Unformatted text preview: [HA] CHEM 162 Exam 1 Review – Winter2013 Percent ionization = [H ] at equilibrium
100% [HA] Convert Ka and Kb: Kw = Ka ∙ Kb = 1.010–14 pH Calculations for Weak Bases – Write equation for reaction of base with H2O. – Write equilibrium expression for the weak base. – The weaker the base, smaller the Kb. – Set up ICE table with [A–] given or calculated. – Solve for x to calculate [OH–] and pOH of weak base solution. Acid‐Base Properties of Salts – salt = ionic compound – Soluble salts dissociate into ions in water. – Classify a given salt as acidic, basic, neutral. Ions that produce acidic solutions – NH4+ – Highly charged metal ions: Al3+, Zn2+, etc., except cations of strong bases Ions that produce basic solutions – anions that are conj. bases of weak acids. – all anions except anions of strong acids – Note: SO42 + H2O HSO4 + OH Ions that produce neutral solutions – do not react with H2O to make H+ or OH Salts with an acidic cation and basic anion – Classify a given salt as acidic, basic, neutral. – If Ka>Kb, salt is acidic. – If Kb>Ka, salt is basic. – Account for different ion concentrations by multiplying initial concentration with Ka or Kb. pH...
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This document was uploaded on 03/22/2014 for the course CHEM 162 at Seattle Central Community College.
- Fall '11