1) If 45.6 milliliters of a nitric acid solution is spilled in lab and it requires 24.2 milliliters of a 4.32 molar aluminum hydroxide solution to completely neutralize the spill, what was the concentration of the nitric acid solution?

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Keith LeannonLv2

13 Dec 2019

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A student is asked to standardize a solution of barium hydroxide. He weighs out 0.965 g potassium hydrogen phthalate (KHC₈H₄O₄, treat this as a monoprotic acid).

It requires 19.0 mL of barium hydroxide to reach the endpoint.

A. What is the molarity of the barium hydroxide solution? M

This barium hydroxide solution is then used to titrate an unknown solution of nitric acid.

B. If 24.6 mL of the barium hydroxide solution is required to neutralize 13.0 mL of nitric acid, what is the molarity of the nitric acid solution? M

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1) If 45.6 milliliters of a nitric acid solution is spilled in lab and it requires 24.2 milliliters of a 4.32 molar aluminum hydroxide solution to completely neutralize the spill, what was the concentration of the nitric acid solution?

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