If the density of methanol is `0.793 kg L^(-1)` what ia its volume needed for making 2.5 L of its `0.25 M` solution?

(i) Define : (a) Mole fraction (b) Mass percentage. (ii) 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 ?

If the density of methanol is 0.8 kg L^(-1) , what is its volume needed for making 4 L of its 0.25 M solution?

Commercially available concentrated hydrochloric acid contains 38 % HCl by mass. (i) What is the molarity of the solution if its density is 1.19 "g cm"^(-2) ? (ii) What volume of concentrated HCl is needed to make 1.0 L of 0.2 M HCl solution ?

At 293.2K, the density of a 60% aqueous solution of methanol is 0.8946 g/mL. Calculate volume of 1 mole of the solution.

The density of 3 M solution of NaCl is 1.25 "g L"^(-1) . The molality of the solution is :

The molality of 1 M solution of sodium nitrate is 0.858 mol kg^(-1) . Determine the density of the solution. How much BaCl_(2) would needed to make 250 L of a solution having same concetration of Cl^(ɵ) as the one containing 3.78 g of NaCl per 100 mL ?