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Unit 3A – Acid/Base

Unit 3A – Acid/Base

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Unit 3A – Acid/Base

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  1. Unit 3A – Acid/Base By: Nikola Popovic, Rory Fencl, Jonathan Hooyman

  2. Strong Acids and Bases • Strong Acids • HCl, HBr, HI, H2SO4, HNO3, HClO4 • Strong Bases • First 2 columns of periodic table + OH-

  3. Example of a typical reaction • “molecular” HCl + NaOH  H2O + NaCl • “total ionic” H+ + Cl- + Na+ + OH- Na+ + Cl- + H2O • “net ionic” H+ + OH- H2O

  4. General pH rules • For a strong acid reacting with a weak base, the pH will be lower then a weak acid with weak base, or strong acid with strong base • For a weak acid reacting with a strong base, the pH will be higher then a weak acid with weak base, or strong acid with strong base

  5. Acid/Base Definitions • Bronsted – Lowery • Acid: proton (H+) donor • Base: proton acceptor • According to Lewis Model • Acid: electron acceptor • Base: electron donor • Lewis acids and bases do not always involve H+ • Ex. When BF3 and NH3 react, the electron rich NH3 donates an electron pair to BF3 to form a stable bonding interaction. BF3 is the Lewis acid, and NH3 is the Lewis base

  6. Example Bronsted-Lowery • H2O + H2O  OH- + H3O+ acid base conjugate conjugate base acid

  7. General pH rules part II • pH scale • 1-6 = acid • 7 = neutral • 8-14 = base • pH = -log[H+] • pOH = -log[OH-] • 14 – pH = pOH

  8. Formulas Equilibrium Equation • NH * VA * CA = NOH * VB * CB