Easy Practice — Set 2

Quick Recap — Ionic Equilibrium & pH

• $K_w=[H^+][OH^-]=10^{-14}$ at 25$^\circ$C; $pH=-\log[H^+]$; $pH+pOH=14$.
• Acidic $pH<7$, basic $pH>7$, neutral $=7$.
• Strong acids/bases ionise completely; weak ones partially ($K_a$, $K_b$). Higher $K_a$ (lower $pK_a$) $\Rightarrow$ stronger acid.
• Buffers resist pH change; common-ion effect suppresses ionisation; $K_{sp}$ governs sparingly soluble salts.