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Chap18Notes - 1036 Chapter 18 1 of 42 1036 Chapter 18 3 of...

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1036 Chapter 18 1 of 42 Chapter 18 Acid-Base Equilibria What are Acids and Bases? Two classes of compounds: acids and bases 3 Definitions of acids and bases: 1. Arrhenius Definition: Acids: Bases: Examples: HCl(aq) NaOH(aq) 1036 Chapter 18 2 of 42 2. Bronsted-Lowry Definition: Acids: Bases: Deprotonation: Protonation: In an acid-base reaction, a proton is transferred from acid to base. Acids: Bases: HA(aq) + H 2 O H 3 O + (aq) + A - (aq) B(aq) + H 2 O(aq) BH + (aq) +OH(aq) HCl(aq) + H 2 O( l ) H 3 O + (aq) + Cl - (aq) NH 3 (aq) +H 2 O( l ) NH 4 + (aq) +OH - (aq) Or HCl(aq) H + (aq) + Cl - (aq) 1036 Chapter 18 3 of 42 HCl(aq) + NH 3 (aq) Cl - (aq) + NH 4 + (aq) Conjugate acid: Conjugate base: Example Problem : What is the conjugate acid of H 2 PO 4 - ? What is the conjugate base of HCO 3 - ? Example Problem : Identify the conjugate acid-base pairs in HIO 3 (aq) + HC 2 O 4 - (aq) IO 3 - (aq) + H 2 C 2 O 4 (aq) 1036 Chapter 18 4 of 42 Water - Acid or Base? Note the two acid-base reactions examined above: HCl(aq) + H 2 O( l ) H 3 O + (aq) + Cl - (aq) NH 3 (aq) +H 2 O( l ) NH 4 + (aq) +OH - (aq) Water is amphiprotic (amphoteric) : H 2 O( l ) + H 2 O( l ) H 3 O + (aq) + OH - (aq) Or H 2 O( l ) H + (aq) + OH - (aq) Printed with FinePrint - purchase at www.fineprint.com
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