13.4 Equilibria for Weak Acids and Bases
pH Calculations for Weak Acids & Bases
|HF||6.8 × 10-4|
|HC2H3O2||1.76 × 10-5|
|HCN||4.9 × 10-10|
KaKb = Kw
A stronger acid has a larger Ka / smaller pKa.
A stronger base has a larger Kb / smaller pKb.
The stronger the acid, the weaker the conjugate base and vice versa.
What is the pH of a 0.1M solution of acetic acid (Ka = 1.76 × 10-5)?
What is the Ka of a weak acid, HA, if the pH of a 0.1M solution is 3?
What is the pH of a 0.1M solution of ammonia (Kb = 1.75 × 10-5)?