100+ Free UPMSP Intermediate Chemistry Practice Questions

Prepare for the Uttar Pradesh UPMSP Intermediate (Class 12) Chemistry — Code 152 exam with instant access — no signup required.

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2026 Statistics

Key Facts: UPMSP Intermediate Chemistry Exam

3h 15m

Duration of UPMSP Class 12 Chemistry theory board examination

UPMSP Official Syllabus

70 Marks

Maximum marks for the written theory question paper

UP Board Marking Scheme

30 Marks

Maximum marks for practical assessment and viva-voce

UPMSP Examination Guidelines

100 MCQs

Verified practice questions available in this question bank

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Prepare for UPMSP Class 12 Chemistry (Code 152) with 100 practice MCQs covering Physical Chemistry calculations, Coordination Chemistry, Organic mechanisms, and Biomolecules.

Sample UPMSP Intermediate Chemistry Practice Questions

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

1According to Raoult's law, for a solution of volatile liquids, the partial vapor pressure of each component in the solution is directly proportional to which quantity?

A.Its mole fraction in the liquid solution

B.Its molarity in the liquid solution

C.Its molality in the liquid solution

D.Its mass percentage in the liquid solution

Explanation: Raoult's law states that for a solution of volatile liquids, the partial vapor pressure of each volatile component in the solution is directly proportional to its mole fraction present in the liquid phase (p₁ = p₁° × x₁).

2When 1.00 g of a non-volatile solute is dissolved in 50.0 g of benzene, the freezing point of benzene is lowered by 0.40 K. If the molal freezing point depression constant (K_f) of benzene is 5.12 K kg mol⁻¹, what is the molar mass of the solute?

A.128 g mol⁻¹

B.256 g mol⁻¹

C.64 g mol⁻¹

D.512 g mol⁻¹

Explanation: Using the freezing point depression formula ΔT_f = K_f × m = K_f × (w_B × 1000) / (M_B × w_A), substitute the values: 0.40 = 5.12 × (1.00 × 1000) / (M_B × 50.0). Rearranging gives M_B = (5.12 × 1000) / (0.40 × 50.0) = 256 g mol⁻¹.

3What is the osmotic pressure exerted by a 0.05 M aqueous solution of glucose at 300 K? (Gas constant R = 0.0821 L atm K⁻¹ mol⁻¹)

A.0.615 atm

B.2.463 atm

C.1.231 atm

D.4.926 atm

Explanation: Osmotic pressure is given by π = CRT. Substituting C = 0.05 M, R = 0.0821 L atm K⁻¹ mol⁻¹ and T = 300 K gives π = 0.05 × 0.0821 × 300 = 1.2315 atm ≈ 1.231 atm.

4How does the Henry's law constant (K_H) of a gas in a liquid solvent change with an increase in temperature, and what is its effect on gas solubility?

A.K_H decreases with increasing temperature, and gas solubility increases

B.K_H remains unchanged, and gas solubility is independent of temperature

C.K_H decreases with increasing temperature, and gas solubility decreases

D.K_H increases with increasing temperature, and gas solubility decreases

Explanation: According to Henry's law (p = K_H × x), K_H increases with an increase in temperature. A higher K_H corresponds to lower gas solubility (x) at a given pressure, which is why aquatic species are more comfortable in cold water.

5A mixture of nitric acid (68%) and water (32%) forms a maximum boiling azeotrope at 393.5 K. What type of deviation from Raoult's law does this solution exhibit?

A.Negative deviation from Raoult's law because A-B interactions are stronger than A-A and B-B interactions

B.Positive deviation from Raoult's law because A-B interactions are weaker than A-A and B-B interactions

C.Zero deviation because it behaves as an ideal solution at the azeotropic composition

D.Positive deviation because the total vapor pressure of the solution is maximum

Explanation: Maximum boiling azeotropes are formed by non-ideal solutions showing large negative deviations from Raoult's law. In nitric acid and water mixture, strong solute-solvent (A-B) hydrogen bonding decreases total vapor pressure, elevating the boiling point above either component.

6A 0.1 M aqueous solution of potassium ferrocyanide, K₄[Fe(CN)₆], dissociates to give a van 't Hoff factor (i) of 4.60. What is the degree of dissociation (α) of the complex salt?

A.0.72

B.0.90

C.0.80

D.0.95

Explanation: Potassium ferrocyanide dissociates as K₄[Fe(CN)₆] → 4K⁺ + [Fe(CN)₆]⁴⁻, giving n = 5 ions. The degree of dissociation is α = (i − 1) / (n − 1) = (4.60 − 1) / (5 − 1) = 3.60 / 4 = 0.90, or 90%.

7The boiling point of pure water is 373.15 K. If 18 g of glucose (C₆H₁₂O₆) is dissolved in 1 kg of water, at what temperature will the solution boil? (K_b for water = 0.52 K kg mol⁻¹)

A.373.67 K

B.372.63 K

C.373.202 K

D.373.098 K

Explanation: Moles of glucose = 18 g / 180 g mol⁻¹ = 0.10 mol. Molality m = 0.10 mol / 1 kg = 0.10 m. Boiling point elevation ΔT_b = K_b × m = 0.52 × 0.10 = 0.052 K. Boiling point of the solution T_b = 373.15 + 0.052 = 373.202 K.

8Which of the following concentration units of a solution is independent of temperature changes?

A.Molarity (M)

B.Normality (N)

C.Formality (F)

D.Molality (m)

Explanation: Molality (m) measures the number of moles of solute per kilogram of solvent mass. Since mass is independent of temperature, molality does not change with temperature, unlike volume-dependent units such as molarity and normality.

9Benzoic acid (C₆H₅COOH) dissolved in benzene undergoes dimerisation to an extent of 100%. What is the theoretical van 't Hoff factor (i) for this solution?

A.0.5

B.1.0

C.2.0

D.1.5

Explanation: When benzoic acid dimerises completely (2 C₆H₅COOH ⇌ (C₆H₅COOH)₂), two molecules associate into one dimer particle. The van 't Hoff factor is i = 1 − α + α/n = 1 − 1 + 1/2 = 0.5.

10The vapor pressure of pure water at 298 K is 23.8 mm Hg. When 50 g of urea (NH₂CONH₂, M = 60 g mol⁻¹) is dissolved in 850 g of water, what is the relative lowering of vapor pressure?

A.0.035

B.0.017

C.0.052

D.0.009

Explanation: The relative lowering of vapor pressure (p° − p) / p° equals the mole fraction of the solute, n(urea) / [n(urea) + n(water)]. Moles of urea = 50/60 = 0.833 mol; moles of water = 850/18 = 47.22 mol. So x(urea) = 0.833 / (0.833 + 47.22) = 0.833 / 48.053 ≈ 0.0173 ≈ 0.017.

About the UPMSP Intermediate Chemistry Exam

The UPMSP Class 12 Chemistry (Code 152) examination evaluates students across Physical Chemistry (Solutions, Electrochemistry, Kinetics), Inorganic Chemistry (d & f block elements, Coordination Compounds), and Organic Chemistry (Haloalkanes, Alcohols, Aldehydes, Amines, Biomolecules). This 100-question practice test suite delivers comprehensive, syllabus-aligned multiple-choice questions complete with step-by-step numerical calculations, reaction mechanisms, and detailed option-by-option explanations to ensure high scoring performance in UP Board examinations.

Assessment

70-mark written theory board examination (3 hours 15 minutes) supplemented by a 30-mark practical examination. The question paper includes multiple-choice questions, short numerical problems, inorganic coordination chemistry concepts, and organic reaction mechanism questions.

Time Limit

3 hours 15 minutes (195 minutes)

Passing Score

33% aggregate pass mark (minimum 23 out of 70 in theory and 10 out of 30 in practicals)

Exam Fee

₹600.75 for institutional (regular) Intermediate candidates and ₹806 for private candidates for the 2026 examination, plus ₹206 per additional subject. UPMSP charges one registration fee per candidate, not per subject paper. (Uttar Pradesh Madhyamik Shiksha Parishad (UPMSP))

UPMSP Intermediate Chemistry Exam Content Outline

10%

Solutions

Concentration terms, Henry's law, Raoult's law, ideal and non-ideal solutions, colligative properties (elevation of boiling point, depression of freezing point, osmotic pressure), and van 't Hoff factor.

12%

Electrochemistry

Galvanic cells, Nernst equation, molar conductivity, Kohlrausch's law, electrolysis and Faraday's laws, cell EMF, free energy change, and commercial batteries.

10%

Chemical Kinetics

Rate of reaction, reaction order and molecularity, integrated rate laws for zero and first order, half-life calculations, Arrhenius equation, and collision theory.

10%

d- and f-Block Elements

Transition metal general properties, oxidation states, magnetic properties, colored ions, lanthanoid contraction, actinoids, and preparations/reactions of K2Cr2O7 and KMnO4.

10%

Coordination Compounds

IUPAC nomenclature, Werner's theory, valence bond theory (VBT), crystal field theory (CFT), structural and stereoisomerism, and biological importance of coordination compounds.

Haloalkanes and Haloarenes

Nomenclature, SN1 and SN2 substitution mechanisms, stereochemistry, Walden inversion, reactions of haloarenes, and environmental impact of polyhalogen compounds.

10%

Alcohols, Phenols and Ethers

Preparation methods, physical properties, acidic nature of phenols vs alcohols, hydration, dehydration mechanism, Reimer-Tiemann and Kolbe reactions, and Williamson synthesis.

12%

Aldehydes, Ketones and Carboxylic Acids

Nucleophilic addition mechanism, carbonyl reactivity, Aldol condensation, Cannizzaro reaction, Clemmensen and Wolff-Kishner reductions, Tollens and Fehling tests, and carboxylic acid acidity.

Amines

Basicity of aliphatic and aromatic amines, Gabriel phthalimide synthesis, Hoffmann bromamide reaction, Hinsberg test, and synthetic applications of diazonium salts.

10%

Biomolecules

Structure of D-glucose and fructose, mutarotation, reducing sugars, disaccharides and polysaccharides, amino acid zwitterions, peptide bond, protein structures, denaturation, DNA/RNA double helix, and vitamins.

How to Pass the UPMSP Intermediate Chemistry Exam

What You Need to Know

Passing score: 33% aggregate pass mark (minimum 23 out of 70 in theory and 10 out of 30 in practicals)
Assessment: 70-mark written theory board examination (3 hours 15 minutes) supplemented by a 30-mark practical examination. The question paper includes multiple-choice questions, short numerical problems, inorganic coordination chemistry concepts, and organic reaction mechanism questions.
Time limit: 3 hours 15 minutes (195 minutes)
Exam fee: ₹600.75 for institutional (regular) Intermediate candidates and ₹806 for private candidates for the 2026 examination, plus ₹206 per additional subject. UPMSP charges one registration fee per candidate, not per subject paper.

Keys to Passing

Complete 500+ practice questions
Score 80%+ consistently before scheduling
Focus on highest-weighted sections
Use our AI tutor for tough concepts

UPMSP Intermediate Chemistry Study Tips from Top Performers

1Master Physical Chemistry formulas for molarity/molality, Raoult's law, Nernst equation, Kohlrausch's law, and first-order half-life kinetics.

2Practice IUPAC nomenclature rules for coordination complexes, including identifying ligand types, coordination number, and oxidation states.

3Memorize transition metal trends, spin-only magnetic moment formula μ = √(n(n+2)) BM, and reasons for lanthanoid contraction.

4Understand organic reaction mechanisms step-by-step, particularly SN1 vs SN2 substitution, acid-catalyzed alcohol dehydration, and nucleophilic addition to carbonyl groups.

5Revise organic named reactions, chemical tests for functional group distinction (Tollens, Fehling, Iodoform, Lucas, Hinsberg, Carbylamine tests), and biomolecule structural features.

Frequently Asked Questions

What is the code and structure for UPMSP Class 12 Chemistry?

Code 152 is the official subject code for Class 12 Chemistry under UPMSP. The evaluation consists of a 70-mark theory paper and a 30-mark practical examination.

How many chapters are included in the revised UPMSP Chemistry syllabus?

The revised rationalized NCERT syllabus for UPMSP Chemistry consists of 10 core chapters split across Physical, Inorganic, and Organic Chemistry.

What is the minimum passing score in UP Board Class 12 Chemistry?

Students must secure at least 33% overall, with a minimum of 23 marks out of 70 in theory and 10 marks out of 30 in practicals.

Are numerical calculations tested in UPMSP Chemistry?

Yes, physical chemistry chapters (Solutions, Electrochemistry, Chemical Kinetics) carry significant weightage in numerical calculations using formulas like Nernst equation, integrated rate laws, and colligative property formulas.

What key organic named reactions should be mastered for UP Board Chemistry?

Important named reactions include Aldol condensation, Cannizzaro reaction, Reimer-Tiemann reaction, Kolbe's reaction, Hoffmann bromamide degradation, Gabriel phthalimide synthesis, Sandmeyer reaction, and HVZ reaction.

100+ Free UPMSP Intermediate Chemistry Practice Questions

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