   Chapter 13.5, Problem 3.2ACP

Chapter
Section
Textbook Problem

At a depth of 20 meters the pressure is about 3.0 atm. Calculate the solubility of O2 in water under 3.0 atm pressure. Then, calculate the mass of oxygen that will dissolve in 1.0 L of water under this pressure.

Interpretation Introduction

Interpretation: The solubility of O2 in water and its mass, which dissolve in 1.0L of water under 3.0atm pressure has to be determined.

Concept introduction:

• Raoult’s law: the vapor pressure of a solvent above a solution (Psolution)is equal to the vapor pressure of the pure solvent(P0solvent ) at the same temperature scaled by the mole fraction of the solvent (XSolvent )present.

Psolution=Xsolvent×P0solvent

• Density=MassVolume
• Henry’s law: The solubility of a gas in liquid is directly proportional to the gas pressure.

Sg= kHPg,where,Sgisthegassolubility(inmol/kg)kHis Henry's constant Pg is the partial pressure of the gaseous solute.

Explanation

Given,Thetotalpresureis3.0atm,thenpartialpressureofO2is,partialpressureofO2 =XO2×(Ptotal) =0.2095(3.0atm)=0.629atm

Solubility of oxygen can be calculated by using Henry’s law.

SolubilityofO2=kHPg =(1.3×10-3mol/kg.bar)(0.629atm)(1bar/0.98692atm) =8

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