Revision Notes: Solutions | Chemistry for JEE Main & Advanced PDF Download

 Page 1


Solutions 
 
? Mixture  
1. Mixtures refer to those substances which consist of two or more elements or compounds, 
mixed together in any ratio and do not give rise to new compound. For example: sea water, 
air, chocolate milk etc. 
2. Mixture is composed of two or more substances mixed together in any ratio i.e. the 
composition is variable and do not possess properties like fixed melting or boiling point. 
3. Mixture shows the properties similar to that of its constituents and they can be separated 
by using physical and chemical methods. 
4. There are two types of mixtures: 
i. Homogeneous mixtures: Such mixtures have only one phase. They have the same 
composition throughout and there is no visible separation of line between the constituents. 
For example: sugar solution, vinegar etc. 
 
ii. Heterogeneous mixture: Mixtures which has more than one phase is known as 
heterogeneous mixture. There is a visible boundary of separation between the components 
and they do not have the same composition throughout. 
5. Homogeneous mixtures are of three types: (i) Solid homogeneous mixture (alloys), (ii) 
Liquid homogeneous mixture (solution of alcohol in water) and (iii) Gaseous homogeneous 
mixture (air). 
6. Heterogeneous mixtures are of three types: (i) Solid heterogeneous mixture (mixture of 
sand and sugar), (ii) Solid-liquid heterogeneous mixture (solution of chalk in water) and 
(iii) Gaseous heterogeneous mixture (smoke in air). 
? Substance – Cannot be separated into its constituent particles by any physical process 
? Solution – Homogeneous mixture of two or more substances  
? Alloys – Homogeneous mixture of metals 
Page 2


Solutions 
 
? Mixture  
1. Mixtures refer to those substances which consist of two or more elements or compounds, 
mixed together in any ratio and do not give rise to new compound. For example: sea water, 
air, chocolate milk etc. 
2. Mixture is composed of two or more substances mixed together in any ratio i.e. the 
composition is variable and do not possess properties like fixed melting or boiling point. 
3. Mixture shows the properties similar to that of its constituents and they can be separated 
by using physical and chemical methods. 
4. There are two types of mixtures: 
i. Homogeneous mixtures: Such mixtures have only one phase. They have the same 
composition throughout and there is no visible separation of line between the constituents. 
For example: sugar solution, vinegar etc. 
 
ii. Heterogeneous mixture: Mixtures which has more than one phase is known as 
heterogeneous mixture. There is a visible boundary of separation between the components 
and they do not have the same composition throughout. 
5. Homogeneous mixtures are of three types: (i) Solid homogeneous mixture (alloys), (ii) 
Liquid homogeneous mixture (solution of alcohol in water) and (iii) Gaseous homogeneous 
mixture (air). 
6. Heterogeneous mixtures are of three types: (i) Solid heterogeneous mixture (mixture of 
sand and sugar), (ii) Solid-liquid heterogeneous mixture (solution of chalk in water) and 
(iii) Gaseous heterogeneous mixture (smoke in air). 
? Substance – Cannot be separated into its constituent particles by any physical process 
? Solution – Homogeneous mixture of two or more substances  
? Alloys – Homogeneous mixture of metals 
? Solution: 
 
o The component of the solution that dissolves the other component in it is called solvent 
(present in larger amount). 
o The component of the solution that is dissolved in the solvent is called solute (present in 
lesser quantity). 
 
? Properties of solution: 
 
o Homogeneous mixture 
o Particles are extremely small, not visible to the naked eye 
o Light path not visible 
o Solute particles cannot be separated by filtration 
Solubility: Solubility of a substance is the maximum amount of the substance that can be 
dissolved in a specified amount of a solvent at a specified temperature. 
 
? Solubility of a solid in a liquid: 
 
-Effect of temperature (Le Chatelier’s principle) – 
 
When the dissolution process is endothermic, the solubility will increase with increase in 
temperature. 
 
When the dissolution process is exothermic, the solubility will decrease with increase in 
temperature. 
 
-Effect of pressure: Pressure does not affect solubility. 
 
? Solubility of a gas in a liquid: 
 
Henry’s law ? The solubility of a gas in a liquid is directly proportional to the pressure of 
the gas. 
Or 
The partial pressure of a gas in vapour phase (p) is proportional to the mole fraction of the 
gas (x) in the solution. 
 
Where, KH ? Henry’s law constant 
 
? Some applications of Henry’s law – 
-The solubility of CO2 in soft drinks and soda water is increased by sealing the bottles under 
high pressure. 
-At high pressure underwater, scuba divers have to cope with high concentrations of 
dissolved gases while breathing air. 
-At high altitudes, climbers become weak and are unable to think clearly, which are 
symptoms of a condition called anoxia 
Page 3


Solutions 
 
? Mixture  
1. Mixtures refer to those substances which consist of two or more elements or compounds, 
mixed together in any ratio and do not give rise to new compound. For example: sea water, 
air, chocolate milk etc. 
2. Mixture is composed of two or more substances mixed together in any ratio i.e. the 
composition is variable and do not possess properties like fixed melting or boiling point. 
3. Mixture shows the properties similar to that of its constituents and they can be separated 
by using physical and chemical methods. 
4. There are two types of mixtures: 
i. Homogeneous mixtures: Such mixtures have only one phase. They have the same 
composition throughout and there is no visible separation of line between the constituents. 
For example: sugar solution, vinegar etc. 
 
ii. Heterogeneous mixture: Mixtures which has more than one phase is known as 
heterogeneous mixture. There is a visible boundary of separation between the components 
and they do not have the same composition throughout. 
5. Homogeneous mixtures are of three types: (i) Solid homogeneous mixture (alloys), (ii) 
Liquid homogeneous mixture (solution of alcohol in water) and (iii) Gaseous homogeneous 
mixture (air). 
6. Heterogeneous mixtures are of three types: (i) Solid heterogeneous mixture (mixture of 
sand and sugar), (ii) Solid-liquid heterogeneous mixture (solution of chalk in water) and 
(iii) Gaseous heterogeneous mixture (smoke in air). 
? Substance – Cannot be separated into its constituent particles by any physical process 
? Solution – Homogeneous mixture of two or more substances  
? Alloys – Homogeneous mixture of metals 
? Solution: 
 
o The component of the solution that dissolves the other component in it is called solvent 
(present in larger amount). 
o The component of the solution that is dissolved in the solvent is called solute (present in 
lesser quantity). 
 
? Properties of solution: 
 
o Homogeneous mixture 
o Particles are extremely small, not visible to the naked eye 
o Light path not visible 
o Solute particles cannot be separated by filtration 
Solubility: Solubility of a substance is the maximum amount of the substance that can be 
dissolved in a specified amount of a solvent at a specified temperature. 
 
? Solubility of a solid in a liquid: 
 
-Effect of temperature (Le Chatelier’s principle) – 
 
When the dissolution process is endothermic, the solubility will increase with increase in 
temperature. 
 
When the dissolution process is exothermic, the solubility will decrease with increase in 
temperature. 
 
-Effect of pressure: Pressure does not affect solubility. 
 
? Solubility of a gas in a liquid: 
 
Henry’s law ? The solubility of a gas in a liquid is directly proportional to the pressure of 
the gas. 
Or 
The partial pressure of a gas in vapour phase (p) is proportional to the mole fraction of the 
gas (x) in the solution. 
 
Where, KH ? Henry’s law constant 
 
? Some applications of Henry’s law – 
-The solubility of CO2 in soft drinks and soda water is increased by sealing the bottles under 
high pressure. 
-At high pressure underwater, scuba divers have to cope with high concentrations of 
dissolved gases while breathing air. 
-At high altitudes, climbers become weak and are unable to think clearly, which are 
symptoms of a condition called anoxia 
Effect of temperature – 
 
With increase in temperature, the solubility of gases in liquids decreases. 
 
Vapour pressure of liquid solutions: 
 
? Vapour pressure of liquid–liquid solutions: 
 
? Raoult’s law ? For a solution of volatile liquids, the partial vapour pressure of each 
component in the solution is directly proportional to its mole fraction. 
 
 
 
 
 
(For an ideal solution at constant temperature) 
 
? Vapour pressure of solutions of solids in liquids: 
 
  
Ideal and non-ideal solutions: 
 
? Ideal solutions – 
Solutions which obey Raoult’s law over the entire range of concentrations 
 
 
-In an ideal solution, the solute–solute and solvent–solvent interactions are nearly equal to 
the solute–solvent interactions. 
 
? Non-ideal solutions – Solutions which do not obey Raoult’s law over the entire range of 
concentrations 
Page 4


Solutions 
 
? Mixture  
1. Mixtures refer to those substances which consist of two or more elements or compounds, 
mixed together in any ratio and do not give rise to new compound. For example: sea water, 
air, chocolate milk etc. 
2. Mixture is composed of two or more substances mixed together in any ratio i.e. the 
composition is variable and do not possess properties like fixed melting or boiling point. 
3. Mixture shows the properties similar to that of its constituents and they can be separated 
by using physical and chemical methods. 
4. There are two types of mixtures: 
i. Homogeneous mixtures: Such mixtures have only one phase. They have the same 
composition throughout and there is no visible separation of line between the constituents. 
For example: sugar solution, vinegar etc. 
 
ii. Heterogeneous mixture: Mixtures which has more than one phase is known as 
heterogeneous mixture. There is a visible boundary of separation between the components 
and they do not have the same composition throughout. 
5. Homogeneous mixtures are of three types: (i) Solid homogeneous mixture (alloys), (ii) 
Liquid homogeneous mixture (solution of alcohol in water) and (iii) Gaseous homogeneous 
mixture (air). 
6. Heterogeneous mixtures are of three types: (i) Solid heterogeneous mixture (mixture of 
sand and sugar), (ii) Solid-liquid heterogeneous mixture (solution of chalk in water) and 
(iii) Gaseous heterogeneous mixture (smoke in air). 
? Substance – Cannot be separated into its constituent particles by any physical process 
? Solution – Homogeneous mixture of two or more substances  
? Alloys – Homogeneous mixture of metals 
? Solution: 
 
o The component of the solution that dissolves the other component in it is called solvent 
(present in larger amount). 
o The component of the solution that is dissolved in the solvent is called solute (present in 
lesser quantity). 
 
? Properties of solution: 
 
o Homogeneous mixture 
o Particles are extremely small, not visible to the naked eye 
o Light path not visible 
o Solute particles cannot be separated by filtration 
Solubility: Solubility of a substance is the maximum amount of the substance that can be 
dissolved in a specified amount of a solvent at a specified temperature. 
 
? Solubility of a solid in a liquid: 
 
-Effect of temperature (Le Chatelier’s principle) – 
 
When the dissolution process is endothermic, the solubility will increase with increase in 
temperature. 
 
When the dissolution process is exothermic, the solubility will decrease with increase in 
temperature. 
 
-Effect of pressure: Pressure does not affect solubility. 
 
? Solubility of a gas in a liquid: 
 
Henry’s law ? The solubility of a gas in a liquid is directly proportional to the pressure of 
the gas. 
Or 
The partial pressure of a gas in vapour phase (p) is proportional to the mole fraction of the 
gas (x) in the solution. 
 
Where, KH ? Henry’s law constant 
 
? Some applications of Henry’s law – 
-The solubility of CO2 in soft drinks and soda water is increased by sealing the bottles under 
high pressure. 
-At high pressure underwater, scuba divers have to cope with high concentrations of 
dissolved gases while breathing air. 
-At high altitudes, climbers become weak and are unable to think clearly, which are 
symptoms of a condition called anoxia 
Effect of temperature – 
 
With increase in temperature, the solubility of gases in liquids decreases. 
 
Vapour pressure of liquid solutions: 
 
? Vapour pressure of liquid–liquid solutions: 
 
? Raoult’s law ? For a solution of volatile liquids, the partial vapour pressure of each 
component in the solution is directly proportional to its mole fraction. 
 
 
 
 
 
(For an ideal solution at constant temperature) 
 
? Vapour pressure of solutions of solids in liquids: 
 
  
Ideal and non-ideal solutions: 
 
? Ideal solutions – 
Solutions which obey Raoult’s law over the entire range of concentrations 
 
 
-In an ideal solution, the solute–solute and solvent–solvent interactions are nearly equal to 
the solute–solvent interactions. 
 
? Non-ideal solutions – Solutions which do not obey Raoult’s law over the entire range of 
concentrations 
-Positive deviation from Raoult’s law – 
 
-Vapour pressure of the solution is higher than that predicted by Raoult’s law. 
-Solute–solvent interactions are weaker than solute–solute and solvent–solvent 
interactions. 
 
-Negative deviation from Raoult’s law – 
 
-Vapour pressure of the solution is lower than that predicted by Raoult’s law. 
-Solute–solute and solvent–solvent interactions are weaker than solute–solvent 
interactions. 
          
(For a two-component solution showing positive deviation from Raoult’s law) 
   
Page 5


Solutions 
 
? Mixture  
1. Mixtures refer to those substances which consist of two or more elements or compounds, 
mixed together in any ratio and do not give rise to new compound. For example: sea water, 
air, chocolate milk etc. 
2. Mixture is composed of two or more substances mixed together in any ratio i.e. the 
composition is variable and do not possess properties like fixed melting or boiling point. 
3. Mixture shows the properties similar to that of its constituents and they can be separated 
by using physical and chemical methods. 
4. There are two types of mixtures: 
i. Homogeneous mixtures: Such mixtures have only one phase. They have the same 
composition throughout and there is no visible separation of line between the constituents. 
For example: sugar solution, vinegar etc. 
 
ii. Heterogeneous mixture: Mixtures which has more than one phase is known as 
heterogeneous mixture. There is a visible boundary of separation between the components 
and they do not have the same composition throughout. 
5. Homogeneous mixtures are of three types: (i) Solid homogeneous mixture (alloys), (ii) 
Liquid homogeneous mixture (solution of alcohol in water) and (iii) Gaseous homogeneous 
mixture (air). 
6. Heterogeneous mixtures are of three types: (i) Solid heterogeneous mixture (mixture of 
sand and sugar), (ii) Solid-liquid heterogeneous mixture (solution of chalk in water) and 
(iii) Gaseous heterogeneous mixture (smoke in air). 
? Substance – Cannot be separated into its constituent particles by any physical process 
? Solution – Homogeneous mixture of two or more substances  
? Alloys – Homogeneous mixture of metals 
? Solution: 
 
o The component of the solution that dissolves the other component in it is called solvent 
(present in larger amount). 
o The component of the solution that is dissolved in the solvent is called solute (present in 
lesser quantity). 
 
? Properties of solution: 
 
o Homogeneous mixture 
o Particles are extremely small, not visible to the naked eye 
o Light path not visible 
o Solute particles cannot be separated by filtration 
Solubility: Solubility of a substance is the maximum amount of the substance that can be 
dissolved in a specified amount of a solvent at a specified temperature. 
 
? Solubility of a solid in a liquid: 
 
-Effect of temperature (Le Chatelier’s principle) – 
 
When the dissolution process is endothermic, the solubility will increase with increase in 
temperature. 
 
When the dissolution process is exothermic, the solubility will decrease with increase in 
temperature. 
 
-Effect of pressure: Pressure does not affect solubility. 
 
? Solubility of a gas in a liquid: 
 
Henry’s law ? The solubility of a gas in a liquid is directly proportional to the pressure of 
the gas. 
Or 
The partial pressure of a gas in vapour phase (p) is proportional to the mole fraction of the 
gas (x) in the solution. 
 
Where, KH ? Henry’s law constant 
 
? Some applications of Henry’s law – 
-The solubility of CO2 in soft drinks and soda water is increased by sealing the bottles under 
high pressure. 
-At high pressure underwater, scuba divers have to cope with high concentrations of 
dissolved gases while breathing air. 
-At high altitudes, climbers become weak and are unable to think clearly, which are 
symptoms of a condition called anoxia 
Effect of temperature – 
 
With increase in temperature, the solubility of gases in liquids decreases. 
 
Vapour pressure of liquid solutions: 
 
? Vapour pressure of liquid–liquid solutions: 
 
? Raoult’s law ? For a solution of volatile liquids, the partial vapour pressure of each 
component in the solution is directly proportional to its mole fraction. 
 
 
 
 
 
(For an ideal solution at constant temperature) 
 
? Vapour pressure of solutions of solids in liquids: 
 
  
Ideal and non-ideal solutions: 
 
? Ideal solutions – 
Solutions which obey Raoult’s law over the entire range of concentrations 
 
 
-In an ideal solution, the solute–solute and solvent–solvent interactions are nearly equal to 
the solute–solvent interactions. 
 
? Non-ideal solutions – Solutions which do not obey Raoult’s law over the entire range of 
concentrations 
-Positive deviation from Raoult’s law – 
 
-Vapour pressure of the solution is higher than that predicted by Raoult’s law. 
-Solute–solvent interactions are weaker than solute–solute and solvent–solvent 
interactions. 
 
-Negative deviation from Raoult’s law – 
 
-Vapour pressure of the solution is lower than that predicted by Raoult’s law. 
-Solute–solute and solvent–solvent interactions are weaker than solute–solvent 
interactions. 
          
(For a two-component solution showing positive deviation from Raoult’s law) 
   
(For a two-component solution showing negative deviation from Raoult’s law) 
 
Colligative properties and determination of molar mass: 
 
? Relative lowering of vapour pressure: 
 
? Relative lowering of vapour pressure is equal to the mole fraction of the solute. 
i.e.,  
However,  
Where, n2 = Number of moles of solute 
n1 = Number of moles of solvent 
Now,  
For dilute solution, n1 >> n2 
Therefore,  
Or,  
Or,  
 
? Elevation of boiling point: 
 
 
? Here, = Elevation of boiling point 
Where,