A 0.1911-g sample of an unknown monoprotic acid was dissolved in34.5 mL of water and titrated with 0.0618 M NaOH solution. Thevolume of base required to bring the solution to the equivalencepoint was 15.6 mL.
(a) Calculate the molar mass of the acid.
g/mol

(b) After 12.0 mL of base had been added during the titration, thepH was determined to be 5.53. What is the Ka of the unknownacid?

answer

watching

112

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

Lelia LubowitzLv2

7 Sep 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 0.1236-g sample of an unknown monoprotic acid was dissolved in25.8 mL of water and titrated with 0.0680 M NaOH solution. Thevolume of base required to bring the solution to the equivalencepoint was 19.1 mL.
(a) Calculate the molar mass of the acid.
___________g/mol

(b) After 11.7 mL of base had been added during the titration, thepH was determined to be 5.17. What is the Ka of the unknownacid?
___________

A sample of an unknown monoprotic acid was dissolved in of water and titrated with solution. The volume of base required to bring the solution to the equivalence point was .

(a) Calculate the molar mass of the acid.

(b) After of base had been added during the titration, the pH was determined to be . What is the Ka of the unknown acid?

plumraccoon473

A sample of 0.2140 g of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The acid required 27.4 mL of base to reach the equivalence point. (a) What is the molar mass of the acid? (b) After 15.0 mL of base had been added in the titration, the pH was found to be 6.50. What is the K_a for the unknown acid?