What is the $pH$ of solution of $7$ $gm$ $N{H_4}OH$ per $500$ $mL$ ? ( ${K_b}$ of $N{H_4}OH 1.8 \times {10^{ - 5}}$, Molecular moles of $N{H_4}OH$ is $35\,g\,mo{l^{ - 1}}$ )
What is the $pH$ of solution of $7$ $gm$ $N{H_4}OH$ per $500$ $mL$ ? ( ${K_b}$ of $N{H_4}OH 1.8 \times {10^{ - 5}}$, Molecular moles of $N{H_4}OH$ is $35\,g\,mo{l^{ - 1}}$ )
$11.43$
Similar Questions
Which of the following base is weakest
Which of the following base is weakest
$0.1$ $mol$ of $H_2S(g)$ is kept in a $0.4$ litre vessel at $1000\,K$. For the reaction -
$2{H_2}S(g)\,\rightleftharpoons\,2{H_2}(g)\, + \,{S_2}(g)\,;\,{K_c} = {10^{ - 6}}\% $ dissociation of $H_2S$ is.......$\%$
$0.1$ $mol$ of $H_2S(g)$ is kept in a $0.4$ litre vessel at $1000\,K$. For the reaction -
$2{H_2}S(g)\,\rightleftharpoons\,2{H_2}(g)\, + \,{S_2}(g)\,;\,{K_c} = {10^{ - 6}}\% $ dissociation of $H_2S$ is.......$\%$
Derive ${K_w} = {K_a} \times {K_b}$ and ${K_w} = p{K_a} \times p{K_b}$ for weak base $B$ and its conjugate acid ${B{H^ + }}$.
Derive ${K_w} = {K_a} \times {K_b}$ and ${K_w} = p{K_a} \times p{K_b}$ for weak base $B$ and its conjugate acid ${B{H^ + }}$.
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.
Which oxychloride has maximum $pH$
Which oxychloride has maximum $pH$