Example:

$[H_{2}S{O}_4]=$ concentration $($initial volume $/$ final volume$)$

$=0\mathrm{.}36M(35m\frac{L}{100}mL)$

$=0\mathrm{.}13M$

The dissociation reaction for sulfuric acid appears as:

$H_{2}S{O}_4+H_{2}OHS{O}_4^{-}+H_3{O}^{+}$

Based on the reaction above, what is the approximate concentration of $H_3{O}^{+}?$

$[H_3{O}^{+}]=$

$M$

M

$[KI]=$ concentration $(initial$ volume $\frac{?}{?}$ final volume $)$

$=0\mathrm{.}025M(10m\frac{L}{100}mL)$

$=$

$M$

The dissociation reaction for potassium iodide appears as:

$K{I}_{(s)}{K}_{(aq)}^{+}+I^{-}(aq)$