[warofnature]

Hey Guys, In a week I will be tested on my analysis of testing ions in a solution. I will be given a solution of ions and i will have to test what types of ions are in the solution. I'm all good with what tests to do between each individual ions and how to write precipitation reactions however how do you differentiate between two ions that give the same result?

e.g. testing for both lead ions and sulfates yield a white precipitate by adding Barium (BaCl). I understand that you can additionally test lead with iodine which gives a yellow precipitate, but how would I go with this process, just simply add in e.g. Potassium Iodine into a second batch of the solution? Then again how does that not prove that are may also be both lead and sulfates in the solution :3

I've thought of basically just putting the solution in individual droplets and testing specifically for individual ions however I heard that some ions like carbonates can precipitate with a large number of other ions.

I've seen before that there is a process in testing ions in a solution (i.e to test for carbonates first, then hydroxide) however I am limited with solutions I can use:
Barium Chloride
Hydrochloric Acid
Potassium Iodine
Silver (I) Nitrate
Sodium Carbonate
Sodium Sulphate
Sodium Hydroxide

thanks in advance/

[Borek]

e.g. testing for both lead ions and sulfates yield a white precipitate by adding Barium (BaCl)

Ba(NO₃)₂, NaCl.

[warofnature]

so basically in that situation the more reactive ion will react? if that is the case then my problem is solved. thanks.

[Borek]

No idea what you mean by "more reactive will react". Just looking at solubility rules it should be obvious why using separately salts I have mentioned is better then using BaCl₂.

There is no need to reinvent the wheel, there are known analytical procedures for qualitative inorganic analysis.

[Darren]

You can make it easier by elimination. Eliminate carbonates by using nitric acid and see if there is effervescence observed.