Chemistry · Class 12 Science

Maharashtra Msbshse Class 12 Chemistry — Real Previous-Year Papers

with complete answers

Real previous-year board papers, year by year — the official exam pattern, the full question paper, and every question solved the concept-first way. Distinct from the chapter-wise textbook bank.

2016–2026
Years of papers: 10
Total Papers: 10
Real Board Papers: 0
Sample papers: 420
Real-paper Q & A: 0
Sample-paper Q & A

Real board-paper questions available, by year

47 Q2026complete

47 Q2025complete

47 Q2024complete

47 Q2023complete

47 Q2022complete

—2021Not available

47 Q2020complete

29 Q2019complete

35 Q2018complete

34 Q2017complete

40 Q2016complete

Maharashtra HSC (MSBSHSE) Board 2026 · Set ANNUAL

Real board examination

About this paper

The real Class-12 board examination held in 2026. Every question below is solved the concept-first way. Sample papers are labelled honestly — never shown as a past exam.

Total marks: 70
Questions: 47
Duration: 180 min
Sections: 5

The marks / questions / duration above are the official exam pattern. We currently have 47 of this paper’s questions (100% of the full paper), with 47 fully solved. Questions we couldn’t yet extract or verify are held — never shown as complete.

Sections & marks

Section	Type	Questions	Marks each	Total
ASection A	compulsory	10	1	10
ASection A	compulsory	8	1	8
BSection B	choice	12	2	24
CSection C	choice	12	3	36
DSection D	choice	5	4	20
Total		47		70

The question paper

The questions we hold for this paper, laid out by section. Solutions are on the Answers tab.

Board Examination

Chemistry

Maharashtra HSC (MSBSHSE) Board 2026 · Set ANNUAL

Series/Set: ANNUALRoll No. ________

Time Allowed: 3 hoursMaximum Marks: 70

General Instructions

This question paper contains 47 questions divided into 5 sections — A, A, B, C, D.
Section A comprises 10 questions of 1 mark each (compulsory).
Section A comprises 8 questions of 1 mark each (compulsory).
Section B comprises 12 questions of 2 marks each (choice).
Section C comprises 12 questions of 3 marks each (choice).
Section D comprises 5 questions of 4 marks each (choice).

Above is the official exam pattern. The questions printed below are those we currently hold for this paper.

Section A

compulsory · 1 mark each · 18 of 10 shown

Q1.

The electrolyte used in H

_2

– O

_2

fuel cell is _____.

(a) aqueous KCl
(b) aqueous KOH
(c) aqueous HCl
(d) aqueous KNO $_3$

[1]

Q2.

The oxidation state of bromine in HOBrO

_2

oxoacid is _____.

(a) +7
(b) +5
(c) +3
(d) +1

[1]

Q3.

Acetonitrile may be prepared by heating the following reactants:

(a) Ethyl chloride with alcoholic KCN
(b) Ethyl chloride with alcoholic AgCN
(c) Methyl chloride with alcoholic KCN
(d) Methyl chloride with alcoholic AgCN

[1]

Q4.

The carbonated water is an example of _____.

(a) solid in liquid solution
(b) liquid in liquid solution
(c) gas in liquid solution
(d) liquid in gas solution

[1]

Q5.

The unit of rate constant is per second, the order of reaction is –

(a) Zero
(b) First
(c) Second
(d) Third

[1]

Q6.

A system releases 10 kJ of heat and performs 15 kJ of work on the surrounding. Hence the change in internal energy is:

(a) +5 kJ
(b) –5 kJ
(c) +25 kJ
(d) –25 kJ

[1]

Page 1 of 9

Q7.

The co-ordination complex ions [Co(NH₃)₅(NO₂)]2oplus and [Co(NH₃)₅(ONO)]2oplus are ___ of each other. (a) ionization isomers (b) solvate isomers (c) linkage isomers (d) co-ordination isomers

[1]

Q8.

The correct order for basic strength of amines and ammonia is ___. (a) NH₃ > R-NH₂ > R₂NH > R₃N (b) NH₃ > R₃N > R₂NH > R-NH₂ (c) NH₃ < R-NH₂ > R₃N > R₂NH (d) NH₃ < R-NH₂ < R₂NH > R₃N

[1]

Q9.

Amongst the following 3d-series elements, having highest value of first ionization enthalpy is ___. (a) Zn (b) Cu (c) Co (d) Sc

[1]

Q10.

The pOH of 0.01 M HCl solution is ___. (a) 1 (b) 2 (c) 11 (d) 12

[1]

Q11.

Write the name of product obtained, when selenium is treated with magnesium metal.

[1]

Q12.

Write the SI unit of cell constant.

[1]

Q13.

Write the name of radioactive element in lanthanide series.

[1]

Q14.

Complete the following reaction: [Phenol (benzene ring with OH)] + 3 H₂ xrightarrow[433K]Nickel ?

[1]

Q15.

Write the IUPAC name of: [benzene ring with -CHO and -OH substituents]

[1]

Q16.

Copper has fcc structure with edge length 495 pm. What is the radius of copper atom in pm?

[1]

Q17.

Write the chemical name of Teflon.

[1]

Page 2 of 9

Q18.

Write the name of nanoparticle which acts as highly effective bacterial disinfectant.

[1]

Section A

compulsory · 1 mark each · 18 of 10 shown

Q1.

The electrolyte used in H₂ – O₂ fuel cell is ___. (a) aqueous KCl (b) aqueous KOH (c) aqueous HCl (d) aqueous KNO₃

[1]

Q2.

The oxidation state of bromine in HOBrO₂ oxoacid is ___. (a) +7 (b) +5 (c) +3 (d) +1

[1]

Q3.

Acetonitrile may be prepared by heating the following reactants: (a) Ethyl chloride with alcoholic KCN (b) Ethyl chloride with alcoholic AgCN (c) Methyl chloride with alcoholic KCN (d) Methyl chloride with alcoholic AgCN

[1]

Q4.

The carbonated water is an example of ___. (a) solid in liquid solution (b) liquid in liquid solution (c) gas in liquid solution (d) liquid in gas solution

[1]

Q5.

The unit of rate constant is per second, the order of reaction is – (a) Zero (b) First (c) Second (d) Third

[1]

Q6.

A system releases 10 kJ of heat and performs 15 kJ of work on the surrounding. Hence the change in internal energy is: (a) +5 kJ (b) –5 kJ (c) +25 kJ (d) –25 kJ

[1]

Q7.

[1]

Q8.

[1]

Page 3 of 9

Q9.

Amongst the following 3d-series elements, having highest value of first ionization enthalpy is ___. (a) Zn (b) Cu (c) Co (d) Sc

[1]

Q10.

The pOH of 0.01 M HCl solution is ___. (a) 1 (b) 2 (c) 11 (d) 12

[1]

Q11.

Write the name of product obtained, when selenium is treated with magnesium metal.

[1]

Q12.

Write the SI unit of cell constant.

[1]

Q13.

Write the name of radioactive element in lanthanide series.

[1]

Q14.

Complete the following reaction: [Phenol (benzene ring with OH)] + 3 H₂ xrightarrow[433K]Nickel ?

[1]

Q15.

Write the IUPAC name of: [benzene ring with -CHO and -OH substituents]

[1]

Q16.

Copper has fcc structure with edge length 495 pm. What is the radius of copper atom in pm?

[1]

Q17.

Write the chemical name of Teflon.

[1]

Q18.

Write the name of nanoparticle which acts as highly effective bacterial disinfectant.

[1]

Page 4 of 9

Section B

choice · 2 marks each · 12 of 12 shown

Q1.

Define: (a) Isomorphism (b) Unit Cell

[2]

Q2.

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

[2]

Q3.

Explain Homoleptic and Heteroleptic complexes with example.

[2]

Q4.

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

[2]

Q5.

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

[2]

Q6.

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 dm³.atm.K⁻¹.mol⁻¹]

[2]

Q7.

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

[2]

Q8.

Write two similarities and two differences between lanthanoids and actinoids.

[2]

Page 5 of 9

Q9.

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

[2]

Q10.

Explain Cannizzaro reaction with suitable example.

[2]

Q11.

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

[2]

Q12.

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

[2]

Section C

choice · 3 marks each · 12 of 12 shown

Q1.

(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]

Q2.

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

[3]

Q3.

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

[3]

Page 6 of 9

Q4.

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

[3]

Q5.

(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]

Q6.

(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) + (1)/(2)O2(g) arrow SO3(g) [Given: R = 8.314 J/K/mol]

[3]

Q7.

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

[3]

Q8.

(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]

Q9.

(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]

Q10.

(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]

Page 7 of 9

Q11.

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

[3]

Q12.

(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]

Section D

choice · 4 marks each · 5 of 5 shown

Q1.

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

[4]

Q2.

(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]

Q3.

(i) Calculate effective atomic number of Fe2oplus in [Fe(CN)₆]4ominus [Given: (Z = 26)]. (ii) Draw neat and labelled diagram of lead accumulator. (iii) Write two advantages of hydrogen–oxygen fuel cell.

[4]

Page 8 of 9

Q4.

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

[4]

Q5.

(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]

Page 9 of 9