Chem 102 1st Edition Lecture 9 Outline of Last Lecture I. Weak AcidsA. Polyprotic AcidsII. Weak BasesOutline of Current LectureI. Relationship Between Ka and KbII. Acid-Base Properties of Salt SolutionsA. StructureIII. Lewis Acids and BaseCurrent Lecture I. Relationship Between Ka and Kb- Used to quantify the relationship between acid and conjugate base. -When 2 reactions are added to give a third, the equilibrium for the third reaction is the product of the equilibrium of the first 2. K1 x K2 = K3-For a conjugate acid-base pair:Ka x Kb = KwII. Acid-Base Properties of Solutions-Nearly all salts are strong electrolytes, salts exist entirely of ions in solution. -Acid-Base properties of salts are a consequence of the reaction oftheir ions in solution. -The reaction in which ions produce H+ or OH- in water is called hydrolysis. -Anions from weak acids are basic-Anions from strong acids are neutral-Anions with ionizable protons are amphotericThese 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.A. Structure-Binary- acid strength increases across a period and down a group. Base strength decreases across a period and down a group. HF is a weak acid because the bond energy is high. The electronegativity difference between C and H is so small that C-H bond is non-polar and CH4 is neither an acid nor a base. -Oxyacids- Conation O-H bonds. All oxyacids have the general structure Y-O-H. The strength of the acid depends on Y and the atoms attached to Y. -Carboxylic acids- These are the organic acids which contain a COOH group. When the proton is removed, the negative charge is delocalized over the carboxylic anion. The strength increases as the number of electronegative R groups. III. Lewis Acids and Bases -Bronsted-Lowry acid is a proton donor. A bronsted-lowry acid can be considered as an electron acceptor pair. Lewis acid: electron pair acceptor. Lewis base: electron pair donor. Lewis acid and bases do not contain protons. Lewis acids generally have an incomplete octet. Transition metals are considered Lewis acids. Lewis acids must have a vacant orbital.-Hydrolysis of Metal Ions- Metal ions are positively charged and attract water molecules. Thehigher the charge, the smaller the metal ion and the stronger the M-OH2
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