Acids, Bases, and Equilibrium Learning Lab
Fourteen guided chemistry lessons that connect particles, reactions, equations, graphs, and worked reasoning for acids, bases, equilibrium, buffers, titrations, and solubility.
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How this tool works
The learning lab organizes fourteen acid–base and equilibrium topics into a five-unit sequence with explicit learning goals, real chemical contexts, guided observations, and live calculations.
Each lesson explains what the model represents, why the result changes, and how the current values connect to particle-level chemistry and laboratory reasoning.
Every numerical value, imported state, solver iteration, and graph sample count is bounded before calculation or rendering.
Core equations
pH = −log₁₀[H⁺] and pH + pOH = 14 at 25 °CKaKb = KwHenderson–Hasselbalch: pH = pKa + log₁₀([A⁻]/[HA])reaction quotient: Q = [C]^c[D]^d / ([A]^a[B]^b)Kp = Kc(RT)^Δnvan’t Hoff: ln(K₂/K₁) = −ΔH/R(1/T₂ − 1/T₁)solubility product: Ksp = [M]^m[X]^nAssumptions
- Aqueous acid–base calculations use Kw = 1.0×10⁻¹⁴ and pKw = 14.00 at 25 °C.
- Weak-acid and weak-base calculations use monoprotic ideal-solution models unless the polyprotic module is selected.
- Activity coefficients are approximated as one, so concentration is used in place of activity.
- Titration models assume additive volumes and complete stoichiometric neutralization by the strong titrant.
- Generic equilibrium modules model one homogeneous reaction of the form aA + bB ⇌ cC + dD.
- Kc–Kp conversion assumes ideal gases.
Limitations
- Highly concentrated solutions, mixed polyprotic systems, activity corrections, simultaneous equilibria, electrochemical equilibria, and full speciation with charge balance are outside this version.
- The Le Châtelier module predicts a new ideal equilibrium from one selected disturbance; it is not a kinetic simulation.
- Results are educational estimates and do not replace laboratory procedures, calibrated analytical software, or chemical safety review.