Ionic EquilibriumHard
Question
The self ionisation constant for pure formic acid, K = [HCOOH2+][HCOO-] has been estimated as 10-6 at room temperature. The density of formic acid is 1.15 g/cm3.The percentage of formic acid molecules in pure fomic acid are converted to formate ion:
Options
A.0.002%
B.0.004%
C.0.006%
D.0.008%
Solution
Given density of formic acid = 1.15 g/cm3
∴ Weight of formic acid in 1 litre solution = 1.15 × 103 g
Thus, [HCOOH] =
= 25 M
Since in case of auto ionisation
[HCOOH2+] = [HCOO-] and [HCOO-] [HCOOH2+] = 10-6 ⇒ [HCOO-] = 10-3
Now % dissociation of HCOOH =
× 100 = 0.004%.
∴ Weight of formic acid in 1 litre solution = 1.15 × 103 g
Thus, [HCOOH] =
= 25 MSince in case of auto ionisation
[HCOOH2+] = [HCOO-] and [HCOO-] [HCOOH2+] = 10-6 ⇒ [HCOO-] = 10-3
Now % dissociation of HCOOH =
× 100 = 0.004%.Create a free account to view solution
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