CHEM 1120 1nd Edition Lecture 12Outline of Last Lecture I. Radiation Units and Dosesa. Gray (Gy)b. Radc. Sievert (Sv)d. Reme. Radon (Rn)II. Begin Chapter 16 (Acids and Bases)-Not on Exam 1III. Acids and Bases: A brief reviewa. Arrhenius acid and base definitionIV. Bronsted-Lowry Acid Base Definitiona. Conjugate Base Pairsb. Strong Acids and BasesOutline of Current Lecture I. Acid-Base Reactionsa. Autoionization of waterb. pH equationc. Acid disassociation constantII. Strong Acids and Basesa. Strong acidsb. Strong basesc. Weak acidsCurrent LectureThese 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.III. Acid-Base reactionsa. Equilibrium will favor the reaction that moves the proton to the stronger baseb. Autoionization of wateri. Water is amphoteric, in pure water, a few molecules act as bases and a few act as acidsii. Water is a very weak electrolyteiii. Kw = [H+][OH-] = 1 x 10 ^-24 at 25 degrees Celsius1. Called ion product constant for waterc. pH = -log10 [H+]i. 2 significant digits = 2 decimal placesii. pOH = -log [OH-]iii. pKw = pH + pOH = 14iv. pH < 7 : acidic, pH > 7 : basicd. Acid dissociation constanti. Ka = [H+][A-] / [HA]ii. Only works for weak acidsIV. Strong Acids and Basesa. Strong acidsi. Strong electrolytes and exist totally as ions in aqueous solutionsb. Strong basesi. Substances completely dissociate in aqueous solutionc. Weak acidsi. Most acidsii. Memorize 7 common strong acidsiii. Ka is a measure of acid strength1. Smaller k weaker acid2. For all acids k>> 13. Calculations using Ka are similar to those using Keq in Chapter 15iv. Must use ICE table to calculate concentrations in weak
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