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.

Step-by-step 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 = (V1 * M1)/(2 * V2)`

`$M2 = (50 * 0.425 )/(2 * 36.8)`

= 0.289 M