Acids and Bases problem set with solutions

FGBC1) Calculate the pH for each of the following solutions.
a) 1.0 × 10–4 M H3O+ b) 0.040 M OH–
2) Calculate [H3O+] or [OH–] as required for each of the following solutions at 24°C,
and state whether the solution is neutral, acidic, or basic.
a) 1.0 × 10–4 M OH– b) 2.0 M H3O+
3) The pH of a solution is 5.85. What is the [H 3O+] for this solution?
4) What is the [OH-] and the percent dissociation of a 0.080 M solution of aniline,
C6H5NH2? (Kb of aniline = 4.3 x 10–10)
5) What concentration of potassium acetate has a pH of 8.9? (K a of HC2H3O2 = 1.8 x
10–5)
6) What is the pH of a buffer solution made from equal volumes of 0.080 M HCN and
0.10 M NaCN? (Ka of HCN = 4.9 x 10–10)
7) A certain weak acid HA forms a sodium salt, NaA. If a 0.10 M solution of NaA has
a pH of 9.2, calculate the ionization constant (K a) of HA.
8) A buffer solution made up of 0.100 M NH 3 and 0.100 M NH4Cl has a pH of 4.74. If
0.005 M of a strong acid is added, reacting with the base and producing an
equivalent amount of conjugate acid, what is the change in pH of the buffer
solution?
9) The pH of a 0.10 M solution of HClO is 4.2, determine the Ka and the pKa of HClO
from this.
10) Citric acid has a pKa of 3.10. What is the pOH of a 0.10 M solution of citric acid?