Chem 113 1st Edition Lecture 23 Outline of Last Lecture I. ΔG, Q, and K7II. ΔG, Equilibrium, and Reaction DirectionIII. ΔG and the Equilibrium ConstantIV. The Effect of a Change in TemperatureV. Temperature and KOutline of Current Lecture VI. Deriving the van’t Hoff equationVII. Aqueous equilibriaVIII. Bronsted-Lowry Acid Base DefinitionIX. Strong and Weak AcidsX. Classifying the relative strengths of acidsXI. Conjugate acid-base pairsCurrent LectureI. Deriving the van’t Hoff equationa. At two different temperatures, T1 and T2, we have two different values for K, K1 and K2i. lnK2=-ΔH°/RT2 and lnK1=-ΔH°/RT1II. Aqueous equilibriaa. The equilibria of aqueated species can have pronounced effects on everything from blossom colors, to coral reef formation and blood pHIII. Bronsted-Lowry Acid Base Definitiona. A Bronsted-Lowry acid is a proton donor, or any species that donates an H+ ioni. A Bronsted-Lowry Acid must contain H in its formulaThese 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.b. A Bronsted-Lowry base is a proton acceptor, or any species that accepts H+ ionsi. A Bronsted-Lowry base must contain a lone pair of electrons to bond to H+c. An acid-base reaction is a proton-transfer processIV. Strong and Weak Acidsa. A strong acid dissociates completely into ions in wateri. A dilute solution of a strong acid contains no HA moleculesii. Kc value will be much larger than 1b. A weak acid dissociates slightly to form ions in wateri. In a dilute solution of a weak acid, most HA molecules are undissociatedii. Kc value will be much less than 1c. Ka reflects acid association, Kb reflects base associationV. Classifying the relative strengths of acidsa. Strong acids includei. The hydrohalic acids (HCl, HBr, and HI)ii. Oxoacids in which the number of O atoms exceeds the number of ionizable protons by two or more (HNO3, H2SO4, HClO4)b. Weak acids includei. The hydrohalic acid HFii. Acids in which H is not bonded to O or to a Halogen (HCN)iii. Oxoacids in which the number of O atoms equals or exceeds the number of ionizable protons by one(HClO, HNO2)iv. Carboxylic acids, which have the general formal RCOOH (e.g., CH3COOH, C6H5COOH)VI. Conjugate acid-base pairsa. A Bronsted-Lowry acid-base reaction occurs when an acid and a base react to form their conjugate base and conjugate acidi. Acid – H+ = conjugate baseii. Base + H+= conjugate
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