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Chemistry
Degree of dissociation of NH4OH in water is 1.8× 10-5, then hydrolysis constant of NH4Cl is:
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Q. Degree of dissociation of $ N{{H}_{4}}OH $ in water is $ 1.8\times {{10}^{-5}}, $ then hydrolysis constant of $ N{{H}_{4}}Cl $ is:
Bihar CECE
Bihar CECE 2004
Equilibrium
A
$ 1.8\times {{10}^{-5}} $
B
$ 1.8\times {{10}^{-10}} $
C
$ 5.55\times {{10}^{-5}} $
D
$ 5.55\times {{10}^{-10}} $
Solution:
$K_{h}=\frac{K_{w}}{K_{b}}$
where $K_{w}=$ ionic product of water $=1 \times 10^{-14}$
$K_{b}=$ degree of dissociation of $NH _{4} OH$ $=1.8 \times 10^{-5}$
$K_{h}=\frac{1 \times 10^{-14}}{1.8 \times 10^{-5}}$
$=0.555 \times 10^{-9}$
$=5.55 \times 10^{-10}$