Chemistry: Solutions - Lecture 1 | CHEMCA

Class 12 / JEE / NEET Chapter 1

Chemistry - Solutions | Lecture 1

By Abhishek Sengar

Lecture Chapters

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Theory & Quick Notes

1 What is a Solution?

A solution is defined as the homogeneous mixture of two or more components. "Homogeneous" means that the composition and properties are uniform throughout the mixture (e.g., salt completely dissolved in water).

Solvent

The component usually present in a higher amount. The physical state of the final solution is identical to the physical state of the solvent.

Solute

The component usually present in a lower amount. A single solution can contain one or more solutes.

2 Concentration Terms

Temp Dependent

Molarity (M)

Number of moles of solute present in 1 Liter of solution.

M = moles of solute / V_solution(L)

Temp Independent

Molality (m)

Number of moles of solute present in 1 kg of solvent.

m = moles of solute / Mass_solvent(kg)

Mole Fraction (χ)

Ratio of moles of a specific component to the total number of moles in the solution. Sum of all fractions equals 1.

χ_A = n_A / (n_A + n_B)

Parts Per Million (ppm)

Used for extremely dilute solutions, such as measuring pollutants in air or water.

ppm = (Mass_solute / Mass_solution) × 10⁶

3 Vital Formulas & Rules

Dilution Equation: Upon adding solvent, moles remain constant: M₁V₁ = M₂V₂
Mixing Solutions: Mixing two solutions of the same solute: M₃ = (M₁V₁ + M₂V₂) / (V₁ + V₂)
Temperature Dependence Rule: Any concentration term containing Volume (like Molarity, %v/v) changes with temperature. Terms based on mass/moles (Molality, Mole Fraction) do not.

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