Question

A student is performing a titration on a solution of HNO3 with an unknown concentration. They used a solution of KOH that they determined the concentration to be 8.2 x 10-2 M beforehand. They use an aliquot of 15.0 mL of HNO3 to titrate.
a. If the equivalence point is reached after the addition of 18.5 mL of titrant, what was the original pH of the analyte? [1.00]
b. What would the pH of the analyte be at the equivalence point? [You should be able to figure this out yourself!]
c. If the student over-titrates the analyte and adds 19.2 mL of titrant, what would the pH of the analyte be? [11.22]
d. If the student under-titrates and only adds 10.0 mL of titrant, what is the pH of the analyte? [1.56]
e. Draw a titration curve for this question.

Answer 1

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