Ionic EquilibriumHard

Question

What will be the pH at the equivalence point during the titration of a 100 mL 0.2 M solution of CH3COONa with 0.2 M solution of HCl ? Ka = 2 × 10-5.

Options

A.3 - log√2
B.3 + log√2
C.3 - log 2
D.3 + log 2

Solution

CH3COONa + HCI  → NaCI + CH3COOH
t=0    20 m eq.         20 meq.           
teq.     -            -                   20 meq.
[CH3COOH] = = 0.1 M
pH = [pKa - log C] = [5 - log2 + 1] = [6 - log2] = 3 - log√2

Create a free account to view solution

View Solution Free
Topic: Ionic Equilibrium·Practice all Ionic Equilibrium questions

More Ionic Equilibrium Questions

pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product (Ksp) of Ba(OH)2 is...At 25oC, the solubility product of Mg(OH)2 is 1.0 × 10-11. At what pH, will Mg2+ ion start precipitating in the for...Which of the following is the strongest base :-...Which may be added to one litre of water to act a buffer:...Fear or excitement, generally cause one to breathe rapidly and it results in the decrease of concentration of CO2 in blo...