00:01
Here in this problem given, if 20 .5 milliliters of 0 .1 to 2 molar barium hydroxide solution are required to neutralize 19 .6 milliliters of the nitric acid, then we have to calculate the concentration of the acid.
00:18
First, we'll write the equation for the neutralization reaction between nitric acid and barium hydroxide.
00:28
And the products are barium nitrate b a no 3 hold twice and water now we'll balance this one here will be two and here will be two this is the balanced neutralization reaction now we'll calculate number of most of barium hydroxide the base barium hydroxide that will be volume of barium hydroxide solution in liters times is smaller concentration.
01:06
And here, volume of barium hydroxide is 20 .5 milliliters.
01:12
If we divide by 1 ,000, we get 0 .0205 liters because 1 liter is 1 ,000 milliliters.
01:22
And here is the molar concentration of the base.
01:25
So we write 0 .0205 liters times 0 .122 molar, that is moles per liter.
01:37
And we get 0 .002 .501 moles of barium hydroxide.
01:47
Now we'll find out moles of nitric acid.
01:50
Here we see one mole base barium hydroxide requires two more.
01:56
Moles of nitric acid...