[alumrock12]

ugh, i'm having a hard time with the steps to these problems.


1. should a precipitate of AgCl form if 10.0 mL of 1.0X10^-4 M AgNO3 is mixed with 10.0 mL of 2.0X10^-6 M NaCL?   (Ksp of AgCl = 1.7X10^-10)

so far, the steps i have.
1. write out reaction
- AgNO3 + NaCl -> NaNO3 (aq.) + AgCl (s.)

2. i noticed that AgCl is going to be our precipitate so i take that and dissociate it?
- AgCl <-> Ag  +  Cl


3. i want to find Q = [Ag] [Cl], but i don't know what or how to find the concentrations to plug into that equation to find Q. i want Q so i can compare it with the Ksp right? and then find out if a precipitate forms or not?


i'm really not sure on my steps... so if someone could write out steps for me to do that'd be great!... i'm just really lost, i kinda know what to look for, just don't know where and how to find it.

[xiankai]

if by Q you mean the ionic product, then yes.

[Ag⁺] = (total amount of Ag⁺ in moles) / (total volume of mixture)

and likewise for [Cl[sup-[/sup]].

if Q > K_sp, a precipitate will form since concentration is higher than maximum solubility.

if Q = K_sp, mixture is saturated, but precipitate will not form.

if Q < K_sp, the mixture is dilute and no precipitate forms.