00:01
So for this question, we are looking at the equilibrium of silver sulfate, but we're trying to dissolve that silver sulfate into solutions that already exist.
00:13
So one, given the equilibrium expression, we know that the ksp is equal to the concentration of silver ion squared times the concentration of sulfate.
00:24
And that value for that ksp was 1 .5 times 10 to the negative fifth.
00:30
So that's the value of the ksp.
00:33
Now notice the silver sulfate is not included because it is it's solid.
00:38
We're looking at it in terms of its solubility product.
00:43
Okay, so we're looking for molar solubility.
00:46
And molar solubility is really if we were looking at dissolving one mole of silver sulfate, what would its concentration be? so it's based on one mole.
00:55
Okay, so the first solution that we have is a solution that contains 0 .24 molar silver nitrate.
01:06
So if i have silver nitrate, what i have to consider is what ions do i have in common with that equilibrium? well, if i have 0 .24 molar of silver nitrate, i have 0 .24 molar of silver and 0 .24 molar of the nitrate ion.
01:25
But if i look, it is the silver ion that is in common.
01:29
And what you have to remember is you always have what you have.
01:32
So i'm going to input that value into that equilibrium to figure out what the molar solubility would be.
01:41
So the concentration of the silver is 0 .24 molar because you have what you have, but that value squared based on the equilibrium expression times, i'm going to give the value of s to the sulfate ion, and there's one mole of it in that equilibrium.
02:02
Right, the coefficient of the so4 is 1.
02:07
And that's going to be equal to 1 .5 times 10 to the negative fifth.
02:12
So when i solve for s, i'm solving for the molar solubility.
02:16
So i take 1 .5 times 10 to the negative fifth divided by 0 .24 squared, and i get 2 .6 times 10 to the negative fourth molar...