00:01
So now we'll work on chapter 17, problem 94.
00:12
So here we're given a generic compound mx and we're asked to calculate the molar solubility of the compound in different environments.
00:25
So first it asks us about in pure water.
00:33
So it will dissolve into its constituents.
00:45
So when pure water, there's no initial concentration of either ion.
00:50
We add s and we have equilibrium concentrations of s.
00:57
We have ksp equal to what's given as 1 .27 times 10 to the minus 36 is equal to s squared.
01:08
If we take the square root of both sides, we get s is equal to 1 .13 times 10 to the minus 18.
01:18
So that is without any any other ionic compound in the water.
01:27
Now the question is what happens if we're working in an environment with one of the other ions? so in the case for part b, we're working in a environment that has this metal chloride, let's say.
01:51
So let's go ahead and draw out the reaction again.
01:59
We have our ice.
02:03
So this time, we're starting with 0 .25 metal plus, no x minus, and we're adding s, adding s, and we have equilibrium of 0 .25 plus s and s...