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
View Solution FreeMore Ionic Equilibrium Questions
How many grams of HCl should be dissolved in sufficient water to get 500 ml of an aqueous solution of pH, 2.0?...The Ksp of Ag2CrO4 = 1.2 × 10–11. What concentration of Ag+ ion in aqueous solution will just fail to give a precipitate...The strength of an aqueous solution of I2 can be determined by titrating the solution with standard solution of:...Which of the following compounds is not an antacid?...The pH of an aqueous solution of 1.0 M ammonium formate assuming complete dissociation is (pKa of formic acid = 3.8 and ...