1 / 12

Chapter 16 Acid-Base Equilibria

CHEMISTRY The Central Science 9th Edition. Chapter 16 Acid-Base Equilibria. 16.1: Acids and Bases: A Brief Review. Acids: taste sour cause dyes to change color Bases: taste bitter feel soapy Arrhenius: acids increase [H + ], bases increase [OH - ] in AQUEOUS solution

coby
Télécharger la présentation

Chapter 16 Acid-Base Equilibria

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. CHEMISTRYThe Central Science 9th Edition Chapter 16Acid-Base Equilibria Chapter 16

  2. 16.1: Acids and Bases: A Brief Review • Acids: taste sour • cause dyes to change color • Bases: taste bitter • feel soapy • Arrhenius: acids increase [H+], bases increase [OH-] in AQUEOUS solution • Arrhenius: acid + base  salt + water • Problem: the definition confines us to aqueous solutions Chapter 16

  3. 16.2: Brønstead-Lowry Acids and Bases • The H+ Ion in Water • The H+(aq) ion is a proton with no electrons • In water, the H+(aq) form clusters • The simplest cluster is H3O+(aq) • A hydrated proton • Larger clusters are H5O2+ and H9O4+ • Generally H+(aq) and H3O+(aq) are used interchangeably Chapter 16

  4. Proton Transfer Reactions • Brønsted-Lowry theory: • Acid donates H+ and base accepts H+ • Brønsted-Lowry base does not need to contain OH- • HCl(aq) + H2O(l)  H3O+(aq) + Cl-(aq) • HCl donates a proton to water (HCl is an acid) • H2O accepts a proton from HCl (H2O is a base) • Water can behave as either an acid or a base • Amphoteric substances can behave as acids and bases • With a stronger base, it is an acid (and vice versa) Chapter 16

  5. Conjugate Acid-Base Pairs • Whatever is left of the acid after the proton is donated is called its conjugate base • Whatever remains of the base after it accepts a proton is called a conjugate acid • After HA (acid) loses its proton it is converted into A- (base) • HA and A- are conjugate acid-base pairs • After H2O (base) gains a proton it is converted into H3O+ (acid) • H2O and H3O+ are conjugate acid-base pairs • Conjugate acid-base pairs differ by only one proton Chapter 16

  6. Relative Strengths of Acids and Bases • The stronger the acid, the weaker the conjugate base Chapter 16 Text, P. 618

  7. Generalizations about Acid and Base Behavior • Strong acids completely transfer their protons to water • The conjugate base of a strong acid has negligible acid-base properties • The conjugate acid of a strong base has negligible acid-base properties • Weak acids partly dissociate in aqueous solution • The conjugate bases of weak acids are weak bases • Substances with negligible acidity (CH4) contain H but don’t behave as acids in water • Their conjugate bases are strong bases (form (OH)- in water) Chapter 16

  8. Proton Transfer Reactions • Strong acids and bases react with water to liberate H+(aq) and (OH)-(aq) ions • The leveling effect of water: one can’t distinguish among the strengths of the strong acids or strong bases • Place HCl, HBr or HI in dilute acetic acid and there is a noticeable difference in their strengths • H+ is the strongest acid that can exist in equilibrium in aqueous solution • OH- is the strongest base that can exist in equilibrium in aqueous solution Chapter 16

  9. Proton Transfer Reactions • In acid-base reactions, the equilibrium favors transfer of the proton from the stronger acid to the stronger base • Strong acid in water: Equilibrium favors the right side • HSO4-(aq) + CO3-2(aq) SO4-2(aq) + HCO3-(aq) • Compare bases: CO3-2 is from HCO3- • SO4-2 is from HSO4- • Use chart ( P. 618) to determine which base is stronger (CO3-2) • The stronger base and acid are consumed • Proton is transferred to the stronger base • Production of the weaker electrolytes is favored Chapter 16

  10. The reaction favors theconsumption of the stronger acid and stronger base and the formation of the weaker acid and weaker base (the weaker electrolytes) Chapter 16

  11. Proton Transfer Reactions • Weak acid in water: Equilibrium favors the left side • The anion of the acid is a stronger base, so it accepts a proton from the H3O+ • HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2-(aq) • Use chart ( P. 618) to determine which base is stronger (C2H3O2-) • The stronger base and acid are consumed • Proton is transferred to the stronger base Chapter 16

  12. The reaction favors the consumption of the stronger acid and stronger base and the formation of the weaker acid and weaker base (the weaker electrolytes) • Complete Sample Problems: • # 5, 7, 9, 11, 15 Chapter 16

More Related