Question

Jack mixes 82 mL of `4.0x10^-4 M` silver acetate with 18 mL of `1.0x10^-4 M` Sodium Chloride. Write the overall reaction. Write the net ionic equation. Will precipitate form if Ksp `AgCl` is `1.6x10^-10`?

Answer 1

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

Explanation:

`K_(sp) = 1.6xx10^-11`.

A precipitate WILL form if `[Ag^+][Cl^-]>K_(sp)`.

`[Ag^+]=(4.0xx10^-4*mol*L^-1xx0.082*L)/(0.082*L+0.018*L)=3.28xx10^-3*mol*L^-1`

`[Cl^-]=(1.0xx10^-4*mol*L^-1xx0.018*L)/(0.082*L+0.018*L)=1.8xx10^-6*mol*L^-1`

Note that I have added the volumes together, but we still have units of `mol*L^-1` in each case; i.e. a concentration.

So the ion product `Q` `=` `1.8xx10^-6xx3.28xx10^-3`

If `"calculated ion product">K_(sp)` precipitatiion will occur.