Problem: Find the molarity of a 40.0% by mass aqueous solution of sulfuric acid, H2SO4, for which the density is 1.3057 g/mL.

🤓 Based on our data, we think this question is relevant for Professor Li's class at CSUF.

$molarity (M) = \frac{moles solute}{L solution}$

mass percent of H₂SO₄ = 40.0%

$% Mass = \frac{mass of {CH}_{3} COOH}{mass of solution}$

This means in 100 g of solution, we have 40.0 g H₂SO₄

$40.0 % = \frac{40.0 g H_{2} {SO}_{4}}{100 g solution}$

molar mass H₂SO₄ = 98.079 g/mol

The moles of H₂SO₄ is:

$moles H_{2} {SO}_{4} = 40.0 g H_{2} {SO}_{4} \times \frac{1 mol H_{2} {SO}_{4}}{98.079 g H_{2} {SO}_{4}}$

moles H₂SO₄ = 0.4078 mol

Find the molarity of a 40.0% by mass aqueous solution of sulfuric acid, H₂SO₄, for which the density is 1.3057 g/mL.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Calculate Molarity concept. You can view video lessons to learn Calculate Molarity. Or if you need more Calculate Molarity practice, you can also practice Calculate Molarity practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Li's class at CSUF.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.