Advanced Chemistry: Acid/Base Worksheet
Name
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1. A solution has a hydroxide-ion concentration of 1.5 x 10-5M. (a) What is the concentration of the hydronium
ions in this solution? (b) What is the pH of this solution? (c) Is the solution acidic, basic, or neutral?
2. Calculate the [H+] for a solution with a pOH of 4.75
3. A 0.001 M solution of HCl is prepared. What are the hydronium & hydroxide ion concentrations?
4. Calculate the pH of a 0.125 M HNO3 solution.
5. Calculate the pH of a 2.0 x 10-3M solution of HCl.
6. Calculate the pOH and the pH of a 5.0 x 10-2 M solution of NaOH.
7. Calculate the pH for a 0.015 M acetic acid solution. The Ka is 1.8 x 10-5 for acetic acid.
8. The pH of a solution is 9.67. Calculate [H+] for the solution
9. Calculate the percentage of benzoic acid ionized in a 0.020 M benzoic acid solution. Ka is 6.6 x 10-5 for benzoic
acid.
10. Calculate the pH of a solution prepared by mixing 2.0 mL of a strong acid (pH = 3.00) and 3.0 mL of a strong
base (pH = 10.00).
12. Calculate the pH of a solution prepared by adding 25 mL of 0.10 M NaOH to 30 mL of 0.20 M acetic acid.
(pKa of HAc = 4.76)
13. If the internal pH of a muscle cell is 6.8, what is the [HPO4-2]/[H2PO4-1] ratio in this cell?
(Ka for H2PO4-1  HPO4-2 is 6.31 x 10-8)
14. The total cellular concentration of the phosphate system is 20 mM, what are the concentrations of the two
anionic forms from #13?
15. Citric acid, a tricarboxylic acid important in intermediary metabolism, can be symbolized as H3A. Its
dissociation reactions are
H3A
H+ + H2ApKa1 = 3.13
H2A
H+ + HA-2
pKa2 = 4.76
-2
+
-3
HA
H + A
pKa3 = 6.40
16. If the total concentration of the acid and its anion forms is 0.02 M, what are the individual concentrations of
H3A, H2A-, HA-2and A-3 at pH 5.2?
17. The Ka for formic acid is 1.78 x 10-4.
a. What is the pH of a 0.1 M solution of formic acid
b. 150 mL of 0.1 M NaOH is added to 200 mL of 0.1 M formic acid, and water is added to give a final
volume of 1L. What is the pH of the final solution?
18. What concentrations of acetic acid and sodium acetate are required to prepare a buffer solution with a pH of
4.60? Ka is 1.8 x 10-5 for acetic acid