Deck 12: Acids Bases

Question 1

Predict the products for HCl (aq) + NaOH (aq) .

A) NaCl (aq) + H₂O (l)
B) NaCl (aq) + NaOH (aq)
C) NaCl (aq) + HCl (aq)
D) NaCl (aq) + H₂ (g)

Answer 1

NaCl (aq) + H₂O (l)

Question 2

Which acid will fully ionize in water?

A) HClO
B) HF
C) HCl
D) HC₂Cl₃O₂

Answer 2

HCl

Question 3

Acids that completely ionize in water are:

A) strong bases.
B) weak bases.
C) strong acids.
D) weak acids.

Answer 3

strong acids.

Question 4

The pH of an unknown solution is 8.5. Its [OH^-] is:

A) 3.2 × 10^-6 M.
B) 3.2 × 10^-9 M.
C) 3.2 × 10⁵ M.
D) 3.2 M.

Question 5

An aqueous solution is found to have an H⁺ concentration of 7.8 × 10^-2 M. What is the concentration of OH^- in this solution?

A) 1.3 × 10^-13 M
B) 7.8 × 10¹² M
C) 2.0 × 10¹⁰ M
D) 7.8 M

Question 6

An aqueous solution is found to have an H⁺ concentration of 2.0 × 10^-4 M. What is the concentration of OH^- in this solution?

A) 5.0 × 10^-11 M
B) 2.0 × 10^-18 M
C) 2.0 × 10¹⁰ M
D) 4.0 M

Question 7

A compound that is a proton (H⁺) donor is a(n):

A) salt.
B) solvent.
C) base.
D) acid.

Question 8

The net ionic equation for the reaction Cu (s) + 2 HNO₃ (aq)  H₂(g) + Cu(NO₃)₂ (aq) is:

A) Cu (s) + H⁺ (aq)  H₂(g) + Cu²⁺ (aq).
B) Cu (s) + 2 H⁺ (aq)  H₂(g) + Cu²⁺ (aq).
C) Cu (s) + 2 H⁺ (aq)  H₂(g) + Cu⁺ (aq).
D) Cu (s) + H⁺ (aq)  H₂(g) + Cu⁺ (aq).

Question 9

In the following equilibrium, which species is the CONJUGATE BASE of compound b?

A) a
B) b
C) c
D) d

Question 10

Identify the Brønsted base in this reaction. H₂O (l) + HNO₃ (aq)  H₃O⁺ (aq) + NO₃^- (aq)

A) H₂O (l)
B) HNO₃ (aq)
C) H₃O⁺ (aq)
D) NO₃^- (aq)

Question 11

Acids that partially ionize in water are:

A) strong bases.
B) weak bases.
C) strong acids.
D) weak acids.

Question 12

The net ionic equation for the reaction Zn (s) + 2 HNO₃ (aq)  H₂(g) + Zn(NO₃)₂ (aq) is:

A) Zn (s) + H⁺ (aq)  H₂(g) + Zn²⁺ (aq).
B) Zn (s) + 2 H⁺ (aq)  H₂(g) + Zn²⁺ (aq).
C) Zn (s) + 2 H⁺ (aq)  H₂(g) + Zn⁺ (aq).
D) Zn (s) + H⁺ (aq)  H₂(g) + Zn⁺ (aq).

Question 13

Identify the Brønsted acid in this reaction. H₂SO₄ (aq) + HNO₃ (aq)  HSO₄^- (aq) + H₂NO₃⁺ (aq)

A) H₂SO₄ (aq)
B) HNO₃ (aq)
C) HSO₄^- (aq)
D) H₂NO₃⁺ (aq)

Question 14

What is the pH of a solution if [H⁺] = 1.0 × 10^-9 M?

A) 6.0
B) 9.0
C) 8.6
D) 5.4

Question 15

A compound that increases the concentration of hydroxide ion in an aqueous solution is a(n):

A) acid.
B) base.
C) salt.
D) solvent.

Question 16

Acid and base combine to form:

A) salt and water.
B) gas and water.
C) salt and gas.
D) only ionic compounds.

Question 17

Which acid can undergo up to a second ionization?

A) H₂SO₄ (aq)
B) HNO₃ (aq)
C) HNO₂ (aq)
D) HCl (aq)

Question 18

The pH of an unknown solution is 2.1. Its [OH^-] is:

A) 0.0079 M.
B) 1.3 × 10^-12 M.
C) 3.2 × 10² M.
D) 3.2 M.

Question 19

In the following equilibrium, which species is the CONJUGATE BASE of compound a?

A) a
B) b
C) c
D) d

Question 20

The neutralization reaction of barium hydroxide with aqueous hydrochloric acid (HCl) leads to what two products?

A) H₂O and BaCl
B) Ba(ClO₂)₂ and H₂
C) HCl and BaOCl
D) BaCl₂ and H₂O

Question 21

A 50.0-mL sample of HNO₃ is neutralized by reaction with 120.0 mL of 2.50 M NaOH. What is the concentration of HNO₃ in the unknown sample?

A) 6.00 M
B) 1.04 M
C) 0.960 M
D) 1.55 M

Question 22

A 50.0-mL sample of H₂SO₄ is neutralized with NaOH solution having a concentration of 2.00 M. If 35.5 mL of NaOH are required to complete the neutralization, what is the concentration of the sulfuric acid solution?

A) 0.710 M
B) 2.84 M
C) 1.41 M
D) 0.355 M

Question 23

A 25.0-mL sample of HBr is neutralized by reaction with 20.0 mL of 3.00 M KOH. What is the concentration of HBr in the unknown sample?

A) 3.8 M
B) 2.4 M
C) 1.7 M
D) 0.55 M

Question 24

Which statement is FALSE?

A) Buffer systems keep pH within a narrow range.
B) A buffer is a solution containing a mixture of acidic and basic components that resist changes in pH.
C) An appropriate buffer is a mixture of a strong acid and its conjugate base.
D) An appropriate buffer is a mixture of a weak acid and its conjugate base.

Question 25

Which combination would make the MOST effective buffer solution?

A) 0.1 M H₂CO₃ and 1.0 M NaHCO₃
B) 0.1 M H₂CO₃ and 0.1 M NaHCO₃
C) 0.1 M H₂CO₃ and 2.0 M NaHCO₃
D) 0.15 M H₂CO₃ and 0.015 M NaHCO₃

Question 26

A buffer solution contains a mixture of acetic acid (HC₂H₃O₂) and potassium acetate (KC₂H₃O₂). What reaction will take place if H⁺ is added to this solution?

A) HC₂H₃O₂ (aq) + H⁺ (aq)  H₂C₂H₃O₂⁺ (aq)
B) C₂H₃O₂^- (aq) + H⁺ (aq)  H₂C₂H₃O₂⁺ (aq)
C) KC₂H₃O₂ (aq) + H⁺ (aq)  KHC₂H₃O₂ (aq)
D) C₂H₃O₂^- (aq) + H⁺ (aq)  HC₂H₃O₂ (aq)

Question 27

A buffer solution contains a mixture of carbonic acid (H₂CO₃) and potassium hydrogen carbonate (KHCO₃). What reaction will take place if H⁺ is added to this solution?

A) H₂CO₃ (aq) + H⁺ (aq)  H₃CO₃⁺ (aq)
B) HCO₃^- (aq) + H⁺ (aq)  H₂CO₃ (aq)
C) KHCO₃ (aq) + H⁺ (aq)  KH₂CO₃ (aq)
D) CO₃^2- (aq) + H⁺ (aq)  HC₂H₃O₂ (aq)

Question 28

Which combination would make a buffer solution?

A) 0.1 M HCl and 0.1 M NaCl
B) 0.1 M H₂CO₃ and 0.1 M NaHCO₃
C) 0.4 M HNO₃ and 0.4 M NaNO₃
D) 0.15 M H₂SO₄ and 0.4 M CaSO₄

Question 29

Which solution will turn litmus paper red?

A) 0.5 M KOH
B) 2.1 M Mg(OH)₂
C) 4.5 M HC₂H₃O₂
D) 0.125 M KNO₃

Question 30

Which solution will turn litmus paper blue?

A) 0.5 M NaOH
B) 2.1 M HCl
C) 4.5 M HC₂H₃O₂
D) 0.125 M HBr