JEE Mains and JEE Advanced

Colligative properties:

• Freezing point depression: (\Delta T_f = K_f * m)
• Boiling point elevation: (\Delta T_b = K_b * m)
• Osmotic pressure: (\pi = M R T)

where (K_f) and (K_b) are the freezing point depression and boiling point elevation constants, respectively, (m) is the molality of the solution, (M) is the molarity of the solution, (R) is the universal gas constant, and (T) is the temperature in Kelvin.

Raoult’s law and Henry’s law:

• Raoult’s law: (P_{\text{total}} = P_A + P_B)
• Henry’s law: (P = k [X])

Solubility and factors affecting it:

Solubility is the maximum amount of solute that can be dissolved in a solvent at a given temperature and pressure. Factors affecting solubility include:

• Temperature: Solubility usually increases with temperature.
• Pressure: Solubility of gases increases with pressure.
• Nature of solute and solvent: Polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes.

Types of solutions:

• Electrolytes: Solutions that conduct electricity.
• Non-electrolytes: Solutions that do not conduct electricity.
• Strong electrolytes: Electrolytes that completely dissociate into ions in solution.
• Weak electrolytes: Electrolytes that partially dissociate into ions in solution.
• Acid-base solutions: Solutions that contain acids and bases.
• Redox solutions: Solutions that contain oxidizing and reducing agents.

Solution stoichiometry:

Solution stoichiometry is used to determine the concentrations of reactants and products in a chemical reaction. It is based on the balanced chemical equation for the reaction and the initial concentrations of the reactants.

Redox reactions:

Redox reactions are chemical reactions that involve the transfer of electrons between atoms or molecules. Redox reactions can be identified by the presence of oxidation and reduction half-reactions.

Chemical equilibrium:

Chemical equilibrium is a state in which the concentrations of the reactants and products of a chemical reaction do not change over time. The equilibrium constant ((K_c)) for a reaction is a measure of the extent to which the reaction proceeds in the forward direction.

Le Chatelier’s principle:

Le Chatelier’s principle states that when a system at equilibrium is subjected to a stress, the system will shift in the direction that opposes the stress.

Solubility product:

The solubility product ((K_{sp})) of a compound is the product of the molar concentrations of its constituent ions raised to their stoichiometric coefficients in the equilibrium equation.

Common ion effect:

The common ion effect is the decrease in the solubility of a sparingly soluble salt when a solution containing a common ion is added to it.

CBSE board exams

Colligative properties:

Freezing point depression:

(\Delta T_f=K_f *m)

Boiling point elevation:

(\Delta T_b=K_b *m)

Raoult’s law:

(P_{\text{total}} = P_A + P_B) where:

(P_{\text{total}}) is the total vapor pressure of the solution (P_A) is the vapor pressure of the pure solvent (P_B) is the vapor pressure of the solute

Solubility and factors affecting it:

Solubility is the maximum amount of solute that can be dissolved in a solvent at a given temperature and pressure. Factors affecting solubility include:

• Temperature
• Pressure
• Nature of solvent
• Nature of solute

Types of solutions:

Electrolytes: Solutions that conduct electricity.

Non-electrolytes: Solutions that do not conduct electricity.

Solution stoichiometry:

Solution stoichiometry is used to determine the concentrations of reactants and products in a chemical reaction. It is based on the balanced chemical equation for the reaction and the initial concentrations of the reactants.

Redox reactions:

Redox reactions are chemical reactions involving the transfer of electrons between atoms or molecules. The main types of redox reactions include:

• Combination reactions: Two or more substances combine to form a single product.
• Decomposition reactions: A single substance breaks down into two or more products.
• Displacement reactions: One element replaces another element in a compound.
• Combustion reactions: A substance reacts with oxygen to produce heat and light.