00:03
We're told that our boss asks us to prepare then standardized sodium hydroxide, which we do.
00:07
The average concentration is found to be 0 .1063 molar n -a -o -h, blah, blah, blah.
00:23
And then we get nitric acid, gives you nitric acid, and it takes 27 .33 milliliters.
00:49
Of 0 .1063 molar and a .o .h.
00:56
4 .24 .79 mills of the acid.
01:06
And we're asked to write an equation and then figure out the molarity of the acid.
01:12
I'm going to leave my states off because i don't need them for this.
01:19
This one will be easy because it's a, um, everything has a coefficient of one.
01:26
So i'm going to take, i get to use milliliters times molarity equals milliliters times molarity.
01:37
And i will go my acid, acid, base, base.
01:42
Doesn't really matter.
01:44
So i've got 24 .79 milliliters of my acid equals 27 .33 mil liters of my base times 0 .13 mil liters of my base times 0 .106 .3 milalmers of my base times 0 .106 .3 milal molar base.
02:04
I just used a and b to save time and space.
02:09
And this should be an x right there.
02:11
I forgot to put my x.
02:12
27 .33 times 0 .163 divided.
02:18
24 .79.
02:20
And i get x equals 0 .11.
02:26
Where are my givens? 1172.
02:33
Molar.
02:37
So 3, first answer.
02:42
Then our boss asks us to titrate the same thing, but this time we're going to be working with sulfuric acid.
02:51
And it takes 43 .88 milliliters of 0 .1063 molar and a .o .h for 22 .54 milliliters of h2s .4.
03:15
This will not be a one -to -one mole ratio, which you will see in a moment.
03:22
There's different ways to do this, but i'm going to do it using a more stoichiometric process.
03:36
So you can see i have a two here and a two here.
03:41
So on this, i'm going to find moles...