PPT-Unit IV Chemical Equilibrium Focusing on Acid-Base Systems

Chemical System A system is described in terms of empirical properties such as temperature pressure volume and amount of substance present By definition all chemical systems are fast quantitative stoichiometric and spontaneous However this assumption is NOT always true. 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. 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, . 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: . Equilibria. Electrolytes. Acids and Bases (review). The Equilibrium Constant. Equilibrium Expressions. “. Special. ”. Equilibrium Expressions. Solubility Products. Common-Ion Effects. Weak Acids and Bases. 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. A Practical Application of the Principles of Equilibrium. Water is always in equilibrium with its ions:. 2H. 2. O(l) .   . H. 3. O. . (. aq. ) . OH. -. (. aq. ). K. W. = [. H. 3. O. . Daley & . Daley. Chapter 5. :. Acid-base theory. 5.1 Acids & bases: overview & basics. 5.2 Acid & base strength. 5.3 Equilibrium acid-base reactions. 5.4 The leveling effect of solvents. Demonstrate understanding of equilibrium principles in aqueous systems. Aqueous systems are limited to those involving sparingly soluble ionic solids and acidic and basic solutions (in which proton transfer occurs). . This achievement standard involves demonstrating understanding . of . chemical reactivity. .. Rates . of Reaction . typically involves:. factors . affecting rates of reaction – restricted to changes in . Lecture Presentation. James F. Kirby. Quinnipiac University. Hamden, CT. © 20. 15. Pearson Education, Inc.. 16.1 & 16.2 Some . Definitions. Arrhenius. An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions.. A.S. 91392. Chemistry 3.6. 5 . external credits. Equilibrium Systems. N. 2. (g) 3H. 2. (g) 2NH. 3. (g) - H. What is the formula for the equilibrium constant Kc?. What can be said about the concentrations if Kc is very small?. Topics:. 3A_Chemical Reactions and . Stoichiometry. 3B_Types of Chemical Reactions. 3C_Driving Forces, Energy Changes and Electrochemistry. Topic 3A_Chemical Reactions and . Stoichiometry. Chemical Equations. 4.1 Introduction for Reactions. A physical change occurs when a substance undergoes a change in properties, but not a change in composition. Changes in the phase of a substance (solid, liquid, gas)or formation/separation of mixtures of substances are common physical changes. Acid. is defined as a substance which when dissolved in water gives hydrogen ions. (H +) . Examples.. Base is defined as a substance which when dissolved in water gives hydroxyl ions. (OH-) . Examples..