Calculate approximate pH of the resultant solution formed by titration of 25mL of 0.4MNa2CO3 with 50mL of 0.025MHCl.
[Given that: pKa1=6.4 and pKa2=10.3 for H2CO3]
A
5.92
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
11.14
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
C
6.4
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
5.88
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution
The correct option is B11.14 The number of millimoles of sodium carbonate =25×0.4=10 millimoles. The number of millimoles of HCl=50×0.025=1.25 millimoles. Out of 10 millimoles of sodium carbonate, 1.25 millimoles will react with 1.25 millimoles of HCl to from 1.25 millimoles of sodium bicarbonate. 8.75 millimoles of sodium carbonate remain unreacted. An acidic buffer solution is obtained in which acid is sodium bicarbonate and salt is sodium carbonate. The expression for the pH of the solution is pH=pKa+log[salt][acid]=10.3+log8.751.25=11.14