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A weak acid, HA, has a K(a) of 1.00xx10^...

A weak acid, HA, has a `K_(a)` of `1.00xx10^(-5)`. If `0.100` mol of the acid is dissolved in 1 L of water, the percentage of the acid dissociated at equilibrium is the closed to

A

`1.0 %`

B

`99.9%`

C

`0.10%`

D

`99.0%`

Text Solution

Verified by Experts

The correct Answer is:
A
`alpha = sqrt((K_(a))/(C)) =sqrt((1xx10^(-5))/(0.1)) =10^(-2) =0.01`
Precentage dissociation =1.0 %
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