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  • 2024-02-06
  • Sanjay Bhandari
  • solutions-short-notes, solutions notes
  • 2929

Solutions Short Notes and Previous Year papers with solutions

Solutions short notes. solution chapter in chemistry class 12 notes pdf download the PDF file below Link:
Chemistry notes
Download Chemistry Short Notes

Solutions:

A perfectly homogeneous mixture of two or more components is called a solution.

Solute: The component which is present in a lesser amount or whose physical state is changed during the formation of the solution is called the solute.

Solvent: The component which is present in a larger amount and determines the physical state of the solution is called the solvent.

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Types of the solution: Depending upon the nature of solute and solvent, solutions are classified as follows:

Gaseous solutions: Solutions in which gas acts as a solvent are known as gaseous solutions.

Liquid solutions: Solutions in which liquids are present in larger amounts.

Solid solutions: Solutions in which solids are present in larger amounts.

Solubility: Maximum amount of substance that can be dissolved in a specified amount of solvent at a specified temperature is called its solubility.

Factors affecting solubility of a solid in a liquid:

Nature of solute and solvent: Polar solutes dissolve in polar solvents and non-polar solutes in non-polar solvents. (i.e., like dissolves like).

Effect of temperature:

– If the dissolution process is endothermic (DsolH > 0), the solubility increases with rise in temperature.

– If dissolution process is exothermic (DsolH < 0), the solubility decreases with rise in temperature.

Effect of pressure: Pressure does not have any significant effect on solubility of solids in liquids as these are highly incompressible.

Factors affecting solubility of a gas in a liquid:

Effect of pressure: Henry’s law states that “the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution” p = KH x where, KH is the Henry’s law constant and is different for different gases at a particular temperature.

Higher the value of KH at a given pressure, the lower is the solubility of the gas in the liquid.

Effect of temperature: As dissolution is an exothermic process, then according to Le Chatelier’s principle, the solubility should decrease with increase of temperature.

Raoult’s law: It states that for a solution of volatile liquids, the partial vapour pressure of each component of the solution is directly proportional to its mole fraction present in solution. p1 = p°1 x1 and p2 = p°2 x2 where p°1 and p°2 are vapour pressures of pure components 1 and 2 respectively, at the same temperature.

Dalton’s law of partial pressures:

Ptotal = p1 + p2 = x1 p1° + x2 p2°

= (1 – x2)p1° + x2 p2°

= p1° + (p2° – p1°)x2

If y1 and y2 are the mole fractions of the components 1 and 2 respectively in the vapour phase then, p1 = y1 Ptotal and p2 = y2 Ptotal

Raoult’s law for solid-liquid solutions: It states that relative lowering in vapour pressure of a solution containing a non-volatile solute is equal to the mole fraction of the solute.

p°− ps  /  p° = x2 where,

p° = vapour pressure of pure solvent

ps = vapour pressure of solution

x2 = mole fraction of solute.

Solution in short chart

Certainly! Here are some key formulas and concepts in solutions chemistry:

  1. Molarity (M): �=moles of solutevolume of solution in litersM=volume of solution in litersmoles of solute​

  2. Molality (m): �=moles of solutemass of solvent in kgm=mass of solvent in kgmoles of solute​

  3. Mass Percentage (% w/w): % �/�=mass of solutemass of solution×100%%w/w=mass of solutionmass of solute​×100%

  4. Volume Percentage (% v/v): % �/�=volume of solutevolume of solution×100%%v/v=volume of solutionvolume of solute​×100%

  5. Parts per Million (ppm): ppm=mass of solutemass of solution×106ppm=mass of solutionmass of solute​×106

  6. Dilution Equation: �1�1=�2�2M1​V1​=M2​V2​

  7. Colligative Properties: These depend only on the number of solute particles, not their identity. Examples include:

    • Boiling Point Elevation: Δ��=�×��×�ΔTb​=i×Kb​×m
    • Freezing Point Depression: Δ��=�×��×�ΔTf​=i×Kf​×m
    • Osmotic Pressure: �=�×�×�×�π=i×M×R×T
  8. Raoult's Law: �solution=�solvent×�solvent∗Psolution​=xsolvent​×Psolvent∗​

  9. Henry's Law: �=��×�P=kH​×c

  10. Solvation: Process of solvent molecules surrounding and interacting with solute particles.


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