Nernst Equation
For electrochemical cell reaction $aA + bB \rightarrow cC + dD$ at $298\text{ K}$:
$$E_{\text{cell}} = E^\circ_{\text{cell}} - \frac{0.0591}{n}\log_{10} \frac{[C]^c [D]^d}{[A]^a [B]^b}$$
$$\Delta G^\circ = -n F E^\circ_{\text{cell}} = -2.303 RT \log K_c$$
Kohlrausch's Law of Independent Migration
Limiting molar conductivity ($\Lambda_m^\circ$) of an electrolyte is the sum of individual ionic conductivities of its cations and anions:
$$\Lambda_m^\circ (\text{NaCl}) = \lambda^\circ(\text{Na}^+) + \lambda^\circ(\text{Cl}^-)$$
- Degree of dissociation: $\alpha = \frac{\Lambda_m}{\Lambda_m^\circ}$
