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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
📄
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