University:
York University
Course:
CHEM 1001 | Chemical Dynamics
Academic year:

2022
Views:

309

Pages:

1
Author:

Niklas

Exam #2 Chapter 7/Chapter 8 02/25/2027 03/02/2022 Lewis Base - any substance that can donate a pair of electrons - has lone pair electrons - may be neutral or anionic - ex. NH₃, OH⁻, Brønsted bases, H₂O, Cl⁻ Hydration of Lewis acid cations - metal ions attract lone pairs on oxygen in H₂O molecules - hydrated metal ions are acidic acidity increases with increasing charge /size ratio of the metal ions - Lewis acid-base interaction with coordinated water weakens the O-H bond Solutions of very dilute strong acids or bases - for very dilute solutions (10⁻⁹ M) we can't ignore H⁺, OH⁻ from water - use mass charge balance with Kw equation - Ex. HA + H₂O mass balance: [HA]₀ = [HA] + [A⁻] charge balance: [H⁺] = [A⁻] + [OH⁻]; [HA]₀ - [OH⁻] = [H⁺] [H⁺]² / [HA]₀ = Kw - pH = pKa when [HA] = [A⁻] Common Ion effect of Buffer Solutions - mixture of weak acid & conjugate base HA + A⁻ NaA + HA A⁻ is the common ion in the reaction - adding more NaA pushes the first equilibrium to the left