NEET Chemistry Preparation (Raftaar 2.0)

Jul 21, 2024

NEET Chemistry Preparation (Raftaar 2.0)

Welcome and Introduction

  • Session: Raftaar 2.0 for NEET 2024
  • Subject: Class 12th Chemistry
  • Objective: Complete Class 12th Chemistry with high-yielding content
  • Expectation: ~55 marks in NEET 2024 Chemistry exam
  • Structure: One chapter per day, in-depth study
  • Addition: Inclusion of Previous Year Questions (PYQs) at the end of each class

Excitement for Raftaar 2.0

  • Promise: Students must follow through religiously
  • Goal: Achieve 160+ marks out of 180 in NEET Chemistry
  • Event: “Udbhav” on March 21st at 6 PM

Telegram Channel

  • Content: Notes, DPPs, short notes, tests available
  • Test Series: Free test series, Yalgaar test scheduled for March 24th

Class 12th Solutions Chapter

Binary Solutions

  • Components: Solvent (A), Solute (B)
  • Definition: Binary solutions have two components
  • Identification: Solute in lesser amount, solvent in more amount
  • Examples: Sugar in water, NaCl in water

Types of Solutions

  • Types: Gaseous, Liquid, Solid solutions based on the phase of the solvent

Concentration Terms

Percentage

  • % v/v: (Volume of solute / Volume of solution) * 100
  • % w/w: (Weight of solute / Weight of solution) * 100
  • % w/v: (Weight of solute / Volume of solution) * 100
  • Temperature Dependency: Volume-related terms are temperature-dependent

Molarity (M)

  • Formula: (Number of moles of solute / Volume of solution in liters)
  • Temperature Dependency: Volume-related, hence temperature-dependent

Molality (m)

  • Formula: (Number of moles of solute / Weight of solvent in kg)
  • Temperature Dependency: Mass-related, hence temperature-independent

Mole Fraction (X)

  • Definition: Ratio of moles of a component to total moles in the solution
  • Formula: XA = nA / (nA + nB), XB = nB / (nA + nB)
  • Sum: XA + XB = 1

Vapor Pressure

  • Concept: Pressure exerted by vapor in equilibrium with its liquid at a given temperature
  • Dependence: Depends on the nature of liquid and temperature, inversely proportional to intermolecular forces

Types of Substances

  • Volatile: Convert to vapor, ex. water, benzene
  • Non-Volatile: Do not easily vaporize, ex. urea, glucose

Raoult's Law

Non-Volatile Solute

  • Formula: Psolution = P₀A * XA
  • Effect: Adding non-volatile solute decreases vapor pressure

Volatile Solute

  • Formula: Ptotal = P₀A * XA + P₀B * XB
  • Effect: Both solute and solvent contribute to vapor pressure

Pressure in Solution (Dalton's Law)

  • Formula: Pa = Xa * Ptotal, Pb = Xb * Ptotal
  • Formula Transformation: Pa = P₀A * XA, Pb = P₀B * XB

Graphs

  • Double-axis graphs: Show ideal and non-ideal behaviors

Types of Solutions

  • Ideal Solution: Obeys Raoult's Law at all concentrations and temperatures
    • Interactions: ΔVA = ΔVB = ΔVAB
    • Key features: ΔVmix = 0, ΔHmix = 0
  • Non-Ideal Solution: Deviates from Raoult's Law
    • Positive Deviation: High vapor pressure, low intermolecular forces
    • Negative Deviation: Low vapor pressure, high intermolecular forces
    • Graphs: Respective deviations from ideal lines

Azeotropes

  • Definition: Mixtures with constant boiling points
  • Types: Minimum Boiling Azeotrope (positive deviation), Maximum Boiling Azeotrope (negative deviation)

Colligative Properties

  • Types: Relative lowering of vapor pressure, Elevation of boiling point, Depression of freezing point, Osmotic pressure
  • Key Characteristic: Depend on the number of solute particles

Van't Hoff Factor (i)

  • Definition: Ratio of particles in solution to original particles
  • Electrolytes: Cause dissociation (i > 1) or association (i < 1)
  • Formulas: Different for dissociation and association conditions

Important Formulas

  • Elev. Boiling Point: ΔTb = i * Kb * m
  • Dep. Freezing Point: ΔTf = i * Kf * m
  • Osmotic Pressure: π = i * CRT

Henry's Law

  • Equation: P = kH * Χ
  • Implication: Solubility is inversely proportional to Henry’s constant

Takeaways

  • Consistency: Follow the series religiously
  • Event: Join “Udbhav” on March 21st
  • Next Class: Chemical Kinetics on March 20th
  • Focus: Prioritize study over distractions for NEET 2024