00:01
Hi, so over here we're told that commercial nitric acid is going to be a solution with a concentration equal to 16 molar.
00:08
We're also told that the density of this solution is going to be equal to 1 .42 grams per milliliter.
00:15
With this information we want to know the percent by mass of nitric acid.
00:23
So remember that the percent by mass is going to tell us then how many grams of of solute we're going to get in 100 grams of solution.
00:40
You can also think about the percent by mass as mass of solute divided by mass of solution multiplied by 100.
00:51
So in this case, we're going to start by expressing the concentration of nitric acid as 16 mol of hno3 in each liter.
01:05
The next thing that we need to do is to transform moles of hno3 into grams of hno3, and for that we're going to employ the molecular weight.
01:17
The molecular weight for this compound is going to be equal to 63 grams per mole.
01:24
So using that information we're going to have 63 grams of hno3 per each mole of hno3.
01:34
Following that, we need to convert liters into milliliters in order to be able to employ the density of the solution...