⚗️ Kenyan Chemistry Practical
🧪 Practical📘 Syllabus💧 Ions🔬 Radicals💧 Solubility🔬 Precipitates🔄 Complex Ions⭐ Upgrade
🐢 Slow
Fast 🐇
| Cation | Anion | Word equation | Products' Colour |
|---|---|---|---|
colourless | colourless | — | — |
🧪 Reactants → Product
—
Cation
—
Anion
?
Product
🧪 About This Chemistry Practical Simulator
🎯 Purpose
This software simulates KCSE Chemistry Paper 3 practical experiments. Students explore ion reactions, flame tests, titration, gas identification, cation tests, enthalpy, solubility, complex ions, redox, electrochemistry, radioactivity, carbonates, rates of reaction, chemical equilibrium, gas laws, and precipitates — all interactively. Covers the entire KCSE practical syllabus.
👨🔬 Who Is It For?
Form 1-2: Word equations with chemical names.
Form 3-4: Ionic equations with symbols.
Teachers: Classroom demonstration tool.
Students: Self-study and exam preparation.
Premium Users: Full access to all simulations.
Form 3-4: Ionic equations with symbols.
Teachers: Classroom demonstration tool.
Students: Self-study and exam preparation.
Premium Users: Full access to all simulations.
💡 Features (Free)
• Ion reactions (72 combos)
• Flame tests (6 cations)
• 2 titration experiments
• Gas identification reference guide
• Cation confirmatory tests
• 1 enthalpy experiment
• 1 solubility curve (KNO₃)
• 1 electrochemistry display
• Radioactivity simulator
• Carbonates heating simulator
• Rates of Reaction simulator
• Chemical Equilibrium simulator
• Gas Laws simulator
• 5 practice questions
• Precipitates, ions & radicals reference
• Flame tests (6 cations)
• 2 titration experiments
• Gas identification reference guide
• Cation confirmatory tests
• 1 enthalpy experiment
• 1 solubility curve (KNO₃)
• 1 electrochemistry display
• Radioactivity simulator
• Carbonates heating simulator
• Rates of Reaction simulator
• Chemical Equilibrium simulator
• Gas Laws simulator
• 5 practice questions
• Precipitates, ions & radicals reference
⭐ Premium Features
• All 12 cations + 9 anions = 108+ reactions (unlimited)
• Animated Gas Test Simulator
• 10 titration experiments
• 5 enthalpy experiments
• Full 7 solubility curves
• Complex ion formation simulator
• Redox reactions simulator
• 5 electrochemistry simulations
• 15+ practice questions
• No reaction limits
• Ad-free
• Animated Gas Test Simulator
• 10 titration experiments
• 5 enthalpy experiments
• Full 7 solubility curves
• Complex ion formation simulator
• Redox reactions simulator
• 5 electrochemistry simulations
• 15+ practice questions
• No reaction limits
• Ad-free
📘 Table of Contents
🧪 Ion Reactions
12 cations, 9 anions. Word & ionic equations. Visual test tubes. 108+ reactions. Premium
🔥 Flame Tests
Li⁺, Na⁺, K⁺, Ca²⁺, Ba²⁺, Cu²⁺, Sr²⁺ flame colours with Bunsen animation.
🧪 Titration
10 experiments: acid-base, redox (KMnO₄/Fe²⁺), back titration. Premium
💨 Gas Tests
O₂, H₂, CO₂, NH₃, Cl₂, SO₂, NO₂, HCl. Animated simulations. Premium
✅ Cation Tests
Fe²⁺, Fe³⁺, Cu²⁺, Zn²⁺, Al³⁺, Pb²⁺, Cr³⁺, Mn²⁺ with NaOH/NH₃.
⚡ Electrochemistry
Visual electrochemical cells with salt bridge, electrodes, and reference data. Premium
☢️ Radioactivity
Alpha, beta, gamma rays. Penetrating power, half-life decay, nuclear equations, magnetic deflection.
🔥 Carbonates
Heat effects on 8 carbonates. Decomposition, colour changes, limewater test, residues.
⚡ Rates of Reaction
Collision theory, concentration, temperature, surface area, catalyst. Particle-level animations.
⚖️ Equilibrium
Dynamic equilibrium, Le Chatelier's principle. NO₂/N₂O₄, Haber, CaCO₃ reactions.
🎈 Gas Laws
Boyle's Law, Charles' Law, Graham's Law. Interactive particle simulations.
🔄 Complex Ions
Interactive step-by-step complex ion formation simulator. Premium
🔥 Enthalpy
5 experiments. Temperature-time graphs. ΔH calculations. Premium
💧 Solubility
7 solubility curves, fractional crystallization, KCSE questions. Premium
📝 Practice
15+ MCQ questions with auto-marking & marking scheme. Premium
💧 Ions Guide
All cations, anions & complex ions reference with colours.
🔬 Radicals
13 polyatomic radicals, oxidation states, redox simulator. Premium
🔬 Precipitates
Full precipitates guide with solubility rules and colours.
🔥 Flame Test Colours Form 1-2 | Practical
Select cation
💡 Select a metal cation.
🧪 Titration Simulator — KCSE Format Form 3-4 | Practical
Pipette: 25.0 cm³ base. Auto-record ON — readings capture automatically at endpoint.
Burette
💧
Flask
Final: 0.00 cm³ | Initial: 0.00 cm³
| Titration number | 1 (Rough) | 2 | 3 |
|---|---|---|---|
| Final burette reading (cm³) | — | — | — |
| Initial burette reading (cm³) | 0.00 | — | — |
| Volume of solution used (cm³) | — | — | — |
📝 Calculations:
💨 Gas Identification Tests — Interactive Simulator Premium Form 1-2 | Practical
Select a gas below to run the confirmatory test. Splint relighting, litmus paper changes, bleaching, and dichromate paper tests are animated.
A
B
💥 POP!
BEFORE TEST
A — Wet Blue Litmus Paper |
B — Wet Blue Litmus Paper
Oxygen (O₂)
👆 Select a gas and click Run Test.
📋 Gas Tests Reference
🟢 O₂ (Oxygen)
Glowing splint relights. Colourless, odourless.
Lab prep: 2H₂O₂ →MnO₂→ 2H₂O + O₂
Lab prep: 2H₂O₂ →MnO₂→ 2H₂O + O₂
💥 H₂ (Hydrogen)
Burning splint: "pop" sound.
Lab prep: Zn + 2HCl → ZnCl₂ + H₂
Lab prep: Zn + 2HCl → ZnCl₂ + H₂
⬜ CO₂ (Carbon dioxide)
Limewater milky. Blue litmus→red. Extinguishes flame.
Lab prep: CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂
Lab prep: CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂
🟡 NH₃ (Ammonia)
Red litmus→blue. Pungent. White fumes with HCl.
Lab prep: NH₄Cl + NaOH → NaCl + H₂O + NH₃
Lab prep: NH₄Cl + NaOH → NaCl + H₂O + NH₃
🟢 Cl₂ (Chlorine)
Blue litmus→red→bleaches. Greenish-yellow.
Lab prep: MnO₂ + 4HCl → MnCl₂ + 2H₂O + Cl₂
Lab prep: MnO₂ + 4HCl → MnCl₂ + 2H₂O + Cl₂
🟤 SO₂ (Sulphur dioxide)
Blue litmus→red→bleaches. K₂Cr₂O₇→green.
Lab prep: Na₂SO₃ + H₂SO₄ → Na₂SO₄ + H₂O + SO₂
Lab prep: Na₂SO₃ + H₂SO₄ → Na₂SO₄ + H₂O + SO₂
🟠 NO₂ (Nitrogen dioxide)
Red-brown gas. Turns blue litmus red.
Lab prep: 2Pb(NO₃)₂ →heat→ 2PbO + 4NO₂ + O₂
Lab prep: 2Pb(NO₃)₂ →heat→ 2PbO + 4NO₂ + O₂
⬜ HCl (Hydrogen chloride)
White fumes with NH₃. Blue litmus→red.
Lab prep: NaCl + H₂SO₄ → NaHSO₄ + HCl
Lab prep: NaCl + H₂SO₄ → NaHSO₄ + HCl
✅ Cation Tests & Complex Ions Form 3-4 | Practical
Fe²⁺
+NaOH: Dirty green ppt
+NH₃: Dirty green ppt
Insoluble in excess
+NH₃: Dirty green ppt
Insoluble in excess
Fe³⁺
+NaOH: Red-brown ppt
+NH₃: Red-brown ppt
Insoluble in excess
+NH₃: Red-brown ppt
Insoluble in excess
Cu²⁺
+NaOH: Blue ppt
+Excess NH₃: Deep blue
+Excess NH₃: Deep blue
Zn²⁺
+NaOH: White ppt
+Excess: Dissolves → [Zn(OH)₄]²⁻
+Excess: Dissolves → [Zn(OH)₄]²⁻
Al³⁺
+NaOH: White gel
+Excess: Dissolves → [Al(OH)₄]⁻
+Excess: Dissolves → [Al(OH)₄]⁻
Pb²⁺
+NaOH: White ppt
+Excess: Dissolves
+KI: Bright yellow ppt
+Excess: Dissolves
+KI: Bright yellow ppt
Cr³⁺
+NaOH: Grey-green ppt
+Excess: → [Cr(OH)₄]⁻ green
+Excess: → [Cr(OH)₄]⁻ green
Mn²⁺
+NaOH: Pale pink ppt
Darkens in air → brown
Darkens in air → brown
🔄 Complex Ion Formation Simulator Premium Form 3-4 | Theory
Step-by-step simulation of complex ion formation with excess reagent.
Initial
0 drops
👆 Select a cation and reagent, then add drops.
🔥 Enthalpy Experiments Form 3-4 | Practical
Plateau, peak-fall, or steady change.
Beaker Therm. 0s 25.0°C |
| 0s | 30s | 60s | 90s | 120s | 150s | 180s | 210s |
|---|---|---|---|---|---|---|---|
| 25.0 | - | - | - | - | - | - | - |
📝 Questions:
⚡ Electrochemistry — Live Simulation Premium Form 4 | Theory
Interactive electrochemical cell with salt bridge, external circuit, electron flow, electrode reactions, and visual indicators.
⏱ 00:00
E° = +1.10V
ELECTROCHEMICAL CELL — DANIELL CELL
ZnSO₄(aq)
CuSO₄(aq)
Salt Bridge — KNO₃(aq)
💡 Press START to begin. Watch: anode dissolves, cathode deposit grows, ions migrate, electrons flow through external circuit, bulb glows, salt bridge maintains neutrality.
📋 Electrochemistry Reference & KCSE Calculations
📐 Cell Data
Cell Diagram: Zn(s)|Zn²⁺(aq)||Cu²⁺(aq)|Cu(s)
E°cell = +1.10V
Anode (oxidation): Zn(s) → Zn²⁺(aq) + 2e⁻
Cathode (reduction): Cu²⁺(aq) + 2e⁻ → Cu(s)
Overall: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)
E°cell = +1.10V
Anode (oxidation): Zn(s) → Zn²⁺(aq) + 2e⁻
Cathode (reduction): Cu²⁺(aq) + 2e⁻ → Cu(s)
Overall: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)
📝 KCSE Exam Questions
Q1. Calculate mass of copper deposited when 2A flows for 30 min. (Cu=63.5, 1F=96500C)
Q = It = 2 × 1800 = 3600C
mass = (63.5 × 3600)/(2 × 96500) = 1.18g
Q2. Why does the anode wear out?
Metal oxidizes: M(s) → Mⁿ⁺ + ne⁻, losing mass as ions dissolve.
Q3. Quantity of electricity to deposit 3.2g Cu?
Moles = 3.2/63.5 = 0.0504; Q = 0.0504 × 2 × 96500 = 9727C
Q4. Why inert electrodes?
Conduct without reacting. Platinized Pt increases surface area.
Q = It = 2 × 1800 = 3600C
mass = (63.5 × 3600)/(2 × 96500) = 1.18g
Q2. Why does the anode wear out?
Metal oxidizes: M(s) → Mⁿ⁺ + ne⁻, losing mass as ions dissolve.
Q3. Quantity of electricity to deposit 3.2g Cu?
Moles = 3.2/63.5 = 0.0504; Q = 0.0504 × 2 × 96500 = 9727C
Q4. Why inert electrodes?
Conduct without reacting. Platinized Pt increases surface area.
☢️ Radioactivity Simulator Premium Form 4 | Theory
Explore alpha, beta, gamma rays — penetrating power, half-life decay, nuclear equations, and magnetic deflection.
☢️
DETECTOR
α — — —
β — — —
γ — — —
💡 Select radiation type and barrier, then click Fire Rays to see penetration.
α Alpha
Stopped by paper or skin. Highly ionizing. Helium nucleus (⁴₂He). Charge: +2
β Beta
Stopped by aluminium (3mm). Fast electron. Charge: -1
γ Gamma
Stopped by thick lead or concrete. EM wave. No charge
🔥 Effects of Heat on Carbonates Premium Form 2 | Practical
Heat various carbonates and observe decomposition, colour changes (hot & cold), and gas tests.
0s | Temp: 25C
Observations
Before: -
During: -
Hot: -
Cold: -
Gas: -
Splint: -
Litmus: -
⚗️ Select a carbonate and heat to see the equation.
📋 Carbonates Heating Reference
🟤 CuCO₃
Green → Black (CuO)
CO₂ evolved
CuCO₃ → CuO + CO₂
CO₂ evolved
CuCO₃ → CuO + CO₂
⬜ CaCO₃
White → White (CaO)
CO₂ evolved, needs strong heat
CaCO₃ → CaO + CO₂
CO₂ evolved, needs strong heat
CaCO₃ → CaO + CO₂
⬜ ZnCO₃
White → Yellow (hot ZnO)
→ White (cold ZnO)
ZnCO₃ → ZnO + CO₂
→ White (cold ZnO)
ZnCO₃ → ZnO + CO₂
⬜ PbCO₃
White → Yellow/Orange (PbO)
CO₂ evolved
PbCO₃ → PbO + CO₂
CO₂ evolved
PbCO₃ → PbO + CO₂
🧂 Na₂CO₃ & K₂CO₃
NO decomposition!
Only melt at high temps
Very stable — Group 1 carbonates
Only melt at high temps
Very stable — Group 1 carbonates
💨 (NH₄)₂CO₃
SUBLIMES — NO residue!
NH₃ + CO₂ + H₂O vapour
White solid disappears completely
Test tube ends up empty & clean
NH₃ + CO₂ + H₂O vapour
White solid disappears completely
Test tube ends up empty & clean
⚡ Rates of Reaction — Collision Theory Simulator Form 3-4 | Theory
Watch particles collide! Change concentration, temperature, surface area, or add a catalyst and see how reaction rate changes in real-time.
Concentration: More particles = more collisions = faster reaction. Compare low vs high concentration.
Conc
Low
REACTANTS → PRODUCTS
REACTANTS
PRODUCTS
Products: 0 | Collisions: 0 | Timer: 0s
💡 Click Low Conc or High Conc to start. Watch how particle count affects reaction speed.
⚖️ Chemical Equilibrium — Le Chatelier's Principle Form 3-4 | Theory
📖 Le Chatelier's Principle: "When a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system shifts to oppose (counteract) the change and restore a new equilibrium."
Watch dynamic equilibrium in action! Particles weave continuously — forward AND reverse reactions happen at the SAME RATE.
R: 0 | P: 0
🔄 Ready. Click Start.
💡 Particles weave left⇄right continuously with glow trails — forward AND reverse at the SAME RATE.
🎈 Gas Laws — Interactive Particle Simulator Form 3 | Theory
Watch gas particles respond to changes in pressure, volume, and temperature. See Boyle's, Charles', and Graham's Laws in action!
📖 Boyle's Law: For a fixed mass of gas at constant temperature, pressure is inversely proportional to volume. P₁V₁ = P₂V₂
Drag the slider to move the piston wall. Watch how pressure changes as particles have less space to bounce!
Volume:
6.5 L
PISTON
📦 Vol: 6.5 L
📊 Pres: 1.0 atm
⬅ Particles bounce off walls ➡
🔍 Observation: As the piston moves LEFT (volume decreases), particles hit walls more often → pressure INCREASES.
💧 Solubility & Solubility Curves Premium Form 3-4 | Theory
Select a salt, heat the solution. All 7 curves plot simultaneously.
Therm.
Beaker
Bunsen
Time: 0sTemp: 20°CSol: 0g
● KNO₃● KCl● NaCl● Ce₂(SO₄)₃● K₂SO₄● NaNO₃● Pb(NO₃)₂
💡 Key Note: Solubility of one salt does NOT interfere with another.
📊 Calculations: Solubility = (Mass of solute ÷ Mass of water) × 100 | Mass crystallized = Mass at T₁ − Mass at T₂
📊 Calculations: Solubility = (Mass of solute ÷ Mass of water) × 100 | Mass crystallized = Mass at T₁ − Mass at T₂
📝 KCSE Exam-Style Questions
- Mass of KNO₃ in 50g water at 60°C?
(110×50)÷100 = 55g KNO₃ - KCl crystallized cooling 70°C→30°C in 200g water?
98g − 74g = 24g KCl - Best salts for fractional crystallization?
KNO₃ and KCl — KNO₃ has steep curve. - Ce₂(SO₄)₃ behaviour when heated?
Solubility DECREASES — dissolves exothermically. - 80g NaNO₃ in 100g water at 30°C — saturated?
80g < 96g → Unsaturated. - Pb(NO₃)₂ crystallized 80°C→20°C in 150g water?
210g − 84g = 126g
📝 Practice Questions 15+ in Premium Form 1-4 | Theory
Answer all. Click Submit & Mark for your score.
💧 Ions Guide — Cations, Anions & Complex Ions Form 1-4 | Reference
🟢 Cations (15)
Na⁺ || Sodium — colourless aq
K⁺ || Potassium — colourless aq
NH₄⁺ || Ammonium — colourless aq
Li⁺ || Lithium — colourless aq
Ca²⁺ || Calcium — colourless aq
Mg²⁺ || Magnesium — colourless aq
Al³⁺ || Aluminium — colourless aq
Zn²⁺ || Zinc — colourless aq
Fe²⁺ || Iron(II) — pale green aq
Fe³⁺ || Iron(III) — yellow-brown aq
Pb²⁺ || Lead(II) — colourless aq
Cu²⁺ || Copper(II) — blue aq
Ba²⁺ || Barium — colourless aq
Cr³⁺ || Chromium(III) — grey-green aq
Mn²⁺ || Manganese(II) — pale pink aq
🟠 Anions (9)
OH⁻ || Hydroxide — colourless aq
SO₄²⁻ || Sulphate — colourless aq
SO₃²⁻ || Sulphite — colourless aq
CO₃²⁻ || Carbonate — colourless aq
Cl⁻ || Chloride — colourless aq
Br⁻ || Bromide — colourless aq
I⁻ || Iodide — colourless dilute aq
NO₃⁻ || Nitrate — colourless aq
HCO₃⁻ || Hydrogen carbonate — colourless aq
🔄 Complex Ions (7)
[Al(OH)₄]⁻ || Al(OH)₃ + OH⁻ → colourless
[Zn(OH)₄]²⁻ || Zn(OH)₂ + 2OH⁻ → colourless
[Pb(OH)₄]²⁻ || Pb(OH)₂ + 2OH⁻ → colourless
[Cr(OH)₄]⁻ || Cr(OH)₃ + OH⁻ → green
[Cu(NH₃)₄]²⁺ || Cu(OH)₂ + 4NH₃ → deep blue
[Ag(NH₃)₂]⁺ || AgCl + 2NH₃ → colourless
[Zn(NH₃)₄]²⁺ || Zn(OH)₂ + 4NH₃ → colourless
🔬 Radicals Guide Premium Form 3-4 | Reference
Common radicals tested in KCSE. Formulas, valencies, oxidation states.
📋 Complete Radicals Reference
| Radical | Formula | Valency | Central Atom | Oxid. State | Appearance |
|---|---|---|---|---|---|
| Ammonium | NH₄⁺ | 1+ | N | -3 | Colourless aq |
| Hydroxide | OH⁻ | 1- | O | -2 | Colourless aq |
| Nitrate(V) | NO₃⁻ | 1- | N | +5 | Colourless aq |
| Sulphate(VI) | SO₄²⁻ | 2- | S | +6 | Colourless aq |
| Carbonate | CO₃²⁻ | 2- | C | +4 | Colourless aq |
| Manganate(VII) | MnO₄⁻ | 1- | Mn | +7 | Purple aq |
| Dichromate(VI) | Cr₂O₇²⁻ | 2- | Cr | +6 | Orange aq |
🔬 Redox Reactions Simulator Premium
Reactant
→Product
⭐ Essential KCSE Radicals
MnO₄⁻
Purple. Oxidizing agent. Redox titrations.
Purple. Oxidizing agent. Redox titrations.
Cr₂O₇²⁻
Orange→green when reduced.
Orange→green when reduced.
S₂O₃²⁻
Iodine titration. "Clock reaction".
Iodine titration. "Clock reaction".
SO₄²⁻
White ppt with Ba²⁺ (BaSO₄).
White ppt with Ba²⁺ (BaSO₄).
CO₃²⁻
Produces CO₂ with acids.
Produces CO₂ with acids.
🔬 Theoretical Precipitates Guide Form 1-4 | Reference
Common precipitates, ionic equations, colours, and excess reagent behaviour.
🟡 Carbonates (CO₃²⁻)
Ca²⁺: CaCO₃ ↓ white
Mg²⁺: MgCO₃ ↓ white
Zn²⁺: ZnCO₃ ↓ white
Fe²⁺: FeCO₃ ↓ green-grey
Cu²⁺: CuCO₃ ↓ blue-green
Pb²⁺: PbCO₃ ↓ white
Ba²⁺: BaCO₃ ↓ white
Soluble: Na⁺, K⁺, NH₄⁺
🟠 Sulphates (SO₄²⁻)
Ca²⁺: CaSO₄ ↓ white
Ba²⁺: BaSO₄ ↓ white (insoluble in acid)
Pb²⁺: PbSO₄ ↓ white
Soluble: Na⁺, K⁺, NH₄⁺, Mg²⁺, Al³⁺, Zn²⁺, Fe²⁺, Fe³⁺, Cu²⁺
⚪ Chlorides (Cl⁻)
Pb²⁺: PbCl₂ ↓ white
Ag⁺: AgCl ↓ white
Soluble: All others
🔵 Hydroxides (OH⁻)
Al³⁺: Al(OH)₃ ↓ white gel → [Al(OH)₄]⁻
Zn²⁺: Zn(OH)₂ ↓ white → [Zn(OH)₄]²⁻
Fe²⁺: Fe(OH)₂ ↓ dirty green
Fe³⁺: Fe(OH)₃ ↓ red-brown
Cu²⁺: Cu(OH)₂ ↓ blue → [Cu(NH₃)₄]²⁺
Cr³⁺: Cr(OH)₃ ↓ grey-green → [Cr(OH)₄]⁻
📋 KCSE Solubility Rules: ✅ Soluble: Na⁺, K⁺, NH₄⁺ salts, all nitrates, most chlorides. ❌ Precipitates: Most carbonates, BaSO₄/PbSO₄/CaSO₄, most hydroxides, AgCl/PbCl₂/PbI₂.