Question

*** I know this a different subject.***
If it requires 23.4 milliliters of 0.65 molar barium hydroxide to neutralize 42.5 milliliters of nitric acid, solve for the molarity of the nitric acid solution. Show all of the work used to solve this problem. Unbalanced equation: Ba(OH)2 + HNO3 Ba(NO3)2 + H2O

Answer 1

I am guessing you are unfamiliar with normality and equivalent concept right ?

Answer 2

A bit

Answer 3

I know stoichiometry

Answer 4

Don't worry, I'll do this with mole concept

Answer 5

but I don't know on how to start

Answer 6

So first of all - Molarity X Volume = No of moles right ?

Answer 7

Not yet

Answer 8

Unless it is 0.65

Answer 9

Why this is definiton of molarity

Answer 10

I wasnt referring to question. Just a general insight.

Answer 11

Yes its is Balanced Equation: Ba(OH)2 2HNO3 ---> Ba(NO3)2 2H2O

Answer 12

What I am trying to say is you know the no of moles of barium hydroxide.

Then from balanced eqaution you get moles of nitric acid corresponding to one mole of barium hydroxide.


Then you equate moles by unitary method

Answer 13

Good ! Now as you can see that 1 mole of Baoh2 reacts with 2 moles of nitric acid

So 15.21 millimoles will react with 30.42 millimoles ?

Answer 14

What unit 15.21 would be in

Answer 15

millimoles. Because you are multipling molarity with millilitres

Answer 16

Any doubt ?

Answer 17

ok so it is15.21 mmol Ba(OH)2

Answer 18

Yes

Answer 19

SO now from balanced equation we need double the millimoles of nitric acid ?

Answer 20

ok

Answer 21

30.42

Answer 22

So we need 30.42 millimoles of nitric acid

Answer 23

Feel free to ask any doubts ?

Answer 24

I got 0.71576471

Answer 25

Yeah that'd be the right answer.

Answer 26

Thank you very much.

Answer 27

You are welcome :)