4

17. An acidic solution at 25°C will have a hydronium ion concentration ________ and a pH value ________. A) [H3O+] > 1 × 10-7 M, pH > 7.00 B) [H3O+] > 1 × 10-7 M, pH < 7.00 C) [H3O+] < 1 × 10-7 M, pH > 7.00 D) [H3O+] < 1 × 10-7 M, pH < 7.00

B) [H3O+] > 1 × 10-7 M, pH < 7.00

13. At 50°C the value of Kw is 5.5 × 10-14. A basic solution at 50°C has A) [H3O+] < [OH-] < 2 × 10-7 M. B) [H3O+] < 2 × 10-7 M < [OH-]. C) [H3O+] = [OH-] < 2 × 10-7 M. D) [H3O+] > 2 × 10-7 M < [OH-].

B) [H3O+] < 2 × 10-7 M < [OH-].

15. A solution with a hydrogen ion concentration of 3.25 × 10-2 M is ________ and has a hydroxide concentration of ________. A) acidic, 3.08 × 10-12 M B) acidic, 3.08 × 10-13 M C) basic, 3.08 × 10-12 M D) basic, 3.08 × 10-13 M

B) acidic, 3.08 × 10-13 M

16. Human tears have a concentration of H3O+ that is 3.16 × 10-8. The concentration of OH- in human tears is A) greater than 3.16 × 10-7 and tears are acidic. B) greater than 3.16 ×10-7 and tears are basic. C) less than 3.16 × 10-7 and tears are acidic. D) less than 3.16 × 10-7 and tears are basic.

B) greater than 3.16 ×10-7 and tears are basic.

23. What is the pH of a solution made by mixing 100.0 mL of 0.10 M HNO3, 50.0 mL of 0.20 M HCl, and 100.0 mL of water? Assume that the volumes are additive. A) 0.30 B) 0.82 C) 1.00 D) 1.10

D) 1.10

22. What is the pH of a solution prepared by dissolving 0.15 gram of solid CaO (lime) in enough water to make 2.00 L of aqueous Ca(OH)2 (limewater)? CaO(s) + H2O(l) → Ca2+(aq) + 2 OH-(aq) A) 2.57 B) 2.87 C) 11.13 D) 11.43

D) 11.43

26. What is the hydronium ion concentration of a 0.100 M hypochlorous acid solution with Ka = 3.5 × 10-8? The equation for the dissociation of hypochlorous acid is: HOCl(aq) + H2O(l) ⇌ H3O+(aq) + OCl-(aq). A) 1.9 × 10-4 B) 5.9 × 10-4 C) 1.9 × 10-5 D) 5.9 × 10-5

D) 5.9 × 10-5

7. The equilibrium constant, K, for the reaction shown below has a value 1.8 × 10-5. In this reaction which is the strongest acid and which is the strongest base? CH3CO2H(aq) + H2O(l) ⇌ H3O+(aq) + CH3CO2-(aq) A) CH3CO2H and CH3CO2- B) CH3CO2H and H2O C) H3O+ and H2O D) H3O+ and CH3CO2-

D) H3O+ and CH3CO2-

9. What is the strongest acid among the following? A) HF B) HCl C) HBr D) HI

D) HI

8. Using the conjugate acid-base pairs listed below, complete the following equation with the pair that gives an equilibrium constant Kc > 1. ________ + HSO3- ⇌ ________ + H2SO3 A) CH3CO2H/ CH3CO2- B) HCO2H/ HCO2- C) HNO2/NO2- D) HNO3/NO3-

D) HNO3/NO3-

3. What is the conjugate base of the Br∅nsted-Lowry acid HPO42-? A) H3PO4 B) H2PO4- C) HPO42- D) PO43-

D) PO43-

D) HI

10. What is the weakest acid among the following? A) SiH4 B) PH3 C) H2S D) HCl

A) SiH4

11. Which of the following should have the lowest bond strength? A) HOI B) HOCl C) HOAt D) HOBr

B) HOCl

12. An acidic solution at 25°C has A) [H3O+] > [OH-] > 1 × 10-7 M. B) [H3O+] > 1 × 10-7 M > [OH-]. C) [H3O+] = [OH-] > 1 × 10-7 M. D) [H3O+] < 1 × 10-7 M > [OH-].

B) [H3O+] > 1 × 10-7 M > [OH-].

13. At 50°C the value of Kw is 5.5 × 10-14. A basic solution at 50°C has A) [H3O+] < [OH-] < 2 × 10-7 M. B) [H3O+] < 2 × 10-7 M < [OH-]. C) [H3O+] = [OH-] < 2 × 10-7 M. D) [H3O+] > 2 × 10-7 M < [OH-].

B) [H3O+] < 2 × 10-7 M < [OH-].

14. Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-3 M in hydronium ion. A) 2.86 × 10-4 M B) 2.86 × 10-11 M C) 2.86 × 10-12 M D) 3.50 × 10-12 M

C) 2.86 × 10-12 M

15. A solution with a hydrogen ion concentration of 3.25 × 10-2 M is ________ and has a hydroxide concentration of ________. A) acidic, 3.08 × 10-12 M B) acidic, 3.08 × 10-13 M C) basic, 3.08 × 10-12 M D) basic, 3.08 × 10-13 M

B) acidic, 3.08 × 10-13 M

16. Human tears have a concentration of H3O+ that is 3.16 × 10-8. The concentration of OH- in human tears is A) greater than 3.16 × 10-7 and tears are acidic. B) greater than 3.16 ×10-7 and tears are basic. C) less than 3.16 × 10-7 and tears are acidic. D) less than 3.16 × 10-7 and tears are basic.

B) greater than 3.16 ×10-7 and tears are basic.

17. An acidic solution at 25°C will have a hydronium ion concentration ________ and a pH value ________. A) [H3O+] > 1 × 10-7 M, pH > 7.00 B) [H3O+] > 1 × 10-7 M, pH < 7.00 C) [H3O+] < 1 × 10-7 M, pH > 7.00 D) [H3O+] < 1 × 10-7 M, pH < 7.00

B) [H3O+] > 1 × 10-7 M, pH < 7.00

18. Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10-3 M hydronium ion. A) 4.65 × 10-12 B) 2.15 × 10-3 C) 2.67 D) 11.33

C) 2.67

19. What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10-4 M? A) 6.67 × 10-10 M, 4.82 B) 6.67 × 10-10 M, 9.18 C) 6.67 × 10-11 M, 3.82 D) 6.67 × 10-11 M, 10.18

B) HBr, CH3C(OH)2+

2. What are the conjugate acid-base pairs in the following chemical reaction? NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq) A) NH3, H2O and NH4+, OH- B) NH3, NH4+ and H2O, OH- C) NH3, OH- and H2O, NH4+ D) NH3 and NH4+

C) 6.67 × 10-11 M, 3.82

20. At 25°C, the pH of a vinegar solution is 2.60. What are the values of [H3O+] and [OH-] in the solution? A) 3.99 × 10-12 M, 2.51 × 10-3 M B) 2.51 × 10-3 M, 3.98 × 10-12 M C) 2.51 × 10-3 M, 11.40 M D) 2.60 M, 11.40 M

B) 2.51 × 10-3 M, 3.98 × 10-12 M

21. What is the pH of a 0.020 M HClO4 solution? A) 0.020 B) 0.040 C) 1.70 D) 12.30

C) 1.70

22. What is the pH of a solution prepared by dissolving 0.15 gram of solid CaO (lime) in enough water to make 2.00 L of aqueous Ca(OH)2 (limewater)? CaO(s) + H2O(l) → Ca2+(aq) + 2 OH-(aq) A) 2.57 B) 2.87 C) 11.13 D) 11.43

D) 11.43

23. What is the pH of a solution made by mixing 100.0 mL of 0.10 M HNO3, 50.0 mL of 0.20 M HCl, and 100.0 mL of water? Assume that the volumes are additive. A) 0.30 B) 0.82 C) 1.00 D) 1.10

D) 1.10

24. HCN (aq) ------------- H 3 O (aq) + + CN (aq) - The correct acid ionization constant relation for HCN is A) Ka = ([H3O+][CN-])/([HCN][H2O]) B) Ka = ([H3O+][CN-])/([HCN]) C) Ka = ([HCN][H2O])/([H3O+][CN-]) D) Ka = ([HCN])/([H3O+][CN-])

B) Ka = ([H3O+][CN-])/([HCN])

25. Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH of 2.87. Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is CH3COOH(aq) + H2O(l) ⇌ H3O+(aq) + CH3CO2-(aq). A) 1.3 × 10-2 B) 1.3 × 10-3 C) 1.8 × 10-5 D) 1.8 × 10-6

C) 1.8 × 10-5

26. What is the hydronium ion concentration of a 0.100 M hypochlorous acid solution with Ka = 3.5 × 10-8? The equation for the dissociation of hypochlorous acid is: HOCl(aq) + H2O(l) ⇌ H3O+(aq) + OCl-(aq). A) 1.9 × 10-4 B) 5.9 × 10-4 C) 1.9 × 10-5 D) 5.9 × 10-5

B) NH3, NH4+ and H2O, OH-

3. What is the conjugate base of the Br∅nsted-Lowry acid HPO42-? A) H3PO4 B) H2PO4- C) HPO42- D) PO43-

D) PO43-

4. Write a balanced equation for the dissociation of the Br∅nsted-Lowry acid HSO4- in water. A) HSO4-(aq) + H2O(l) ⇌ H2SO4(aq) + OH-(aq) B) HSO4-(aq) + H2O(l) ⇌ SO42-(aq) + H3O+(aq) C) HSO4-(aq) + H2O(l) ⇌ SO32-(aq) + OH-(aq) D) HSO4-(aq) + H2O(l) ⇌ SO3(g) + OH-(aq) + H2O(l)

B) HSO4-(aq) + H2O(l) ⇌ SO42-(aq) + H3O+(aq)

5. What is the strongest Br∅nsted-Lowry acid in the chemical reaction shown below? 2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l) A) HNO3 B) Ba(OH)2 C) Ba(NO3)2 D) H2O

A) HNO3

6. From the following chemical reactions determine the relative Br∅nsted-Lowry acid strengths (strongest to weakest). HClO4(aq) + H2O(l) → H3O+(aq) + ClO4-(aq) HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO2-(aq) A) HClO4 > H3O+ > HNO2 B) HClO4 > HNO2 > H3O+ C) H3O+ > HClO4 > HNO2 D) H3O+ > HNO2 > HClO4

A) HClO4 > H3O+ > HNO2

7. The equilibrium constant, K, for the reaction shown below has a value 1.8 × 10-5. In this reaction which is the strongest acid and which is the strongest base? CH3CO2H(aq) + H2O(l) ⇌ H3O+(aq) + CH3CO2-(aq) A) CH3CO2H and CH3CO2- B) CH3CO2H and H2O C) H3O+ and H2O D) H3O+ and CH3CO2-

D) H3O+ and CH3CO2-

8. Using the conjugate acid-base pairs listed below, complete the following equation with the pair that gives an equilibrium constant Kc > 1. ________ + HSO3- ⇌ ________ + H2SO3 A) CH3CO2H/ CH3CO2- B) HCO2H/ HCO2- C) HNO2/NO2- D) HNO3/NO3-

20. At 25°C, the pH of a vinegar solution is 2.60. What are the values of [H3O+] and [OH-] in the solution? A) 3.99 × 10-12 M, 2.51 × 10-3 M B) 2.51 × 10-3 M, 3.98 × 10-12 M C) 2.51 × 10-3 M, 11.40 M D) 2.60 M, 11.40 M

B) 2.51 × 10-3 M, 3.98 × 10-12 M

1. What are the Br∅nsted-Lowry acids in the following chemical reaction? HBr(sol) + CH3COOH(sol) ⇌ CH3C(OH)2+(sol) + Br-(sol) A) HBr, CH3COOH B) HBr, CH3C(OH)2+ C) CH3COOH, CH3C(OH)2+ D) CH3COOH, Br-

B) HBr, CH3C(OH)2+

11. Which of the following should have the lowest bond strength? A) HOI B) HOCl C) HOAt D) HOBr

B) HOCl

4. Write a balanced equation for the dissociation of the Br∅nsted-Lowry acid HSO4- in water. A) HSO4-(aq) + H2O(l) ⇌ H2SO4(aq) + OH-(aq) B) HSO4-(aq) + H2O(l) ⇌ SO42-(aq) + H3O+(aq) C) HSO4-(aq) + H2O(l) ⇌ SO32-(aq) + OH-(aq) D) HSO4-(aq) + H2O(l) ⇌ SO3(g) + OH-(aq) + H2O(l)

B) HSO4-(aq) + H2O(l) ⇌ SO42-(aq) + H3O+(aq)

24. HCN (aq) ------------- H 3 O (aq) + + CN (aq) - The correct acid ionization constant relation for HCN is A) Ka = ([H3O+][CN-])/([HCN][H2O]) B) Ka = ([H3O+][CN-])/([HCN]) C) Ka = ([HCN][H2O])/([H3O+][CN-]) D) Ka = ([HCN])/([H3O+][CN-])

B) Ka = ([H3O+][CN-])/([HCN])

2. What are the conjugate acid-base pairs in the following chemical reaction? NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq) A) NH3, H2O and NH4+, OH- B) NH3, NH4+ and H2O, OH- C) NH3, OH- and H2O, NH4+ D) NH3 and NH4+

B) NH3, NH4+ and H2O, OH-

12. An acidic solution at 25°C has A) [H3O+] > [OH-] > 1 × 10-7 M. B) [H3O+] > 1 × 10-7 M > [OH-]. C) [H3O+] = [OH-] > 1 × 10-7 M. D) [H3O+] < 1 × 10-7 M > [OH-].

B) [H3O+] > 1 × 10-7 M > [OH-].

D) HNO3/NO3-

9. What is the strongest acid among the following? A) HF B) HCl C) HBr D) HI

6. From the following chemical reactions determine the relative Br∅nsted-Lowry acid strengths (strongest to weakest). HClO4(aq) + H2O(l) → H3O+(aq) + ClO4-(aq) HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO2-(aq) A) HClO4 > H3O+ > HNO2 B) HClO4 > HNO2 > H3O+ C) H3O+ > HClO4 > HNO2 D) H3O+ > HNO2 > HClO4

A) HClO4 > H3O+ > HNO2

5. What is the strongest Br∅nsted-Lowry acid in the chemical reaction shown below? 2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l) A) HNO3 B) Ba(OH)2 C) Ba(NO3)2 D) H2O

A) HNO3

10. What is the weakest acid among the following? A) SiH4 B) PH3 C) H2S D) HCl

A) SiH4

21. What is the pH of a 0.020 M HClO4 solution? A) 0.020 B) 0.040 C) 1.70 D) 12.30

C) 1.70

25. Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH of 2.87. Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is CH3COOH(aq) + H2O(l) ⇌ H3O+(aq) + CH3CO2-(aq). A) 1.3 × 10-2 B) 1.3 × 10-3 C) 1.8 × 10-5 D) 1.8 × 10-6

C) 1.8 × 10-5

18. Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10-3 M hydronium ion. A) 4.65 × 10-12 B) 2.15 × 10-3 C) 2.67 D) 11.33

C) 2.67

14. Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-3 M in hydronium ion. A) 2.86 × 10-4 M B) 2.86 × 10-11 M C) 2.86 × 10-12 M D) 3.50 × 10-12 M

C) 2.86 × 10-12 M

19. What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10-4 M? A) 6.67 × 10-10 M, 4.82 B) 6.67 × 10-10 M, 9.18 C) 6.67 × 10-11 M, 3.82 D) 6.67 × 10-11 M, 10.18

C) 6.67 × 10-11 M, 3.82