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Maharashtra HSC Chemistry Board Paper March 2026 with Solutions

Written board papers. Physics and Chemistry: 70 marks, 3 hours. Mathematics & Statistics: 80 marks, 3 hours.

2026, March 180 minutes 70 marks Save WhatsApp

Sections

Section A : Q.1 Multiple choice questions (10 marks) 10 questions
Section A : Q.2 Very short answer questions (8 marks) 8 questions
Section B : Attempt any eight, Q.3 to Q.14 (16 marks) 12 questions
Section C : Attempt any eight, Q.15 to Q.26 (24 marks) 12 questions
Section D : Attempt any three, Q.27 to Q.31 (12 marks) 5 questions

About this paper

This is the actual Maharashtra State Board (MSBSHSE) HSC (Class 12) Science Chemistry (55) board paper of the February–March 2026 examination (Day 08). The paper code printed on the question paper is J-155. The questions are transcribed in full from the board’s own printed question paper as published in the AglaSem Docs archive (‘MH 12th Question Paper March 2026 Chemistry’); structures printed in the paper are written out or described in words. The model answers are original Doubtly answers, worked out and checked independently, not the board’s official answer key.

Paper pattern

Maximum marks 70, time 3 hours, four sections. Section A: Q.1 has ten MCQs (1 mark each) and Q.2 has eight very short answer questions (1 mark each) — 18 marks, all compulsory. Section B: Q.3 to Q.14, twelve 2-mark questions, attempt any eight (16 marks). Section C: Q.15 to Q.26, twelve 3-mark questions, attempt any eight (24 marks). Section D: Q.27 to Q.31, five 4-mark questions, attempt any three (12 marks). Log tables are allowed, calculators are not. Constants printed on the paper: NA = 6.022 × 1023, R = 0.08206 L atm K−1 mol−1, 1 F = 96500 C.

How to use it

Attempt the paper in one 3-hour sitting without a calculator, choosing questions as the board allows. Then compare with the model answers: for conversions and named reactions, check the reagent and conditions over the arrow; for numericals, check the formula, substitution, units and final value; for derivations and diagrams, check that every step and label is present.

FAQs

Is this the official board paper?

Yes, the questions are from the board’s March 2026 Chemistry paper (J-155). The solutions are Doubtly’s own model answers; the board does not publish a full answer key.

Which answer is right for Q.31 (i), 2.5 × 10−4 or 2.63 × 10−4?

The usual board method uses Ka = cα2 because α is small, giving 2.5 × 10−4. Using the full expression cα2/(1 − α) gives 2.63 × 10−4; both methods are shown.

How many questions must I answer in Section C?

Any eight of the twelve 3-mark questions (Q.15 to Q.26), for 24 marks.

Chapters covered

Instructions

Solve on paper with a timer, then check against the solutions. Sections: A (MCQ and very short answers), B (short answers, attempt any 8 of 12), C (attempt any 8 of 12), D (long answers with choice).

Section A : Q.1 Multiple choice questions (10 marks)

  1. Q.1 (i) The electrolyte used in H2 – O2 fuel cell is _____.

    1. (A) aqueous KCl
    2. (B) aqueous KOH
    3. (C) aqueous HCl
    4. (D) aqueous KNO3
    1 mark See answer →

  2. Q.1 (ii) The oxidation state of bromine in HOBrO2 oxoacid is _____.

    1. (A) + 7
    2. (B) + 5
    3. (C) + 3
    4. (D) + 1
    1 mark See answer →

  3. Q.1 (iii) Acetonitrile may be prepared by heating the following reactants :

    1. (A) Ethyl chloride with alcoholic KCN
    2. (B) Ethyl chloride with alcoholic AgCN
    3. (C) Methyl chloride with alcoholic KCN
    4. (D) Methyl chloride with alcoholic AgCN
    1 mark See answer →

  4. Q.1 (iv) The carbonated water is an example of _____.

    1. (A) solid in liquid solution
    2. (B) liquid in liquid solution
    3. (C) gas in liquid solution
    4. (D) liquid in gas solution
    1 mark See answer →

  5. Q.1 (v) The unit of rate constant is per second, the order of reaction is –

    1. (A) Zero
    2. (B) First
    3. (C) Second
    4. (D) Third
    1 mark See answer →

  6. Q.1 (vi) A system releases 10 kJ of heat and performs 15 kJ of work on the surrounding. Hence the change in internal energy is :

    1. (A) + 5 kJ
    2. (B) – 5 kJ
    3. (C) + 25 kJ
    4. (D) – 25 kJ
    1 mark See answer →

  7. Q.1 (vii) The co-ordination complex ions [Co(NH3)5(NO2)]2⊕ and [Co(NH3)5(ONO)]2⊕ are _____ of each other.

    1. (A) ionization isomers
    2. (B) solvate isomers
    3. (C) linkage isomers
    4. (D) co-ordination isomers
    1 mark See answer →

  8. Q.1 (viii) The correct order for basic strength of amines and ammonia is _____.

    1. (A) NH3 > R–NH2 > R2NH > R3N
    2. (B) NH3 > R3N > R2NH > R–NH2
    3. (C) NH3 < R–NH2 > R3N > R2NH
    4. (D) NH3 < R–NH2 < R2NH > R3N
    1 mark See answer →

  9. Q.1 (ix) Amongst the following 3d-series elements, having highest value of first ionization enthalpy is _____.

    1. (A) Zn
    2. (B) Cu
    3. (C) Co
    4. (D) Sc
    1 mark See answer →

  10. Q.1 (x) The pOH of 0.01 M HCl solution is _____.

    1. (A) 1
    2. (B) 2
    3. (C) 11
    4. (D) 12
    1 mark See answer →

Section A : Q.2 Very short answer questions (8 marks)

  1. Q.2 (i) Write the name of product obtained, when selenium is treated with magnesium metal.

    1 mark See answer →

  2. Q.2 (ii) Write the SI unit of cell constant.

    1 mark See answer →

  3. Q.2 (iii) Write the name of radioactive element in lanthanide series.

    1 mark See answer →

  4. Q.2 (iv) Complete the following reaction :
    Phenol (C6H5OH, a benzene ring carrying an –OH group) + 3 H2 —(Nickel, 433 K)→ ?

    1 mark See answer →

  5. Q.2 (v) Write the IUPAC name of :
    (Structure: a benzene ring carrying a –CHO group, and an –OH group on the adjacent (ortho) carbon.)

    1 mark See answer →

  6. Q.2 (vi) Copper has fcc structure with edge length 495 pm. What is the radius of copper atom in pm?

    1 mark See answer →

  7. Q.2 (vii) Write the chemical name of Teflon.

    1 mark See answer →

  8. Q.2 (viii) Write the name of nanoparticle which acts as highly effective bacterial disinfectant.

    1 mark See answer →

Section B : Attempt any eight, Q.3 to Q.14 (16 marks)

  1. Q.3

    Define : (a) Isomorphism (b) Unit Cell

    2 marks See answer →

  2. Q.4

    Explain the trends in the following properties of group 17 elements : (i) Atomic radii (ii) Electronegativity

    2 marks See answer →

  3. Q.5

    Explain Homoleptic and Heteroleptic complexes with example.

    2 marks See answer →

  4. Q.6

    (a) Write the reaction of bromine water on glucose.
    (b) Define – Enantiomers

    2 marks See answer →

  5. Q.7

    (i) Write example of one dimensional nanostructure of size less than 100 nm.
    (ii) Write the hydrolysis reaction of ethyl methyl ether.

    2 marks See answer →

  6. Q.8

    Calculate the osmotic pressure of solution containing 0.822 gm of sucrose in 300 mL of water at 298 K. [ Given : Molar mass of sucrose 342 g/mol, R = 0.08205 dm\(^3\) atm K\(^{-1}\) mol\(^{-1}\) ]

    2 marks See answer →

  7. Q.9

    Write the mathematical equation of first law of thermodynamics for following processes : (a) Isochoric process (b) Adiabatic process

    2 marks See answer →

  8. Q.10

    Write two similarities and two differences between lanthanoids and actinoids.

    2 marks See answer →

  9. Q.11

    What is the action of following reagents on chlorobenzene? (i) conc. HNO3 (ii) fuming H2SO4

    2 marks See answer →

  10. Q.12

    Explain Cannizzaro reaction with suitable example.

    2 marks See answer →

  11. Q.13

    A chemical reaction occurs in two steps :
    (i) NO2Cl(g) —(slow)→ NO2(g) + Cl(g)
    (ii) NO2Cl(g) + Cl(g) —(fast)→ NO2(g) + Cl2(g)
    (a) Write down the rate law.
    (b) Identify the reaction intermediate.

    2 marks See answer →

  12. Q.14

    The standard potential of electrode Cu++ (0.02 M) | Cu(s) is 0.337 volt. Calculate its potential in volt.

    2 marks See answer →

Section C : Attempt any eight, Q.15 to Q.26 (24 marks)

  1. Q.15

    (i) Derive relationship between relative lowering of vapour pressure and molar mass of non volatile solute.
    (ii) Write statement of second law of thermodynamics.

    3 marks See answer →

  2. Q.16

    (i) Convert, acetamide into ethyl amine.
    (ii) Explain amphoteric nature of water.

    3 marks See answer →

  3. Q.17

    Convert the following :
    (i) Ethanol into sodium ethoxide.
    (ii) Phenol into o-phenol sulfonic acid.
    (iii) Bromomethane into methoxyethane.

    3 marks See answer →

  4. Q.18

    (i) What is peptide linkage?
    (ii) Write general characteristics of interhalogen compounds.

    3 marks See answer →

  5. Q.19

    (i) Write observed electronic configuration of chromium (Z = 24).
    (ii) Calculate magnetic moment of Ti3+ by using spin only formula. (Z of Ti = 22)
    (iii) Define Green chemistry.

    3 marks See answer →

  6. Q.20

    (i) Write examples of coordination metal complexes in biology.
    (ii) Calculate the work done in oxidation of 2 moles of SO2 at 298K, if SO2(g) + ½ O2(g) → SO3(g) [ Given : R = 8.314 J/K/mol ]

    3 marks See answer →

  7. Q.21

    (i) Write the formula to measure % atom economy according to green chemistry.
    (ii) Convert : (a) Benzene into benzaldehyde (b) Cyclohexene into adipic acid

    3 marks See answer →

  8. Q.22

    (i) Write a reaction for preparation of Nylon-6.
    (ii) The salt of Sc3+ ion is colourless and the salt of Mn3+ ion is coloured. Explain. [ Z of Sc = 21 and Z of Mn = 25 ]

    3 marks See answer →

  9. Q.23

    (i) Write the postulates of Werner’s theory of co-ordination complexes.
    (ii) What is the action of ethane –1, 2 – diol on acetone?

    3 marks See answer →

  10. Q.24

    (i) Write Tollen’s reagent test for acetaldehyde.
    (ii) Write the structure of zwitter ion of sulfanilic acid. Write the reaction between benzene diazonium chloride and phenol in alkaline medium.

    3 marks See answer →

  11. Q.25

    (i) Define : Common ion effect.
    (ii) Write preparation of glucose from starch.

    3 marks See answer →

  12. Q.26

    (i) Draw the structure of 2, 4 – dinitrophenylhydrazone of acetaldehyde.
    (ii) The rate of A + B → P is 3.6 × 10−2 mol/dm3/s. When [A] = 0.2 M and [B] = 0.1 M. Calculate the rate constant if reaction is first order in B and second order in A.

    3 marks See answer →

Section D : Attempt any three, Q.27 to Q.31 (12 marks)

  1. Q.27

    (i) Define : (a) Isotonic solution (b) Molecularity of reaction
    (ii) State and explain Hess’s law of constant heat summation.

    4 marks See answer →

  2. Q.28

    (i) Define : (a) Schottky defect (b) Ferromagnetism
    (ii) Write the name of catalyst used in preparation of HDP.
    (iii) Draw structure of isoprene unit of natural rubber.

    4 marks See answer →

  3. Q.29

    (i) Calculate effective atomic number of Fe2⊕ in [Fe(CN)6]4⊖ [ Given : (Z = 26) ]
    (ii) Draw neat and labelled diagram of lead accumulator.
    (iii) Write two advantages of hydrogen – oxygen fuel cell.

    4 marks See answer →

  4. Q.30

    (i) Convert, ethanoic acid to ethanol.
    (ii) Explain the mechanism of alkaline hydrolysis of bromomethane.

    4 marks See answer →

  5. Q.31

    (i) Acetic acid is 5% ionised in its decimolar solution. Calculate the dissociation constant of acetic acid.
    (ii) Write chemical formula of epsom salt. Give two uses of H2SO4.

    4 marks See answer →