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

$20 \ mL$ of $0.5 \ N \ HCl$ and $35 \ mL$ of $0.1 \ N \ NaOH$ are mixed. The resulting solution will

What is the concentration of hydrogen ion in the solution when the concentration of hydroxyl ion is $0.08 \text{ mol/dm}^3$ at $298 \text{ K}$?

Calcium lactate is a salt of a weak organic acid. $A$ $0.5 \ L$ saturated solution of calcium lactate contains $0.13 \ mol$ of the salt. If the $p^{OH}$ of the solution is $5.6$,what will be the $K_a$ of lactic acid,assuming complete dissociation of the salt?

The first ionization constant of $H_2S$ is $9.1 \times 10^{-8}$. Calculate the concentration of $HS^{-}$ ion in its $0.1 \ M$ solution. How will this concentration be affected if the solution is $0.1 \ M$ in $HCl$ also? If the second dissociation constant of $H_2S$ is $1.2 \times 10^{-13}$,calculate the concentration of $S^{2-}$ under both conditions.

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