Question

What is the concentration of the barium hydroxide solution if 50.0 mL of a 0.425 M HNO3 solution is required to neutralize a 36.8 mL sample?

Answer 1

The molarity of Barium Hydroxide is 0.289 M.

Explanation:

We have to write the balanced equation as,

Ba(OH)₂ + 2 HNO₃ → Ba(NO₃)₂ + 2 H₂O

We need 2 moles of nitric acid to react with a mole of Barium hydroxide, so we can write the law of volumetric analysis as,

V1M1 = 2 V2M2

Here V1 and M1 are the volume and molarity of nitric acid

V2 and M2 are the volume and molarity of Barium hydroxide.

So the molarity of Ba(OH)₂, can be found as,

$M2 = \frac{V1 \times M1}{2 \times V2}$

   $M2 = \frac{50 \times 0.425 }{2 \times 36.8}$

      = 0.289 M