The dissociation constant of acetic acid is $10^{-6}$ and the dissociation constant of formic acid is $10^{-5}$. What is the value of $pK_a(\text{acetic acid}) - pK_a(\text{formic acid})$?
- A$10$
- B$1$
- C$10^{-1}$
- D$-1$
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Calculate the pH of a centimolar solution of a monoacidic weak base which is $10 \%$ dissociated in its aqueous solution.
At $27^{\circ} C$,the degree of dissociation of a weak acid $(HA)$ in its $0.5 \ M$ aqueous solution is $1 \%$. Its $K_{a}$ value is approximately:
The $pH$ of $0.1 \ M$ monobasic acid is $4.50$. Calculate the concentration of species $H^{+}$,$A^{-}$ and $HA$ at equilibrium. Also,determine the value of $K_{a}$ and $pK_{a}$ of the monobasic acid.
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View SolutionIf the $pH$ of $0.10 \ M$ monoacidic base at $298 \ K$ is $9.0$,the value of $K_{b}$ and $pK_{b}$ at the same temperature are respectively:
$HClO$ is a weak acid. The concentration of ${H^+}$ ions in $0.1 \ M$ solution of $HClO$ $(K_a = 5 \times 10^{-8})$ will be equal to:
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