The $pH$ of $0.1$ $M$ $HCN$ solution is $5.2$ calculate ${K_a}$ of this solution.
The $pH$ of $0.1$ $M$ $HCN$ solution is $5.2$ calculate ${K_a}$ of this solution.
$3.98 \times 10^{-10}$
Similar Questions
$p{K_a}$ of a weak acid is defined as
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A weak acid, $HA,$ has a $K_a$ of $1.00 \times 10^{-5}.$ If $0.100 \,mol$ of this acid is dissolved in one litreof water, the percentage of acid dissociated at equilibrium is closest to.....$\%$
A weak acid, $HA,$ has a $K_a$ of $1.00 \times 10^{-5}.$ If $0.100 \,mol$ of this acid is dissolved in one litreof water, the percentage of acid dissociated at equilibrium is closest to.....$\%$
- [AIPMT 2007]
The hydrogen ion concentration of a $0.006\,M$ benzoic acid solution is $({K_a} = 6 \times {10^{ - 5}})$
The hydrogen ion concentration of a $0.006\,M$ benzoic acid solution is $({K_a} = 6 \times {10^{ - 5}})$
Write characteristics and uses of ${K_a}$ value.
Write characteristics and uses of ${K_a}$ value.