Henry’s law states that the solubility of a gas in a liquid is directly proportional to pressure of the gas; temperature constant.
Mathematically, P = KH x
x=mole fraction of gas in solution
P is partial pressure of gas,
KH is Henry's constant.
(1) 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.
(2) For deep divers, oxygen diluted with less soluble He gas is used as breathing gas and it minimises the painful effects due to higher solubility of N2 gas in blood.
(3) In lungs, where oxygen is present in air with high partial pressure, haemoglobin combines with O2 to form oxyhaemoglobin. In tissues where partial pressure of O2 is low, oxyhaemoglobin releases the oxygen for utilisation in cellular activities.
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
Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride.
Let the total mass of the solution be 100g and mass of benzene be 30 g
therefore mass of tetrachloride= (100-30)g = 70g
Molar mass of benzene,
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.