Ommercially available aqueous nitric acid has a density of 1.42 g/mL and a concentration of 16 M. Calculate the mass percent of HNO3 (molar mass = 63.01 g/mol) in the solution.

The mass percent of nitric acid in the solution is 70.99 %

Explanation:

We are given:

Molarity of nitric acid = 16 M

This means that 16 moles of nitric acid is present in 1 L or 1000 mL of solution

Density of solution = 1.42 g/mL

Volume of solution = 1000 mL

Putting values in above equation, we get:

Moles of nitric acid = 16 moles

Molar mass of nitric acid = 63.01 g/mol

Putting values in above equation, we get:

To calculate the mass percentage of nitric acid in solution, we use the equation:

Mass of solution = 1420 g

Mass of nitric acid = 1008.16 g

Putting values in above equation, we get:

Hence, the mass percent of nitric acid in the solution is 70.99 %

if you're asking what comes out, it's steam.

idk what the question is about