1 / 8

Unit 3A – Acid/Base

Unit 3A – Acid/Base. By: Nikola Popovic, Rory Fencl, Jonathan Hooyman. Strong Acids and Bases. Strong Acids HCl, HBr, HI, H2SO 4 , HNO 3 , HClO 4 Strong Bases First 2 columns of periodic table + OH -. Example of a typical reaction. “molecular” HCl + NaOH  H 2 O + NaCl

brandy
Download Presentation

Unit 3A – Acid/Base

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  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

More Related