PDF-Assignment 161. What is the pKof a base whose conjugate acid has a pKo

OH HN pH Solution This is a salt of a weak acid The reaction is 14 10 Now we can write the equilibrium constant 33 And make a reaction table Molecule 3 3 Initial 0450 00 00 D. Amine nomenclature. diisopropylamine. pyrrole. nicotine. histamine. pyrrolidine. Formation of amines. triethylamine. Mechanism for LAH reduction of amides. 1-methylpiperidine. One equivalent . SN2 is faster the more R groups on N. Marissa Levy. Boyi. Zhang. Shana . Zucker. What is an acid? What is A Base?. Arrhenius. Acid- An acid is a substance that when dissolved increases H. +. concentration. Base- A base is a substance that when dissolved increases OH. Common Ion Effect. Learning Outcomes and . Prereqs. Pre-. reqs. :. Identify how changing concentrations of reactants or products shift an equilibrium (Le . Chatelier’s. Principle). Learning Outcomes. of Salts. Acid-Base Properties of Salts. Type of Salt. Examples. Comment. pH of solution. Cation is from a strong base, anion from a strong acid. KCl, KNO. 3. NaCl. NaNO. 3. Both ions are neutral. Neutral. 17 Acids & Bases. The basics:. it’s just equilibrium. same K expressions, with new names: K. a. , K. b. same equilibrium calculations. What’s new:. the concept of . K. w. . p. -functions (pH, . of Salts. Acid-Base Properties of Salts. Type of Salt. Examples. Comment. pH of solution. Cation is from a strong base, anion from a strong acid. KCl, KNO. 3. NaCl. NaNO. 3. Both ions are neutral. Neutral. Different definitions of acids and bases. Acids are proton donors (. Brønsted. Lowry definition). they generate H. 3. O. +. in water (Arrhenius definition). Bases are proton acceptors. they generate OH. Different definitions of acids and bases. Acids are proton donors (. Brønsted. Lowry definition). they generate H. 3. O. +. in water (Arrhenius definition). Bases are proton acceptors. they generate OH. Acid-Base chemistry & pH. Recognizing acid/base and conjugate base/acid. Calculation of pH, . pOH. , [H. 3. O. +. ], [OH. -. ]. Calculating pH for solutions of strong acids/base. Ionization constant: . Principles of Chemical Reactivity: . The Chemistry of Acids and Bases. In Chapter 3, you were introduced to two definitions of acids and bases: the Arrhenius and the Brønsted–Lowry definition.. Arrhenius acid: Any substance that when dissolved in water increases the concentration of hydrogen ions, H. 2009, Prentice-Hall, Inc.. Titration. In . this technique a known concentration of base (or acid) is slowly added to a solution of acid (or base. ).. The . analyte. - is the solutions being evaluated and is of unknown concentration.. Different definitions of acids and bases. Acids are proton donors (. Brønsted. Lowry definition). they generate H. 3. O. +. in water (Arrhenius definition). Bases are proton acceptors. they generate OH. Just a few reminders. What makes an acid an acid?. A . Bronsted. -Lowry Acid is a compound that donates a proton (a hydrogen ion with a positive charge, H. +. ). Think of the standard acids that are commonly mentioned in Gen . Taken from State University of West Georgia Chemistry Dept.. Acid and Base Strengths. Taken from State University of West Georgia Chemistry Dept.. Hydronium Ions. Hydronium Ions. H. 5. O. 2. +. Dissociation of Water.