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A chemist titrates $190\mathrm{.}0mL$ of a $0\mathrm{.}8017M$ dimethylamine $((C{H}_3{)}_{2}NH)$ solution with $0\mathrm{.}2334MHN{O}_3$ solution at $25C.$ Calculate the pH at equivalence. The

$p{K}_b$ of dimethylamine is $3\mathrm{.}27.$

Round your answer to $2$ decimal places.

Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of $HN{O}_3$ solution added.

$pH=10\mathrm{.}73$