Dissociation constant for NH₄OH if at a given temperature its 0.1,N solution has pH = 11.27 and io

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6-2.Equilibrium-II (Ionic Equilibrium)

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What is the dissociation constant for $NH_4OH$ if at a given temperature its $0.1\,N$ solution has $pH = 11.27$ and the ionic product of water is $7.1 \times 10^{-15}$ (antilog $0.73 = 5.37$ )

$3\times 10^{-5}$

$1.86\times 10^{-6}$

$1.75\times 10^{-5}$

$2.86\times 10^{-5}$

Solution

$\quad\left[\mathrm{H}^{+}\right]=\cdot 10^{-11.27}=10^{-12}, 10^{0.73}=5.37 \times 10^{-12}$

$\left[\mathrm{OH}^{-}\right]=\frac{\mathrm{K}_{\mathrm{w}}}{\left[\mathrm{H}^{+}\right]}=\frac{7.1 \times 10^{-15}}{5.37 \times 10^{-12}}=\frac{7.1}{5.37} \times 10^{-3}\, \mathrm{M}=\sqrt{\mathrm{K}_{\mathrm{b}} \mathrm{C}}$

$\left(\frac{7.1}{5.37}\right)^{2} \times 10^{-6}=\mathrm{K}_{\mathrm{b}} \times 0.1$

$\boxed{{K_b} = 1.747 \times {{10}^{ – 5}}}$

Standard 11

Chemistry

At $25\,^oC$, the dissociation constant of $CH_3COOH$ and $NH_4OH$ in aqueous solution are almost the same. The $pH$ of a solution $0.01\, N\, CH_3COOH$ is $4.0$ at $25\,^oC$. The $pH$ of $0.01\, N\, NH_4OH$ solution at the same temperature would be

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Ionisation constant of $CH_3COOH$ is $1.7 \times 10^{-5}$ and concentration of $H^+$ ions is $3.4 \times 10^{-4}$. Then find out initial concentration of $CH_3COOH$ Molecules

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The degree of dissociation of acetic acid $\left(0.1\, mol\, L ^{-1}\right)$ in water $\left(K_a\right.$ of acetic acid is $\left.10^{-5}\right)$ is

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(KVPY-2013)

In aqueous solution the ionization constants for carbonic acid are

$K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$

Select the correct statement for a saturated $0.034\, M$ solution of the carbonic acid.

normal

(AIEEE-2010)

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

What is the dissociation constant for $NH_4OH$ if at a given temperature its $0.1\,N$ solution has $pH = 11.27$ and the ionic product of water is $7.1 \times 10^{-15}$ (antilog $0.73 = 5.37$ )

Solution

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In aqueous solution the ionization constants for carbonic acid are

$K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$

Select the correct statement for a saturated $0.034\, M$ solution of the carbonic acid.