tailieunhanh - Chapter 16: Acid-Base Equilibria
Invite you to consult the lecture content "Chapter 16: Acid Base Equilibria" below. Contents of lectures introduce to you the content: Acids and bases: a brief review, bronsted lowry acids and bases, the autoionization of water, strong acids and bases, acid base behavior and chemical structure. Hopefully document content to meet the needs of learning, work effectively. | Copyright 1999, PRENTICE HALL Chapter 16 Acid-Base Equilibria Chapter 16 David P. White University of North Carolina, Wilmington 1 1 1 1 Copyright 1999, PRENTICE HALL Chapter 16 Acids and Bases: A Brief Review Acid: taste sour and cause dyes to change color. Bases: taste bitter and feel soapy. Arrhenius: acids increase [H+] bases increase [OH-] in solution. Arrhenius: acid + base salt + water. Problem: the definition confines us to aqueous solution. Copyright 1999, PRENTICE HALL Chapter 16 Brønsted-Lowry Acids and Bases The H+ Ion in Water The H+(aq) ion is simply a proton with no electrons. (H has one proton, one electron, and no neutrons.) In water, the H+(aq) form clusters. The simplest cluster is H3O+(aq). Larger clusters are H5O2+ and H9O4+. Generally we use H+(aq) and H3O+(aq) interchangeably. Copyright 1999, PRENTICE HALL Chapter 16 Brønsted-Lowry Acids and Bases The H+ Ion in Water Copyright 1999, PRENTICE HALL Chapter 16 Brønsted-Lowry Acids and . | Copyright 1999, PRENTICE HALL Chapter 16 Acid-Base Equilibria Chapter 16 David P. White University of North Carolina, Wilmington 1 1 1 1 Copyright 1999, PRENTICE HALL Chapter 16 Acids and Bases: A Brief Review Acid: taste sour and cause dyes to change color. Bases: taste bitter and feel soapy. Arrhenius: acids increase [H+] bases increase [OH-] in solution. Arrhenius: acid + base salt + water. Problem: the definition confines us to aqueous solution. Copyright 1999, PRENTICE HALL Chapter 16 Brønsted-Lowry Acids and Bases The H+ Ion in Water The H+(aq) ion is simply a proton with no electrons. (H has one proton, one electron, and no neutrons.) In water, the H+(aq) form clusters. The simplest cluster is H3O+(aq). Larger clusters are H5O2+ and H9O4+. Generally we use H+(aq) and H3O+(aq) interchangeably. Copyright 1999, PRENTICE HALL Chapter 16 Brønsted-Lowry Acids and Bases The H+ Ion in Water Copyright 1999, PRENTICE HALL Chapter 16 Brønsted-Lowry Acids and Bases Proton Transfer Reactions Focus on the H+(aq). Brønsted-Lowry: acid donates H+ and base accepts H+. Brønsted-Lowry base does not need to contain OH-. Consider HCl(aq) + H2O(l) H3O+(aq) + Cl-(aq): HCl donates a proton to water. Therefore, HCl is an acid. H2O accepts a proton from HCl. Therefore, H2O is a base. Water can behave as either an acid or a base. Amphoteric substances can behave as acids and bases. Copyright 1999, PRENTICE HALL Chapter 16 Brønsted-Lowry Acids and Bases Proton Transfer Reactions Copyright 1999, PRENTICE HALL Chapter 16 Brønsted-Lowry Acids and Bases Conjugate Acid-Base Pairs Whatever is left of the acid after the proton is donated is called its conjugate base. Similarly, whatever remains of the base after it accepts a proton is called a conjugate acid. Consider After HA (acid) loses its proton it is converted into A- (base). Therefore HA and A- are conjugate acid-base pairs. After H2O (base) gains a proton it is converted into H3O+ (acid). Therefore,
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