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
The acidic hydrolysis of ether (X) shown below is fastest when   Â...When 100 ml of 0.4 M CH3COOH are mixed with 100 ml of 0.2 M NaOH, the [H3O+] in the solution is approximately : [Ka(CH3C...Solid Ba (NO3)2 is gradually dissolved in a 1.0 × 10-4 M Na2CO3 solution. At what concentration ofBa2+ will a preci...Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH ...Which may be added to one litre of water to act a buffer:...