16.5 pH Calculations for Weak Acids and Bases
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| WEAK ACIDS | WEAK BASES |
|---|---|
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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.
The stronger the base, the weaker the conjugate acid.
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 percent dissociation of this acid?
What is the pH of a 0.1M solution of ammonia (Kb = 1.75×10-5)?
What is the Kb of a weak base, A-, if the pH of a 0.1M solution is 10.2?