[fozul_mahale]

How do i identify the metal ion from these tests?
I think it is barium because you get a white ppt with sulfuric acid. and the solubility of the sulfates decreases down group 2. am  i right?


NaOH > thin white ppt
Sulfuric acid > thick white ppt
Potassium dichromate and HCL > thick yellow ppt --> redissolves in HCL to form a yellow solution
Nitric acid + silver nitrate > no change
Sodium carbonate > thick white ppt

[SirRoderick]

I'm thinking it's lead.
First thing I saw was yellow solution which is often a dead giveaway. The others match up as well.

Lead Carbonate and Lead Sulfide are white ppt.

[fozul_mahale]

I'm thinking it's lead.
First thing I saw was yellow solution which is often a dead giveaway. The others match up as well.

Lead Carbonate and Lead Sulfide are white ppt.

thanks for the response do you think it could be magnesium sulphate?

[AWK]

NaOH > thin white ppt

Barium hydroxide is soluble in water but diluted NaOH always contain a bit of sodium carbonate ant the later form precipitate

Potassium dichromate and HCL > thick yellow ppt --> redissolves in HCL to form a yellow solution

Chromate redissolved in acid forms orange solution, and since HCl was used this solution became green then blue soon

Sulfuric acid > thick white ppt

to be sure this is barium sulfate you should add some nitric or hydrochloric acid (barium sulfate is insoluble in strong diluted acids)


Lead hydroxide is soluble in an excess of NaOH
Magnesium sulfate is soluble in water

[SirRoderick]

So it could be barium OR lead still?

[AWK]

fozul_mahale data are incomplete and partially false

[fozul_mahale]

fozul_mahale data are incomplete and partially false

i did these tests in the lab and these are the exact observations, so they cant be false

[AWK]

Color of solution after treatment of chromate with HCl is incorrect, but will be just this after treatment with HNO₃
You should check solubility of BaSO₄ in HCl or HNO₃ to be sure the precipitate is in fact BaSO₄ - so your observation is insufficient.
Colourless precipitate after treatment with NaOH is only possible when your NaOH contains carbonates - so your observation is rather incorrect.