The Solubility of Gases in a Liquid

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  • 0:02 Introduction to Gas…
  • 1:26 What is Solubility?
  • 3:17 Effect of Pressure
  • 5:22 Effect of Temperature
  • 7:55 Lesson Summary
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Lesson Transcript
Instructor: Nicola McDougal

Nicky has taught a variety of chemistry courses at college level. Nicky has a PhD in Physical Chemistry.

In this video lesson, you will learn what solubility is and the factors that affect gas solubility. We will use real-life examples to illustrate the importance of understanding solubility. A quick quiz will then test our new knowledge.

Introduction to Gas Solubility

It is a hot summer day and you and your best friend each take out a cool can of soda from the refrigerator. As you open the can, you hear the reassuring fizz as it bubbles out a little. You both take a sip. Ah, that is good. Suddenly your mom calls you from outside; you're needed right away. You put your opened can on the counter and run out to her. However, your best friend, who aced her chemistry class, chooses to put her open can in the refrigerator before catching up with you.

It was a smart move to put the soda in the refrigerator, but do you know why? Let us see what happens. Two hours later you come back inside and you need a drink. You pick up the open can of the soda you left on the counter and take a gulp. Not only is it warm, but it is flat! All of the fizz, which of course you know is carbon dioxide, has gone.

Your best friend takes her open can out of the refrigerator, and she drinks some. Not only is it cold, as you would expect, but amazingly it is still fizzy! So, how can we explain this? Why is there still carbon dioxide left in the cold can of cola, but not in the warm can? It is all to do with the solubility of gases in a liquid.

What is Solubility

Before we move onto looking at gases specifically, let us briefly remind ourselves of some important terms. A solution is a homogenous mixture of substances. In other words, the solution is mixed in a uniform way. The substance that is dissolved is called the solute. The solute can be a liquid, a solid or a gas. The solvent is the substance that does the dissolving. The solvent is usually in excess, and can also be a gas, liquid or a solid.

Now, we come across solutions all the time in our daily lives. Take, for example, a cup of tea. Here, the solute is the tea and the water is the solvent - together they form a solution of tea. Another example of a solution is our can of soda. In this case, the solute is the carbon dioxide; this is dissolved in a solvent that is basically flavored water to make the solution, which is the soda.

Solubility is defined as the maximum amount of solute that dissolves in a given amount of solvent. When a solution contains the maximum amount of solute it is called saturated. Solubility is affected by three main factors:

  • Firstly, the nature of the solvent and solute particles and how they interact together
  • Secondly, the temperature
  • Thirdly, the pressure of a gaseous solute

In this lesson, we are going to focus on the solubility of gases in a liquid, so that covers our first factor, which was just the nature of the solvent and the solute. We will consider the effects of temperature and pressure in the next sections.

Effect of Pressure

Pressure has a major effect on the solubility of gas-liquid systems. At a constant temperature, raising the pressure increases the solubility of the gas. This occurs because increasing the gas pressure increases the concentration of gas molecules. To overcome this change and to maintain equilibrium, more gas molecules enter the liquid solution.

This property is used in the soda-making industry. Sodas are bottled and canned under very high pressure of carbon dioxide, often as high as four units of atmospheric pressure (or atm). Once the can or the bottle is open, the pressure above the can opening is just normal atmospheric pressure, which is one atm, four times lower than what is in the can. This then lowers the pressure inside the soda can. The carbon dioxide rapidly bubbles out of the soda solution. You see this effect when you first open your can of soda.

A serious consequence on the effect of pressure on gas solubility is the painful, sometimes deadly condition called the bends. Scuba divers have to be very careful when they come back to the surface after a deep dive. This is because deeper water is at higher pressure than surface water. As divers breathe, more gas is being dissolved in their blood and other fluids.

You already know that gases are less soluble at lower pressure. If divers come back up too quickly, the air that is dissolved in their blood bubbles out of solution. These bubbles can seriously affect blood circulation and nerve impulses. To help overcome this problem, deep sea divers breathe a helium-oxygen mixture rather than compressed air, which is a nitrogen-oxygen mixture. Helium is much less soluble than nitrogen and, therefore, less gas comes out of their blood when they come back to the surface of the water.

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