*** 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

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*** 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

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I am guessing you are unfamiliar with normality and equivalent concept right ?
A bit
I know stoichiometry

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Don't worry, I'll do this with mole concept
but I don't know on how to start
So first of all - Molarity X Volume = No of moles right ?
Not yet
Unless it is 0.65
Why this is definiton of molarity
I wasnt referring to question. Just a general insight.
|dw:1436897699148:dw|
Yes its is Balanced Equation: Ba(OH)2 2HNO3 ---> Ba(NO3)2 2H2O
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
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 ?
What unit 15.21 would be in
millimoles. Because you are multipling molarity with millilitres
Any doubt ?
ok so it is15.21 mmol Ba(OH)2
Yes
SO now from balanced equation we need double the millimoles of nitric acid ?
ok
30.42
So we need 30.42 millimoles of nitric acid |dw:1436898445233:dw|
Feel free to ask any doubts ?
I got 0.71576471
Yeah that'd be the right answer.
Thank you very much.
You are welcome :)

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