🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
Chemistry
1
answer
0
watching
121
views
13 Dec 2019

A 0.041 mol sample of a weak acid, HA, is dissolved in 463 mL of water and titrated with 0.41 M NaOH. After 35 mL of the NaOH solution has been added, the overall pH = 4.834. Calculate the Ka value for the HA?

Watch
1
answer
0
watching
121
views

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

Jean Keeling
Jean KeelingLv2
17 Dec 2019

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

[1300 Points :)] [Please provide the process] A monoprotic weak acid, HA, 1.00g, 100g/mol is titrated with NaOH (0.250 M). After the addition of 20.0 ml of NaOH the pH was 5.81. Calculate the initial moles of HA, the moles NaOH added, the moles of HA and A- after the addition of the addition of the NAOH and the pKaof HA. Use the Henderson Hasselbach equation.

HA(aq) + OH-(aq) -> A-(aq) + H2O

1) molHAinitial:

2) molNaOHadded:

3) mol HA after NaOH added:

4) mol A- after NaOH added:

5) pKa:

While titrating 25 mL of a weak acid HA, with 0.15 M NaOH, you reach the equivalence point after adding 27 mL of the NaOH. The pH of the acid initally was 2.48. What is the dissociation constant of the acid?25 mL of a 0.12 M weak acid, HA, was titrated with 0.1 M NaOH. The pH of the solution was 4.2 after 10 mL of NaOH was added. What is the dissociation constant of the this acid?

A 20.00-mL sample of a 0.200 M weak acid HA is titrated with 0.400 M NaOH as the titrant. At the equivalence point, the pH of the sample is 8.71. What is Ka of the weak acid?

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in