Podcast
Questions and Answers
What is the observation when mixing barium chloride (BaCl2) with a solution containing sulfate ions (SO4–2)?
What is the observation when mixing barium chloride (BaCl2) with a solution containing sulfate ions (SO4–2)?
- A yellow precipitate forms.
- A white precipitate of barium sulfate forms. (correct)
- A red solution is formed.
- No precipitation occurs.
Which reaction produces a white precipitate that is soluble in mineral acids?
Which reaction produces a white precipitate that is soluble in mineral acids?
- Salt solution + BaCl2 with PO4-3 (correct)
- Salt solution + FeCl3 with PO4-3
- Salt solution + BaCl2 with SO4-2 (correct)
- Salt solution + AgNO3 with SO4-2
What occurs when NO2 is produced in a reaction mixture during a test for nitrate ions?
What occurs when NO2 is produced in a reaction mixture during a test for nitrate ions?
- A white precipitate forms.
- A brown solid forms.
- The mixture turns blue. (correct)
- No change occurs.
What color is the vapor produced when mixing HF with I2?
What color is the vapor produced when mixing HF with I2?
Which of the following methods would confirm the presence of phosphate ions (PO4–3)?
Which of the following methods would confirm the presence of phosphate ions (PO4–3)?
When heating a mixture that includes copper turnings and nitrate, which observation is expected?
When heating a mixture that includes copper turnings and nitrate, which observation is expected?
If no gas is evolved during the testing for acidic radicals, what can be inferred?
If no gas is evolved during the testing for acidic radicals, what can be inferred?
What is the result of adding sodium hydroxide to a solution containing manganous ions?
What is the result of adding sodium hydroxide to a solution containing manganous ions?
Which ion produces a black precipitate when treated with hydrogen sulfide in the presence of ammonium chloride and hydroxide?
Which ion produces a black precipitate when treated with hydrogen sulfide in the presence of ammonium chloride and hydroxide?
What happens to the cobalt hydroxide precipitate when warmed with excess sodium hydroxide?
What happens to the cobalt hydroxide precipitate when warmed with excess sodium hydroxide?
Which confirmatory test results in a red precipitate?
Which confirmatory test results in a red precipitate?
Which statement about zinc testing is false?
Which statement about zinc testing is false?
What indicates the presence of carbonate ion when dil.HCl is added to a solid salt?
What indicates the presence of carbonate ion when dil.HCl is added to a solid salt?
What is produced when sodium carbonate reacts with hydrochloric acid?
What is produced when sodium carbonate reacts with hydrochloric acid?
What color indicates a positive test for sulphide ion using lead acetate paper?
What color indicates a positive test for sulphide ion using lead acetate paper?
What is the result of treating sulphite ions with warm dilute HCl?
What is the result of treating sulphite ions with warm dilute HCl?
Which of the following tests would confirm the presence of bicarbonate ions?
Which of the following tests would confirm the presence of bicarbonate ions?
What is the confirmatory test for sulphite ion using barium chloride?
What is the confirmatory test for sulphite ion using barium chloride?
Which gas is evolved when sulfide ions react with warm dilute HCl?
Which gas is evolved when sulfide ions react with warm dilute HCl?
What is formed when sodium sulfite and hydrochloric acid react?
What is formed when sodium sulfite and hydrochloric acid react?
What color change occurs in potassium dichromate paper when exposed to sulfur dioxide gas?
What color change occurs in potassium dichromate paper when exposed to sulfur dioxide gas?
What gas is evolved when thiosulphate ion is treated with warm dilute hydrochloric acid?
What gas is evolved when thiosulphate ion is treated with warm dilute hydrochloric acid?
What color does potassium dichromate paper turn when exposed to the gas evolved from thiosulphate ion treatment?
What color does potassium dichromate paper turn when exposed to the gas evolved from thiosulphate ion treatment?
What precipitate is formed when thiosulphate ion is mixed with barium chloride solution?
What precipitate is formed when thiosulphate ion is mixed with barium chloride solution?
Which of the following indicates the presence of nitrite ions in a solution?
Which of the following indicates the presence of nitrite ions in a solution?
What happens to the solution when a solid nitrite is warmed with dilute hydrochloric acid?
What happens to the solution when a solid nitrite is warmed with dilute hydrochloric acid?
What is the resultant gas formed when nitrous acid decomposes?
What is the resultant gas formed when nitrous acid decomposes?
Which of the following is NOT a confirmatory test for nitrite ions?
Which of the following is NOT a confirmatory test for nitrite ions?
What color is the precipitate formed during the formation of lead thiosulphate?
What color is the precipitate formed during the formation of lead thiosulphate?
What is observed when ferric chloride solution is added to thiosulphate ion?
What is observed when ferric chloride solution is added to thiosulphate ion?
What is produced when sodium thiosulphate is treated with dilute hydrochloric acid?
What is produced when sodium thiosulphate is treated with dilute hydrochloric acid?
What is the result of adding disodium hydrogen phosphate to a magnesium salt solution with NH4Cl?
What is the result of adding disodium hydrogen phosphate to a magnesium salt solution with NH4Cl?
Which color is produced during the flame test for sodium ions?
Which color is produced during the flame test for sodium ions?
What is the precipitate formed when chromic ion Cr3+ reacts with a buffer solution?
What is the precipitate formed when chromic ion Cr3+ reacts with a buffer solution?
Which compound is indicated by the formation of a dark blue precipitate when ferrous ions react with potassium ferricyanide?
Which compound is indicated by the formation of a dark blue precipitate when ferrous ions react with potassium ferricyanide?
What happens when aluminium ions Al3+ react with ammonium sulfate?
What happens when aluminium ions Al3+ react with ammonium sulfate?
What is the outcome when ferric ion Fe3+ is treated with NaOH?
What is the outcome when ferric ion Fe3+ is treated with NaOH?
In the presence of sodium peroxide, which color solution is obtained from chromic ions?
In the presence of sodium peroxide, which color solution is obtained from chromic ions?
What is the identity of the precipitate formed when ferrous ammonium sulfate reacts with a buffer solution?
What is the identity of the precipitate formed when ferrous ammonium sulfate reacts with a buffer solution?
What distinguishes aluminium hydroxide from aluminium sulphide in reactions with ammonium sulphate?
What distinguishes aluminium hydroxide from aluminium sulphide in reactions with ammonium sulphate?
Which precipitation form occurs for group III cations consisting of chromic, aluminium, ferrous, and ferric ions?
Which precipitation form occurs for group III cations consisting of chromic, aluminium, ferrous, and ferric ions?
Flashcards
Sulphate Ion Test
Sulphate Ion Test
Adding barium chloride (BaCl2) to a salt solution will produce a white precipitate if sulphate ions (SO42-) are present. The precipitate is barium sulphate, which is insoluble in mineral acids.
Phosphate Ion Test
Phosphate Ion Test
Adding barium chloride (BaCl2) to a salt solution will produce a white precipitate if phosphate ions (PO43-) are present. The precipitate is barium phosphate, which is soluble in mineral acids.
Confirmatory Test for Sulphate
Confirmatory Test for Sulphate
Adding silver nitrate (AgNO3) to a concentrated salt solution containing sulphate ions (SO42-) will yield a white precipitate of silver sulphate.
Confirmatory Test for Phosphate
Confirmatory Test for Phosphate
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Bromide Iodide Test
Bromide Iodide Test
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Nitrate Test
Nitrate Test
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Acidic Radical Group II/III
Acidic Radical Group II/III
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Carbonate ion test
Carbonate ion test
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Carbonate ion confirmatory test (MgSO4)
Carbonate ion confirmatory test (MgSO4)
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Bicarbonate ion confirmatory test(HgCl2)
Bicarbonate ion confirmatory test(HgCl2)
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Sulfide ion test
Sulfide ion test
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Sulfide ion confirmatory test (Sodium Nitroprusside)
Sulfide ion confirmatory test (Sodium Nitroprusside)
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Sulfite ion confirmatory test (Barium)
Sulfite ion confirmatory test (Barium)
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Carbonate ion confirmatory test (BaCl2)
Carbonate ion confirmatory test (BaCl2)
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Carbonate ion confirmatory test (AgNO3)
Carbonate ion confirmatory test (AgNO3)
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Test for sulfite ion
Test for sulfite ion
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Thiosulfate ion test
Thiosulfate ion test
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Thiosulfate confirmation test
Thiosulfate confirmation test
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Nitrite ion test
Nitrite ion test
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Nitrite confirmation tests
Nitrite confirmation tests
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Sulfite + HCl
Sulfite + HCl
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Thiosulfate + HCl
Thiosulfate + HCl
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Nitrite + HCl
Nitrite + HCl
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Group V Basic Radicals
Group V Basic Radicals
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Barium Chloride ppt
Barium Chloride ppt
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Manganese Ion Test
Manganese Ion Test
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Nickel Ion Test
Nickel Ion Test
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Cobalt Ion Test
Cobalt Ion Test
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Zinc Ion Test
Zinc Ion Test
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Confirmatory Test for Zinc
Confirmatory Test for Zinc
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Magnesium Ion Test
Magnesium Ion Test
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Sodium Ion Test
Sodium Ion Test
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Chromic Ion (Cr3+) Test
Chromic Ion (Cr3+) Test
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Aluminium Ion (Al3+) Test
Aluminium Ion (Al3+) Test
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Ferrous Ion (Fe2+) Test
Ferrous Ion (Fe2+) Test
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Ferric Ion (Fe3+) Test
Ferric Ion (Fe3+) Test
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Group III Cations
Group III Cations
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Group Reagent
Group Reagent
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Precipitate Formation
Precipitate Formation
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Group IV Cations
Group IV Cations
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Study Notes
Acidic Radicals Scheme
- Experiment: Salt + dilute HCl
- Observation 1: Effervescence on cold, CO₂ gas evolved, which renders limewater turbid
- Result 1: CO₃⁻² or HCO₃⁻
- Observation 2: SO₂ gas suffocating odour on warming, turns acidified potassium dichromate paper to green and solution clear
- Result 2: SO₃⁻²
- Observation 3: SO₂ gas suffocating odour on warming, turns acidified potassium dichromate paper to green and solution becomes yellow due to sulphide precipitation
- Result 3: S₂O₃⁻² (S + SO₃⁻²)
- Observation 4: H₂S gas evolves on warming, has odour like rotten eggs, and blackens lead acetate paper
- Result 4: S⁻²
- Observation 5: NO₂ gas evolves, brown fumes, and solution turns faint blue
- Result 5: NO₃⁻
- Observation 6: No gas evolved
- Result 6: Acidic radical is not from group I; it may be from group II or group III
Acidic Radicals Scheme (cont.)
- Experiment: Salt + concentrated H₂SO₄
- Observation 1: HCl: colourless gas evolves which gives dense white fumes when a rod dipped in ammonium hydroxide is brought near the mouth of the test tube
- Result 1: Chloride (Cl⁻)
- Observation 2: Mix of HBr and Br₂: reddish-brown gases, solution turns reddish brown
- Result 2: Bromide (Br⁻)
- Observation 3: Mix of HF and I₂: violet vapours, which turn starch paper blue and a layer of violet sublimate is formed on the sides of the tube (sulphur ppt on walls of tube)
- Result 3: Iodide (I⁻)
- Observation 4: NO₂: Brown fumes evolve which become dense upon heating the reaction mixture after addition of copper turnings and the solution becomes faint blue
- Result 4: Nitrate (NO₃⁻)
- Observation 5: No gas evolved
- Result 5: Acidic radical is not from group II; it may be from group III
Acidic Radicals Scheme (cont.)
- Experiment: Salt solution + BaCl₂ solution
- Observation 1: White ppt of insoluble in mineral acids (barium sulphate)
- Result 1: SO₄⁻²
- Observation 2: White ppt of soluble in mineral acids (barium phosphate or barium metaborate)
- Result 2: PO₄⁻³ or B₄O₇⁻²
Acidic Radicals (SO₄⁻², PO₄⁻³, B₄O₇⁻²) Group III
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Test 1: Sulphate ions [SO₄⁻²] -Procedure: Salt solution + Barium chlorides (BaCl₂): White ppt of barium sulphate, insoluble in mineral acids -Confirmation tests: Concentrated Salt solution + AgNO₃: White ppt (Ag₂SO₄) -Procedure: Salt solution + lead acetate: White ppt soluble in ammonium acetate - NaOH
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Test 2: Phosphate ions [PO₄⁻³] -Procedure: Salt solution + Barium chlorides (BaCl₂): White ppt of barium phosphate, soluble in mineral acids -Confirmation tests: Salt solution + AgNO₃: Yellow ppt soluble in NH₄OH -Procedure: Salt solution + FeCl₃: Yellow ppt (FePO₄) soluble in mineral acids -Procedure: Salt solution + excess of ammonium molybdate + conc HNO₃ and heat: Canary yellow ppt
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Test 3: Borate ions [B₄O₇⁻²] -Procedure: Salt solution + Barium chlorides (BaCl₂): White ppt of (Ba(BO₂)₂), soluble in mineral acids
Acidic Radicals (Cl⁻, Br⁻, I⁻, NO₃⁻) Group II
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Test 1: Chloride anion [Cl⁻] -Procedure: Solid + a few drops of concentrated H₂SO₄ and warm: HCl evolves, recognized by formation of white clouds of ammonium chloride when a glass rod wetted with ammonia solution is held near the tube's mouth -Confirmation test: Salt solution + AgNO₃: White ppt (AgCl) soluble in dilute ammonia solution -Procedure: Concentrated salt solution + lead acetate: White ppt of lead chloride soluble in hot water
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Test 2: Bromide anion [Br⁻] -Procedure: Solid + concentrated H₂SO₄ and warm: Reddish-brown vapours of Br₂ + HBr are evolved, the solution becomes reddish-brown
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Confirmation Tests: Salt solution + AgNO₃: Pale yellow ppt soluble in dilute HNO₃ -Procedure: Salt solution + lead acetate: White ppt soluble in boiling water
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Test 3: Iodide anion [I⁻] -Procedure: Solid + concentrated H₂SO₄ and warm: Violet vapours (I₂) are evolved, which turn starch paper blue
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Confirmation Tests: Salt solution + AgNO₃: Yellow ppt soluble in ammonia solution
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Procedure: Salt solution + HgCl₂: Scarlet red ppt of mercuric iodide, soluble in excess KI
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Test 4: Nitrate anion [NO₃⁻] -Procedure: Solid + concentrated H₂SO₄ and heat: Brown fumes of NO₂ evolve, become dense upon heating the reaction mixture after addition of copper turnings, and the solution acquires blue colour
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Confirmation Tests: Salt solution + AgNO₃: Pale yellow ppt
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Procedure: Salt solution + FeSO₄ + conc H₂SO₄: Brown ring
Acidic Radicals (CO₃⁻², HCO₃⁻, S⁻², SO₃⁻², S₂O₃⁻², NO₃⁻) Group I
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Test 1: Carbonate and Bicarbonate -Procedure: If effervescence occurs with evolution of colourless, odourless gas upon adding dilute HCl to solid salt, carbonate or bicarbonate ion is present.
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Procedure: The gas turns lime water milky due to the formation of calcium carbonate. (Na₂CO₃ + HCl→NaCl + H₂O + CO₂) (Ca(OH)₂) + CO₂→CaCO₃ + H₂O Confirmatory Tests (CO₃⁻²): ----Salt solution+ MgSO₄: White ppt (MgCO₃) ----Salt solution + HgCl₂: Reddish brown ppt (HgCO₃-3HgO) if no ppt on cold. ----Salt solution + BaCl₂: White ppt (BaCO₃) ----Salt solution + AgNO₃: White ppt (Ag₂CO₃)
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Test 2: Sulphide ion [S⁻²]
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Confirmatory Tests: (S⁻²) Salt solution + Sodium Nitroprusside : Purple/Black ppt is formed, (S⁻²) Salt solution + Lead Acetate : Black ppt of lead sulphide (PbS),
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Test 3: Sulphite ion [SO₃⁻²]
- Procedure: Sulphite treated with warm dilute HCl, SO₂ gas is given off with smell of burning sulfur. This gas turns acidified potassium dichromate paper green and the solution becomes clear. K₂Cr₂O₇ + H₂SO₄ + 3SO₂ → K₂SO₄ + Cr₂(SO₄)₃ + H₂O
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Test 4: Thiosulphate ion [S₂O₃⁻²]
- On treating thiosulphate with warm dilute HCl, SO₂ gas is evolved with suffocating smell of burning sulfur. The gas turns potassium dichromate paper acidified with dil H₂SO₄ to green and the solution becomes clear.
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Test 5: Nitrite ion [NO₂⁻]
- On treating a solid nitrite with dilute HCl and warming, reddish brown fumes of NO₂ gas are evolved and the solution becomes pale blue.
Basic Radicals (Ba²⁺, Sr²⁺, Ca²⁺) Group V
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Test 1: Barium Ion [Ba²⁺]
- Procedure: Salt solution + (NH₄Cl) + (NH₄OH) + (NH₄)₂CO₃: White ppt of barium carbonate (BaCO₃)
- Confirmation Tests: -Salt solution + Potassium chromate (K₂CrO₄) : Yellow ppt of barium chromate (BaCrO₄) soluble in mineral acids -5 drops of salt solution + 4 drops of Ammonium oxalate solution: White ppt of barium oxalate (BaC₂O₄)
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Test 2: Strontium Ion [Sr²⁺]
- Procedure: Salt solution + (NH₄Cl) + (NH₄OH) + (NH₄)₂CO₃: White ppt of strontium carbonate (SrCO₃)
- Confirmation Tests: 6 drops of salt solution + 6 drops of Ammonium oxalate solution: White ppt of strontium oxalate (SrC₂O₄)
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Test 3: Calcium Ion [Ca²⁺]
- Procedure: Salt solution + (NH₄Cl) + (NH₄OH) + (NH₄)₂CO₃: White ppt of calcium carbonate (CaCO₃)
Basic Radicals (NH₄⁺, K⁺, Mg²⁺, Na⁺) Group VI
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Test 1: Ammonium Ion [NH₄⁺]
- Procedure: Salt solution + NaOH, solid and solution boiled: NH₃ gas evolved, and exposed to glass rod wetted with HCl, forming white fumes
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Procedure: Salt solution + Sodium cobalt nitrite (Na₃[Co(NO₂)₆]): Yellow ppt of ammonium cobalt nitrite (NH₄)₃[Co(NO₂)₆]
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Test 2: Potassium Ion [K⁺]
- Procedure: Salt solution + Sodium cobalt nitrite (Na₃[Co(NO₂)₆]): Yellow ppt of potassium cobalt nitrite (K₃[Co(NO₂)₆]).
-
Procedure: Flame test: Salt colors the flame violet
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Test 3: Magnesium Ion [Mg²⁺]
- Procedure: Salt solution + NH₄Cl + NH₄OH + Na₂HPO₄: White ppt of magnesium ammonium phosphate (MgNH₄PO₄)
- Procedure: Salt solution + NaOH: White ppt of magnesium hydroxide (Mg(OH)₂)
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Test 4: Sodium Ion [Na⁺]
- Procedure: Flame test: Salt colors the flame golden yellow.
Basic Radicals (Cr³⁺, Al³⁺, Fe²⁺, Fe³⁺) Group III
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Test 1: Chromic Ion [Cr³⁺] -Procedure: Soln of chromic nitrate + buffer: Pale green ppt Cr(OH)₃
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Test 2: Aluminium Ion [Al³⁺]
- Procedure: Soln of aluminium nitrate + buffer: Gelatinous white ppt Al(OH)₃
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Test 3: Ferrous Ion [Fe²⁺]
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Procedure: Soln of ferrous ammonium sulphate + buffer soln: Green ppt Fe(OH)₂
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Test 4: Ferric Ion [Fe³⁺]
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Procedure: Soln of Ferric Chloride + buffer soln: Brown ppt Fe(OH)₃.
Basic Radicals (Mn²⁺, Ni²⁺, Co²⁺, Zn²⁺) Group IV
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Test 1: Manganous Ion [Mn²⁺]
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Procedure: Salt solution + NH₄Cl + NH₄OH + H₂S: Buff ppt of manganese sulfide (MnS)
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Confirmatory Tests: Salt solution + NaOH: White ppt of manganous hydroxide (Mn(OH)₂), insoluble in excess reagent . Salt solution + Na₂HPO₄: White ppt of Manganese(II) Hydrogen Phosphate (MnHPO₄)
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Test 2: Nickel Ion [Ni²⁺] -Procedure: Salt solution + NH₄Cl + NH₄OH + H₂S: Black ppt of nickel sulphide (NiS) insoluble in mineral acid and soluble in aqua regia
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Confirmatory Tests: Salt solution + NaOH: Green ppt of nickel hydroxide (Ni(OH₂) insoluble in excess of the reagent. Salt solution + NH₄OH + Dimethylglyoxime: Red ppt of Nickel dimethylglyoxime (Ni(DMG)₂)
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Test 3: Cobalt Ion [Co²⁺]
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Procedure: Salt solution + NH₄Cl + NH₄OH + H₂S: Black ppt of cobalt sulfide (CoS) insoluble in mineral acid and soluble in aqua regia
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Confirmatory Tests: Salt solution + NaOH: Blue ppt changes to pink Co(OH)₂ on warming with excess of NaOH. Salt solution + Ammonium thiocyanate + drop of alcohol: Blue solution due to the formation of a complex salt of ammonium cobalt thiocyanate [(NH₄)₂Co(CNS)₄]
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Test 4: Zinc Ion [Zn²⁺]
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Procedure: Salt solution + NH₄Cl + NH₄OH + H₂S: White ppt of zinc sulphide (ZnS)
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Confirmatory Tests: Salt solution + NaOH: White ppt of zinc hydroxide (Zn(OH)₂) soluble in excess of the reagent Salt solution + Potassium ferrocyanide (K₄[Fe(CN)₆]): White ppt of zinc ferrocyanide (Zn₂[Fe(CN)₆])
Basic Radicals (Pb²⁺, Ag⁺, Hg₂²⁺) Group I
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Test 1: Lead Cation [Pb²⁺]
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Procedure: Soln of lead nitrate + dilute HCl: White ppt of lead chloride (PbCl₂), soluble in hot water.
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Confirmatory Tests: Soln + KI: Yellow ppt (PbI₂), soluble in hot water giving golden crystals, and Soln+K₂CrO₄: Yellow ppt (PbCrO₄) soluble in alkali hydroxides and nitric acid but insoluble in acetic acid.
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Test 2: Mercurous Cation [Hg₂²⁺]
- Procedure: Soln of mercurous nitrate + dilute HCl: White ppt of (Hg₂Cl₂), insoluble in hot water
- Confirmatory Tests: Soln+ KI: Yellow ppt (Hg₂I₂), soluble in excess of KI, forming complex K₂[HgI₄] Soln+ K₂CrO₄: Brown ppt of Hg₂CrO₄ in cold
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Test Silver Cation [Ag⁺]:
- Procedure: Soln of Silver nitrate + dilute HCl: White ppt (AgCl)
- Confirmatory Tests: -Soln + KI: Yellow ppt (AgI) -Soln +K₂CrO₄: Scarlet red ppt (Ag₂CrO₄) soluble in dilute nitric acid.
Group II-B
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Test 1: Stannous ions [Sn²⁺] -Procedure: Soln stannous chloride + dil HCl +H₂S: Brown ppt SnS, Soln + NaOH: White ppt Sn(OH₂) , Soln+HgCl₂: White ppt
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Test 2: Stannic ion [Sn⁴⁺]
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Procedure: Soln of stannic chloride + dil HCl +H₂S: yellow ppt, Soln +NaOH: White gelatinous Sn(OH)₄ soluble in excess of NaOH, Soln+HgCl₂: NO Preciptate
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Test 3: Antimonious ion [Sb³⁺]
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Procedure: Soln of antimony trichloride + dil HCl + H₂S: Orange ppt Sb₂Sз -Procedure: Soln +NaOH: White ppt
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Description
Explore the Acidic Radicals Scheme through detailed observations and results of various chemical experiments. This quiz covers the reactions of salts with dilute HCl and concentrated H₂SO₄, highlighting the gases evolved and their corresponding acidic radicals. Test your knowledge on identifying the outcomes and implications of these chemical reactions.
