A 1.00M solution of a hypothetical weak acid (HB) has a pH of 2.85. A solution is created using 0.10M of a salt NaB ('B' being the anion of the weak acid HB) and 50.0 ml of 2.0M acid HB (assume no change in volume). What would be the pH of the solution and what would you call the solution?

Question

A 1.00M solution of a hypothetical weak acid (HB) has a pH of 2.85. A solution is created using 0.10M of a salt NaB ('B' being the anion of the weak acid HB) and 50.0 ml of 2.0M acid HB (assume no change in volume).  What would be the pH of the solution and what would you call the solution?

DrBob222 · Answer

Use the 1 M HB and pH of 2.85 to determine pKa for HB. The remaining part of the BUFFER problem is solved by using the Henderson-Hasselbalch equation.