$word_{count}$: 150

For weak electrolytes, Ka = Calpha^$\frac{2}{1-alpha}$. When alpha << 1 (under 5%): Ka approximately equals C$alpha^2$, giving alpha = sqrt$\frac{Ka}{C}$. Key implications: (1) alpha increases with dilution — at infinite dilution, alpha approaches 1. (2) [H+] = Calpha = sqrt(KaC) decreases with dilution. (3) These two trends are not contradictory: a larger fraction dissociates, but the absolute number of ions per unit volume decreases. The van't Hoff factor i = 1 + (n-1)*alpha connects dissociation to colligative properties, where n = number of ions. For strong electrolytes, alpha approximately equals 1 and i approximately equals n. Always verify alpha < 5% before using the approximation; otherwise solve the quadratic.