Henry’s law states that the solubility of a gas in a liquid is directly proportional to pressure of the gas keeping temperature constant.
Mathematically, P = KH x
x mole fraction of gas in solution
P is partial pressure of gas,
KH is Henry's constant.
Applications: Henry's law finds various applications in industry and enables us to explain and understand some biological phenomena. The some of important applications are: CO2 solubility in soft drinks, beverages, soda water etc. is increased by applying high pressure and bottles are sealed under high pressure.
Molarity (M) is defined as number of moles of solute dissolved in one litre (or one cubic decimetre) of solution.
(a) Mol. mass of
Volume of solution = 4.3 L
(b) Number of moles present in 1000 ml of 0.5M H2SO4= 0.5 mol
therefore number of moles present in 30ml of 0.5M H2SO4=mol =0.015mol
therefore molarity =0.015/0.5L
thus molarity is 0.03M
Molality (m) is defined as the number of moles of the solute per kilogram (kg) of the solvent and is expressed as:
Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density of 20% (mass/mass) aqueous KI is 1.202 g mL-1.