Interactive 3D Chemistry Virtual Lab
Explore chemical reactions, acid–base titrations, pH indicators, qualitative ionic analysis, and solution chemistry through accurate computational models.
Chemistry Learning & Reference Guide for School and University Students
The 3D virtual chemistry lab provides a safe practice space where learners can look up reactions, predict observations, and calculate concentrations accurately.
Secondary Students (Grades 8–12)
Practice acid–base titration, identify ions by precipitates, balance redox equations, and study atomic structure and periodic trends.
- Observe the pH jump at equivalence and indicator color changes.
- Look up solubility, precipitate colors, and gases formed in ionic reactions.
- Prepare effectively for national, IGCSE, and AP Chemistry exams.
University & Specialist Students
Model VSEPR geometry, reaction thermodynamics ΔH, ΔS, ΔG, equilibria Kc and Kp, and electrochemical cells with the Nernst equation.
- Rotate 3D models to study orbitals, bond angles, and dipole moments.
- Analyze reaction order and Arrhenius activation energy Ea.
- Study buffer solutions, solubility products Ksp, and transition-metal complexes.
Quick Chemistry Reference
Look up atomic structure, periodic trends, the metal activity series, molar masses, standard electrode potentials, and solubility rules.
- Data for 118 elements: electron configuration, electronegativity, and atomic radius.
- Indicator library including litmus, phenolphthalein, and bromothymol blue.
- English–Vietnamese IUPAC nomenclature aligned with international standards.
Key Chemistry Modules & Reaction Models
1. Acid - Base Titration & pH Equilibrium
Neutralization Reaction: $\text{H}^+ + \text{OH}^- \rightarrow \text{H}_2\text{O}$
pH Definition: $\text{pH} = -\log[\text{H}^+], \quad \text{pOH} = -\log[\text{OH}^-], \quad \text{pH} + \text{pOH} = 14$
Simulate titration curves of strong acid - strong base and weak acid - strong base with Phenolphthalein and Methyl Orange indicators.
2. Precipitation & Qualitative Ionic Analysis
Precipitation Example: $\text{Ba}^{2+} + \text{SO}_4^{2-} \rightarrow \text{BaSO}_4 \downarrow \text{ (White)}$
Silver Halide Test: $\text{Ag}^+ + \text{Cl}^- \rightarrow \text{AgCl} \downarrow \text{ (White)}, \quad \text{Ag}^+ + \text{I}^- \rightarrow \text{AgI} \downarrow \text{ (Yellow)}$
Identify cation and anion unknown solutions via characteristic precipitate colors and solubility rules.
3. Ideal Gas Laws & Thermochemistry
Ideal Gas Equation: $PV = nRT = \frac{m}{M}RT$
Enthalpy Change: $\Delta H = \sum \Delta H_f^\circ(\text{Products}) - \sum \Delta H_f^\circ(\text{Reactants})$
Measure gas volume production over time and calculate reaction rates under varying temperature and concentration conditions.
4. Chemical Kinetics & Iodine Clock Reaction
Rate Law & Arrhenius: $v = k[\text{S}_2\text{O}_8^{2-}]^m [\text{I}^-]^n, \quad k = A \exp\left(-\frac{E_a}{RT}\right)$
Clock Mechanism: $\text{S}_2\text{O}_8^{2-} + 2\text{I}^- \rightarrow 2\text{SO}_4^{2-} + \text{I}_2 \quad (\text{Starch} \rightarrow \text{Deep Blue-Black})$
Explore reaction order determination, sacrificial thiosulfate timing step, and instantaneous starch-iodine color flip delay.
5. Electrochemistry & Daniell Galvanic Cell
Nernst Cell EMF: $E = E^\circ - \frac{0.0592}{n}\log\left(\frac{[\text{Zn}^{2+}]}{[\text{Cu}^{2+}]}\right) \quad (E^\circ = +1.10\text{ V})$
Gibbs Free Energy: $\Delta G^\circ = -n F E^\circ = -212.3\text{ kJ/mol} \quad (F = 96485\text{ C/mol})$
Trace spontaneous electron flow from Zinc anode to Copper cathode and ion migration across the KCl agar salt bridge.
6. Buffer Solutions & Henderson-Hasselbalch
Buffer Equation: $\text{pH} = \text{p}K_a + \log\left(\frac{[\text{CH}_3\text{COO}^-]}{[\text{CH}_3\text{COOH}]}\right) \quad (\text{p}K_a = 4.75)$
Buffer Capacity: Resists drastic pH shifts upon addition of strong acids HCl or strong bases NaOH.
Compare buffered acetate resistance against unbuffered pure water showing dramatic 10,000-fold jump in $[\text{H}^+]$.
7. Complexometric EDTA Titration & Water Hardness
Chelation Equilibrium: $\text{Ca}^{2+} + \text{EDTA}^{4-} \rightarrow [\text{Ca(EDTA)}]^{2-} \quad (\log K_f = 10.7)$
Metallochromic Indicator: $[\text{Ca-EBT}] \text{ (Wine-Red)} \rightarrow \text{Free EBT} \text{ (Pure Sky-Blue at pH 10)}$
Quantitative assay of total mineral water hardness ($Ca^{2+}, Mg^{2+}$) expressed in $\text{mg CaCO}_3/\text{L}$ (ppm).
8. Triglyceride Saponification & Salting-Out
Saponification Reaction: $(\text{RCOO})_3\text{C}_3\text{H}_5 + 3\text{NaOH} \xrightarrow{\Delta} 3\text{RCOONa} \downarrow + \text{C}_3\text{H}_5(\text{OH})_3$
Salting-Out Effect: Saturated NaCl brine lowers sodium soap solubility through the common-ion Na⁺ effect.
Industrial soap making from vegetable oils, separation of glycerol, and solidification of white curd soap layers.
9. Molecular Spectroscopy & Beer-Lambert Law
Beer-Lambert Absorbance: $A = \varepsilon \cdot l \cdot c = -\log(T) = -\log(I / I_0)$
Quantitative Analysis: Linear absorbance calibration curve A = f(c) for an unknown solution concentration.
Measure photon attenuation across cuvettes with UV-Vis spectrophotometry for transition metal complexes and organic dyes.
