Acids Quiz #2 Conjugates, Reactions, Amphiprotic, Arrhenius, Bronsted Bases, KB, & Strength

1. A test that could be safely used to distinguish a strong base from a weak base is

A. taste

B. touch

C. litmus paper

D. electrical conductivity

2. Identify the two substances that act as Bronsted-Lowry bases in the equation

HS^- + SO₄^2- ⇄ S^2- + HSO₄^-

A. HS^- and S^2-

B. SO₄ ^2-and S^2-

C. HS^- and HSO₄^-

D. SO₄^2- and HSO₄^-

3. The conjugate acid of H₂C₆H₅O^-₇ is

A. C₆H₅O₇^3-

B. HC₆H₅O₇^2-

C. H₂C₆H₅O₇

D. H₃C₆H₅O₇

4. Which one of the following substances is/are amphiprotic?

(1) H₃PO₄ (2) H₂PO₄^- (3) HPO₄^2-

A. 2 only

B. 3 only

C. 1 and 2

D. 2 and 3

5. The net ionic equation for the neutralization of HBr by Ca(OH)₂ is

A. H⁺_(aq) + OH^-_(aq) ® H₂O_(l)

B. Ca2+(aq) + 2Br-(aq) ® CaBr2(s)

C. 2HBr_(aq) + Ca(OH)_2(aq) ® 2H₂O_(l) + CaBr_2(s)

D. 2H⁺_(aq) + Ca(OH)_2(aq) ® 2H₂O_(l) + Ca²⁺_(aq)

6. If reactants are favored in the following equilibrium, the stronger base must be

HCN + HS ^- ⇄ H₂S + CN ^-

A. H₂S

B. HS^-

C. CN^-

D. HCN

7. The hydronium ion, H₃O⁺ is a water molecule that has

A. lost a proton

B. gained a proton

C. gained a neutron

D. gained an electron

8. The complete ionic equation for the neutralization of acetic acid by sodium

hydroxide is

A. H⁺ + OH^- ⇄ H₂O

B. CH₃COOH + OH^- ⇄ CH₃COOH^- + H₂O

C. CH₃COOH + NaOH ⇄ NaCH₃COOH + H₂O

D. CH₃COOH + Na⁺ + OH^- ⇄ Na⁺ + CH₃COO^- + H₂O

9. In the following Bronsted – Lowry acid-base equation:

NH₄⁺ _(aq) + H₂O_(l) ⇄ NH_3(aq) + H₃O⁺_(aq)

The stronger base is

A. NH₄⁺

B. H₂O

C. NH₃

D. H₃O⁺

10. Consider the following equilibrium system:

OCl^-_(aq) + HC₇H₅O_2(aq) ⇄ HOCl_(aq) + C₇H₅O₂^-_(aq) K_eq= 2.1 x 10³

At Equilibrium

A. products are favored and HOCl is the stronger acid

B. reactants are favored and HOCl is the stronger acid

C. products are favored and HC₇H₅O₂ is the stronger acid

D. reactants are favored and HC₇H₅O₂ is the stronger acid

11. In the equilibrium system

H₂BO₃^- _(aq) + HCO₃^-_(aq) ⇄ H₂CO_2(aq) + HBO₃^2-_(aq)

            The two species acting as Bronsted-Lowry acids are

A. HCO₃^- and H₂CO₃

B. H₂BO₃^- and H₂CO₃

C. HCO₃^- and HBO₃^2-

D. H₂BO₃^- and HBO₃^2-

12. Consider the following equilibrium HS^- + H₂C₂O₄ ⇄ HC₂O₄^- + H₂S

The stronger acid is

A. HS^-

B. H₂C₂O₄

C. HC₂O₄^-

D. H₂S

13. Which species is not amphiprotic?

A. H₂O

B. H₃BO₃

C. HPO₄^2-

D. HC₆H₅O₇^2-

14. Given the equilibrium: H₂BO₃^- + H₂PO₄^- ⇌ H₃BO₃ + HPO₄^2-

Which is the strongest acid?

A. H₂PO₄^-

B. H₃BO₃

C. HPO₄^2-

D. H₂BO₃^-

15. Which equation represents the reaction of a Brønsted-Lowry base with water?

A. 2Na + 2H₂O ® 2NaOH + H₂

B. P₂H₄ + H₂O ⇌ P₂H₅⁺ + OH^-

C. H₂PO₄^- + H₂O ⇌ H₃O⁺ + HPO₄^2-

D. H₂C₂O₄ + H₂O ⇌ H₃O⁺ + HC₂O₄^-

16. A definition for a Brønsted-Lowry acid should contain which of the following

phrases?

A. the donation of H⁺

B. the donation of OH^-

C. the acceptance of H⁺

D. the acceptance of OH^-

17. Which of the following would be a typical pH of soda pop?

A. 1.0

B. 3.2

C. 6.8

D. 7.2

18. When three 25.0 mL samples of the strong acid H₂SO₄ were titrated with 0.25 M NaOH the following results were obtained:

Volume of NaOH_(aq) 47.2 mL 39.9 mL 40.1 mL

What is the concentration of the H₂SO₄ sample?

A. 0.20 M

B. 0.21 M

C. 0.40 M

D. 0.42 M

19. Which of the following is a common base found in drain cleaners?

A. baking soda

B. vinegar

C. milk of magnesia

D. sodium hydroxide

20. Identify the common acid found in the stomach.

A. benzoic acid

B. sulphuric acid

C. perchloric acid

D. hydrochloric acid

21. Which of the following solutions would typically show the greatest electrical

conductivity?

A. 1.0 M weak acid

B. 0.8 M weak base

C. 0.5 M strong acid

D. 0.1 M strong base

22. Which of the following are amphiprotic in aqueous solutions?

I. H₃BO₃ II. H₂BO₃^- III. H₃BO₂^- IV. BO₃^3-

A. I only

B. IV only

C. I and II only

D. II and III only

23. Which of the following best describes an acidic solution?

Litmus Colour Reaction with Mg

A. red reaction

B. red no reaction

C. blue no reaction

D. blue reaction

24. What is the Ka expression for H₃PO₄ ?

A. Ka = [H⁺]³

[PO₄^3-]

B. Ka = [H⁺]³

[H₃PO₄]

C.        Ka   = [H⁺][H₂PO₄^-]  

[H₃PO₄]

D. Ka = [H⁺][HPO₄^2-]

[H₃PO₄]

25. What volume of 0.250 M KOH is required to titrate 0.00230 mol of the weak acid

H₂C₂O₄ ?

A. 1.15 mL

B. 4.60 mL

C. 9.20 mL

D. 18.4 mL

26. What is the net ionic equation for the titration of H₃PO_4(aq) with Sr(OH)_2(aq) ?

            A. H⁺_(aq) + OH^- _(aq) ® H₂O_(l)

B. 6H⁺_(aq) + 6OH^-_(aq) ® 6H₂O_(l)

C. 2H₃PO_4(aq) + 3Sr²⁺_(aq) + 6OH^-_(aq) ® Sr₃(PO₄)_2(s) + 6H₂O_(l)

D. 6H⁺_(aq) + 2PO₄^3-_(aq) + 3Sr²⁺_(aq) + 6OH^- _(aq) ® 3Sr²⁺ + 2PO₄^3-_(aq) + 6H₂O_(l)

27. Which of the following is a piece of equipment typically used in acid-base

titrations?

A. burette

B. test tube

C. litmus paper

D. graduated cylinder

28. Water has the greatest tendency to act as an acid with which of the following?

A. Cl^-

B. NO₂^-

C. H₂PO₄^-

D. CH₃COO^-

29. Which net ionic equation best describes the reaction between NaOH and H₂S?

A. H⁺_(aq) + OH^- _(aq) ® H₂O_(l)

B. H₂S_(aq) + 2OH^- ® 2H₂O_(l) + S^2-_(aq)

C. H₂S_(aq) + 2NaOH ® 2H₂O_(l) + Na₂S_(aq)

D. 2H⁺_(aq) + S^2-_(aq) + 2NaOH_(aq) ® 2H₂O_(l) + 2Na⁺_(aq) + S^2-_(aq)

30. Which of the following is a general characteristic of Arrhenius acids?

A. They produce H⁺ in solution.

B. They accept an H⁺ from water.

C. They donate a proton.

D. They accept a proton.

31. Which of the following is a general characteristic of Bronstead acids?

A. They produce H⁺ in solution.

B. They accept an H⁺ from water.

C. They donate a proton.

D. They accept a proton.

32. Which of the following is a general characteristic of Arrhenius bases?

A. They produce OH^- in solution.

B. They produce H₃O⁺ in water.

C. They donate a proton.

D. They accept a proton.

33. Which of the following is a general characteristic of Bronstead base?

A. They produce H⁺ in solution.

B. They accept an H⁺ from water.

C. They donate a proton.

D. They accept a proton