Ionic EquilibriumEasy
Question
The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, Ka of this acid is :-
Options
A.1 × 10 -7
B.3 × 10 -7
C.1 × 10 -3
D.1 × 10 -5
Solution
pH = -log[H+] pH = 3
[H+] = 10-pH = 10-3
For weak acid
[H+] =
[H+]2 = Ka × C
(10-3)+ = Ka × 0.1
Ka = 10-5
[H+] = 10-pH = 10-3
For weak acid
[H+] =
[H+]2 = Ka × C
(10-3)+ = Ka × 0.1
Ka = 10-5
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
The relation pKa = 14 – pKb is true for which of the following pair(s)?...How many grams of NaOH should be added in 500 ml of 2 M acetic acid solution to get a buffer solution of maximum buffer ...Which is/are correct statements : (a) When 100 ml of 0.1 M NaCN solution is titrated with 0.1 M HCl solution the variati...Which of the following is not correct :...pH of 0.01 M HS- will be:...