XNa2CrO4 = 0.367.
XH2O = 1-0.367 = 0.633
Suppose we have 1 mol of solution. That means we have 0.367 mol Na2CrO4 and 0.633 mol H2O. 0.633 mole H2O = 0.633*18 g/mol = 11.4 g H2O. g Na2CrO4 = mols x molar mass = 0.367*about 162 = about 59.5. Total mass of solution = 59.5+11.4 = about 71 grams. mass = volume x density or volume = mass/density = 71/1.42 = about 50 mL and 0.367moles/0.050 L = ??M Check my work. It's late. I've estimated so you need to clean up the numbers.
The mole fraction of an aqueous solution of sodium dichromate is 0.367. Calculate the molarity (in mol/L) of the sodium dichromate solution, if the density of the solution is 1.42 g mL-1.
1 answer