PPT-Acid – Base Equilibrium

Problem 13 Example Calculate the number of grams of NH 4 Br that have to be dissolved in 100L of water at 25 o C to have a solution with a pH of 51 Example Calculate the number of grams of NH. 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. Definitions . Strong Acids. HCl. HBr. HI. HNO. 3. HClO. 4. H. 2. SO. 4. Acid: a species that supplies H. +. ions to water. Strong acid: an acid that completely ionizes in water forming an H. +. ion and an anion. Titration. Acid–Base Titration. The concentration of a weak acid or a weak base in water is difficult – if not impossible – to measure directly.. But we can calculate the concentration from the results of titration.. 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. When carbon dioxide d_______ in water it forms carbonic acid. The more c______ dioxide the more a_______ the solution becomes . ie. . The pH d_________!. If distilled water (pH 7.0) is exposed to air the carbon dioxide from the air will form dilute carbonic acid (pH 5.5-6.0). 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. 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.. Coakley. 2/27/2014. Quick Review: Acids. Acids are compounds which function as. hydrogen (H+) donors . in biochemical equations/solutes. The more free H+ ions available for donation, the more acidic the compound. For cells to function optimally, . a steady balance . between the acids and the bases . is necessary.. Acid-base balance represents homeostasis of hydrogen (H+) ion . concentration in . body fluids. . 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. . When the rates of the forward and reverse reactions become equal, the concentrations of the reactants and the products remain constant. This is the stage of chemical equilibrium. This equilibrium is . 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.. 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..