If the density of methanol is 0.793 kg L^–1, what is its volume needed for making 2.5 L of its 0.25 M solution?

Given:

Density of methanol = 0.793 kg/L

Molarity of solution = 0.25 M

Molecular Formula of Methanol = [CH₃OH]

Atomic Mass of Hydrogen = 1g

Atomic Mass of Oxygen = 16g

Atomic Mass of Carbon = 12g

So Molecular Mass of sugar = [12×1] + [4×1] + [16×1]

= 12 + 4 + 16

= 32g

= 0.032kg

Molarity of methanol solution = [0.793]/0.032

= 24.781 mol/L

Applying the relation, M₁V₁ = M₂V₂

24.781×X = 2.5×0.25

X = [2.5×0.25]/24.781

= 0.025 L

= 25.22 ml

Therefore, volume needed for making 2.5 L of its 0.25 M solution is 25.22 ml.