11: Ionic Equilibrium, Weak Acid/Base Ionization (Ostwald's Law), K_w, and pH/pOH — الكيمياء الصف الثاني الثانوي لغات

درس «11: Ionic Equilibrium, Weak Acid/Base Ionization (Ostwald's Law), K_w, and pH/pOH» فى مادة الكيمياء لـالصف الثاني الثانوي لغات من وحدة «Change and Equilibrium of Matter». This lesson details ionic equilibrium in aqueous solutions, contrasting strong, weak, and non-electrolytes. It derives Ostwald's Dilution Law (α = √(K_a/C)) and weak acid/base formulas ([H⁺] = √(K_a C)). It covers the autoionization of water, establishing K_w = [H⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 25 ^{\circ}\text{C}, and the logarithmic pH and pOH scales (pH + pOH = 14.00). هتتعلم فى الدرس ده: Strong electrolytes dissociate 100%; Weak electrolytes establish dynamic ionic equilibrium.، Acid ionization constant: K_a =...

الدرس ده من وحدة «Change and Equilibrium of Matter» فى مادة الكيمياء لـالصف الثاني الثانوي لغات على منصة دروسات.

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ملخص الدرس

This lesson details ionic equilibrium in aqueous solutions, contrasting strong, weak, and non-electrolytes. It derives Ostwald's Dilution Law (α = √(K_a/C)) and weak acid/base formulas ([H⁺] = √(K_a C)). It covers the autoionization of water, establishing K_w = [H⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 25 ^{\circ}\text{C}, and the logarithmic pH and pOH scales (pH + pOH = 14.00).

هتتعلم إيه فى الدرس ده

• Strong electrolytes dissociate 100%; Weak electrolytes establish dynamic ionic equilibrium.
• Acid ionization constant: K_a = [H₃O⁺][A⁻]/[HA].
• Ostwald's law: Degree of ionization α = √(K_a / C) increases upon dilution.
• Weak acid [H⁺] = √(K_a * C); Weak base [OH⁻] = √(K_b * C).
• Water autoionization: K_w = [H⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 25 ^{\circ}\text{C}.
• pH = -log[H⁺], pOH = -log[OH⁻], and pH + pOH = 14.00.