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
B
1×109
C
3.33×109
D
3.33×1010

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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