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Question

The chloride salt of a certain weak monoacidic organic base is hydrolysed to an extent of $$3$$% in its $$0.1M$$ solution at $${25}^{o}C$$. Given that the ionic product of water is $${10}^{-14}$$ at this temperature, what is the dissociation constant of the base?


A
1×1010
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B
1×109
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C
3.33×109
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D
3.33×1010
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Solution

The correct option is B $$\approx 1\times { 10 }^{ -10 }$$
$$h = 0.03$$, $$C = 0.1 M$$ , $$K_{w} = 10^{-14}$$       
We know, $$K_{a} = Ch^{2}   $$
$$\cfrac{K_{w}}{K_{b}} = Ch^{2}    \Rightarrow \cfrac{10^{-14}}{K_{b}} = (0.1)(0.03)^{2} \Rightarrow  \cfrac{10^{-9}}{9} \approx 1 \times 10^{-10}$$

Chemistry

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