Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumpH of Strong and Weak Acids and BasesMedium2 minQB

ChemistryMediumsingle choice

What is the $[CH_{3} COO^{-}]$ in a solution that contains 0.02 M $CH_{3} COOH$ and 0.05 M $HCl$ ? $K_{a} (CH_{3} COOH) = 1.8 \times 1 0^{- 5}$ .

Answer:

Solution:

$HCl$ gives $[H^{+}] = 0.05 M$ and suppresses the acetic acid ionisation, so $[CH_{3} COOH] = 0.02 M$ .

$[CH_{3} COO^{-}] = K_{a} \frac{[ CH _{3} COOH ]}{[ H ^{+} ]} = 1.8 \times 1 0^{- 5} \times \frac{0.02}{0.05} = 7.2 \times 1 0^{- 6} M$ .

Answer: (B).

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:pH of Strong and Weak Acids and Bases

⏱ 2mℹ️ Source: QB

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