posted by Cindy on .
A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the pH after the addtion of the following volumes of acid, and plot the pH versus millimeters of HNO3 added.
a. 0.00 mL
b. 10.2 mL
c. 19.9 mL
d. 30.0 mL
e. 39.8 mL
First determine where the equivalence point is (how many mL HNOe are required).
At zero mL, calculate pH from pure Ba(OH)2.
All points from zero to the equivalence point, use an ICE chart to determine how much Ba(OH)2 remains, then determine pH from that. Remember to take into account the dilution of the base.
At equivalence point, the pH is the pH of pure water since this is a strong acid/strong base titration.
All points after the equivalence point, use an ICE chart to determine how much HNO3 is in excess and determine pH from that. Post your work if you get stuck.