Lecture 4 part III Chem 102

Lecture 4 part III Chem 102 - Chapter 4 Types of Chemical...

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Chapter 4 Types of Chemical Reactions Part III
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Types of Chemical Reactions Acid–Base Reactions Oxidation–Reduction Reactions
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Acid—proton donor Base—proton acceptor S trong acid and base reaction H + ( aq ) + OH ( aq ) H 2 O( l ) NaOH +HCl NaCl + H 2 O Base and Acid Salt and Water Acid–Base Reactions Neutralization reaction
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Titration – delivery of a measured volume of a solution of known concentration ( the titrant ) into a solution containing the substance being analyzed ( the analyte ). Equivalence point – the smallest amount of titrant that is sufficient to fully neutralize or react with the analyte. Use indicator to see it. (moles of H + = OH - ) Endpoint – the indicator changes color so you can tell the equivalence point has been reached. Endpoint not always at the equivalence point Acid–Base Titrations
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Acid–Base Titrations Permanent color change= Endpoint Read off the volume added ! Burette with solution of known concentration Erlenmeyer flask with solution of unknown concentration Solution and indicator
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Example 8. What volume of 0.468 M H 2 SO 4 is needed to neutralize 215.00 ml of a 0.125 M LiOH solution? Calculate the number of moles of base: V base x M base = 0.21500 L x 0.125 M = 0.0269 mol LiOH From the balanced equation find the moles of acid needed: 2 LiOH (aq) + H 2 SO 4 (aq) 2 H 2 O (l) + Li 2 SO 4 (aq) We will need half as much sulfuric acid as we have lithium hydroxide: 0.0134 mol H 2 SO 4 Volume of acid: Moles acid M acid V acid = = = 0.0286 L H 2 SO 4 28.6 mL 0.0134 moles 0.468 mol/L Neutralization
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Example 9. For the titration of sulfuric acid (H 2 SO 4 ) with sodium hydroxide (NaOH), how many
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This note was uploaded on 04/21/2011 for the course CHEM 102 taught by Professor Peterpastos during the Spring '08 term at CUNY Hunter.

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Lecture 4 part III Chem 102 - Chapter 4 Types of Chemical...

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