Class 12 Chemistry Notes: Solutions Chapter
Chapter 12: Solutions
1. Introduction:
- A solution is a homogeneous mixture of two or more substances.
- The substance present in a smaller amount is called the solute, and the substance present in a
larger amount is the solvent.
2. Types of Solutions:
- Solid in liquid (e.g., sugar in water).
- Gas in liquid (e.g., carbonated drinks).
- Liquid in liquid (e.g., alcohol in water).
3. Concentration Terms:
- Molarity (M): Moles of solute per liter of solution. M = moles of solute / volume of solution in liters.
- Molality (m): Moles of solute per kilogram of solvent. m = moles of solute / mass of solvent in kg.
- Mole Fraction: Ratio of moles of a component to the total moles of the solution.
- Mass Percent: Mass of solute divided by mass of solution multiplied by 100.
- Normality (N): Gram equivalent of solute per liter of solution.
4. Vapour Pressure of Solutions:
- Raoult's Law: For an ideal solution, the partial vapor pressure of each volatile component is
proportional to its mole fraction.
- Ideal Solutions: Solutions that obey Raoult's law over the entire range of concentration.
- Non-Ideal Solutions: Deviate from Raoult's law, showing either positive or negative deviations.
Chapter 12: Solutions
1. Introduction:
- A solution is a homogeneous mixture of two or more substances.
- The substance present in a smaller amount is called the solute, and the substance present in a
larger amount is the solvent.
2. Types of Solutions:
- Solid in liquid (e.g., sugar in water).
- Gas in liquid (e.g., carbonated drinks).
- Liquid in liquid (e.g., alcohol in water).
3. Concentration Terms:
- Molarity (M): Moles of solute per liter of solution. M = moles of solute / volume of solution in liters.
- Molality (m): Moles of solute per kilogram of solvent. m = moles of solute / mass of solvent in kg.
- Mole Fraction: Ratio of moles of a component to the total moles of the solution.
- Mass Percent: Mass of solute divided by mass of solution multiplied by 100.
- Normality (N): Gram equivalent of solute per liter of solution.
4. Vapour Pressure of Solutions:
- Raoult's Law: For an ideal solution, the partial vapor pressure of each volatile component is
proportional to its mole fraction.
- Ideal Solutions: Solutions that obey Raoult's law over the entire range of concentration.
- Non-Ideal Solutions: Deviate from Raoult's law, showing either positive or negative deviations.
