aq)

Question 20

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

Exam 15: Acids and Bases

What concentration of potassium hydroxide will result from the reaction of 0.170 g of potassium with 100.mL of water?

Identify the conjugate acid of HCO3- in the reaction HCO3- + HPO42- H2CO3 + PO43-

What is the H+ ion concentration in a 4.8 * 10-2 M KOH solution?

Acid strength decreases in the series: HCl > HSO4- > HCN. Which of these species is the strongest base?

Calculate the concentration of chromate ion (CrO42-)in a 0.450 M solution of chromic acid (H2CrO4).[For chromic acid, Ka1 = 0.18, Ka2 = 3.2 * 10-7.]

The pH of a Ba(OH)2 solution is 10.00. What is the H+ ion concentration of this solution?

The pH of a 0.6 M solution of a weak acid is 4.0.What percent of the acid has ionized?

Predict the direction in which the equilibrium will lie for the reaction H3PO4 + NO3- H2PO4- + HNO3 Ka(H3PO4)= 7.5 * 10-3

Arrange the acids HOBr, HBrO3, and HBrO2 in order of increasing acid strength.

Write the chemical formula for perchloric acid.

When comparing acid strength of binary acids HX, as X varies within a particular group of the periodic table, which one of these factors dominates in affecting the acid strength?

The equilibrium constant for the reaction C7H15COOH(aq)+ HCOO-(aq) C7H15COO-(aq)+ HCOOH(aq) Is 7.23 * 10-2 at 25°C. If Ka for formic acid (HCOOH)is 1.77 * 10-4, what is the acid dissociation constant for C7H15COOH?

In the reaction HNO3 + NH3 NH4+ + NO3-, NH4+ and NH3 are a conjugate acid-base pair.

Predict the direction in which the equilibrium will lie for the reaction H3PO4(aq)+ HSO4-(aq) H2PO4-(aq) + H2SO4(aq). Ka1(H3PO4)= 7.5 * 10-3; Ka(H2SO4)= very large

An unknown substance was added to a solution and the pH decreases. What type of substance was added?

The OH- concentration in a 2.5 * 10-3 M Ba(OH)2 solution is

Calculate the concentration of malonate ion (C3H2O42-)in a 0.200 M solution of malonic acid (C3H4O4).[For malonic acid, Ka1 = 1.4 * 10-3, Ka2 = 2.0 * 10-6.]

If the pH of seawater is 8.0, what is the hydroxide ion concentration in seawater?

Which one of these equations represents the reaction of a weak acid with a weak base?

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

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Identify the conjugate acid of HCO₃^- in the reaction HCO₃^- + HPO₄^2- H₂CO₃ + PO₄^3-

What is the H⁺ ion concentration in a 4.8 * 10^-2 M KOH solution?

Acid strength decreases in the series: HCl > HSO₄^- > HCN. Which of these species is the strongest base?

Calculate the concentration of chromate ion (CrO₄^2-)in a 0.450 M solution of chromic acid (H₂CrO₄).[For chromic acid, K_a1 = 0.18, K_a2 = 3.2 * 10^-7.]

The pH of a Ba(OH)₂ solution is 10.00. What is the H⁺ ion concentration of this solution?

Predict the direction in which the equilibrium will lie for the reaction H₃PO₄ + NO₃^- H₂PO₄^- + HNO₃ K_a(H₃PO₄)= 7.5 * 10^-3

Arrange the acids HOBr, HBrO₃, and HBrO₂ in order of increasing acid strength.

The equilibrium constant for the reaction C₇H₁₅COOH(aq)+ HCOO^-(aq) C₇H₁₅COO^-(aq)+ HCOOH(aq) Is 7.23 * 10^-2 at 25°C. If K_a for formic acid (HCOOH)is 1.77 * 10^-4, what is the acid dissociation constant for C₇H₁₅COOH?

In the reaction HNO₃ + NH₃ NH₄⁺ + NO₃^-, NH₄⁺ and NH₃ are a conjugate acid-base pair.

Predict the direction in which the equilibrium will lie for the reaction H₃PO₄(aq)+ HSO₄^-(aq) H₂PO₄^-(aq)+ H₂SO₄(aq). K_a1(H₃PO₄)= 7.5 * 10^-3; K_a(H₂SO₄)= very large

The OH^- concentration in a 2.5 * 10^-3 M Ba(OH)₂ solution is

Calculate the concentration of malonate ion (C₃H₂O₄^2-)in a 0.200 M solution of malonic acid (C₃H₄O₄).[For malonic acid, K_a1 = 1.4 * 10^-3, K_a2 = 2.0 * 10^-6.]

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