Dalton, a
contemporary of Henry, also
concluded independently that the
solubility of a gas in a liquid
solution is a function of partial
pressure of the gas If we use the mole fraction of a gas in
the solution as a measure of its solubility, then it can be
said that the mole fraction of gas in the solution is
proportional to the partial pressure of the gas over
the solution The most commonly used form of Henry’s
law states that “the partial pressure of the gas in
vapour phase (p) is proportional to the mole fraction
of the gas (x) in the solution” and is expressed as:
p = KH x
(1 11)
Here KH is the Henry’s law constant