300 mL of a 1.65 M HCl solution has a density of 1.50 g/mL. Express the conclusion of this solution in:?

The following answers are according to the data given in the question.

a.
Number of moles of HCl = (1.65 mol/L) × (300/1000 L) = 0.495 mol
Molar mass of HCl = (1.0 + 35.5) g/mol = 36.5 g/mol
Mass of HCl in the solution = (36.5 g/mol) × (0.495 mol) = 18.1 g

Mass of the solution = (1.50 g/mL) × (300 mL) = 450 g

Percentage of HCl = (18.1/450) × 100(%) = 4.02(%)

b.
It is given that: Molarity of HCl = 1.65 M

c.
Mass of H₂O (solvent) = (450 - 18.1) g = 432 g
Molar mass of H₂O = (1.0×2 + 16.0) g/mol = 18.0 g/mol
Number of moles of H₂O = (432 g) / (18.0 g/mol) = 24 mol

Mole fraction of HCl (solute) = 0.495 / (0.495 + 24) = 0.0202
Mole fraction of H₂O (solvent) = 24 / (0.495 + 24) = 0.980

Where do these totally imaginary density figures come from . It is impossible for a 1.65M solution of HCl to have density = 1.50g/mL
A 1.65M solution of HCl will contain 60.1g HCl /L solution . The density of this solution is 1.03g/mL