Unformatted text preview: ate base reacting with H2O to form the conjugate acid and OH. • Know Lewis definitions for acids and bases. – Be able to identify the Lewis acid or base in a given reaction. – Know why nitrogen‐containing compounds are generally Lewis bases. – Know highly charged cations (Al3+, Cu2+, etc.) can act as Lewis acids and why. • Recognize how structure, bond strength and bond polarity influence the properties of an acid. – Be able to explain: – Why HF is weak while HCl, HBr, HI are strong – Why CH4 does not display acidic properties – Why some ternary oxyacids are strong while others are weak (e.g. HNO3 vs HNO2) – Ka values for different acids based on structure page 2 of 4 Chapter 17: Acids And Bases (Continued) • Water is amphoteric; it can act as an acid or a base. • Autoionization of water: 2 H2O(l) H3O+(aq) + OH (aq) Kw = [H+][OH–]=1.0x10–14 Kw = water’s ion‐product or dissociation constant – When [H+] = [OH–], the solution is neutral. – When [H+] > [OH–], the solution is acidic. – When [H+] < [OH–], the solution is basic. – Be able to so...
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This document was uploaded on 03/22/2014 for the course CHEM 162 at Seattle Central Community College.
- Fall '11