122_BLB9_16_V2 notes

122_BLB9_16_V2 notes - Chapter 16 Acid-Base Equilibria...

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Chapter 16 Acid-Base Equilibria • Acids: taste sour and cause dyes to change color. • Bases: taste bitter and feel soapy. • Acids increase [H + ] in solution • Bases increase [OH - ] in solution • acid + base salt + water Acids and Bases Acids and Bases A Brief Review A Brief Review The H + Ion in Water • The H + ( aq ) ion is a “proton” (no electrons) • The simplest acid “cluster” is H 3 O + ( aq ) others are H 5 O 2 + and H 9 O 4 + . Generally we use H + ( aq ) and H 3 O + ( aq ) interchangeably Br Br ønsted nsted -Lowry Acids Lowry Acids
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Proton Transfer Reactions Brønsted-Lowry acids and bases are defined as: • An acid donates H + • A base accepts H + (Brønsted-Lowry base does not need to contain OH - ) • Amphoteric substances can behave as acids and bases. Br Br ønsted nsted -Lowry Lowry Acids and Acids and Bases Bases Conjugate Acid-Base Pairs HA( aq ) + H 2 O( l ) H 3 O + ( aq ) + A - ( aq ) ACID BASE Conjugate ACID Conjugate BASE * H 2 O (the base) accepts a proton to become its conjugate acid * The conjugate base can remove a proton from H 3 O + to then become the acid, HA
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• The stronger the acid, the weaker the conjugate base!
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This note was uploaded on 07/17/2008 for the course CHEM 122 taught by Professor Zellmer during the Winter '07 term at Ohio State.

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122_BLB9_16_V2 notes - Chapter 16 Acid-Base Equilibria...

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