Ionic EquilibriumHard
Question
When 10 mL of 0.1 M acetic acid (pKa = 5.0), is titrated against 10mL of 0.1 M ammonia solution (pKa = 5.0), the equivalence point occurs at pH :
Options
A.5.0
B.6.0
C.7.0
D.9.0
Solution
CH3COOH + NH4OH → CH3COONH4 + H2O for salt of weak base & weak acid
pH = -
[log Ka + logKw - log Kb]
= -[-pKa + kogKw - logKb]
= -[-5 + log10-14 + 5]
= 7
pH = -
[log Ka + logKw - log Kb]= -
[-pKa + kogKw - logKb]= -
[-5 + log10-14 + 5]= 7
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