A 15.00 mL sample of hydrofluoric acid, Ka = 6.8x10^-4, was titrated with 0.475 M KOH. The equivalence point was reached after addition of 19.35 mL of base. Determine the molar concentration of the original hydrofluoric acid solution, and find the pH of the original hydrofluoric acid solution.

answer

watching

862

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Collen VonLv2

29 Jul 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

A 1.170-g sample of a solid, weak, monoprotic acid is used to make 100.0 mL of solution. 55.0 mL of this solution was titrated with 0.07445-M NaOH. The pH after the addition of 17.77 mL of base was 3.24, and the equivalence point was reached with the addition of 40.84 mL of base.

a) How many millimoles of acid are in the original solid sample? Hint: Don't forget the dilution. mmol acid

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

c) What is the pKa of the acid?

pKa =

A 3.750-g sample of a solid, weak, monoprotic acid is used to make100.0 mL of solution. 25.0 mL of this solution was titrated with0.08989-M NaOH. The pH after the addition of 16.67 mL of base was6.84, and the equivalence point was reached with the addition of47.64 mL of base.

a) How many millimoles of acid are in the original solid sample?Hint: Don't forget the dilution.