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Salt Analysis Flowchart and Worksheet

Lab activitiesCBSE Class 11–12 · ISC · A-level · IB10 items · answer key included

A printable salt analysis flowchart and worksheet for CBSE Class 11 and Class 12 chemistry practicals (NCERT lab manual conventions). Part A is a qualitative analysis flowchart for cation group separation — zero group NH₄⁺, Group I Pb²⁺, Group II Cu²⁺/Pb²⁺, Group III Al³⁺/Fe³⁺, Group IV Zn²⁺/Mn²⁺/Ni²⁺/Co²⁺, Group V Ba²⁺/Sr²⁺/Ca²⁺ and Group VI Mg²⁺ — with blanks for group reagents and precipitates. Parts B–D are observation/inference tables for anion tests (dilute H₂SO₄ group CO₃²⁻, S²⁻, SO₃²⁻, NO₂⁻; concentrated H₂SO₄ group Cl⁻, Br⁻, I⁻, NO₃⁻; independent SO₄²⁻ and PO₄³⁻) and confirmatory tests for cations, followed by reasoning and identify-the-salt questions. The answer key gives the completed salt analysis chart.

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Salt Analysis Flowchart and Worksheet

Name Class Date

Part A — Cation group separation flowchart

Fill in the group reagent, the precipitate (with colour) and the ions present in each group.

1.
Zero group
Group reagent:
 
→
Precipitate / observation:
 
Ion(s):  
Original solution (O.S.) of the salt in water / dil. HCl
↓
Group I
Group reagent:
 
→
Precipitate / observation:
 
Ion(s):  
↓ filtrate (if no precipitate, use the same solution)
Group II
Group reagent:
 
→
Precipitate / observation:
 
Ion(s):  
↓ filtrate (if no precipitate, use the same solution)
Group III
Group reagent:
 
→
Precipitate / observation:
 
Ion(s):  
↓ filtrate (if no precipitate, use the same solution)
Group IV
Group reagent:
 
→
Precipitate / observation:
 
Ion(s):  
↓ filtrate (if no precipitate, use the same solution)
Group V
Group reagent:
 
→
Precipitate / observation:
 
Ion(s):  
↓ filtrate (if no precipitate, use the same solution)
Group VI
Group reagent:
 
→
Precipitate / observation:
 
Ion(s):  

Zero group (NH4+) is tested on the solid salt; Groups I–VI are tested in order on the original solution, using the filtrate from each group for the next.

Zero group
Group reagent:
Heat the salt with NaOH solution
→
Precipitate / observation:
Ammonia gas: pungent smell, dense white fumes with a glass rod dipped in conc. HCl
Ion(s): NH4+
Original solution (O.S.) of the salt in water / dil. HCl
↓
Group I
Group reagent:
Original solution + dil. HCl
→
Precipitate / observation:
White precipitate of PbCl2
Ion(s): Pb2+
↓ filtrate (if no precipitate, use the same solution)
Group II
Group reagent:
Pass H2S gas through the acidic (dil. HCl) solution
→
Precipitate / observation:
Black precipitate of CuS / PbS
Ion(s): Cu2+, Pb2+
↓ filtrate (if no precipitate, use the same solution)
Group III
Group reagent:
Boil off H2S, add a few drops of conc. HNO3 and heat; then solid NH4Cl + excess NH4OH
→
Precipitate / observation:
White gelatinous Al(OH)3 / reddish-brown Fe(OH)3
Ion(s): Al3+, Fe3+
↓ filtrate (if no precipitate, use the same solution)
Group IV
Group reagent:
Pass H2S gas through the ammoniacal solution (NH4Cl + NH4OH)
→
Precipitate / observation:
ZnS white (dirty white), MnS buff / flesh-coloured, NiS and CoS black
Ion(s): Zn2+, Mn2+, Ni2+, Co2+
↓ filtrate (if no precipitate, use the same solution)
Group V
Group reagent:
(NH4)2CO3 solution in the presence of NH4Cl + NH4OH
→
Precipitate / observation:
White precipitate of BaCO3 / SrCO3 / CaCO3
Ion(s): Ba2+, Sr2+, Ca2+
↓ filtrate (if no precipitate, use the same solution)
Group VI
Group reagent:
Disodium hydrogen phosphate (Na2HPO4) + NH4OH; scratch the sides of the test tube
→
Precipitate / observation:
White crystalline precipitate of Mg(NH4)PO4
Ion(s): Mg2+

Zero group (NH4+) is tested on the solid salt; Groups I–VI are tested in order on the original solution, using the filtrate from each group for the next.

Part B — Anions: dilute H₂SO₄ group (preliminary test)

Complete the missing observations and inferences.

2.
ExperimentObservationInference
Salt + dil. H₂SO₄Brisk effervescence; colourless, odourless gas turns lime water milkyCO₃²⁻
Salt + dil. H₂SO₄Colourless gas with rotten-egg smell; turns lead acetate paper blackS²⁻
Salt + dil. H₂SO₄Colourless gas with suffocating (burning sulfur) smell; turns acidified K₂Cr₂O₇ paper greenSO₃²⁻
Salt + dil. H₂SO₄ (cold)Light brown fumes; turn acidified KI–starch paper blueNO₂⁻

Part C — Anions: conc. H₂SO₄ group and confirmatory tests

Complete the missing observations and inferences.

3.
ExperimentObservationInference
Salt + conc. H₂SO₄, warmColourless pungent gas; dense white fumes with a glass rod dipped in NH₄OHCl⁻
Salt + conc. H₂SO₄, warmReddish-brown vapours, intensified on adding MnO₂Br⁻
Salt + conc. H₂SO₄, warmViolet vapours that turn starch paper blueI⁻
Salt + conc. H₂SO₄ + copper turnings, heatBrown fumes (NO₂), intensified by copper; solution turns bluishNO₃⁻
4.
Confirmatory / independent testObservationInference
Sodium carbonate extract + dil. HNO₃ + AgNO₃White precipitate, soluble in NH₄OHCl⁻ confirmed
Sodium carbonate extract + dil. HNO₃ + AgNO₃Pale yellow precipitate, partially (sparingly) soluble in NH₄OHBr⁻ confirmed
Sodium carbonate extract + dil. HNO₃ + AgNO₃Yellow precipitate, insoluble in NH₄OHI⁻ confirmed
Salt solution + freshly prepared FeSO₄; pour conc. H₂SO₄ slowly down the sideDark brown ring at the junction of the two liquidsNO₃⁻ confirmed (ring test)
Sodium carbonate extract + dil. HCl + BaCl₂ solutionWhite precipitate, insoluble in conc. HClSO₄²⁻
Salt + conc. HNO₃ + ammonium molybdate, heatCanary-yellow precipitatePO₄³⁻

Part D — Confirmatory tests for cations

Write the expected observation for each confirmatory test.

5.
IonConfirmatory testObservation
NH₄⁺Salt solution + Nessler's reagentBrown precipitate
Pb²⁺Dissolve PbCl₂ in hot water; add KI solutionYellow precipitate (PbI₂), golden spangles on cooling
Cu²⁺Dissolve CuS in 50 % HNO₃; add excess NH₄OHDeep blue solution
Fe³⁺Dissolve precipitate in dil. HCl; add K₄[Fe(CN)₆]Prussian blue colour / precipitate
Al³⁺Lake test: dissolve in dil. HCl, add blue litmus, then NH₄OH dropwiseBlue lake floating in a colourless solution
Zn²⁺Dissolve ZnS in dil. HCl, boil off H₂S; add NaOH dropwiseWhite precipitate, soluble in excess NaOH
Mn²⁺Boil precipitate with PbO₂ and conc. HNO₃Pink / purple supernatant (MnO₄⁻)
Ni²⁺Solution + NH₄OH + dimethylglyoximeRose-red (bright red) precipitate
Co²⁺Neutralised solution + acetic acid + KNO₂Yellow precipitate
Ba²⁺Dissolve in acetic acid; add K₂CrO₄Yellow precipitate; apple-green flame
Sr²⁺Dissolve in acetic acid; add (NH₄)₂SO₄White precipitate; crimson flame
Ca²⁺Dissolve in acetic acid; add ammonium oxalateWhite precipitate; brick-red flame
Mg²⁺Solution + magneson reagent + NaOHBlue precipitate

Part E — Reasoning and identification

Answer in full sentences; write equations where possible.

6.
Why is H2S passed in the presence of dil. HCl for Group II, but in ammoniacal medium for Group IV?
In acid, H+ suppresses the ionisation of H2S (common-ion effect), so [S2−] is very low and only sulfides with very low Ksp (CuS, PbS) precipitate. In ammoniacal solution OH− removes H+, ionisation increases and [S2−] becomes high enough to exceed the larger Ksp of ZnS, MnS, NiS and CoS.
7.
Why are a few drops of conc. HNO3 added and the solution heated before adding the Group III reagent?
To oxidise any Fe2+ to Fe3+. Fe(OH)2 is too soluble to precipitate completely in Group III, whereas Fe(OH)3 (very low Ksp) precipitates fully.
8.
Why must the solution be boiled to remove H2S after Group II?
Otherwise, when NH4OH is added in Group III, S2− concentration rises and Group IV sulfides (e.g. ZnS, NiS) would precipitate early with Group III.
9.
A white salt gives no gas with dil. H2SO4. With conc. H2SO4 it gives a colourless pungent gas forming white fumes with NH4OH. Its solution gives a white precipitate with AgNO3, soluble in NH4OH. Heated with NaOH it gives a gas that turns Nessler's reagent brown. Identify the salt.
Anion Cl−; cation NH4+ → ammonium chloride, NH4Cl.
10.
A blue salt gives a white precipitate with BaCl2 (insoluble in conc. HCl). With H2S in dil. HCl it gives a black precipitate; dissolved in HNO3 and treated with excess NH4OH it gives a deep blue solution. Identify the salt.
Anion SO42−; cation Cu2+ (Group II) → copper(II) sulfate, CuSO4 (CuSO4·5H2O).

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Answer key: Salt Analysis Flowchart and Worksheet

Part A — Cation group separation flowchart

1.
Zero group
Group reagent:
Heat the salt with NaOH solution
→
Precipitate / observation:
Ammonia gas: pungent smell, dense white fumes with a glass rod dipped in conc. HCl
Ion(s): NH4+
Original solution (O.S.) of the salt in water / dil. HCl
↓
Group I
Group reagent:
Original solution + dil. HCl
→
Precipitate / observation:
White precipitate of PbCl2
Ion(s): Pb2+
↓ filtrate (if no precipitate, use the same solution)
Group II
Group reagent:
Pass H2S gas through the acidic (dil. HCl) solution
→
Precipitate / observation:
Black precipitate of CuS / PbS
Ion(s): Cu2+, Pb2+
↓ filtrate (if no precipitate, use the same solution)
Group III
Group reagent:
Boil off H2S, add a few drops of conc. HNO3 and heat; then solid NH4Cl + excess NH4OH
→
Precipitate / observation:
White gelatinous Al(OH)3 / reddish-brown Fe(OH)3
Ion(s): Al3+, Fe3+
↓ filtrate (if no precipitate, use the same solution)
Group IV
Group reagent:
Pass H2S gas through the ammoniacal solution (NH4Cl + NH4OH)
→
Precipitate / observation:
ZnS white (dirty white), MnS buff / flesh-coloured, NiS and CoS black
Ion(s): Zn2+, Mn2+, Ni2+, Co2+
↓ filtrate (if no precipitate, use the same solution)
Group V
Group reagent:
(NH4)2CO3 solution in the presence of NH4Cl + NH4OH
→
Precipitate / observation:
White precipitate of BaCO3 / SrCO3 / CaCO3
Ion(s): Ba2+, Sr2+, Ca2+
↓ filtrate (if no precipitate, use the same solution)
Group VI
Group reagent:
Disodium hydrogen phosphate (Na2HPO4) + NH4OH; scratch the sides of the test tube
→
Precipitate / observation:
White crystalline precipitate of Mg(NH4)PO4
Ion(s): Mg2+

Zero group (NH4+) is tested on the solid salt; Groups I–VI are tested in order on the original solution, using the filtrate from each group for the next.

Part B — Anions: dilute H₂SO₄ group (preliminary test)

2.
ExperimentObservationInference
Salt + dil. H₂SO₄Brisk effervescence; colourless, odourless gas turns lime water milkyCO₃²⁻
Salt + dil. H₂SO₄Colourless gas with rotten-egg smell; turns lead acetate paper blackS²⁻
Salt + dil. H₂SO₄Colourless gas with suffocating (burning sulfur) smell; turns acidified K₂Cr₂O₇ paper greenSO₃²⁻
Salt + dil. H₂SO₄ (cold)Light brown fumes; turn acidified KI–starch paper blueNO₂⁻

Part C — Anions: conc. H₂SO₄ group and confirmatory tests

3.
ExperimentObservationInference
Salt + conc. H₂SO₄, warmColourless pungent gas; dense white fumes with a glass rod dipped in NH₄OHCl⁻
Salt + conc. H₂SO₄, warmReddish-brown vapours, intensified on adding MnO₂Br⁻
Salt + conc. H₂SO₄, warmViolet vapours that turn starch paper blueI⁻
Salt + conc. H₂SO₄ + copper turnings, heatBrown fumes (NO₂), intensified by copper; solution turns bluishNO₃⁻
4.
Confirmatory / independent testObservationInference
Sodium carbonate extract + dil. HNO₃ + AgNO₃White precipitate, soluble in NH₄OHCl⁻ confirmed
Sodium carbonate extract + dil. HNO₃ + AgNO₃Pale yellow precipitate, partially (sparingly) soluble in NH₄OHBr⁻ confirmed
Sodium carbonate extract + dil. HNO₃ + AgNO₃Yellow precipitate, insoluble in NH₄OHI⁻ confirmed
Salt solution + freshly prepared FeSO₄; pour conc. H₂SO₄ slowly down the sideDark brown ring at the junction of the two liquidsNO₃⁻ confirmed (ring test)
Sodium carbonate extract + dil. HCl + BaCl₂ solutionWhite precipitate, insoluble in conc. HClSO₄²⁻
Salt + conc. HNO₃ + ammonium molybdate, heatCanary-yellow precipitatePO₄³⁻

Part D — Confirmatory tests for cations

5.
IonConfirmatory testObservation
NH₄⁺Salt solution + Nessler's reagentBrown precipitate
Pb²⁺Dissolve PbCl₂ in hot water; add KI solutionYellow precipitate (PbI₂), golden spangles on cooling
Cu²⁺Dissolve CuS in 50 % HNO₃; add excess NH₄OHDeep blue solution
Fe³⁺Dissolve precipitate in dil. HCl; add K₄[Fe(CN)₆]Prussian blue colour / precipitate
Al³⁺Lake test: dissolve in dil. HCl, add blue litmus, then NH₄OH dropwiseBlue lake floating in a colourless solution
Zn²⁺Dissolve ZnS in dil. HCl, boil off H₂S; add NaOH dropwiseWhite precipitate, soluble in excess NaOH
Mn²⁺Boil precipitate with PbO₂ and conc. HNO₃Pink / purple supernatant (MnO₄⁻)
Ni²⁺Solution + NH₄OH + dimethylglyoximeRose-red (bright red) precipitate
Co²⁺Neutralised solution + acetic acid + KNO₂Yellow precipitate
Ba²⁺Dissolve in acetic acid; add K₂CrO₄Yellow precipitate; apple-green flame
Sr²⁺Dissolve in acetic acid; add (NH₄)₂SO₄White precipitate; crimson flame
Ca²⁺Dissolve in acetic acid; add ammonium oxalateWhite precipitate; brick-red flame
Mg²⁺Solution + magneson reagent + NaOHBlue precipitate

Part E — Reasoning and identification

6.
In acid, H+ suppresses the ionisation of H2S (common-ion effect), so [S2−] is very low and only sulfides with very low Ksp (CuS, PbS) precipitate. In ammoniacal solution OH− removes H+, ionisation increases and [S2−] becomes high enough to exceed the larger Ksp of ZnS, MnS, NiS and CoS.
7.
To oxidise any Fe2+ to Fe3+. Fe(OH)2 is too soluble to precipitate completely in Group III, whereas Fe(OH)3 (very low Ksp) precipitates fully.
8.
Otherwise, when NH4OH is added in Group III, S2− concentration rises and Group IV sulfides (e.g. ZnS, NiS) would precipitate early with Group III.
9.
Anion Cl−; cation NH4+ → ammonium chloride, NH4Cl.
10.
Anion SO42−; cation Cu2+ (Group II) → copper(II) sulfate, CuSO4 (CuSO4·5H2O).

How to use this worksheet

  1. Give the blank flowchart before the first salt analysis practical; students complete it from the NCERT lab manual and keep it in their practical file.
  2. Use the answer key as a wall chart or bench card — it prints on one A4 page.
  3. Parts B–D mirror the Experiment | Observation | Inference format required in CBSE practical record books.
  4. Part E checks understanding of why each group reagent works (common-ion effect, solubility products) — common viva questions.
  5. Set the title, student lines and answer option on the left, then press Download PDF and choose “Save as PDF” (or print directly). Your choices are remembered on this device.

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Frequently asked questions

What are the group reagents in salt analysis?

Group I dil. HCl; Group II H₂S in dil. HCl; Group III NH₄Cl + NH₄OH; Group IV H₂S in ammoniacal medium (NH₄Cl + NH₄OH); Group V (NH₄)₂CO₃ with NH₄Cl + NH₄OH; Group VI Na₂HPO₄ (Mg²⁺). NH₄⁺ (zero group) is tested by heating the salt with NaOH.

Why is NH₄Cl added before NH₄OH in Group III?

NH₄Cl supplies NH₄⁺ ions that suppress the ionisation of NH₄OH (common-ion effect). The OH⁻ concentration is then high enough to precipitate only Fe(OH)₃ and Al(OH)₃, which have very low solubility products, and not the hydroxides of Groups IV–VI.

Why does Pb²⁺ appear in both Group I and Group II?

PbCl₂ is slightly soluble in cold water, so precipitation in Group I is incomplete. The Pb²⁺ left in solution is precipitated as black PbS when H₂S is passed in Group II.

Which anions are detected with dilute and concentrated sulfuric acid?

Dilute H₂SO₄ group: CO₃²⁻, S²⁻, SO₃²⁻, NO₂⁻ (and CH₃COO⁻). Concentrated H₂SO₄ group: Cl⁻, Br⁻, I⁻, NO₃⁻ (and C₂O₄²⁻). SO₄²⁻ and PO₄³⁻ are detected by independent tests.

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