Class 12 Chemistry - ODISHA
Solutions
The Chapter 'Solutions' in Class 12 Chemistry for Odisha BSE students explores homogeneous mixtures of two or more components. It covers types of solutions, methods of expressing concentration like molarity and molality, and solubility of gases and solids in liquids. A major focus is on liquid-liquid solutions, Raoult's Law for ideal and non-ideal solutions, and colligative properties which depend on the number of solute particles. Understanding abnormal molecular masses and Van 't Hoff factor is crucial. This chapter carries significant weightage in the board exams, frequently featuring numerical problems and conceptual reasoning questions about vapor pressure, boiling point elevation, and osmotic pressure.
Start Learning FreeKey Concepts
Concentration Terms
Ways to express the amount of solute in a solution, including Molarity, Molality, Mole Fraction, and Mass Percentage.
Henry's Law
States that the partial pressure of a gas in vapor phase is proportional to the mole fraction of the gas in the solution.
Raoult's Law
States that for a solution of volatile liquids, the partial vapor pressure of each component is directly proportional to its mole fraction.
Colligative Properties
Properties of solutions that depend only on the number of solute particles, such as lowering of vapor pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.
Van 't Hoff Factor
A factor 'i' used to account for the extent of association or dissociation of solutes in solution when calculating colligative properties.
Important Formulas
Board Exam Info
In the Odisha BSE (CHSE) Class 12 Chemistry board examination, the Solutions chapter typically carries around 5 to 7 marks. Questions usually consist of 1-mark objective questions, 2-mark short conceptual questions, and a mandatory 3 or 5-mark numerical problem based on colligative properties or concentration terms.
Frequently Asked Questions
What is the difference between molarity and molality?
Molarity is the number of moles of solute per liter of solution and changes with temperature. Molality is the number of moles of solute per kilogram of solvent and is independent of temperature.
Why do colligative properties depend on the number of solute particles?
Because they are physical properties of solutions that rely strictly on the collective presence of solute particles rather than their chemical identity, affecting the solvent's thermodynamic state.
What causes deviations from Raoult's Law?
Deviations occur due to differences in solute-solvent interactions compared to pure solute-solute and solvent-solvent interactions, leading to positive or negative deviations.
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