Question

If aqueous silver nitrate is added what happens to the system in terms of color change?

CoCl4 (2-) + 6H2O <-> Co(H2O)6 (charge 2+) + 4Cl- + heat
The left side is blue, the right side is pink

If silver nitrate is added what happens color-wise and why?

Answer 1

We would assume the equilibrium SHIFTS to the right as we face the page....

Explanation:

And so we gots...

`CoCl_4^(2-) + 6H_2O(l)` `rightleftharpoons` `[Co(OH_2)_6]^(2+)+4Cl^(-)`

`Ag^+ Cl^(-) rarr AgCl(s)darr`

The addition of silver nitrate EFFECTIVELY REMOVES chloride ion from the equilibrium...i.e. `Cl^-` precipitates as `AgCl(s)`, a curdy white solid which is as souble as a brick. And so as chloride is REMOVED from the equilibrium...we would assume that the equilibrium is DRIVEN to the right as we face the page....the solution should become pinker...certainly the precipitation of silver chloride will occur.