Question

If it requires 18.2 milliliters of 0.45 molar barium hydroxide to neutralize 38.5 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 yields Ba(NO3)2 + H2O

I need help with this (: thanks!

Answer 1

Okay, so balance this first, we shall!

\[\huge Ba(OH)_{2} + 2HNO _{3} -> Ba(NO _{3})_{2} +2 H _{2} O\]

Answer 2

now, 18.2 ml of 0.45M barium hydroxide means, 0.0081 moles of it. Now this is being used for some 'x' moles of of nitric acid. according to the balanced equation above, the no. of moles of nitric acid required is 2 times that of barium hydroxide. so, that means, we neutralised a total of 2*0.0081 moles of nitric acid. so, that means the solution contained 2*0.0081 moles of nitric acid, that is 0.0162 moles, in 38.5 ml of solution of it.


so, you know now, 0.0.162 moles in --> 38.5ml of the solution.

Can you try to find the molarity now?

Answer 3

I think so, I'll try, thank you.

Answer 4

Okay, post your answer, if you need to verify. :)

Answer 5

Okay, I will (:

Answer 6

I have a feeling I did it wrong, but is it 0.210 M ?

Answer 7

I think I plugged in a wrong number O:
Ooopsies!

Answer 8

easy fix though o.O Maybe

Answer 9

Uh-oh. the answer should be just the double of that.


Molarity ---> moles of solute per litre of the solution


Okay, you must have plugged in, 0.081 right? yeah easy fix. :)

Answer 10

Should it be 0.420?

Answer 11

:D yay! I am glad I did it right other than that one mistake! Thank you so much ^__^

Answer 12

No problems! =]

Answer 13

hey @lowcard2