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!

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Okay, so balance this first, we shall! \[\huge Ba(OH)_{2} + 2HNO _{3} -> Ba(NO _{3})_{2} +2 H _{2} O\]

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?

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

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