Exams › JEE Main › Chemistry

A sulphuric acid solution is 13% H2SO4 by mass and has density 0.98 g/mL. Calculate its molarity. (Molar mass of H2SO4 = 98 g/mol)

1. 1.30 M
2. 0.13 M
3. 2.60 M
4. 1.00 M

Correct answer: 1.30 M

Solution

Using M = (10 * mass% * d)/M_molar = (10 * 13 * 0.98)/98 = 1.30 mol/L.

Related JEE Main Chemistry questions

• A 100 mL sample of a urea solution contains 6.02 × 10²⁰ molecules of urea. What is the molarity of the solution? (Take Avogadro constant, N_A = 6.02 × 10²³ mol^−1.)
• When 4.9 g of H2SO4 reacts with NaCl, the products formed are 6 g of sodium hydrogen sulphate and 1.825 g of HCl. What mass of NaCl was decomposed?
• Which of the following has the least mass?
• What amount of magnesium phosphate, Mg3(PO4)2, in moles is needed to provide 0.25 mole of oxygen atoms?
• Haemoglobin has 0.33% iron by mass. If its molecular mass is about 67200 and the atomic mass of iron is 56, how many iron atoms are present in a single haemoglobin molecule?
• For the reaction 2Al(s) + 6HCl(aq) → 2Al³+(aq) + 6Cl^−(aq) + 3H₂(g), which statement is correct?

⚔️ Practice JEE Main Chemistry free + battle 1v1 →