In: Chemistry
Find the pH of a 0.150M solution of a weak monoprotic acid having Ka= 0.20.
Solution
Given data
Concentration of acid = 0.150 M
Ka = 0.20
pH= ?
lets say monoprotic acid is HA
now lets write reaction of acid with water and make the ICE table
HA + H2O -----> H3O+ + A-
I 0.150 M 0 0
C -x +x +x
E 0.150-x x x
Now write the ka equation for this reaction
Ka = [H3O+ ][ A-]/[ HA]
Now lets put the values in the formula
0.20 = [x][x]/[0.150-x]
0.20 * [0.150-x] = x2
By solving this using quadratic equation we get
[H3O+]=X= 0.1 M
Now using this concentration calculate the pH
pH= -log [H3O+]
pH