Why is a gas less soluble in an aqueous solution of electrolytes than pure water? [closed]








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Please help me out! This was given as a fact in my textbook but I don't understand the logic behind it.




*Gist of the matter...*


When an ionic salt dissolves in water the ions and water molecules don't just bounce around independently. The ions have a charge and water molecules are polar. So the water molecules form a cluster, which is a number of concentric layers of water molecules, around the ions. A gas molecule dissolved in the water can't get into a cluster. Hence there is effectively less water in which the gas can dissolve. 


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