Chem 113 1st Edition Lecture 24 Outline of Last Lecture I. Deriving the van’t Hoff equationII. Aqueous equilibriaIII. Bronsted-Lowry Acid Base DefinitionIV. Strong and Weak AcidsV. Classifying the relative strengths of acidsVI. Conjugate acid-base pairsOutline of Current Lecture I. Reactions of acids and bases in waterII. Relative strengths of some acids and basesCurrent LectureI. Reactions of acids and bases in watera. Strong bases (Kb>>1) includei. Water soluble compounds containing an O2- or OH- ionii. Cations are usually though of the most active metals (Group 1 or two metals)1. M2O or MOH, where M = Group 1A(1) metal (Li, Na, K, Rb, Cs)2. MO or M(OH)2 where M = group 2A(2) metal (Ca, Sr, Ba).b. Weak bases (Kb<1) includei. Ammonia (NH3)ii. Amines, which have the general formula RNH2, R2NH, or R3Niii. The common structural feature is an N atom with a lone electron pairiv. Compounds containing nitrogen in aqueous environments act as weak bases because the lone pair is used to bond to free hydrogen atoms in the solutionThese 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.II. Relative strengths of some acids and basesa. The major structural difference between strong and weak acids is the structure of the conjugate basei. Strong acids have weak conjugate basesii. Weak bases are better at stabilizing (-) chargeb. The major structural difference between strong and weak bases is the structure of the conjugate acidi. Strong bases have weak conjugate acidsii. Strong bases are bad at stabilizing (-)
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