September 09, 2024, 07:50:20 AM
Forum Rules: Read This Before Posting

### Topic: Ion separation  (Read 3738 times)

0 Members and 1 Guest are viewing this topic.

#### Johatan3WE

• Very New Member
• Posts: 2
• Mole Snacks: +0/-0
##### Ion separation
« on: December 09, 2023, 01:38:15 PM »
I'm kinda desperate here, I could really use some help.

Magnesium oxalate has a Ksp of 8.6x10-5, and the calcium one has a Ksp of 2.3x 10-9. What pH must be maintained to achieve the maximum separation of the calcium ion from the magnesium ion, if both have a concentration of 0.1 mol/L, and the concentration of oxalic acid is maintained at 0.1 mol/L?

Data: For oxalic acid: Ka1 = 6.5x 10-2, Ka2 = 6.1x10 -5

Well, I have tried to calculate the molar concentration of C2O42- using the ksp equation of MgC2O4, letÂ´s name it y.

h2c2o4--->2h+ + c2o42-   K=Ka1.Ka2
?                0          Y
-X              +2X     +X
0,1            2X        Y+X

I'm not sure if what I did gives the maximum separation, any suggestions?

#### Borek

• Mr. pH
• Deity Member
• Posts: 27780
• Mole Snacks: +1805/-411
• Gender:
• I am known to be occasionally wrong.
##### Re: Ion separation
« Reply #1 on: December 09, 2023, 04:15:28 PM »
The highest separation will be when you precipitate as much calcium oxalate as possible, but without precipitating magnesium oxalate.
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

#### Johatan3WE

• Very New Member
• Posts: 2
• Mole Snacks: +0/-0
##### Re: Ion separation
« Reply #2 on: December 09, 2023, 05:28:54 PM »
So what I did is correct? Because if the concentration of C2O4^2- is greater than 'y,' magnesium oxalate will begin to precipitate.

#### Borek

• Mr. pH
• Deity Member
• Posts: 27780
• Mole Snacks: +1805/-411
• Gender:
• I am known to be occasionally wrong.
##### Re: Ion separation
« Reply #3 on: December 09, 2023, 05:48:36 PM »
So what I did is correct? Because if the concentration of C2O4^2- is greater than 'y,' magnesium oxalate will begin to precipitate.

That's a good starting point, but as far as I can tell your approach ignores fact some of the oxalate is protonated only partially.
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info