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An in-depth exploration of acids and bases, including self-ionization of water, Arrhenius and Bronsted-Lowry models, characteristics, calculating pH and pOH, neutralization reactions, monoprotic and polyprotic acids, and titrations. Topics cover the definitions, dissociation, and reactions of acids and bases, as well as the importance of pH and pOH in determining acidity and basicity.
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a) Water molecules collide, causing a very small number to ionize in a reversible reaction: H 2 O(l) + H 2 O(l) ↔ H 3 O+(aq) + OH-(aq) water molecules hydronium ion hydroxide ion b) The hydronium ion (H 3 O+) consists of a water molecule attached to a hydrogen ion (H+) by a covalent bond; thus, H 3 O+^ and H+^ can be used interchangeably in a chemical equation to represent a hydrogen ion in aqueous solution. Simplified equation for self-ionization of water: H 2 O(l) ↔ H+(aq) + OH-(aq) c) Water is considered neutral since it produces equal numbers of H+^ and OH-^ ions. Hydrogen ion concentration , shown as [H+] , for water = 1.0 x 10-7M Hydroxide ion concentration , shown as [OH-] , for water = 1.0 x 10-7M Self-ionization produces a tiny number of ions but explains how pure water can behave as a very weak electrolyte. d) Water is the usual solvent for acids and bases; the dissociation of acids or bases in an aqueous solution increases either the [H+] or [OH-], resulting in an aqueous solution that is no longer neutral.
b) Bronsted-Lowry Model of Acids and Bases
a) Acids
b) HONORS ONLY
a) A titration is a method for determining the unknown concentration of an acid or base solution by reacting it with a known volume and concentration of an opposing base or acid. b) Neutralization occurs when all H+^ ions in solution have bonded with all OH-^ ions in solution to produce water, a compound with a neutral pH of 7.0. c) Titrations are performed by carefully adding an acid in a burette to a base in a receiving flask until the pH of the base is neutralized to 7.0. The receiving flask contains a chemical “indicator” which turns color when a neutral pH in the base is achieved. The titration is complete at this point, referred to as the endpoint. The same process can be performed by adding a base to an acid in the receiving flask. d) Equation for calculating an unknown concentration of acid/base from a titration: (Macid)(Vacid)( # of H+) = (Mbase)(Vbase)( # of OH-) Where Macid = Molarity of acid Vacid = Volume of acid Mbase = Molarity of base Vbase = Volume of base
e) Examples:
e) The oxidizing agent is the substance that facilitates oxidation by accepting lost electrons; it is the substance that is reduced. f) The reducing agent is the substance that facilitates reduction by losing electrons; it is the substance that is oxidized. g) Analyzing redox reactions
APPENDIX: pH SCALE WITH COMMON SUBSTANCES