🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
Chemistry
2
answers
0
watching
14
views
18 Nov 2019

Calculate the concentrations of acetic acid and acetate in the buffer solution:

6 mL of pH 4 buffer solution

6 mL of pH 7 buffer solution

I'm not sure where to start this; do I work backward to find [OH-] and [H3O+] by using 10^-pH?

Thank you.

Watch
2
answers
0
watching
14
views

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

Unlock all answers

Get 1 free homework help answer.
Get unlimited access
Already have an account? Log in
Share
Bunny Greenfelder
Bunny GreenfelderLv2
18 Nov 2019
Get unlimited access
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

One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations of acetic acid and sodium acetate), and another contains 10.0 mL of pure water. Calculate the hydronium ion concentration and the pH after the addition of 0.25 mL of 0.10 M HCl to each one. What accounts for the difference in the hydronium ion concentrations? Explain this based on equilibrium concepts; in other words, saying that “one solution is a buffer” is not sufficient. H3O+(aq) + C2H3O2-(aq) ⇄ HC2H3O2(aq) +H2O Ka of acetic acid = 1.8 x 10-5 Acetic acid/sodium acetate buffer: Acetic acid = 0.1M, Sodium acetate = 0.1M

All three please help me!! I'm so lost!

CH3COOH <-------> CH3COO- + H+

Prepared 200 ml of 0.1 M sodium acetate solution using acetic acid (1.74M, 11.493 mL) and sodium acetate (1.641g).

Prepated 200 mL of 0.1 M acetic acid solution using the stock 1.74M acetic acid solution (11.494 mL).

testing buffer capacity of solutions

Used teh acetic acid and sodium acetate soltuions containing the volumes below:

1 2 3 4 5 6 7
Acetic Acid 18 mL 15 mL 12 mL 9 mL 6 mL 3 mL 0 mL
Acetate 0 mL 3 mL 6 mL 9 ml 12 mL 15 mL 18 mL
Buffer pH 3.27 4.14 4.45 4.73 5.01 5.39 7.41
pH with HCl 2.65 3.63 4.22 4.51 4.79 5.13 5.69
pH with NaOH 4.04 4.43 4.74 4.96 5.35 6.09 11.54

From the inital pH and ratio of weak acid to base, calculate the pKa of acetic acid using teh Henderson-Hasselbalch equation for all the effective buffering solutions and average th?e values. How does this compare to the actual pKa of acetic acid of 4.76? (Please show step-by-step process)

What is the observed effective pH buffering range for inital acetate buffers?

Which mixtures of acetate buffer resist pH changes to BOTH HCl and NaOH? How did you decide? Which would be the best buffer solution against added acid and base? Why?

Weekly leaderboard

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