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### 15 Cards in this Set

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 Bronsted-Lowry Acid Lewis Acid Arrhenius Acid proton donor e- pair acceptor produces H+ Bronsted-Lowry Base Lewis Base Arrhenius Base proton acceptor e- pair donor produces OH- If the anion ends in -ite, it has ____ oxygen atoms and its acid should end with ___ If the anion ends in -ate, it has ____ oxygen atoms and its acid should end with ___ 1 or 2, -ous acid more than 2, -ic acid definition of pH and its generic equation definition of pOH and its generic equation a measure of H+ concentration pH=-log[H+] a measure of OH- concentration pOH==log[OH-] Kw definition and equation water dissociation constant, a constant that describes an equilibrium reaction. Kw=[H+][OH-]=10^-14 Rewrite the Kw equation in logarithmic form and another form pH+pOH=14 Kw=Ka x Kb= 1 x 10^-14 Log x^n = _____ Log 10^x = _____ -Log 10^-x = _____ nLog x x x Common strong Acids Hydrogen halides:HCl,HBr,HI Oxyacids of halogens:HClO3,HClO4,HBrO3,HBrO4 ,HIO3,HIO4 Sulfuric acid:H2SO4 Nitric acid:HNO3 Common strong Bases NaOH KOH CsOH Ca(OH)2 *mostly from the alkali group and some alkaline group the difference b/n strong acids/bases and weak acid/bases strong acids and bases dissociate completely into their component ions in aq solution. weaker species partially dissociate. common weak acids Formic HCOOH Acetic CH3COOH Trichloroacetic CCl3COOH Hydrofluoric HF Hydrocyanic HCN Hydrogen sulfide H2S Water H2O Conjugate acids of weak bases NH4+ common weak bases ammonia NH3 trimethyl ammonia N(CH3)3 pyridine C5H5N ammonium hydroxide NH4OH water H2O HS- ion HS- conjugate bases of weak acids e.g.: HCOO- HA+H20->H30+ + A- Ka equation [H30+][A-]/[HA] *only for aq molecules define conjugate acid define conjugate base the acid formed when a base gains a proton formed when an acid loses a proton Neutralization reaction The reverse of this is called _____ HA + BOH -> BA + H20 hydrolysis