Question

influence so lubility of gases in liquid​

Answer 1

Answer:

The gas solubility in liquids is greatly affected by temperature and pressure as well as the nature of the solute and the solvent. 

Answer 2

For any substance, solubility is the maximum amount of solute that can be dissolved in a given solvent at a particular temperature. Now our concern is gas solubility in liquids. The gas solubility in liquids is greatly affected by temperature and pressure as well as the nature of the solute and the solvent.There are many gases that readily dissolve in water, while there are gases that do not dissolve in water under normal conditions. Oxygen is only sparingly soluble in water while HCl or ammonia readily dissolves in water.

Factors Affecting Solubility

1. Effect of Pressure: It has been found that the gas solubility in liquids increases with increase in pressure. To have a better understanding of the effect of pressure on gas solubility let us consider a system of a gas solution in a solvent in a closed container in a state of dynamic equilibrium. Now the solution is in equilibrium and hence the rate of gaseous molecules entering the solution is equal to the rate of gaseous molecules leaving the solution. Now suppose we increase the pressure of the system by compressing the gas molecules present in the solution. As a result of an increase in pressure, the gases molecules will now be concentrated in a smaller volume. This will result in an increase in the number of gas molecules per unit volume available above the solution. Since the number of gas molecules presents above the solution has increased, the rate with which the gas molecules will be entering the solution will also increase. The end result is an increase in the number of gas molecules in the solution until a new equilibrium point is attained. Thus the solubility of gases increases with an increase in the pressure of a gas above the solution.
2. The solubility of gases in liquids – Henry’s Law gives a quantitative relation between pressure and gas solubility in a liquid. It states that: The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas present above the surface of liquid or solution.

The most general way of using Henry’s Law is that the partial pressure of a gas above a solution is proportional to the mole fraction of the gas in the solution.

P = KHx

Where, p = partial pressure of the gas

x = mole fraction of the gas in solution KH = Henry’s law constant

Effect of Temperature:

Gas solubility in liquids is found to decrease with increase in temperature. The gas molecules in a liquid are dissolved by the process of dissolution. During this process, heat is evolved. According to Le Chatelier’s Principle which states that when the equilibrium of a system is disturbed, the system readjusts itself in such a way that the effect that has caused the change in equilibrium is countered. So, as we know that dissolution is an exothermic process, the solubility should decrease with an increase in temperature to validate Le Chatelier’s Principle.