Acids Quiz #5 pH calculations for Strong and Weak Acids Answers

 

1. The 1.0 M acidic solution with the highest pH is

A. H2S

B HNO2

C. HNO3

D. H3BO3

 

2. At 25 oC, the equation representing the ionization of water is

A H2O + H2O 2H2 + O2

B. H2O + H2O H2O2 + H2

C. H2O + H2O 4H+ + 2O2-

D. H2O + H2O H3O+ +OH-

 

3. The pH of a 0.3 M solution of NH3 is approximately

A. 14.0

B. 11.0

C. 6.0

D. 3.0

 

4. The pH of an aqueous solution is 4.32. The [OH-] is

A. 6.4 x 10-1 M

B. 4.8 x 10-5 M

C. 2.1 x 10-10 M

D. 1.6 x 10-14 M

 

5. The pH of an aqueous solution is 10.32. The [OH-] is

A. 5.0 x 10-12 M

B. 2.0 x 10-11 M

C. 4.8 x 10-11 M

D. 2.1 x 10-4 M

 

6. The pH of a 0.025 M HClO4 solution is

A. 0.94

B. 1.60

C. 12.40

D. 13.06

 

7. Consider the following equilibrium

H2O(l) H2O(l) H3O+(aq) + OH-(aq)

The equilibrium constant for this system is referred to as

A. Kw

B. Ka

C. Kb

D. Ksp

8. The [H3O-] in a solution of pH 0.60 is

A. 4.0 x 10-14 M

B. 2.2 x 10-1 M

C. 2.5 x 10-1 M

D. 6.0 x 10-1 M

 

9. A solution is prepared by adding 100 mL of 10 M of HCl to a 1 litre volumetric

flask and filling it to the mark with water. The pH of this solution is

 

A. -1

B. 0

C. 1

D. 7

 

10. The approximate pH of a 0.06 M solution of CH3COOH is

A. 1

B. 3

C. 11

D. 13

 

11. The [OH-] is greater than the [H3O+] in

A. HCl(aq)

B. NH3(aq)

C. H2O(aq)

D. CH3COOH(aq)

 

12. The pH of 0.15 M HCl is

A. 0.15

B. 0.71

C. 0.82

D. 13.18

 

13. Which of the following equations correctly relates pH and [H3O+] ?

A. pH= log [H3O+]

B. pH= 14 - [H3O+]

C. pH= -log [H3O+]

D. pH= pKw [H3O+]

 

14. The pH of 0.20 M HNO3 is

A. 0.20

B. 0.63

C. 0.70

D. 1.58

 

15. The [OH-] in 0.050 M HNO3 at 25oC is

A. 5.0 x 10-16 M

B. 1.0 x 10-14 M

C. 2.0 x 10-13 M

D. 5.0 x 10-2 M

 

16. What is the approximate pH of a 1.0 M solution of the salt NH4Cl?

A. 0.0

B. 5.0

C. 7.0

D. 10.0

 

17. What is the approximate pH of a 1.0 M solution of the salt NH3?

A. 2.0

B. 5.0

C. 7.0

D. 10.0

 

18. What is the approximate pH of a 1.0 M solution of the salt NaHCO3?

A. 2.0

B. 5.0

C. 7.0

D. 9.0

 

19. What is the approximate pH of a 1.0 M solution of the salt AlCl3?

A. 0.0

B. 3.0

C. 7.0

D. 9.0

 

20. What is the approximate pH of a 1.0 M solution of the salt NaHSO4?

A. 0.0

B. 3.0

C. 7.0

D. 9.0

 

21. Which of the following is a definition of pH?

A. pH = +Log[H3O+]

B. pH = -Log[OH-]

C. pH = -Log[H3O+]

D. pH = pOH + pKw

 

22. What is the mass of NaOH required to prepare 100.0 mL of NaOH(aq) that has a

pH = 13.62 ?

A. 0.38 g

B. 0.42 g

C. 1.67 g

D. 0.14 g

23. What is the [KOH] in a KOH solution that has a pH =12.00?

A. 0.010 M

B. 0.56 M

C. 2.0 M

D. 2.0 x 10-12 M

 

24. What is the [H3O+] in 0.70 M HCN ?

A. 0.70 M

B. 1.9 x 10-5 M

C. 1.0 x 10-6 M

D. 2.4 x 10-10 M

 

25. What is the value of pKw for water at 25 0C ?

A. 10 x 10-14

B. 10 x 10-7

C. 7.00

D. 14.00

 

26. What pH would most likely result when CO2 dissolves naturally in rainwater?

A. 3.5

B. 6.5

C. 7.2

D. 7.8

 

27. What is the pOH of 0.05 M Ba(OH)2 ?

A. 1.0

B. 1.3

C. 12.7

D. 13.0

 

28. What is the pH of 0.5 M Sr(OH)2 ?

A. 0.0

B. 0.3

C. 12.7

D. 14.0

 

29. Which of the following statements is true for an acidic solution at 25 0C ?

A. pH > 7.0

B. pOH < 7.0

C. [H3O+] < [OH-]

D. [H3O+] > [OH-]

 

30. What is the [OH-] in 0.025 M HCl ?

A. 2.5 x 10-16 M

B. 4.0 x 10-13 M

C. 2.5 x 10-2 M

D. 1.6 M