Misconception: At equilibrium, concentrations of reactants = concentrations of products. Correction: Concentrations are constant, not equal. The ratio is fixed by K, which can be very large or very small.

Misconception: A catalyst increases K and shifts equilibrium toward products. Correction: Catalyst increases rate of attainment only. No shift in position; no change in K.

Misconception: Adding more reactant increases K. Correction: K depends only on temperature. Adding reactant shifts equilibrium forward but leaves K unchanged.

Misconception: pH of 10^{-8} M HCl = 8. Correction: A strong acid cannot produce a basic solution. Water's autoionisation contribution (~10^{-7} M $H^{+}$) must be included. Correct pH ≈ 6.98.

Misconception: pH = 7 always means neutral. Correction: Neutral means [$H^{+}$] = [$OH^{-}$]. At temperatures above 25°C, Kw > 10^{-14}, so neutral pH < 7.

Misconception: Inert gas addition always shifts equilibrium. Correction: At constant volume → no effect (partial pressures unchanged). Only at constant pressure does it shift toward more gas moles.

Misconception: Ka = Cα (not Cα^{2}). Correction: Ka = Cα^{2}; the hydrogen ion concentration [$H^{+}$] = Cα = √(Ka·C).

Misconception: Ksp of $Ag_{2}CrO_{4}$ = [$Ag^{+}$][$CrO_{4}^{2-}$]. Correction: Ksp = [$Ag^{+}$]^{2}[$CrO_{4}^{2-}$]; stoichiometric coefficients become exponents.

Misconception: Higher Ksp always means higher solubility. Correction: Only valid for salts of the same formula type. Compare s values, not Ksp directly, across different formula types.

Misconception: Buffer pH depends on actual concentrations, not ratio. Correction: Henderson-Hasselbalch shows pH depends on [salt]/[acid] ratio; diluting a buffer does not change its pH.