Chem_208_Lecture_15 - Finish Buffer Solutions; Indictors...

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1 This week: Finish Buffer Solutions; Indictors (17-3); Ions as Acids and Bases (16-7); Polyprotic Acids (16-6); Titrations (17-4); Lewis Acids/Bases (16-9) We will not cover material in 16-8. PS6 due Fri. March 14 PS7 will go out in lecture on Thursday, 3/13
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2 Recall Professor Davis’s final demo: CH 3 COOH + H 2 O CH 3 COO + H 3 O + Initial 1.5 M 1.2 M Finish Buffers Finish Buffers Calculate the pH after addition of 10.0 mL of 2.0 M HCl to 1.0 liter of this buffer solution. pH = pK a + log [ CH 3 COO ] [ CH 3 COOH ] = 4.74 + log 1.2 1.5 = 4.65 pH = 4.63
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3 Indicators are weak acids that are usually complex organic molecules HIn + H 2 O In + H 3 O + Indicators Indicators The abbreviationHIn is used because of the complexity of the structure
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4 Bromothymol Blue Bromothymol Blue
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5 Phenol Red Phenol Red
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6 Phenolphthalein Phenolphthalein
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7 HIn + H 2 O In + H 3 O + Color A Color B The differentiating feature of indicators is that HIn and In have different colors The color observed for any aqueous solution containing an indicator will
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Chem_208_Lecture_15 - Finish Buffer Solutions; Indictors...

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