Solubility is the process or property of a matter (Solid, liquid, or gas) which helps them dissolve in another matter called solvent (Solid, liquid, or gas). Therefore, a matter is called soluble if it dissolves in a solvent. For instance, take a small amount of salt and dissolve it in water. Here, salt is known as a solute, and water is a solvent to make a solution of saltwater. Therefore, you can say salt is soluble in water and solubility is the property of salt (or solute).
Further, there are several factors affecting solubility depending upon which state this solute is in. Read on to know more about the various factors which affect the solubility property of solutes present in various states.
Here, the solvent is taken as a liquid, and the solute will be taken for all three states to help you understand these factors that affect solubility.
Liquid as solvent.
Solids as solvent.
Gases as solvent.
Read further to learn in details about the 3 factors that affect solubility.
Solubility is the property of a solvent which can be described as the bond formation between a solvent and solute. In other words, you can describe solubility as the maximum solute concentration, which is to be dissolved in this given value of solvent concentration at a known temperature.
Based upon this property, any solvent can be categorised into three types –
Highly soluble substance: If 0.1 g of solute is capable of dissolving in a 100g of solvent, then it falls into the highly soluble category.
Sparingly or partially soluble substance: If less than 0.1 g of solute is capable of dissolving in a 100g of solvent, then it falls into the sparingly soluble category.
Insoluble: Understandably, this solute cannot be dissolved into a solvent.
While this proves solubility as a quantitative expression, there are several factors affecting the solubility.
Chemical and physical properties of the solute affect its solubility. Here are some significant factors which affect the solubility property.
It affects solutes in their gaseous state more than the ones in a solid or liquid state. The solubility property of a gas is said to increase with the increase in partial pressure of the gas. You can think of a soda bottle as an example. Here, carbon-di-oxide is bottled under a condition of high pressure.
Water is called the universal solvent and can dissolve most of the solutes at a temperature of 200C or 1000C. In the case of sparingly soluble substances which are liquid, the solubility increases with upsurge in temperature. In the case of gases, the solubility declines with a rise in temperature of the solvent.
Bonds and forces
The bonds and forces between these molecules of solute are one of the factors affecting solubility. Since the kind of bonds and intermolecular forces between two substances vary, the solute is known to be more soluble if it is dissolved in a likewise solvent. For instance, you can dissolve Ethanol (a polar solute) easily into a polar solvent such as water.
It is seen that if the solute is a similar kind to that of solvent, it is soluble in nature. For instance, you can easily dissolve salt, sugar, or ethanol in the water where all these are polar solute and solvent. However, it is rather challenging to dissolve a nonpolar solute like naphthalene into water.
Crystallisation – When you add a solid solute into a given concentration of this liquid solvent, the particles (solid) gets dissolved in the solution. This process is termed as dissolution. Crystallisation occurs when the particles of solute collide with the particles present in solution, and some of it separates from the solution.
Subsequently, a dynamic equilibrium state will be achieved when the number of solute molecules entering a solution becomes equal to the number of molecules leaving it. Further, there can be a situation wherein you cannot add more solute to the solution as it will not be dissolved. In such a case, you have reached saturation, and the solution is known as a saturated solution.
Therefore, solubility can be defined as the solute concentration present in this solution at saturation for a known value of temperature and pressure. Further addition of solute in this solution turns it into an unsaturated solution with extra undissolved solute.
Since solids are highly incompressible in nature and small change in pressure have nearly no impact on it, the solubility factors like pressure do not cause many changes.
As per Le Chatelier’s Principle, the solubility of a solvent should increase if the process of dissolution is endothermic. On the contrary, solubility decreases if this dissolution process turns out to be exothermic.
If Gases as a solute needs to be dissolved in a solvent, there are factors influencing solubility, such as temperature, nature of solvent and solute, and pressure. There can be several gas solutes which can readily dissolve in solvent whereas few gas solutes which do not dissolve under normal conditions.
For instance, you can easily dissolve ammonia or HCl into the water, but oxygen acts as a sparingly soluble substance for water.
As there is a rise in temperature, the solubility of a gas solute in liquids must increase. This can be inferred from Le Chatelier's Principle. As per this principle, the system readjusts itself whenever a state of equilibrium is disturbed.
Now, gas molecules are dissolved in liquid with the help of the dissolution process, which is an exothermic process. In an exothermic process, heat is evolved, which causes a change in the equilibrium state. Therefore, to readjust the system and validate the principle of Le Chateliers, increase in temperature of the solution should decrease the solubility. Hence, the temperature is one of the 4 factors that affect solubility.
As per the experiments and observation, the pressure increase is likely to cause an increase in solubility of gases. To better understand the things that affect solubility (In this case, Pressure), consider a closed cylinder in a dynamic equilibrium state with gas as solute and liquid as a solvent. Therefore, the number of molecules entering a solution must be equal to the number of molecules leaving that solution at dynamic equilibrium state.
Now consider increasing the amount of pressure applied to the system. This results in compressing gas molecules of this solution, which causes them to concentrate in a small volume.
Therefore, with the increase in pressure, this concentration of gas molecules present per unit volume above the solution is increased. Resultantly, this rate with which number of molecules enters the solution will also increase. Consequently, this number of gas (solute) molecules in a solution will also increase unless the solution undergoes into a new dynamic equilibrium state.
Hence, you can infer that pressure increment of this solute can cause an increase in the solubility of solutes or gases. So, pressure is one of the factors that affect the rate of solubility significantly.
According to Henry’s law, the solubility of solute or gas in a liquid solvent is proportional to the pressure applied to the gas above the liquid solution’s surface.
It provides the quantitative relation between solubility of gas and pressure of gas as expressed in the equation below –
P = KHX
P is the partial pressure of solute /gas.
KH is Henry’s law constant.
X indicates the mole fraction of gas in a liquid solution.
These are a few factors affecting the solubility of substances. You can increase or decrease factors like pressure, temperature, bonds, and forces to increase or decrease the solubility rate of elements.
Reading this, you will be able to cover which factors affect solubility and how it affects the entire process of dissolution. For a comprehensive approach, you can download Vedantu’s app and refer to the study material there. Learn the intricacies of the chapter with quality notes prepared by professional tutors and improve your academic score.
1. What is a Saturated Solution?
Ans. A saturated solution is said to be one that has the maximum amount of solute dissolved in it beyond which adding solute is not possible.
2. What is Le Chatelier's Principle?
Ans. Often known as ‘The equilibrium law’, it states that any changes in pressure, temperature, concentration, or volume of a system at equilibrium will be followed by opposing changes to attain a new equilibrium state.
3. What do you Understand by Solubility Limit?
Ans. Solubility limit is the maximum amount of solute that can be added unto a solution for a given temperature, pressure and concentration of solution so that it dissolves.
4. What are the 4 Factors Affecting Solubility?
Ans: The different factors affecting solubility can be pressure, temperature, polarity, bonds and forces. There can be varying effects depending upon the state of solute.