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 $1.6x10^-10$ ?

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Answer 1 · 2016-06-18T04:16:42

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

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

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.

Jack mixes 82 mL of 4.0x10^-4 M4.0x10^-4 M silver acetate with 18 mL of 1.0x10^-4 M1.0x10^-4 M Sodium Chloride. Write the overall reaction. Write the net ionic equation. Will precipitate form if Ksp AgClAgCl is 1.6x10^-101.6x10^-10?