CBSE Class 11 chemistry · qualitative salt analysis · Salt analysis

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

Qualitative salt analysis (one cation, one anion) (Class 11 chemistry practical)

You follow the analytical scheme in your NCERT/laboratory manual for Class 11 — usually one cation from groups II–IV simplified set and one anion from the anion list taught.

The unknown salt code is assigned by your teacher; do not guess the answer on this page.

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.

Strong acids.
Toxic gases in dry tests.
Never work alone on unknowns.

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 identify one cation and one anion present in the unknown salt supplied, using the qualitative tests prescribed in your laboratory manual.

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

Apparatus and chemicals

Apparatus and chemicals
Item	Note
Test tubes and rack	Clean; avoid cross-contamination.
Glass rod and dropper	Separate for NH₃ and H₂S sources if used.
Filter paper and funnel	If precipitation steps needed.
Bunsen burner	Flame test for some cations.
Platinum/nichrome loop or wooden splint	As school allows for flame colour.
Unknown salt (unknown)	Teacher-coded sample.
Dilute HCl / H₂SO₄ / HNO₃ (acids)	As manual for anion and group separation.
NaOH / NH₄OH (bases)	Precipitation and confirmatory tests.
Confirmatory reagents (reagents)	BaCl₂, AgNO₃, NH₄OH, (NH₄)₂CO₃, etc. as manual lists.

Burette and conical flask set up for titration — Read the burette at eye level. The end-point colour in a diagram is only a guide — your titre is the volume you measure.

Theory and reaction

Open

Cations are separated into groups by selective precipitation with group reagents (e.g. group II with H₂S in acidic medium — exact scheme from manual).

Anions are detected by dry tests (salt + conc. H₂SO₄) and wet tests (specific precipitates and reactions).

Confirmatory tests must match the ion you claim — write balanced equations only for ions you actually identified.

Illustrative precipitation equations — use those matching your identified ions.

Procedure

Note appearance and solubility of the unknown in water.
Perform flame test or dry tests if manual lists them for preliminary cation hint.
Prepare solution in distilled water (or acid if manual says). Run anion tests in the order of the manual table.
Separate cation groups with group reagents; identify the cation present using confirmatory tests.
Write conclusion: cation … and anion … with at least one confirmatory test each.

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

S. No.	Test (—)	Observation (—)	Inference (—)
1
2
3

Calculation

No numerical calculation — logical inference from observations.

Result

State identified cation and anion. Leave blank until your tests are complete.

Precautions

Follow the test order in the manual — skipping steps gives false conclusions.
Conc. H₂SO₄ and H₂S (if generated) are hazardous — teacher supervision.
Do not mix up test tubes.

Viva questions

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

Question 1 of 4

A white precipitate with BaCl₂ in acidified solution suggests…

A. Always Cl⁻B. SO₄²⁻ (among common anions)C. Only Fe³⁺D. No anion

Pick an answer first.

Show all questions and answers

A white precipitate with BaCl₂ in acidified solution suggests…
Answer: SO₄²⁻ (among common anions). Reason: BaSO₄ is white and insoluble in dilute acid.
AgCl precipitate is…
Answer: White, curdled, soluble in NH₄OH. Reason: Classic chloride confirmatory behaviour.
Group reagents are used to…
Answer: Separate cations into groups by selective precipitation. Reason: Systematic cation analysis scheme.
Before starting wet tests you should…
Answer: Prepare a clear solution or note insolubility as manual directs. Reason: Solution preparation is the usual starting point.

Common mistakes

Reporting an ion without a confirmatory test.
Using flame colour alone without wet confirmation where manual requires both.
Writing equations for ions you did not test.

Frequently asked questions

Can I do this at home?: No. Use this page to practise the order of steps and viva. 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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