Commercially 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 % of HNO3 in the solution is 71.0 %

Explanation:

Step 1: Data given

Density of HNO3 = 1.42 g/mL

Concentration = 16 M = 16 mol /L

Molar mass HNO3 = 63.01 g/mol

Assume the volume = 1L or 1000 mL

Step 2: Calculate mass of the solution

Mass = density * volume

Mass = 1.42 g/mL * 1000 mL

Mass = 1420 grams

Step 3: Calculate moles HNO3

Moles = molarity * volume

Moles = 16 M * 1L

Moles = 16 moles

Step 4: Calculate mass HNO3

Mass HNO3 = moles * molar mass

Mass HNO3 = 16.0 moles * 63.01 g/mol

Mass HNO3 = 1008.16 grams

Step 5: Calculate the mass percent

mass % = (1008.16 grams / 1420 grams) *100%

mass % = 71.0 %

The mass % of HNO3 in the solution is 71.0 %

The empirical formula : C₁₁O₁₄O₃

The assumption of the compound consists of C, H, and O

mass of C in CO₂ =

mass of H in H₂O =

mass of O :

mass sample-(mass C + mass H)

mol of  C :

mol of H :

mol of O :

divide by 0.0155(the lowest ratio)

C : H : O ⇒