CEM142 1nd Edition Lecture 8Outline of Last Lecture I. Weak acidsII. Weak basesOutline of Current Lecture II. Bronsted-Lowry acid-base equilibriaIII. Conjugate acid-base pairsCurrent Lecture-Arrhenius definition of acids and bases-acid: releases H+-base: releases OH--Bronsted-Lowry definition (best definition)-acid: H+ donor-base: H+ acceptor-acid: HA (acid) + H2O (base) A- (base) + H3O+ (acid)-there are 2 couples called conjugate acid-base pairs-HA/A- and H3O+/H2O-note: acids are typically listed on the left and bases are typically listed on the right-amphiprotic: molecules that can act as an acid or base, depending on the molecule that they are reacting with-main one: H2O-as an acid: H2O/OH- or -as a base: H3O+/H2O-HSO3-These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.-as an acid: HSO3-/SO32- or -as a base: H2SO3/HSO3--NH3-as an acid: NH3/NH2- or -as a base: NH4+/NH3-a strong acid has a weak conjugated base-a weak acid has a strong conjugated base-Ka x Kb = Kw = 10-14-if Ka is large, Kb is small-if Ka is small, Kb is
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