An ideal-dilute solution of chloroform and ethanol with a mole fraction of ethanol in the liquid phase χEtOH=0.9900 has a total vapor pressure of 177.95 torr. The vapor pressure of pure ethanol at this temperature is P*EtOH=172.76 torr. a. Calculate the partial pressures of ethanol and chloroform in the vapor phase. b. Calculate the mole fractions of chloroform and ethanol in the vapor phase. c. Calculate the Henry’s law constant for chloroform, KCHCl3, at this temperature

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.