What is the molarity and molality of a 13 % solution (by weight) of sulphuric acid with a density of 1.02 g/mL ? To what volume should 100 mL of this solution be diluted in order to prepare a 1.5 N solution ?

Question

What is the molarity and molality of a 13 % solution (by weight) of sulphuric acid with a density of 1.02 g/mL ? To what volume should 100 mL of this solution be diluted in order to prepare a 1.5 N solution ? (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Let us consider 1.0 L of solution. Weight of solution = 1000 × 1.02 = 1020 g Weight of H2SO4 =1020 × (13/100) = 132.60 g Weight of H2O =1020-132.60=887.40 g ⇒ Molarity =(132.60/98)=1.353 M Molarity =(132.60/98) × (1000/887.40)=1.525 m Normality =2 × M =2.706 ⇒ 2.706 × 100 =1.5 V ⇒ V=180.40 mL

Q. What is the molarity and molality of a 13% solution (by weight) of sulphuric acid with a density of 1.02g/mL ? To what volume should 100mL of this solution be diluted in order to prepare a 1.5N solution ?

Let us consider 1.0L of solution. Weight of solution =1000×1.02=1020g Weight of H2​SO4​=1020×10013​=132.60g Weight of H2​O=1020−132.60=887.40g ⇒ Molarity =98132.60​=1.353M Molarity =98132.60​×887.401000​=1.525m Normality =2×M=2.706 ⇒2.706×100=1.5V ⇒V=180.40mL

Q. What is the molarity and molality of a $13%$ solution (by weight) of sulphuric acid with a density of $1.02 g / m L$ ? To what volume should $100 m L$ of this solution be diluted in order to prepare a $1.5 N$ solution ?