Dissolution is the process where a solute in gaseous, liquid, or solid phase dissolves in a solvent to form a solution.
Solubility is the maximum concentration of a solute that can dissolve in a solvent at a given temperature. At the maximum concentration of solute, the solution is said to be saturated. The units of solubility can be provided in mol/L or g/L.
Factors that affect solubility include:
The rate of dissolution is represented by the Noyes-Whitney equation: dm/dt = D*A*(Cs - C)/h
Effect of temperature on liquid and solid solutes
As temperature increases, the solubility of a solid or liquid can increase or decrease depending on whether the dissolution reaction is exothermic or endothermic.
Increasing solubility with increasing temperature
Decreasing solubility with increasing temperature
Effect of temperature on gas solutes
A gas becomes less soluble as temperate increases. This is because in general heat energy is released as gas dissolves in solution i.e. the process is exothermic.
Increasing temperature (increased heat energy) results in increased kinetic energy. This increase in kinetic energy allows greater movement of the gas particles resulting in the intermolecular bonds between the gas solute and solvent being broken.
Pressure: Henry’s Law
The solubility of gas is affected by changes in pressure on the system. A gas dissolves in liquids to form solutions. This results in equilibrium in the system where a proportion of gas molecules is dissolved in liquid while a proportion remains in the gas above the liquid.
Henry’s law states that: “At constant temperature, the amount of gas that dissolves in a volume of liquid is proportional to the partial pressure of the gas in equilibrium with the liquid.”
C = kP
Hence as the pressure of the gas above the liquid in the system increases, the gas molecules become more soluble in the solvent. Likewise, if the pressure of the gas in the system decreases, gas becomes less soluble in the solvent.
Limitations of Henry’s Law on gas solubility:
Le Chatelier’s principle:
If stress (e.g., pressure and heat) is applied to the equilibrium, the system will respond by adjusting to minimize the effects of this stress.
For example, if pressure is applied to a system, the dissolution reaction will respond to minimize this stress by reducing the pressure in the system.
Heat of solution
Solids and liquids are a result of individual particles being held together by inter-particulate bonds. To form a solution, energy is required to break the bonds between the particles within the solid or liquid. Heat energy is also required to break the bonds in a solvent to insert one of the molecules into solution. Hence these processes are endothermic. Heat energy is released when the solute molecules form bonds with the solvent molecules i.e. this process is exothermic.
Depending on whether more energy is used to break the bonds within the solute and solvent or is released when new bonds are formed between the solute and solvent, the reaction overall can be exothermic or endothermic.
The total amount of heat energy released or absorbed from the system = sum of heat energy absorbed when bonds are broken – the sum of heat energy released when bonds are formed
Example of Henry’s Law: Decompression Sickness
Henry’s Law explains the phenomena of decompression sickness. When scuba divers submerge themselves in deep water, the pressure in their body increases. This causes the nitrogen in their body to dissolve in their blood. Nitrogen is physiologically inert, so it is not used in tissue metabolism. If the scuba diver ascends to the surface too quickly, the sudden drop in pressure causes nitrogen bubbles to come out of solution and form painful and potentially fatal gas embolisms.
Dissolution is important for health practitioners because, for drugs to be absorbed and have a physiological effect in the human body, they must be in solution. For solid preparations, such as tablets and suppositories, the rate of dissolution affects how fast a drug is absorbed in the body.
Aqueous solubility is often considered when formulating drugs. Poorly soluble formulations provide difficulties in the development of pharmaceuticals. Chloramphenicol, phenytoin, and digoxin are some examples. Drugs, particularly those for oral administration, which have low aqueous solubility may have low bioavailability leading to insufficient exposure in the body causing the drug to be not as effective.
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