Dimethyl amine ${\left( {C{H_3}} \right)_2}NH$ is weak base and its ionization constant $ 5.4 \times {10^{ - 5}}$. Calculate $\left[ {O{H^ - }} \right],\left[ {{H_3}O} \right]$, $pOH$ and $pH$ of its $0.2$ $M$ solution at equilibrium.
Dimethyl amine ${\left( {C{H_3}} \right)_2}NH$ is weak base and its ionization constant $ 5.4 \times {10^{ - 5}}$. Calculate $\left[ {O{H^ - }} \right],\left[ {{H_3}O} \right]$, $pOH$ and $pH$ of its $0.2$ $M$ solution at equilibrium.
$\left[\mathrm{OH}^{-}\right]=1.04 \times 10^{-3} \mathrm{M},\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=9.6 \times 10^{-12} \mathrm{M}, \mathrm{pOH}=2.98, \mathrm{pH}=11.02$
Similar Questions
The $pH$ of $0.1$ $M$ $HCN$ solution is $5.2$ calculate ${K_a}$ of this solution.
The $pH$ of $0.1$ $M$ $HCN$ solution is $5.2$ calculate ${K_a}$ of this solution.
A monoprotic acid in a $0.1\,\,M$ solution ionizes to $0.001\%$. Its ionisation constant is
A monoprotic acid in a $0.1\,\,M$ solution ionizes to $0.001\%$. Its ionisation constant is
Write examples of weak acids and weak bases and give ionic equilibrium in its aqueous solution.
Write examples of weak acids and weak bases and give ionic equilibrium in its aqueous solution.
At $298\,K$ a $0.1 \,M $ $C{H_3}COOH$ solution is $ 1.34\%$ ionized. The ionization constant ${K_a}$ for acetic acid will be
At $298\,K$ a $0.1 \,M $ $C{H_3}COOH$ solution is $ 1.34\%$ ionized. The ionization constant ${K_a}$ for acetic acid will be
Derive the equation of ionization constants ${K_a}$ of weak acids $HX$.
Derive the equation of ionization constants ${K_a}$ of weak acids $HX$.