Ostwald's dilution law: alpha = sqrt$\frac{Ka}{C}$ for weak acids (when alpha << 1). As dilution increases (C decreases), alpha increases — more molecules dissociate. However, [H+] = sqrt(Ka*C) decreases with dilution. At infinite dilution, alpha approaches 1 (complete dissociation) but [H+] approaches 0. For strong electrolytes, apparent degree of dissociation is described by the van't Hoff factor i = 1 + (n-1)*alpha, where n = number of ions per formula unit. For weak electrolytes, i is close to 1. For strong electrolytes, i approaches n (the theoretical maximum). Degree of dissociation affects colligative properties through the van't Hoff factor.