00:01
Because we have such a large kf value, we can assume the reaction goes to completion.
00:09
Thus, one mole of nickel 2 plus reacts with six moles of ammonia to produce one mole of the complex ion, where kf is equal to this ratio.
00:24
In looking at the amounts of ammonia and nickel 2 plus that we have available, the limiting reactant ends up being ammonia itself.
00:35
We have more moles of nymphs of nil2 plus that we have available.
00:37
Nickel 2 plus found in nickel two chloride than we do in 100 mill liters of 0 .2 molar ammonia.
00:47
So the maximum amount of complex ion will be limited by the ammonia we have.
00:54
We have 100 milliliters, which is 0 .100 milliliters, which is 0 .10 liters at 0 .2 molar.
01:01
So we have 0 .02 moles of ammonia, but we need 6 moles of ammonia to make one mole of the complex ion.
01:08
Once we have moles of the complex ion limited by ammonia, we divide by the volume of the solution, still 100 milliliters or 0 .1 liters.
01:19
And we get a concentration of 0 .033 molar...