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The self ionisation constant for pure HC...

The self ionisation constant for pure `HCOOH, K = [HCOO overset(o+)H_(2)] [HCOO^(Θ)]` is `10^(-6)` at room temperature. What percentage of `HCOOH` molecules are converted to `HCOO^(Θ)` ions. The density of `HCOOH` iws `1.22 g cm^(-3)`.

A

`0.002%`

B

`0.004%`

C

`0.006%`

D

`0.008%`

Text Solution

Verified by Experts

Given density of formic acid =`1.15g//cm^(3)`
:.Weight of formic acid in `1` litre solution =`1.15xx10^(3)g`
thus `[HCOOH]=(1.15xx10^(3))/(46)=25M`
since in case of auto ionisation
`[HCOOH_(2)^(+)]=[HCOO^(-)]` and `[HCOO^(-)][HCOOH_(2)^(+)]=10^(-6)rArr [HCOO^(-)]=10^(-3)`
Now `%` dissociation of `HCOOH=([HCOO^(-)]xx100)/([HCOOH])=(10^(-3))/(25)xx100=0.004%`
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