Question 1

If one solution has an H3O+ concentration that is 10 times less than that of another solution, the difference in pH is 10 units.

Accepted Answer

A) True 
 B)False  False

Question 2

Calculate the pH of a solution that has [OH-] = 1.0 x 10-8 M.

Accepted Answer

A) pH = 1.00 
B) pH = 7.00 
C) pH = 14.00 
D) pH = 8.00 
E) pH = 6.00 
A) pH = 1.00 
B) pH = 7.00 
C) pH = 14.00 
D) pH = 8.00 
E) pH = 6.00 E

Question 3

Select the solution below that is the most basic.

Accepted Answer

A) [OH-] = 1.0 x 10-4 M 
B) [OH-] = 1.0 x 10-5 M 
C) [OH-] = 1.0 x 10-7 M 
D) [OH-] = 1.0 x 10-9 M 
E) [OH-] = 1.0 x 10-11 M 
A) [OH-] = 1.0 x 10-4 M 
B) [OH-] = 1.0 x 10-5 M 
C) [OH-] = 1.0 x 10-7 M 
D) [OH-] = 1.0 x 10-9 M 
E) [OH-] = 1.0 x 10-11 M A

Question 4

The conjugate base of HCO3- is:

Accepted Answer

A) H2CO3  
B) HCO2-  
C) CO32-  
D) CO2  
E) H3CO3+  
A) H2CO3  
B) HCO2-  
C) CO32-  
D) CO2  
E) H3CO3+

Question 5

Calculate the pH of a solution that has [OH-] = 5.9 x 10-5 M.

Accepted Answer

A) pH = 5.90 
B) pH = 5.00 
C) pH = 4.23 
D) pH = 9.77 
E) pH = 5.59 
A) pH = 5.90 
B) pH = 5.00 
C) pH = 4.23 
D) pH = 9.77 
E) pH = 5.59

Question 6

Select the two Brønsted-Lowry acids in the following equation: CO32-(aq) + HF(aq) ⇌ HCO3-(aq) + F-(aq)

Accepted Answer

A) CO32- and HF 
B) CO32- and HCO3-  
C) HF and F-  
D) CO32- and F-  
E) HF and HCO3-  
A) CO32- and HF 
B) CO32- and HCO3-  
C) HF and F-  
D) CO32- and F-  
E) HF and HCO3-

Question 7

Given an OH- concentration of 1.0 x 10-6 M, calculate the H3O+ concentration, and then identify the solution as acidic, basic, or neutral.

Accepted Answer

A) [H3O+] = 1.0 x 10-7, neutral 
B) [H3O+] = 1.0 x 10-6, acidic 
C) [H3O+] = 1.0 x 10-8, acidic 
D) [H3O+] = 1.0 x 10-8, basic 
E) [H3O+] = 1.0 x 10-6, basic 
A) [H3O+] = 1.0 x 10-7, neutral 
B) [H3O+] = 1.0 x 10-6, acidic 
C) [H3O+] = 1.0 x 10-8, acidic 
D) [H3O+] = 1.0 x 10-8, basic 
E) [H3O+] = 1.0 x 10-6, basic

Question 8

Select the pair that consists of an acid and its conjugate base in that order.

Accepted Answer

A) NH4+/NH2-  
B) CO32-/HCO3-  
C) CO32-/H2CO3-  
D) H2PO4-/H3PO4  
E) H2CO3/HCO3-  
A) NH4+/NH2-  
B) CO32-/HCO3-  
C) CO32-/H2CO3-  
D) H2PO4-/H3PO4  
E) H2CO3/HCO3-

Question 9

Rank the following 0.100 M solutions in order of increasing H3O+ concentration: HOCl, Ka = 4.0 x 10-8; HCN, Ka = 6.2 x 10-10; NH4+, Ka = 5.6 x 10-10

Accepted Answer

A) HOCl 4+  
B) HOCl 4+ 4+ 4+  
E) NH4+ < HCN < HOCl 
A) HOCl 4+  
B) HOCl 4+ 4+ 4+  
E) NH4+ < HCN < HOCl

Question 10

Rank the following 0.100 M solutions in order of increasing H3O+ concentration: HF, Ka = 6.3 x 10-4; HCN, Ka = 6.2 x 10-10; HOCl, Ka = 4.0 x 10-8

Accepted Answer

A) HF < HCN < HOCl 
B) HF < HOCl < HCN 
C) HOCl < HF < HCN 
D) HOCl < HCN < HF 
E) HCN < HOCl < HF 
A) HF < HCN < HOCl 
B) HF < HOCl < HCN 
C) HOCl < HF < HCN 
D) HOCl < HCN < HF 
E) HCN < HOCl < HF

Question 11

The substance HCl(aq) is:

Accepted Answer

A) a strong acid. 
B) a weak acid. 
C) a strong base. 
D) a weak base. 
E) neither an acid nor a base. 
A) a strong acid. 
B) a weak acid. 
C) a strong base. 
D) a weak base. 
E) neither an acid nor a base.

Question 12

The conjugate acid of HCO3- is:

Accepted Answer

A) H2CO3  
B) HCO2-  
C) CO32-  
D) CO2  
E) H3CO3+  
A) H2CO3  
B) HCO2-  
C) CO32-  
D) CO2  
E) H3CO3+

Question 13

The H3O+ concentration in a 0.050 M solution of HClO4 is 0.050 M.

Accepted Answer

A) True 
 B)False

Question 14

Select the two Brønsted-Lowry acids in the following equation: HF(aq) + H2O(l) ⇌ F-(aq) + H3O+(aq)

Accepted Answer

A) HF and H2O 
B) HF and F-  
C) H2O and F-  
D) HF and H3O+  
E) H3O+ and F-  
A) HF and H2O 
B) HF and F-  
C) H2O and F-  
D) HF and H3O+  
E) H3O+ and F-

Question 15

Which of the following bases is not commonly found in household products or antacids?

Accepted Answer

A) sodium hydroxide, NaOH 
B) ammonia, NH3  
C) calcium carbonate, CaCO3  
D) magnesium hydroxide, Mg(OH)2  
E) methyl amine, CH3NH2  
A) sodium hydroxide, NaOH 
B) ammonia, NH3  
C) calcium carbonate, CaCO3  
D) magnesium hydroxide, Mg(OH)2  
E) methyl amine, CH3NH2

Question 16

Select the strong acid from the following list.

Accepted Answer

A) HNO3(aq) 
B) HClO3(aq) 
C) HF(aq) 
D) H3PO4(aq) 
E) HCN(aq) 
A) HNO3(aq) 
B) HClO3(aq) 
C) HF(aq) 
D) H3PO4(aq) 
E) HCN(aq)

Question 17

Which of the following equations represents the behavior of H2PO4- as an acid?

Accepted Answer

A) H2PO4-(aq) + H3O+(aq) ⇌ H3PO4(aq) + H2O(l) 
B) H2PO4-(aq) + HF(aq) ⇌ H3PO4(aq) + F-(aq) 
C) H2PO4-(aq) + HCN(aq) ⇌ H3PO4(aq) + CN-(aq) 
D) H2PO4-(aq) + OH-(aq) ⇌ HPO4-(aq) + H2O(l) 
E) H2PO4-(aq) + H2O(l) ⇌ H3PO4(aq) + OH-(aq) 
A) H2PO4-(aq) + H3O+(aq) ⇌ H3PO4(aq) + H2O(l) 
B) H2PO4-(aq) + HF(aq) ⇌ H3PO4(aq) + F-(aq) 
C) H2PO4-(aq) + HCN(aq) ⇌ H3PO4(aq) + CN-(aq) 
D) H2PO4-(aq) + OH-(aq) ⇌ HPO4-(aq) + H2O(l) 
E) H2PO4-(aq) + H2O(l) ⇌ H3PO4(aq) + OH-(aq)

Question 18

Given 0.10 M solutions of the following acids, which contains the highest concentration of H3O+?

Accepted Answer

A) HNO2, Ka = 5.6 x 10-4  
B) HCN, Ka = 6.2 x 10-10  
C) NH4+, Ka = 5.6 x 10-10  
D) CH3CO2H, Ka = 1.8 x 10-5  
E) HCO2H, Ka = 1.8 x 10-4  
A) HNO2, Ka = 5.6 x 10-4  
B) HCN, Ka = 6.2 x 10-10  
C) NH4+, Ka = 5.6 x 10-10  
D) CH3CO2H, Ka = 1.8 x 10-5  
E) HCO2H, Ka = 1.8 x 10-4

Question 19

Select the two Brønsted-Lowry acids in the following equation: HCN(aq) + H2O(l) ⇌ CN-(aq) + H3O+(aq)

Accepted Answer

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

Question 20

Which of the following statements regarding bases is incorrect?

Accepted Answer

A) A base is a substance that may act as an antacid. 
B) A base is a substance that will not change the color of red litmus paper. 
C) A base is a substance that tastes bitter. 
D) A base is a substance that produces hydroxide ions, OH-, in aqueous solution. 
E) A base is a substance that is an electrolyte. 
A) A base is a substance that may act as an antacid. 
B) A base is a substance that will not change the color of red litmus paper. 
C) A base is a substance that tastes bitter. 
D) A base is a substance that produces hydroxide ions, OH-, in aqueous solution. 
E) A base is a substance that is an electrolyte.

If one solution has an H₃O⁺ concentration that is 10 times less than that of another solution, the difference in pH is 10 units.

Calculate the pH of a solution that has [OH^-] = 1.0 x 10^-8M.

Select the solution below that is the most basic.

The conjugate base of HCO₃^- is:

Calculate the pH of a solution that has [OH^-] = 5.9 x 10^-5M.

Select the two Brønsted-Lowry acids in the following equation: CO₃^2-(aq) + HF(aq) ⇌ HCO₃^-(aq) + F^-(aq)

Given an OH^- concentration of 1.0 x 10^-6 M, calculate the H₃O⁺concentration, and then identify the solution as acidic, basic, or neutral.

Select the pair that consists of an acid and its conjugate base in that order.

Rank the following 0.100 M solutions in order of increasing H₃O⁺ concentration: HOCl, K_a = 4.0 x 10^-8; HCN, K_a = 6.2 x 10^-10;NH₄⁺, K_a = 5.6 x 10^-10

Rank the following 0.100 M solutions in order of increasing H₃O⁺ concentration: HF, K_a = 6.3 x 10^-4; HCN, K_a = 6.2 x 10^-10; HOCl, K_a = 4.0 x 10^-8

The substance HCl(aq) is:

The conjugate acid of HCO₃^- is:

The H₃O⁺concentration in a 0.050 M solution of HClO₄is 0.050 M.

Select the two Brønsted-Lowry acids in the following equation: HF(aq) + H₂O(l) ⇌ F^-(aq) + H₃O⁺(aq)

Which of the following bases is not commonly found in household products or antacids?

Select the strong acid from the following list.

Which of the following equations represents the behavior of H₂PO₄^- as an acid?

Given 0.10 M solutions of the following acids, which contains the highest concentration of H₃O⁺?

Select the two Brønsted-Lowry acids in the following equation: HCN(aq) + H₂O(l) ⇌ CN^-(aq) + H₃O⁺(aq)

Which of the following statements regarding bases is incorrect?

Matter and Energy

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Exam 13: Acids and Bases

If one solution has an H3O+ concentration that is 10 times less than that of another solution, the difference in pH is 10 units.

Calculate the pH of a solution that has [OH-] = 1.0 x 10-8 M.

Select the solution below that is the most basic.

The conjugate base of HCO3- is:

Calculate the pH of a solution that has [OH-] = 5.9 x 10-5 M.

Select the two Brønsted-Lowry acids in the following equation: CO32-(aq) + HF(aq) ⇌ HCO3-(aq) + F-(aq)

Given an OH- concentration of 1.0 x 10-6 M, calculate the H3O+ concentration, and then identify the solution as acidic, basic, or neutral.

Select the pair that consists of an acid and its conjugate base in that order.

Rank the following 0.100 M solutions in order of increasing H3O+ concentration: HOCl, Ka = 4.0 x 10-8; HCN, Ka = 6.2 x 10-10; NH4+, Ka = 5.6 x 10-10

Rank the following 0.100 M solutions in order of increasing H3O+ concentration: HF, Ka = 6.3 x 10-4; HCN, Ka = 6.2 x 10-10; HOCl, Ka = 4.0 x 10-8

The substance HCl(aq) is:

The conjugate acid of HCO3- is:

The H3O+ concentration in a 0.050 M solution of HClO4 is 0.050 M.

Select the two Brønsted-Lowry acids in the following equation: HF(aq) + H2O(l) ⇌ F-(aq) + H3O+(aq)

Which of the following bases is not commonly found in household products or antacids?

Select the strong acid from the following list.

Which of the following equations represents the behavior of H2PO4- as an acid?

Given 0.10 M solutions of the following acids, which contains the highest concentration of H3O+?

Select the two Brønsted-Lowry acids in the following equation: HCN(aq) + H2O(l) ⇌ CN-(aq) + H3O+(aq)

Which of the following statements regarding bases is incorrect?

Matter and Energy

Atoms, Ions, and the Periodic Table

Chemical Compounds

Chemical Composition

Chemical Reactions and Equations

Quantities in Chemical Reactions

Electron Structure of the Atom

Chemical Bonding

The Gaseous State

The Liquid and Solid States

Solutions

Reaction Rates and Chemical Equilibrium

Oxidation-Reduction Reactions

Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

If one solution has an H₃O⁺ concentration that is 10 times less than that of another solution, the difference in pH is 10 units.

Calculate the pH of a solution that has [OH^-] = 1.0 x 10^-8M.

The conjugate base of HCO₃^- is:

Calculate the pH of a solution that has [OH^-] = 5.9 x 10^-5M.

Select the two Brønsted-Lowry acids in the following equation: CO₃^2-(aq) + HF(aq) ⇌ HCO₃^-(aq) + F^-(aq)

Given an OH^- concentration of 1.0 x 10^-6 M, calculate the H₃O⁺concentration, and then identify the solution as acidic, basic, or neutral.

Rank the following 0.100 M solutions in order of increasing H₃O⁺ concentration: HOCl, K_a = 4.0 x 10^-8; HCN, K_a = 6.2 x 10^-10;NH₄⁺, K_a = 5.6 x 10^-10

Rank the following 0.100 M solutions in order of increasing H₃O⁺ concentration: HF, K_a = 6.3 x 10^-4; HCN, K_a = 6.2 x 10^-10; HOCl, K_a = 4.0 x 10^-8

The conjugate acid of HCO₃^- is:

The H₃O⁺concentration in a 0.050 M solution of HClO₄is 0.050 M.

Select the two Brønsted-Lowry acids in the following equation: HF(aq) + H₂O(l) ⇌ F^-(aq) + H₃O⁺(aq)

Which of the following equations represents the behavior of H₂PO₄^- as an acid?

Given 0.10 M solutions of the following acids, which contains the highest concentration of H₃O⁺?

Select the two Brønsted-Lowry acids in the following equation: HCN(aq) + H₂O(l) ⇌ CN^-(aq) + H₃O⁺(aq)