Log in
Chemistry
1
answer
0
watching
65
views
12 Dec 2019

A buffer solution consists of 0.5 M acetic acid and 0.5 M sodium acetate (conjugate base). Ka = 1.8 × 10−5 If 0.15 M NaOH is added to the solution, what is the final pH? (a) 5.0 (b) 4.5 (c) 4.7 (d) 4.3

Watch
1
answer
0
watching
65
views

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

Hubert Koch
Hubert KochLv2
13 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
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
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




Write reaction equations to explain how acetic acid-acetate buffer reacts with an acid and reacts with a base.

Say, for example, that you had prepared a Buffer C, in which you mixed 1.35 g of sodium acetate, NaC2H3O2, with 100.0 mL of 1.0 M acetic acid.

a. What would be the initial pH of Buffer C?

b. If you add 5.0 mL of 0.5 M NaOH solution to 20.0 mL each of Buffer B and Buffer C, which buffer’s pH would change less? Explain.

Weekly leaderboard

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