MrChemCoach – Qualitative Analysis Virtual Lab

🧴 Reagents

Few Drops Excess

Dilute HNO₃

Dilute HCl

AgNO₃ (aq)

Ba(NO₃)₂ (aq)

NaOH (aq)

NH₃ (aq)

NaOH + Al (warm)

KMnO₄ (acidified)

💡 Note: Always acidify with HNO₃ before testing for Halides or Sulfates to avoid interference.

🔬 Unknown Samples

📓 Coach's Notebook

Observations Log

Select a tube and add reagents…

🔬 Identified Anion: ⚛️ Identified Cation:

🏆 Score: 0 / 0

Anion	Test Method	Positive Result
Carbonate (CO₃²⁻)	Add dilute acid (HCl)	Effervescence, carbon dioxide produced (turns limewater milky)
Chloride (Cl⁻)	Acidify with dilute HNO₃, then add AgNO₃	White curdy ppt.
Bromide (Br⁻)	Acidify with dilute HNO₃, then add AgNO₃	Cream ppt.
Iodide (I⁻)	Acidify with dilute HNO₃, then add AgNO₃	Yellow ppt.
Nitrate (NO₃⁻)	Add aqueous NaOH, then Al foil; warm	Ammonia gas produced (turns damp red litmus blue)
Sulfate (SO₄²⁻)	Acidify with dilute HNO₃, then add Ba(NO₃)₂	Dense white ppt. (insoluble in acid)
Sulfite (SO₃²⁻)	Add dilute HCl, warm gently	SO₂ produced turns acidified KMnO₄ from purple to colorless

Cation	Effect of aqueous NaOH	Effect of aqueous NH₃
Aluminium (Al³⁺)	White ppt., soluble in excess (colorless)	White ppt., insoluble in excess
Ammonium (NH₄⁺)	Ammonia gas produced on warming	-
Calcium (Ca²⁺)	White ppt., insoluble in excess	No ppt. or very slight white ppt.
Chromium(III) (Cr³⁺)	Grey-green ppt., soluble in excess (green)	Grey-green ppt., insoluble in excess
Copper(II) (Cu²⁺)	Light blue ppt., insoluble in excess	Light blue ppt., soluble in excess giving a dark blue solution
Iron(II) (Fe²⁺)	Green ppt., insoluble in excess	Green ppt., insoluble in excess
Iron(III) (Fe³⁺)	Red-brown ppt., insoluble in excess	Red-brown ppt., insoluble in excess
Zinc (Zn²⁺)	White ppt., soluble in excess (colorless)	White ppt., soluble in excess (colorless)

📖 CBSE & IGCSE Qualitative Analysis Theory