If it requires 48.3 milliliters of 0.55 molar nitric acid to neutralize 15.0 milliliters of barium hydroxide, solve for the molarity of the barium hydroxide solution. Show all of the work used to solve this problem.

Unbalanced equation: Ba(OH)2 + HNO3 yields Ba(NO3)2 + H2O

Question

If it requires 48.3 milliliters of 0.55 molar nitric acid to neutralize 15.0 milliliters of barium hydroxide, solve for the molarity of the barium hydroxide solution. Show all of the work used to solve this problem.

Unbalanced equation: Ba(OH)2 + HNO3 yields Ba(NO3)2 + H2O

anonymous · Answer

First you have to moles so multiply .0483L X .55M= .026565
Multiply moles by mole ratio which is 1/2, so the moles becomes .013283
now molarity=moles/volume; divide .013283/.015L=.885533M
significant figures and you final answer is 0.89M