$0.1 \, M$ acetic acid is $1\%$ ionized. If its ionization increases to $10\%$,what will be its new concentration (in $, M$)?

The dissociation constant of a weak acid is $1 \times 10^{-4}$. The equilibrium constant of its reaction with a strong base is:

The hydrolysis constants of salts $M_1X$ and $M_2X$ formed from a strong acid and weak bases are $10^{-7}$ and $10^{-4}$ respectively. For base $M_3OH$,$K_b = 10^{-4}$. The decreasing order of basic strength is:

If the equilibrium constant of $CH_3COOH + H_2O \rightleftharpoons CH_3COO^{-} + H_3O^{+}$ is $1.8 \times 10^{-5}$,what is the equilibrium constant for the reaction $CH_3COOH + OH^{-} \rightleftharpoons CH_3COO^{-} + H_2O$?

For the equilibrium $2H_2O \rightleftharpoons H_3O^{+} + OH^{-}$,the value of $\Delta G^o$ at $298 \ K$ is approximately ....... $kJ \ mol^{-1}$.

Which of the following,when added to $20 \ mL$ of a $0.01 \ M$ solution of $HCl$,would decrease its $pH$?