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Le Chatelier's Principle for Del N Lesser Than Zero

By applying t...

Question

By applying the law of mass action, the equilibrium constant $K$ for the reaction:
$H A + H_{2} O ⇌ H_{3} O^{+} + A^{-}$

K = \frac{[H A] [H_{2} O]}{[H_{3} O^{+}] [A^{-}]}

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K = \frac{[H_{3} O^{+}] [A^{-}]}{[H A] [H_{2} O]}

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K = \frac{[H_{3} O^{+}] [H_{2} O]}{[A^{-}] [H A]}

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K = \frac{[H A] [A^{-}]}{[H_{2} O] [H_{3} O^{+}]}

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Solution

The correct option is B $K = \frac{[H_{3} O^{+}] [A^{-}]}{[H A] [H_{2} O]}$
By applying the law of mass action, the equilibrium constant $K$ for the reaction:
$H A + H_{2} O ⇌ H_{3} O^{+} + A^{-}$
$K = \frac{[H_{3} O^{+}] [A^{-}]}{[H A] [H_{2} O]}$
The concentrations of products appear in the numerator.
The concentrations of reactants appear in the denominator.

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