If the Density of Methanol is 0.793kg/L what is its volume needed for making 2.5L of its 0.25M solution

Answer: The given density of methanol =0.793kg/L

The mass of methanol = CH3OH = [12 + 1 (3) + 16 + 1] g/mol = [12 + 3 + 16 + 1] g/mol = [15 + 17] g/mol = 32u.

Let x g of methanol (molar mass = 32g) be expected to set up a 0.25 Molar solution of methanol.

Consequently, we have 0.25 = (x/32) X (1/2.5)

x = 20g = 0.02 Kg

Current Density = Mass/Volume

It is given in the question that density of methanol is 0.793 KgL^-1.

We know, Volume = Mass/Density

Volume of methanol required = m/ρ

V = 20/0.793

So, V = 25.22 mL

Hence, to make 2.5L of solution, we need 25.22 mL of methanol.