00:01
To calculate the concentration of silver at equilibrium, we're going to be using the ksp expression.
00:07
The ksp for silver iodate corresponds to this equilibrium, producing one mole silver and one mole iodate, and ksp is the product of those two concentrations, with a numerical value provided at 3 .0 times 10 to the negative 8.
00:24
If you look closely, you'll notice that we are adding far more moles of iodate than we are, of silver.
00:33
So the first step is to assume that all of the silver iodate and that there will be left over iodate.
00:43
To calculate the concentration of the leftover iodate, we need to take the total moles of iodate, which will be the 50 milliliters we start with, or 0 .050 liters multiplied by its concentration of 0 .01.
00:58
That's the moles of iodate we start with.
01:00
We'll then subtract the moles of iodate that reacts, which will be the moles of silver that was added, the 50 milliliters at a .002 molar concentration...