Chem 113 1st Edition Lecture 27 Outline of Last Lecture I. Consequences of KwII. The pH ScaleIII. pH, pOH, and pKwIV. The Acid Dissociation Constant, KaOutline of Current Lecture V. The Acid Dissociation Constant KaVI. Percent ionizationVII. The Base Dissociation Constant KbVIII. Aqueous Solutions of AmmoniaCurrent LectureI. The Acid Dissociation Constant Kaa. The value of Ka is an indication of acid strengthi. Stronger acid higher % dissociation of HAlarger Kaii. Weaker acid lower % dissociation of HA smaller Kaiii. Kc= Ka=HA¿−¿¿¿¿[¿ ¿3 O ]¿¿¿b. Use RICE tables when solving for Ka at equilibriumII. Percent ionizationa. [H+] at equilibrium represents the percent ionization of the acidb. As the concentration of a weak acid decreases, the percent ionization increasesIII. The Base Dissociation Constant Kba. Kc= Kb=OH¿−¿¿ ¿¿BaH +¿¿¿¿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.b. The value of Kb is an indication of base strengthi. Stronger base higher % accepting H+ from H2O larger Kbii. Weaker base lower % accepting H+ from H2O smaller KbIV. Aqueous Solutions of Ammoniaa. Ammonia (NH3) is a weak base and can accept a proton from water via the following equilibriumi. NH3 (aq)+H2O (l) NH4+ (aq)+OH- (aq)ii. The pH of the solution is dependatnt on [OH-]1. [OH-] at equilibrium can be found using RICE
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