Log in
Chemistry
1
answer
1
watching
768
views
13 Dec 2019

Suppose you have 0.3562g of Na2C2O4 and is dissolved in 250 mL volumetric flask. If 10 mL of this solution requires 48.36 mL of KMnO4 solution for titration, what is the molarity of the permanganate solution. Step by step solution and will rate 5 STARS! please please help.

Watch
1
answer
1
watching
768
views

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

Avatar image
Liked by OC5298185
Elin Hessel
Elin HesselLv2
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
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

You standardize a solution of KMnO4 by titration with a solutionof oxalic acid. You weight out 1.378g H2C2O4ร‚ยท2H2O and dissolve itwith deionized water in a 25.00 mL volumetric flask.

1. What is the molarity of this oxalic acid solution?
2. What is the balanced overall net-ionic equation for the reactionbetween oxalic acid and the permanganate ion, MnO4-?
3. What is the molarity of the KMnO4 solution if it requires 15.42mL of KMnO4 solution to reach the endpoint in a titration with10.00 mL of the oxalic acid solution?

Please show work! Thank you!

One of the analyses of the composition of the green oxalato-iron complex requires the redox titration of oxalate against potassium permanganate.

In the preparation of the potassium permanganate solution, what approximate mass of potassium permanganate is required to make 400 mL of a 0.02 M solution?

1) Approximate mass of KMnO4 required = g

Suppose that you weighed out approximately this amount of potassium permanganate and dissolved it in distilled water to make 400 mL of solution.

0.1089 grams of pure dry sodium oxalate was placed in an Erlenmeyer flask and dissolved in 75 mL of 0.75 M sulfuric acid. This acidic solution of sodium oxalate was titrated against the potassium permanganate solution.

The volume of potassium permanganate required to reach the end point was 15.79 mL.

How many moles of sodium oxalate were used in the titration?

2) Moles of sodium oxalate = mol

Calculate the equivalent number of moles of potassium permanganate.

3) Moles of potassium permanganate = mol

Therefore, calculate the molarity of the potassium permanganate solution.

4) Molarity of the potassium permanganate solution = M

I. Standardization of KMNO4 solution

Procedure:

Add 0.010 g samples of sodium oxalate (Na2C2O4) to separate Erlenmeyer flasks. In each flask put 30 mL DI H2O, 1.0 mL 9 M sulfuric acid (H2SO4), and 2 drops of 0.1 M manganese (II) sulfate (MnSO4). Use a graduated pipet with 0.02 M KMnO4 to titrate each solution.

Mass Na2C2O4- Sample 1: 0.010 g , Sample 2: 0.010 g , Sample 3: 0.010 g

Volume KMnO4- Sample 1: 1.35 mL , Sample 2: 1.42 mL , Sample 3: 1.39 mL --- this is the amount of KMnO4 that was used to turn solution a faint pink color

From this data:

*What is the molarity of KMnO4 for sample 1?

*What is the molarity of KMnO4 for sample 2?

*What is the molarity of KMnO4 for sample 3?

*What is the average molarity of the KMnO4 solution?

*Calculate the standard deviation of the molarity of the KMnO4 solution.

Weekly leaderboard

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