Ionic EquilibriumHard
Question
When weak base solution (50 ml of 0.1 N NH4OH) is titrated with strong acid 0.1 N HCl, the pH of solution initially decreases fast and then decreases slowly till near equivalence point (as shown) in the figure. Which of the following is true.
Options
A.The slow decrease of pH is due to formation of an acidic buffer solution after addition of some HCl
B.The slope of shown pH graph will be minimum when 25 ml of 0.1 N HCl is added
C.The slow decrease of pH is due to formation of a basic buffer solution
D.The initial fast decrement in pH is due to fast consumption of free OH- ions by HCl.
Solution
Initial decrement is due to consumption of free OH– ions, then slow decrement in pH is due to basic buffer solution and minimum slope will be there when there is best buffer action ([salt] / [base] = 1)
Create a free account to view solution
View Solution Free