For the reaction $B^{-} + H_2O \rightleftharpoons HA + OH^{-}$,the value of the hydrolysis constant at equilibrium is equal to $K_a^{-1} = \dots \dots$
- A$\frac{[HA]}{[H^{+}][A^{-}]}$
- B$\frac{[H^{+}][A^{-}]}{[HA]}$
- C$[H^{+}][A^{-}]$
- D$\frac{[H^{+}][OH^{-}]}{[B^{-}]}$
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Similar Questions
At $90\,^{\circ}C$ pure water has $[H_3O^{+}] = 10^{-6}\,M$. The value of $K_w$ at this temperature will be:
MediumAIPMT 1993
View SolutionWhen the $pH$ of a solution is $2$,the hydrogen ion concentration in moles per litre is
Medium
View SolutionObserve the following solutions:
$I$. Black coffee
$II$. $0.2 \ M \ NaOH$
$III$. Lemon juice
$IV$. Lime water
$V$. Human Saliva
$VI$. Tomato juice
The number of solutions with $pH$ less than $7$ is
$I$. Black coffee
$II$. $0.2 \ M \ NaOH$
$III$. Lemon juice
$IV$. Lime water
$V$. Human Saliva
$VI$. Tomato juice
The number of solutions with $pH$ less than $7$ is
The $[OH^{-}]$ in a solution is $1 \times 10^{-12} \ mol \ dm^{-3}$. What is the concentration of $H^{+}$ ions?
Get the equation of ionic product $(K_w)$ of water.
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