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Chem Unit 3

QuestionAnswer
Arrhenius acid H+ generater in solutions
Arrhenius base OH- generator in solutions
Brosnted-Lowry acid H+ donor
Bronsted-Lowry base H+ acceptor
Lewis acid e- pair acceptor
Lewis base e- pair donor
strong acid and base completely dissociated and reactions use a single arrow
weak acids and bases partially dissociate and reaction uses on equilibrium arrow
the strong acids HCL, HBr, HI, HNO3, HCLO3, HCLO4, H2SO4
the strong bases LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
monoprotic acids acids that contain only one ionizable proton
conjugate acid-base pairs two substances related to each other by a single proton (H+)
conjugate base an acid that donates a proton
conjugate acid a base that accepts a proton
amphoteric substance can act as an acid or base
autoionization when pure water reacts as both an acid and a base within itself
ion product constant for water Kw = [H3O+] [OH-] = 1.0x10^-14
neutral when [H3O+] = [OH-] or when pH = 7
acidic when [H3O+] > [OH-] or when pH < 7
basic when [H3O+] < [OH-] or when pH is > 7
how to calculate pH -log[H3O+]
how to calculate pOH -log[OH-]
salt formed during an acid-base neutralizing reaction
what is the pH when the cation nor the anion act as an acid nuetral
what is the pH when the cation does not act as an acid, but the anion acts as a base basic
what is the pH when the cation acts as an acid, but the anion does not act as a base acidic
polyprotic acids contains two or more acidic protons that dissociate in sequential steps, each with a unique Ka value
binary acid contains a hydrogen atom bonded to another atom
oxoacids contain a hydrogen atom bonded to an oxygen atom, which is then bonded to another atom
Created by: user-1972564
 

 



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