Problem set # 14
Chemistry 200
Acids and Bases
Name:
1. If the [HO-] of a solution is 2.63×10-4 M, what is the pOH and pH of the solution.
Find the [H3O+].
2. A sample of 96.3 mL of 0.23 M Ca(OH)2 is titrated with 0.549 M H3PO4. How many
milliliters of the H3PO4 solution are required to reach the end point (point of neutralization)?
3. Identify (a) the Bronsted acid and base in the follwoing reactions, and (b) the conjugate
base and acid formed:
CH3COOH + H2PO4-
CH3COO- + H3PO4
Mg(OH)2 + 2HCl
MgCl2 + 2H2O
4. Write the Lewis structure of each reactant, indentify the Lewis acid and the Lewis base, and
then write the Lewis structure of the product (acomplex) for the follwoing Lewis acid-base
reactions: Show the arrows for the movement of electrons and atoms.
CH3COOH + Br- 
CH3NH2 + HCl 
Dr. Behrang Madani
Chem 200
IVC
5. Calculate the [H3O+], pH, pOH, and [OH-] in an aqueous solution that contains 0.59 g of
H2SO4 in 250 mL of solution. Imagine H2SO4 can dissociate completely in water.
6. If the pH of a an acidic solution is 3.45, find the [H+], pOH, and [OH-] of this solution.
7. In each pair, select the stronger acid.
a) Pyruvic acid (pKa = 2.49) or Lactic acid (pKa = 3.08)
b) Citric acid (pKa = 3.08) or Phosphoric acid (pKa = 2.10)
c) Benzoic acid (Ka = 6.5×10-5) or Lactic acid (Ka = 8.4×10-4)
d) Carbonic acid (Ka = 4.3×10-7) or Boric acid (Ka = 7.3×10-10)
8. Determine which acid in each of the following pairs is stronger and explain why:
a) H2S or HCl
b) HClO4 or H3PO4
c) HBrO3 or HBrO
d) H2CO3 or H2GeO3
Dr. Behrang Madani
Chem 200
IVC
9. Calculate the pH of 0.16 M hydrazine, NH2NH2(aq), given that Kb for acetic acid is
1.7×10-6.
10. For each equilibrium, label the stronger acid, stronger base, weaker acid, and weaker base.
For which reaction(s) does the position of equilibrium lie toward the right? For which does it
lie toward the left?
a) H3PO4 + OH- ↔ H2PO4- + H2O
b) H2O + Cl- ↔ HCl +OH-
c) HCO3- + OH- ↔ CO32- + H2O
11. Determine whether an aqueous solution of each of the following salts has a pH equal to,
greater than, or less than 7. If pH > 7 or pH < 7, write a chemical equation to justify your
answer.
a) AgCl3
b) NH4Br
c) Cu(NO3)2
12. Calculate the pH of 0.56 M NH4Cl (Ka = 5.6×10-10)
Dr. Behrang Madani
Chem 200
IVC
13. Sulfuric acid is a strong acid, and the pKa2 of HSO4- is 1.92 (pKa1 is large). What is the pH
of a 0.100 M NaHSO4 solution?
14. Estimate the pH of (a) 0.15 M NaHSO3(aq); (b) 0.110 M KHCO3.
15. Write the formula for the conjugate base of each acid.
a) H2SO4
d) HCO3-
b) H3PO4
e) NH4+
c) H2S
f) HPO42-
16. Write the formula for the conjugate acid of each base.
a) H2O
d) NH3
b) C6H5O-
e) OH-
c) CO32-
f) HPO42-
Dr. Behrang Madani
Chem 200
IVC