A S.492 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 31.00 mL of the resulting acid solution is then titrated with 0.09653 M NaOH. The pH after the addition of 16.00 mL of the base is 5.27, and the endpoint is reached after the addition of 47.39 mL of the base.

 (a) How many moles of acid were present in the 31.00 mL sample? 40.004575 mol

(b) What is the molar mass of the acid? 371.1 x g/mol

(c) What is the pk of the acid? 4 5.56

Answer rating: 100% (QA)

HA NaOH NOA 10 moles of Naon molariti x volume b solution 009... View the full answer