Question 1

Calculate the H3O+ concentration in 0.10 M NaOH.

Accepted Answer

A) 1.0 × 10-1 M 
B) 1.0 × 10-2 M 
C) 1.0 × 1013 M 
D) 1.0 × 10-12 M 
E) 1.0 × 10-13 M 
A) 1.0 × 10-1 M 
B) 1.0 × 10-2 M 
C) 1.0 × 1013 M 
D) 1.0 × 10-12 M 
E) 1.0 × 10-13 M E

Question 2

Polyprotic acids possess more than one ionizable hydrogen atom.

Accepted Answer

A) True 
 B)False  True

Question 3

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− D

Question 4

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

Accepted Answer

A) NH3/NH4+ 
B) SO42−/HSO3− 
C) H2SO3/HSO3− 
D) H2PO4−/H3PO4 
E) CO32−/HCO32− 
A) NH3/NH4+ 
B) SO42−/HSO3− 
C) H2SO3/HSO3− 
D) H2PO4−/H3PO4 
E) CO32−/HCO32−

Question 5

Select the strong acid from the following list.

Accepted Answer

A) H2SO3(aq) 
B) H2C2O4(aq) 
C) H2S(aq) 
D) HNO2(aq) 
E) HI(aq) 
A) H2SO3(aq) 
B) H2C2O4(aq) 
C) H2S(aq) 
D) HNO2(aq) 
E) HI(aq)

Question 6

Calculate the H3O+ concentration in 0.0010 M HCl.

Accepted Answer

A) 1.0 × 10-2 M 
B) 1.0 × 10-3 M 
C) 1.0 × 103 M 
D) 1.0 × 102 M 
E) 3.0 M 
A) 1.0 × 10-2 M 
B) 1.0 × 10-3 M 
C) 1.0 × 103 M 
D) 1.0 × 102 M 
E) 3.0 M

Question 7

Given an OH- concentration of 0.10 M, calculate the H3O+ concentration, and then identify the solution as acidic, basic, or neutral.

Accepted Answer

A) [H3O+] = 1.0 × 10-7, neutral 
B) [H3O+] = 1.0 × 10-1, acidic 
C) [H3O+] = 1.0 × 10-13, acidic 
D) [H3O+] = 1.0 × 10-13, basic 
E) [H3O+] = 1.0 × 10-1, basic 
A) [H3O+] = 1.0 × 10-7, neutral 
B) [H3O+] = 1.0 × 10-1, acidic 
C) [H3O+] = 1.0 × 10-13, acidic 
D) [H3O+] = 1.0 × 10-13, basic 
E) [H3O+] = 1.0 × 10-1, basic

Question 8

Select the two Brønsted-Lowry bases in the following equation: CO32−(aq)+ H2O(l)⇌ HCO3−(aq)+ OH−(aq)

Accepted Answer

A) CO32− and H2O 
B) CO32− and HCO3− 
C) H2O and OH− 
D) CO32− and OH− 
E) H2O and HCO3− 
A) CO32− and H2O 
B) CO32− and HCO3− 
C) H2O and OH− 
D) CO32− and OH− 
E) H2O and HCO3−

Question 9

Identify orange juice, pH = 3.5, as acidic, basic, or neutral.

Accepted Answer

Orange juice with a pH of 3.5 is acidic.

Question 10

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

Accepted Answer

A) [OH-] = 1.0 × 10-7, neutral 
B) [OH-] = 1.0 × 10-6, acidic 
C) [OH-] = 1.0 × 10-8, acidic 
D) [OH-] = 1.0 × 10-8, basic 
E) [OH-] = 1.0 × 10-6, basic 
A) [OH-] = 1.0 × 10-7, neutral 
B) [OH-] = 1.0 × 10-6, acidic 
C) [OH-] = 1.0 × 10-8, acidic 
D) [OH-] = 1.0 × 10-8, basic 
E) [OH-] = 1.0 × 10-6, basic

Question 11

Which of the following ionizes to the greatest extent?

Accepted Answer

A) HF, Ka = 6.3 × 10−4 
B) HCN, Ka = 6.2 × 10−10 
C) HOCl, Ka = 4.0 × 10−8 
D) CH3CO2H, Ka = 1.8 × 10−5 
E) HCO2H, Ka = 1.8 × 10−4 
A) HF, Ka = 6.3 × 10−4 
B) HCN, Ka = 6.2 × 10−10 
C) HOCl, Ka = 4.0 × 10−8 
D) CH3CO2H, Ka = 1.8 × 10−5 
E) HCO2H, Ka = 1.8 × 10−4

Question 12

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.

Question 13

Which of the following ionizes to the greatest extent?

Accepted Answer

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

Question 14

The image shows a molecular-level representation of part of a solution after ammonia, NH3, is dissolved in water. (Besides water, there are 2 NH4+ ions, 6 NH3 molecules, and 2 OH− ions present in the solution.). Which of the following best describes NH3?

Accepted Answer

A) strong acid 
B) strong base 
C) weak acid 
D) weak base 
E) amphoteric 
A) strong acid 
B) strong base 
C) weak acid 
D) weak base 
E) amphoteric

Question 15

How does a buffered solution resist changes in pH due to added acid or base?

Accepted Answer

A buffered solution resists changes in p

Question 16

All of the following species are weak bases except:

Accepted Answer

A) KCN(aq) 
B) NaNO2(aq) 
C) LiCl(aq) 
D) C6H5NH2(aq) 
E) CH3CH2NH2(aq) 
A) KCN(aq) 
B) NaNO2(aq) 
C) LiCl(aq) 
D) C6H5NH2(aq) 
E) CH3CH2NH2(aq)

Question 17

If you take an antacid tablet, the pH in your stomach will increase. This means your stomach juice becomes more acidic.

Accepted Answer

A) True 
 B)False

Question 18

When fluoride ion, F−, reacts with water, what are the products?

Accepted Answer

A) H+(aq)and OH−(aq) 
B) F+(aq)and OH−(aq) 
C) F+(aq)and H2O(aq) 
D) HF(aq)and H−(aq) 
E) HF(aq)and OH−(aq) 
A) H+(aq)and OH−(aq) 
B) F+(aq)and OH−(aq) 
C) F+(aq)and H2O(aq) 
D) HF(aq)and H−(aq) 
E) HF(aq)and OH−(aq)

Question 19

Is it possible for an indicator to change color in two different pH ranges? If so, under what circumstances is this possible?

Accepted Answer

Yes, it is possible for an indicator to

Question 20

Calculate the pOH of a solution that has [H3O+] = 5.2 × 10-7 M.

Accepted Answer

A) pOH = 7.72 
B) pOH = 7.00 
C) pOH = 6.28 
D) pOH = 5.27 
E) pOH = 5.20 
A) pOH = 7.72 
B) pOH = 7.00 
C) pOH = 6.28 
D) pOH = 5.27 
E) pOH = 5.20

Calculate the H₃O⁺ concentration in 0.10 M NaOH.

Polyprotic acids possess more than one ionizable hydrogen atom.

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

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

Select the strong acid from the following list.

Calculate the H₃O⁺ concentration in 0.0010 M HCl.

Given an OH^- concentration of 0.10 M, calculate the H₃O⁺ concentration, and then identify the solution as acidic, basic, or neutral.

Select the two Brønsted-Lowry bases in the following equation: CO₃²⁻(aq)+ H₂O(l)⇌ HCO₃⁻(aq)+ OH⁻(aq)

Identify orange juice, pH = 3.5, as acidic, basic, or neutral.

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

Which of the following ionizes to the greatest extent?

Which of the following statements regarding bases is incorrect?

Which of the following ionizes to the greatest extent?

The image shows a molecular-level representation of part of a solution after ammonia, NH₃, is dissolved in water. (Besides water, there are 2 NH₄⁺ ions, 6 NH₃ molecules, and 2 OH⁻ ions present in the solution.). Which of the following best describes NH₃?

How does a buffered solution resist changes in pH due to added acid or base?

All of the following species are weak bases except:

If you take an antacid tablet, the pH in your stomach will increase. This means your stomach juice becomes more acidic.

When fluoride ion, F⁻, reacts with water, what are the products?

Is it possible for an indicator to change color in two different pH ranges? If so, under what circumstances is this possible?

Calculate the pOH of a solution that has [H₃O⁺] = 5.2 × 10^-7 M.

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

Exam 13: Acids and Bases

Calculate the H3O+ concentration in 0.10 M NaOH.

Polyprotic acids possess more than one ionizable hydrogen atom.

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

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

Select the strong acid from the following list.

Calculate the H3O+ concentration in 0.0010 M HCl.

Given an OH- concentration of 0.10 M, calculate the H3O+ concentration, and then identify the solution as acidic, basic, or neutral.

Select the two Brønsted-Lowry bases in the following equation: CO32−(aq)+ H2O(l)⇌ HCO3−(aq)+ OH−(aq)

Identify orange juice, pH = 3.5, as acidic, basic, or neutral.

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

Which of the following ionizes to the greatest extent?

Which of the following statements regarding bases is incorrect?

Which of the following ionizes to the greatest extent?

The image shows a molecular-level representation of part of a solution after ammonia, NH3, is dissolved in water. (Besides water, there are 2 NH4+ ions, 6 NH3 molecules, and 2 OH− ions present in the solution.). Which of the following best describes NH3?

How does a buffered solution resist changes in pH due to added acid or base?

All of the following species are weak bases except:

If you take an antacid tablet, the pH in your stomach will increase. This means your stomach juice becomes more acidic.

When fluoride ion, F−, reacts with water, what are the products?

Is it possible for an indicator to change color in two different pH ranges? If so, under what circumstances is this possible?

Calculate the pOH of a solution that has [H3O+] = 5.2 × 10-7 M.

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

Calculate the H₃O⁺ concentration in 0.10 M NaOH.

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

Calculate the H₃O⁺ concentration in 0.0010 M HCl.

Given an OH^- concentration of 0.10 M, calculate the H₃O⁺ concentration, and then identify the solution as acidic, basic, or neutral.

Select the two Brønsted-Lowry bases in the following equation: CO₃²⁻(aq)+ H₂O(l)⇌ HCO₃⁻(aq)+ OH⁻(aq)

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

The image shows a molecular-level representation of part of a solution after ammonia, NH₃, is dissolved in water. (Besides water, there are 2 NH₄⁺ ions, 6 NH₃ molecules, and 2 OH⁻ ions present in the solution.). Which of the following best describes NH₃?

When fluoride ion, F⁻, reacts with water, what are the products?

Calculate the pOH of a solution that has [H₃O⁺] = 5.2 × 10^-7 M.