Ionic EquilibriumHard
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
Which is not true about acetaminophen ?...Which of the following when added to 1.0 L of 0.5 M HCl would result in maximum increase in pH :-...What is the aqueous ammonia concentration of a solution prepared by dissolving 0.15 mole of NH4+CH3COO− in 1 L of water?...Which one is the correct graph (figure) for the corresponding acid base titration?...What concentration of free CN– must be maintained in a solution that is 1.8 M-AgNO3 and 0.16 M-NaCl to prevent AgCl from...