Question #191310

How many liters of nitric acid solution, with a concentration of 0.05 mol / dm3, can be made if we have 150 cm3 of 60% nitric acid, whose density is 1.37 g / cm3?

Expert's answer

**Solution:**

Calculate the mass of nitric acid solution:

Mass of HNO_{3} solution = Solution volume × Density of solution

Mass of HNO_{3} solution = 150 cm^{3} × 1.37 g/cm^{3} = 205.5 g

Calculate the mass of nitric acid (HNO_{3}) in the solution:

Mass of HNO_{3} = Mass of HNO_{3} solution × w(HNO_{3})

Mass of HNO_{3} = 205.5 g × 0.6 = 123.3 g

Calculate the moles of nitric acid (HNO_{3}) in the solution:

Moles of HNO_{3} = Mass of HNO_{3} / Molar mass of HNO_{3}

The molar mass of HNO_{3} is 63.01 g mol^{-1}.

Moles of HNO_{3} = (123.3 g) / (63.01 g mol^{-1}) = 1.9568 mol

Calculate liters of nitric acid solution:

Liters of HNO_{3} solution = Moles of HNO_{3} / Molarity of HNO_{3}

Liters of HNO_{3} solution = (1.9568 mol) / (0.05 mol dm^{-3}) = 39.137 dm^{3} = **39.14 L**

**Answer: 39.14 L of nitric acid solution.**

Learn more about our help with Assignments: Chemistry

## Comments

## Leave a comment