00:01
First we need a balanced chemical reaction.
00:03
And that balanced chemical reaction is the permanganate of potassium permanganate in the presence of an acidic environment reacting with 5 -fe2 +, the fe2 +, being found with the moore's salt, to produce mn2 +, 5 fe3 +, and 4 h2o.
00:37
So we know the stoichiometry between the permanganate and the iron 2 plus and the morse salt is 1 to 5.
00:45
This then allows us to carry out the calculations.
00:48
I'm going to skip trial 1 because we know we added way too much it went way pink and the volumes the volume added 12 .4 is significantly greater than the other three so for trials two and three where the volume is exactly 11 .35 in both cases we can calculate the concentration of the more salt which will be the concentration of the iron two plus by determining the moles of iron 2 plus and dividing it by the volume of the more salt.
01:32
The volume of the more salt used in each case is 10 milliliters so we know what that already is.
01:41
To get the moles of iron we use the permanganate information 11 .35 milliliters titrated is 0 .01135 liters, which we can convert into moles of permanganate using the molarity of permanganate.
02:07
They tell us the molarity of permanganate in all of the cases is 0 .01043...