Question 1

The substance HNO3(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 2

Calculate the pH of a solution that has [OH-] = 1.0 × 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

Question 3

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

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

Which of the following is not an attribute of a base?

Accepted Answer

A) It provides OH− ions in aqueous solution. 
B) It is an electrolyte. 
C) It reacts with some organic dyes to cause them to change color. 
D) It has the ability to neutralize acids. 
E) It would taste sour. 
A) It provides OH− ions in aqueous solution. 
B) It is an electrolyte. 
C) It reacts with some organic dyes to cause them to change color. 
D) It has the ability to neutralize acids. 
E) It would taste sour.

Question 6

Calculate the pOH of a solution that has [OH-] = 3.1 × 10-8 M.

Accepted Answer

A) pOH = 3.10 
B) pOH = 8.00 
C) pOH = 7.51 
D) pOH = 3.18 
E) pOH = 6.49 
A) pOH = 3.10 
B) pOH = 8.00 
C) pOH = 7.51 
D) pOH = 3.18 
E) pOH = 6.49

Question 7

When ammonia, NH3, is dissolved in water, which ions are formed?

Accepted Answer

A) NH3−(aq)and OH−(aq) 
B) NH3+(aq)and OH−(aq) 
C) NH4+(aq)and OH−(aq) 
D) NH4+(aq)and H−(aq) 
E) NH2−(aq)and H+(aq) 
A) NH3−(aq)and OH−(aq) 
B) NH3+(aq)and OH−(aq) 
C) NH4+(aq)and OH−(aq) 
D) NH4+(aq)and H−(aq) 
E) NH2−(aq)and H+(aq)

Question 8

Select the solution below that is the most basic.

Accepted Answer

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

Question 9

When carbonate ion, CO32−, reacts with water, what are the products?

Accepted Answer

A) H+(aq)and OH−(aq) 
B) HCO3(aq)and OH−(aq) 
C) HCO3+(aq)and H2O(aq) 
D) HCO3−(aq)and H−(aq) 
E) HCO3−(aq)and OH−(aq) 
A) H+(aq)and OH−(aq) 
B) HCO3(aq)and OH−(aq) 
C) HCO3+(aq)and H2O(aq) 
D) HCO3−(aq)and H−(aq) 
E) HCO3−(aq)and OH−(aq)

Question 10

Select the solution below that is the most acidic.

Accepted Answer

A) [OH-] = 1.0 × 10-10 M 
B) [OH-] = 1.0 × 10-5 M 
C) [H3O+] = 1.0 × 10-6 M 
D) [H3O+] = 1.0 × 10-8 M 
E) [H3O+] = 1.0 × 10-10 M 
A) [OH-] = 1.0 × 10-10 M 
B) [OH-] = 1.0 × 10-5 M 
C) [H3O+] = 1.0 × 10-6 M 
D) [H3O+] = 1.0 × 10-8 M 
E) [H3O+] = 1.0 × 10-10 M

Question 11

What is the pH of a 0.015 M HNO3 solution?

Accepted Answer

A) 0.015 
B) 1.82 
C) 7.00 
D) 12.18 
E) −1.82 
A) 0.015 
B) 1.82 
C) 7.00 
D) 12.18 
E) −1.82

Question 12

Calculate the pH of a solution that has [H3O+] = 1.0 × 10-6 M.

Accepted Answer

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

Question 13

Which of the following is the strongest acid?

Accepted Answer

A) HOCl, Ka = 4.0 × 10−8 
B) HCN, Ka = 6.2 × 10−10 
C) NH4+, Ka = 5.6 × 10−10 
D) CH3CO2H, Ka = 1.8 × 10−5 
E) HCO2H, Ka = 1.8 × 10−4 
A) HOCl, Ka = 4.0 × 10−8 
B) HCN, Ka = 6.2 × 10−10 
C) NH4+, Ka = 5.6 × 10−10 
D) CH3CO2H, Ka = 1.8 × 10−5 
E) HCO2H, Ka = 1.8 × 10−4

Question 14

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 15

The indicator phenol red changes from yellow to red between pH 6.8 and pH 8.4. If phenol red is added to a solution, and the solution turns yellow, then

Accepted Answer

A) the solution is basic, and the pH must be at or below 7.0. 
B) the pH of the solution must be below 6.8, and the solution is basic. 
C) the pH of the solution must be below 6.8, and the solution is acidic. 
D) the pH of the solution must be above 8.4, and the solution is basic. 
E) the pH of the solution is above 8.4, and the solution is acidic. 
A) the solution is basic, and the pH must be at or below 7.0. 
B) the pH of the solution must be below 6.8, and the solution is basic. 
C) the pH of the solution must be below 6.8, and the solution is acidic. 
D) the pH of the solution must be above 8.4, and the solution is basic. 
E) the pH of the solution is above 8.4, and the solution is acidic.

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

Is it possible for a solution of a weak acid to have a higher hydronium ion concentration, [H3O+], than a solution of a strong acid? Explain.

Accepted Answer

No, under typical circumstances, a solut

Question 18

The conjugate base of H2PO4− is:

Accepted Answer

A) HPO42− 
B) H2PO3− 
C) H3PO4 
D) PO43− 
E) H2PO4OH− 
A) HPO42− 
B) H2PO3− 
C) H3PO4 
D) PO43− 
E) H2PO4OH−

Question 19

The pH of an aqueous HCl solution can be greater than 7.

Accepted Answer

A) True 
 B)False

Question 20

Which of the following is the strongest acid?

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

The substance HNO₃(aq)is

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

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

The conjugate base of HCO₃^- is:

Which of the following is not an attribute of a base?

Calculate the pOH of a solution that has [OH^-] = 3.1 × 10^-8 M.

When ammonia, NH₃, is dissolved in water, which ions are formed?

Select the solution below that is the most basic.

When carbonate ion, CO₃²⁻, reacts with water, what are the products?

Select the solution below that is the most acidic.

What is the pH of a 0.015 M HNO₃ solution?

Calculate the pH of a solution that has [H₃O⁺] = 1.0 × 10^-6 M.

Which of the following is the strongest acid?

The substance HCl(aq)is

The indicator phenol red changes from yellow to red between pH 6.8 and pH 8.4. If phenol red is added to a solution, and the solution turns yellow, then

Select the strong acid from the following list.

Is it possible for a solution of a weak acid to have a higher hydronium ion concentration, [H₃O⁺], than a solution of a strong acid? Explain.

The conjugate base of H₂PO₄⁻ is:

The pH of an aqueous HCl solution can be greater than 7.

Which of the following is the strongest acid?

Matter and Energy

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Exam 13: Acids and Bases

The substance HNO3(aq)is

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

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

The conjugate base of HCO3- is:

Which of the following is not an attribute of a base?

Calculate the pOH of a solution that has [OH-] = 3.1 × 10-8 M.

When ammonia, NH3, is dissolved in water, which ions are formed?

Select the solution below that is the most basic.

When carbonate ion, CO32−, reacts with water, what are the products?

Select the solution below that is the most acidic.

What is the pH of a 0.015 M HNO3 solution?

Calculate the pH of a solution that has [H3O+] = 1.0 × 10-6 M.

Which of the following is the strongest acid?

The substance HCl(aq)is

The indicator phenol red changes from yellow to red between pH 6.8 and pH 8.4. If phenol red is added to a solution, and the solution turns yellow, then

Select the strong acid from the following list.

Is it possible for a solution of a weak acid to have a higher hydronium ion concentration, [H3O+], than a solution of a strong acid? Explain.

The conjugate base of H2PO4− is:

The pH of an aqueous HCl solution can be greater than 7.

Which of the following is the strongest acid?

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

The substance HNO₃(aq)is

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

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

The conjugate base of HCO₃^- is:

Calculate the pOH of a solution that has [OH^-] = 3.1 × 10^-8 M.

When ammonia, NH₃, is dissolved in water, which ions are formed?

When carbonate ion, CO₃²⁻, reacts with water, what are the products?

What is the pH of a 0.015 M HNO₃ solution?

Calculate the pH of a solution that has [H₃O⁺] = 1.0 × 10^-6 M.

Is it possible for a solution of a weak acid to have a higher hydronium ion concentration, [H₃O⁺], than a solution of a strong acid? Explain.

The conjugate base of H₂PO₄⁻ is: