Question

What is the net ionic equations for the formation of each of the precipitates observed?

A solution contains one or more of the following ions: Ag+, Ca2+, and Cu2+. When sodium chloride is added to the solution, no precipitate forms. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered off and sodium carbonate is added to the remaining solution, producing a precipitate.

Answer 1

Well it is NOT `Ag^+`....

Explanation:

`AgCl(s)` is as soluble as a brick, and would precipitate from solution as a curdy white solid.

And the precipitation of a white solid upon addition of `SO_4^(2-)` is consistent with the formation of `CaSO_4(s)`

`Ca^(2+) + SO_4^(2-) rarr CaSO_4(s)darr`

The copper ion, which would not precipitate as `CuSO_4` is likely to be precipitated as `CuCO_3`...tho this is usually formulated as `Cu_2(OH)_2CO_3`...

And so the data are consistent with the presence of `Cu^(2+)` and `Ca^(2+)` ions....