Percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅N^+H) in a 0.10, M aqueous pyr

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6-2.Equilibrium-II (Ionic Equilibrium)

hard

The percentage of pyridine $(C_5H_5N)$ that forms pyridinium ion $(C_5H_5N^+H)$ in a $0.10\, M$ aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is

$0.0060 \%$

$0.013\%$

$0.77\%$

$1.6\%$

(NEET-2016)

Solution

$\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}+\mathrm{H}_{5} \mathrm{O} \longrightarrow \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}^{+} \mathrm{H}+\mathrm{OH}^{-}$

$\alpha=\sqrt{\frac{K_{b}}{c}}=\sqrt{\frac{1.7 \times 10^{-9}}{0.1}}=\sqrt{1.7 \times 10^{-8}}$

$\% a=1.3 \times 10^{-4} \times 100$

$=1.3 \times 10^{-2}=0.013$

Standard 11

Chemistry

A certain amount of $H_2CO_3$ & $HCl$ are dissolved to form $1$ litre solution. At equilibrium it is found that concentration of $H_2CO_3$ & $CO_3^{-\,-}$ are $0.1\,M$ & $0.01\,M$ respectively. Calculate the $pH$ of solution. Given that for $H_2CO_3$ $K_{a_1} =10^{-5}$ & $K_{a_2} =10^{-8}$

hard

$K_b$ for $NH_4OH$ is $1.8\times 10^{-5}.$ The $[\mathop O\limits^\Theta H]$ of $0.1\,M\,NH_4OH$ is

medium

The ionization constant of dimethylamine is $5.4 \times 10^{-4}$. Calculate its degree of ionization in its $0.02$ $M$ solution. What percentage of dimethylamine is ionized if the solution is also $0.1 \,M$ in $NaOH ?$

hard

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.

hard

What is $[{H^ + }]$ of a solution that is $0.01\,M$ in $HCN$ and $0.02\,M$ in $NaCN$ $({K_a}$for $HCN = 6.2 \times {10^{ – 10}})$

medium

The percentage of pyridine $(C_5H_5N)$ that forms pyridinium ion $(C_5H_5N^+H)$ in a $0.10\, M$ aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is

Solution

Similar Questions

A certain amount of $H_2CO_3$ & $HCl$ are dissolved to form $1$ litre solution. At equilibrium it is found that concentration of $H_2CO_3$ & $CO_3^{-\,-}$ are $0.1\,M$ & $0.01\,M$ respectively. Calculate the $pH$ of solution. Given that for $H_2CO_3$ $K_{a_1} =10^{-5}$ & $K_{a_2} =10^{-8}$

$K_b$ for $NH_4OH$ is $1.8\times 10^{-5}.$ The $[\mathop O\limits^\Theta H]$ of $0.1\,M\,NH_4OH$ is

The ionization constant of dimethylamine is $5.4 \times 10^{-4}$. Calculate its degree of ionization in its $0.02$ $M$ solution. What percentage of dimethylamine is ionized if the solution is also $0.1 \,M$ in $NaOH ?$

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.

What is $[{H^ + }]$ of a solution that is $0.01\,M$ in $HCN$ and $0.02\,M$ in $NaCN$ $({K_a}$for $HCN = 6.2 \times {10^{ – 10}})$

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