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Class 11 chemistry · linked to Redox reactions · Physical chemistry experiments

Source: CBSE Class 11 chemistry practical syllabus · use your school laboratory manual (NCERT Lab Manual where your school uses it).

Displacement redox reaction (Class 11 chemistry practical)

You observe a metal strip in a salt solution and decide which species is oxidised and which is reduced.

Which metals and what concentrations you use come from your manual — not invented here.

Published practice page. Concentrations, masses, and numerical answers come from your school laboratory manual and your own readings — not invented here. Not yet reviewed by a named chemistry reviewer. Version 1.0.0, updated 2026-10-03.

Safety — read before you start

Safety warning. Practise here. Perform the real experiment only in your school lab, with your teacher present.

  • Metal salt solutions can be toxic or irritant.
  • Some metals react vigorously — only use the pair and amount your teacher assigns.

Wear: Lab coat, Splash goggles, Gloves, as your teacher directs.

Follow your teacher’s disposal instructions. Do not pour leftovers down a household drain.

Loads only after you tap. Use the lab hands to pick up and use equipment (pointer hidden in the scene). Falls back to a flat diagram if WebGL is unavailable.

Aim

To carry out a displacement reaction between a metal and a salt solution specified in your laboratory manual, and to identify the oxidising and reducing agents.

Methods and quantities can differ between schools. Follow your teacher's instructions.

Apparatus and chemicals

Apparatus and chemicals
ItemNote
Test tubes / beakerClean and dry as your teacher directs.
Metal strip or granulesAs named in the manual.
Forceps and emery paperClean the metal surface if required.
Salt solution (manual) (salt solution)Identity and concentration not printed here until checked.
Metal sample (manual) (metal)Do not substitute a different metal without your teacher.

Theory and reaction

Open

Oxidation = loss of electrons; reduction = gain of electrons.

The metal that dissolves is oxidised (reducing agent). The ion that plates out or is consumed in solution is reduced (oxidising agent).

Example pattern only: Zn + Cu2+ → Zn2+ + Cu. Your manual’s pair may differ.

Metal M displaces ion of N from solution when M is more reactive.

Picture guide

Metal strip in a coloured salt solution in a beaker
A more reactive metal can displace another from solution. Watch colour change and any coating on the strip — write what you actually see.

Procedure

  1. Clean the metal sample if the manual says to.
  2. Pour the assigned volume of salt solution into a clean tube or beaker.
  3. Add the metal. Note colour of solution and surface of the metal at the start.
  4. Wait the time your manual states. Record changes (deposit, colour fade, gas, heat).
  5. Write half-reactions and the net ionic equation using only the pair you actually used.

Observation table

Enter the readings from your school lab in the practical file below. This page does not fill them in for you.

Type the readings in your practical file

Calculation

No titre unless your manual adds a quantitative follow-up. Identify ox. nos. before and after.

Result

State the displacement you observed and name the oxidising and reducing agents.

Precautions

  • Do not taste solutions. Do not pipette by mouth.
  • Dispose of metal ions as your teacher instructs — many are environmental hazards.

Viva questions

Answer one question at a time. The full answers stay closed until you open them.

Question 1 of 3

In Zn + Cu²⁺ → Zn²⁺ + Cu, what is oxidised?

Answer choices

Pick an answer first.

Show all questions and answers

  1. In Zn + Cu²⁺ → Zn²⁺ + Cu, what is oxidised?

    Answer: Zn. Reason: Zinc loses electrons.

  2. The oxidising agent is the species that…

    Answer: Is reduced. Reason: It gains electrons / is reduced.

  3. Oxidation number of an element in free form is…

    Answer: 0. Reason: Free elements are 0.

Common mistakes

  • Calling the ion that gains electrons the reducing agent.
  • Using a metal/solution pair not in the reactivity order your syllabus teaches.
  • Inventing a balanced equation for chemicals you did not use.

Frequently asked questions

Can I do this at home?
No. Use this page to practise the order of ideas and steps. Do the real experiment only in your school laboratory, with your teacher present.

Your practical file

Name, school, and roll number are optional and are not sent anywhere.

The practical file opens on this device.

Review

Not yet reviewed by a named chemistry reviewer. Published for practice only — follow your teacher and laboratory manual for quantities and safety.

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Related notes

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