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100+ Free KSEAB II PUC Chemistry Practice Questions

Karnataka School Examination and Assessment Board II PUC Chemistry (Class 12 Pre-University, Subject Code 34) practice questions are available now; exam metadata is being verified.

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Key Facts: KSEAB II PUC Chemistry Exam

~3 h 15 min

Typical duration of the II PUC Chemistry theory paper under KSEAB (subject code 34)

Karnataka II PUC science theory paper scheduling practice / model papers

Code 34

KSEAB II PUC Chemistry subject code used on model and annual papers

Karnataka DPUE/KSEAB Chemistry subject coding

Theory + practical

Official assessment mixes objective/written theory with a practical component; this bank is an English MCQ study adaptation only

KSEAB II PUC Chemistry paper pattern

Fee via college

Examination fees are typically paid through the PU college under KSEAB/DPUE notifications (not a fixed chemistry-only marketplace price)

KSEAB/DPUE fee notification practice

Pass as notified

Pass criteria (including separate theory/practical rules) are as published by KSEAB/DPUE for the sitting

KSEAB/DPUE result and promotion circulars

100 FREE MCQs

Local practice bank size for concept and calculation drill (not the official item count)

OpenExamPrep practice bank

Free 100-question English MCQ study bank for KSEAB II PUC Chemistry (Class 12, code 34). Official exams are ~3 h 15 min theory plus practical; pass as notified with separate theory/practical rules; fee via college as notified by KSEAB/DPUE. Not an official full-format simulation. Sources: kseab.karnataka.gov.in, dpue-exam.karnataka.gov.in, and NCERT Class 12 Chemistry.

Sample KSEAB II PUC Chemistry Practice Questions

Try these sample questions to test your KSEAB II PUC Chemistry exam readiness. Each question includes a detailed explanation. Start the interactive quiz above for the full 100+ question experience with AI tutoring.

1Molarity of a solution is defined as the number of moles of solute per:
A.Litre of solution
B.Kilogram of solvent
C.Litre of solvent
D.Kilogram of solution
Explanation: Molarity (M) = moles of solute / volume of solution in litres. Molality uses kilograms of solvent.
2Which concentration unit does not change with temperature for a dilute solution of fixed composition?
A.Molarity
B.Normality
C.Molality
D.Formality expressed per litre of solution
Explanation: Molality is moles of solute per kilogram of solvent. Mass is temperature-independent, so molality does not change with T at fixed composition, unlike volume-based units.
3Raoult's law for a non-volatile solute states that the vapour pressure of the solvent in solution equals:
A.Mole fraction of solvent × vapour pressure of pure solvent
B.Mole fraction of solute × vapour pressure of pure solvent
C.Mole fraction of solvent × vapour pressure of pure solute
D.Total moles × vapour pressure of pure solvent
Explanation: For a non-volatile solute, p_solvent = x_solvent × p°_solvent (Raoult's law).
4Colligative properties of dilute solutions depend primarily on the:
A.Number of solute particles, not their chemical identity
B.Chemical nature of the solute only
C.Colour of the solution
D.Molecular mass of the solvent only
Explanation: Colligative properties (relative vapour-pressure lowering, ΔTb, ΔTf, osmotic pressure) depend on the concentration of solute particles, not on their chemical identity (ideal dilute limit).
5A solution is prepared by dissolving 5.85 g of NaCl (M = 58.5 g mol^-1) in water to make 500 mL of solution. Its molarity is:
A.0.10 M
B.0.20 M
C.0.50 M
D.1.0 M
Explanation: n(NaCl) = 5.85/58.5 = 0.10 mol; V = 0.500 L; M = 0.10/0.500 = 0.20 M.
6The relative lowering of vapour pressure of a dilute solution of a non-volatile solute equals:
A.Mole fraction of the solute
B.Mole fraction of the solvent
C.Molality of the solution
D.Molarity of the solution
Explanation: For ideal dilute solutions, (p° − p)/p° = x_solute.
7The elevation of boiling point of a solution is given by ΔTb = Kb · m · i. Here m stands for:
A.Molality of the solute
B.Molarity of the solute
C.Mass of solvent in grams
D.Mole fraction of solute
Explanation: In the colligative formula ΔTb = i Kb m, m is molality (mol kg^-1 solvent).
8A 0.1 m aqueous solution of a non-electrolyte freezes at −0.186 °C. If Kf(H2O) = 1.86 K kg mol^-1, the van't Hoff factor i is approximately:
A.1.0
B.0.1
C.2.0
D.0.5
Explanation: ΔTf = i Kf m ⇒ 0.186 = i × 1.86 × 0.1 ⇒ i = 0.186/0.186 = 1.0 for a non-electrolyte.
9Osmotic pressure π of a dilute solution is given by π = cRT (van't Hoff), where c is:
A.Molar concentration of solute particles (mol L^-1)
B.Molality only
C.Mole fraction of solvent
D.Density of the solution
Explanation: In the van't Hoff equation π = cRT, c is molar concentration (often written as moles of particles per litre for electrolytes with i).
10Compared with pure water, the vapour pressure of a 1 m aqueous glucose solution is:
A.Lower
B.Higher
C.The same
D.Zero
Explanation: A non-volatile solute lowers the solvent vapour pressure (Raoult's law).

About the KSEAB II PUC Chemistry Practice Questions

Verified exam format metadata for Karnataka School Examination and Assessment Board II PUC Chemistry (Class 12 Pre-University, Subject Code 34) is pending. The practice questions above remain available while official exam length, timing, passing score, fee, and administrator details are reviewed.