CHEM 122 11th Edition Lecture 25 Outline of Last LectureI. Acids and Basesa. Arrhenius’s definitionb. Bronsted’s definitionc. CharacteristicsII. Conjugate Acid-Base PairsIII. Chemical structure of acidsa. Binary Hydridesb. Oxoacidsc. Carboxylic AcidsOutline of Current Lecture I. Strong Basesa. Properties of binary oxidesII. Lewis Acids and BasesIII. Autoionization of WaterIV. pH Scale for Acids and BasesCurrent LectureStrong Bases: bases that completely dissociate to ions in a solution.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.- All alkali metal hydroxides are strong bases: LiOH, NaOH, KOH, RbOH and CsOH- The heavier alkaline earth metal hydroxides are strong bases: Ca(OH)2, Sr(OH)2, Ba(OH)2o Be(OH)2 and Mg(OH)2 are weak basesAcid/Base Properties of Binary Oxides:- Basic anhydrides: “Bases without water” Made from metal oxides reacting with water to form bases. - Acid Anhydrides: “Acids without water) Mae from nonmetal oxides reacting with water to form acids.Lewis Acids and Bases: focuses on the electron pairs.- Lewis Acid: An electron pair acceptor.- Lewis Base: an electron pair donor.- Lewis developed Lewis electron dot structures based on electron pairs.Autoionization of Water: pure water dissociates to yield ions.- Ion product constant: + ¿H¿¿−¿OH¿¿Kw=¿ when the temperature is 25 degrees Celsius.- Electrolytic solution: aqueous solutions that contain high concentration of dissolved ionsthat conduct electricity- Nonelectrolyte solution: aqueous solutions that do not contain dissolved ions that do not conduct electricity.- If an acid is added to water, then the H+ concentration increases. The position of the equilibrium shifts to the left until the product of the ion concentrations equal Kw.- If a base is added then the OH- concentration increases and H+ decreases.pH scales for Acids and Bases: - pH= -log[H+]- as [H+] concentration decreases, pH increases.- P-function: pX= -log[X] X= any
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