0:00
All right.
00:01
So we have 110 milliliters of 0 .190 molar k -oh and 260 milliliters of 0 .170 molar nickel sulfate.
00:10
And there's a series of questions, and you had to answer the first couple of ones.
00:15
And the first one is right on the correct chemical equation, and you do that here.
00:19
And then you correctly identify which one's going to be the precipitate, and that's going to be our nickel hydroxide, your nickel -2 hydroxide, and our limit your reactant will be the k -o -h.
00:27
So these are all correct.
00:28
And so you get the chemistry down.
00:31
And so the only remaining questions all have to do with math, basically.
00:35
And so the first step in figuring this out is we have to figure out, what we're dealing with here.
00:41
And i approach this in moles.
00:43
You can keep everything in molar, but i did everything in moles this time.
00:48
And so molar is moles per liter.
00:50
So we times these concentrations by the liters of substance we have.
00:54
We'll find out how many moles of k -o -h and how many moles if niso -4 we were dealing with.
00:59
So let's convert these milliliters into liters.
01:02
So we have 110 milliliters.
01:04
And if we divide by 1 ,000 milliliters per liter, we get 0 .1 -1 -0.
01:09
Liters of k -o -h.
01:11
We can do the same math for the nickel.
01:14
We get 0 .26 liters of nickel sulfate.
01:21
So now we can multiply these liters by our concentrations to get at moles.
01:27
And so let's do that.
01:28
So we have 0 .190 molar k -o -h times the volume of k -o -h, 0 .110 -0 liters.
01:37
And that will come out to 0 .0 .02.
01:42
09 moles of k -o -h and 0 .170 molar niso4 times 0 .260 liters means you have 0 .0442 moles of niso4.
02:02
Alright so now we have the amount of moles of each of the species so we can start forming an ice table here for our initial conditions.
02:15
Yeah and so the reaction will happen and we already identified that case.
02:18
Which is going to be a limiting reactant, so that one is going to go to zero.
02:29
And so we can subtract that from our other reactant, but we have to adjust for these coefficients.
02:35
So we're going to have that, because we're using half as much nickel sulfate as we are in koh.
02:41
So we have to have that.
02:43
We can then also add that to our product side.
02:49
And again, we need to have that because all these coefficients are one.
02:52
We're going to have every time.
02:59
So if you ever confused about what to multiply it at 1 half, 1 3rd, or multiply the coefficient you come in from, and that's going to be on the bottom, and the coefficient going to on top.
03:12
So we're going from all these numbers are starting to k -o -h, and we're going to each of these, and so ones are on the top because that's what we're going to, and we're all coming from k -o -h, so that's what's going to be on the bottom.
03:22
All right, so we're going to have zero potassium hydroxide left over.
03:27
This works out to 0 .03375 moles.
03:35
These are all moles here.
03:37
And then these are 0 .010 or 5.
03:48
So we now know the moles of all our remaining substances.
03:54
So the first one is grams of precipitate.
03:56
Well, we already have moles of precipitate...