Question

Why did my professor choose NiCl? (Finding g of NiCO3)

Answer 1

The answer is there, I just want to know why.

Answer 2

To carry out this analysis, we need a soluble salt of Ni++ to make an aqueous solution.
NiSO4 would have done the same job, since NaSO4 and NaCl will both remain in solution.
Also, NiCl2 and NiSO4 have more or less the same solubility, so no problem with the aqueous solution.

To directly answer your question why the choice NiCl2, I don't know! Maybe he tossed a die to choose, maybe he had more NiCl2 in the lab, maybe he chose it at random! lol

Answer 3

@mathmate lol! I'm supposed to be able to do it on my own but I'm still confused. There is no NaSO4 though??? Hahaha

Answer 4

There is no such a thing as NaSO4, but Na2SO4 (Epsom salt) is a soluble salt (also a mineral).
If NiSO4 were used, we expect to balance the equation differently.
If you have difficulties balancing the new equation, please post again.
Note: It does not have to be NiSO4, it could have been Ni(NO3)2 as well, since all nitrates are soluble.

Answer 5

@mathmate ok, im confused. trying to get g of NiCO3 but he picked NiCl2 to find it instead of Na2CO3

Answer 6

Is it because we know the ml of one of NiCl2?

Answer 7

You have already calculated the volume of 0.25M NiCl2 as 12 mL (before reaction)
How much NiCl2 is left after the reaction?
So all you have to do is to calculate the mass of NiCl2 in 12 mL of 0.25M solution with molecular mass of 129.6 g/mol (anhydrous NiCl2) \(before\) reaction.
Note: NiCl2 also comes in crystals of hexahydrate, so beware.