Question

concentrated nitric acid(HNO3) used in the laboratory is 68% nitric acid(w/w) in 3 aqueous solution. calculate the molality and molarity of the solution. ( given density of the solution=1.504 g/ml.​

Answer 1

Answer:

For example

Explanation:

The molar mass of nitric acid is 63 g/mol.

It is given that the nitric acid used in the laboratory is 68% by mass in aqueous solution.

100 g of solution contains 68 g of nitric acid  or $\frac{68}{63}$ =1.079 moles of nitric acid.

Density of solution is 1.504 g/mL.

100 g of solution corresponds to $\frac{100}{1.504}$=66.5 mL or 0.0665 L

Molarity of the solution is the number of moles of nitric acid present in 1 L of solution.

It is

$\frac{1.079}{0.0665}$ = 16.22 M