Chap 4 Sec 4 & part 5

Chap 4 Sec 4 & part 5 - 4.4 Acid-Base Reactions...

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Chap 4 sec 4 & part 5 F09.doc Page 1 4.4 Acid-Base Reactions Arrhenius: Acids give off H + , bases have OH 1– Bronsted-Lowry: Acid = proton donor, base = proton acceptor Writing equations: Example 1: HNO 3 + NaOH -----> Balanced Equation HNO 3 + NaOH -----> NaNO 3 + H(OH) or H 2 O Strong acid + soluble base -----> soluble salt + molecule Check solubility and for molecules or weak acids All these substances are soluble but H 2 O is a MOLECULE! It stays together ! Total ionic equation H + + NO 3 1– + Na + + OH 1– -----> Na + + NO 3 1– + H 2 O Net Ionic Equation + + OH 1– -----> H 2 Example 2: HC 2 H 3 O 2 + Mg(OH) 2 ------> products: Mg(C 2 H 3 O 2 ) 2 + H(OH) Balanced equation 2 HC 2 H 3 O 2 + Mg(OH) 2 ------> Mg(C 2 H 3 O 2 ) 2 + 2 H 2 O weak acid insoluble base soluble salt molecule Total Ionic Equation 2 HC 2 H 3 O 2 + Mg(OH) 2 ------> Mg +2 + 2 C 2 H 3 O 2 1– + 2 H 2 O Net Ionic Equation 2 HC 2 H 3 O 2 + Mg(OH) 2 ------> Mg +2 + 2 C 2 H 3 O 2 1– + 2 H 2 What is driving these reactions? The formation of a covalent bond which is exothermic . The formation of other molecules will also drive reactions. Examples are HC 2 H 3 O 2 , H 2 CO 3 and H 2 SO 3 . Note these are weak acids.
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This note was uploaded on 04/06/2010 for the course CHEM 1A taught by Professor Okamura during the Fall '08 term at UC Riverside.

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Chap 4 Sec 4 & part 5 - 4.4 Acid-Base Reactions...

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