$word_{count}$: 200

Conductance G = 1/R (Siemens). Conductivity kappa = G * $cell_{constant}$ $\frac{S}{cm}$. Molar conductivity $Lambda_m$ = kappa * 1000/C (S.$cm^2$/mol). Upon dilution: kappa decreases (fewer ions per $cm^3$), but $Lambda_m$ increases (more dissociation per mole). For strong electrolytes, $Lambda_m$ increases linearly with decreasing sqrt(C) — Debye-Huckel-Onsager equation. Lambda_m_{infinity} is found by extrapolation. For weak electrolytes, $Lambda_m$ increases sharply near infinite dilution — cannot extrapolate. Use Kohlrausch's law. Degree of dissociation: alpha = \frac{Lambda_m}{Lambda_m_infinity}. Combined with Ostwald's dilution law: Ka = C*alpha^$\frac{2}{1-alpha}$. H+ (349.6) and OH- (198) have anomalously high ionic conductivities due to the Grotthuss proton-hopping mechanism.