00:01
The equation for the dissociation of barium iodate and water is given here, as i've shown.
00:08
And the expression for the ion product constant is qsp equals the concentration barium 2 plus, which is over here, times concentration of iodate.
00:30
I forgot the 3 on that one.
00:34
Minus and that is squared because of that two right there.
00:41
Okay, so barium chloride is a salt.
00:46
So it dissociates completely in water to barium and chloride ions.
00:51
So if we want to calculate the barium ion concentration formed from 7 .5 milligrams of barium chloride, b .a .c .l .2, then we do it like this.
01:07
We take this expression and we say barium 2 plus equals 7 .5 times 10 to the negative 3 grams times moles of barium chloride over the total mass of barium chloride.
01:41
This is just to convert it to moles.
01:43
And we multiply it by moles of barium 2 plus and moles of barium chloride.
02:06
Because like i said, it dissociates completely.
02:09
This is all over 500 milliliters, and we need to convert that to liters.
02:18
So we say one liter over 1 ,000 millimeters.
02:28
Okay...