The molarity (in mol/liter) of a 13% solution (by weight) of sulphuric acid with a density of 1.02 g/mL is (Note: Report your answer in the required format by relevant rounding up.)

Step-by-step solution

13% solution of Sulfuric acid consists of 13 g of H 2 SO 4 and 87 g (100 g-13g) of water. The molarity is, M = number of moles volume = n V = ( given mass of H 2 SO 4 molar mass ) ( total mass of solution / density ) M = ( 13 g 98 g/mol ) ( 100 g/1 .02 g/mL ) = 0.133 mol 98 mL = 0.133 mol 0.098 L M = 1.357 mol/L ≃ 1.36