Log in
Chemistry
1
answer
0
watching
209
views
23 Nov 2019

53.576g of MgSO4.2H2O are dissolved in 250.00mL of 1.50 MBa(NO3)2 solution to produce barium sulfate precipitate. Bariumsulfate formed 80.0 g after the reaction. Assume that the solutionvolume is constant and calculate the following concentrations.

a)what is the concentration of magnesium nitrate in solution ,and the concentration of nitrate ion in solution?

Watch
1
answer
0
watching
209
views

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

Patrina Schowalter
Patrina SchowalterLv2
31 Oct 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


Show transcribed image text

You have an aqueous solution of chromium(III) nitrate that you titrate with an aqueous solution of sodium hydroxide. After a certain amount of titrant has been added, you observe a precipitate forming. You add more sodium hydroxide solution and the precipitate dissolves, leaving a solution again. What has happened?

You have an aqueous solution of chromium(III) nitrate that you titrate with an aqueous solution of sodium hydroxide. After a certain amount of titrant has been added, you observe a precipitate forming. You add more sodium hydroxide solution and the precipitate dissolves, leaving a solution again. What has happened?

The precipitate was chromium hydroxide, which dissolved once more solution was added, forming Cr3+(aq).
The precipitate was sodium nitrate, which reacted with more nitrate to produce the soluble complex ion Na(NO3)2−.
The precipitate was sodium hydroxide, which re-dissolved in the larger volume.
The precipitate was chromium hydroxide, which then reacted with more hydroxide to produce a soluble complex ion, Cr(OH)4−.

A chemist attempts to seperate barium ions from lead ions by using the sulfate ion as a precipitating agent.

a) What sulfate ion concentrations are required for the precipitation of BaSO4 and pbSO4 from a solution containing 0.010M Ba^2+ aq and 0.010M Pb^2+ aq?

b) What is the concentration of barium ions when the lead sulfate begins to precipitate?

Weekly leaderboard

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