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#?

1 Answer
Jun 18, 2016

Answer:

#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.