C__DOCUME~1_NICHOL~1_LOCALS~1_Temp_plugtmp-9_ProblemSet_8_final

C__DOCUME~1_NICHOL~1_LOCALS~1_Temp_plugtmp-9_ProblemSet_8_final

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Unformatted text preview: Chem 208, Spring 2008 Problem Set 8 Due Friday, April 4, 2:00 PM Ch 17: 97, 98, 101, 103 Name: Ch18z3,9,11,15, l9,25,45,47 LabTAName: Lab Time/Room: 1. Calculate the equilibrium constants for the following reactions in agueous solutions: a) N113 + H30+ ¢> NH,+ + H20 b) HF + (CH3)3N <=> F’+ (CH3)3NH* c) HNo3 + KOH a» KNO3+H20 2. The K,,, of BaSO4 is 1.1 x 10'“). Calculate [Bay] in a saturated aqueous solution of BaSO4. A “barium milkshake”, a saturated solution of BaSO4 dissolved in a flavored liquid, is often administered prior to the x-ray imaging of a person’s digestive system because Ba absorbs erays. Assuming that an oral dose of 50mg/kg of Ba is toxic to a human, what volume of barium milkshake would a 70kg person have to drink for it to be lethal? You can assume that the solubility of BaSO4 in the flavored liquid is the same as in water. Chem 208, Spring 2008 Problem Set 8 Due Friday, April 4, 2:00 PM 3. A 0.164 gram sample of phosphorous acid, H3PO3, (K31 = 3.7 x 1072;1(82 = 2.1 x 10*?) is dissolved in enough water to make 50.0 mL of solution. This solution is then titrated with 0.122 M NaOH. ' I (a) Calculate the volume of 0.122 M NaOH required to reach the first equivalence point of the titratlon. (b) Calculate the pH of the titrated solution at the second equivalence point. 4. Recall the titration of 20.0 mL of 0.10 M H3PO4 with 0.10 M NaOH from lecture. (a) Calculate the pH halfway between the second and third equivalence points using the Henderson- Hasselbalch relationship. (b) Calculate [P0437] at the third equivalence point. (c) Calculate the pH at the third equivalence point assuming P043“ to be the major species present in solution. ((1) Are your answers to (a) and (0) what you expected? Justify your yes or no answer in one sentence. I Chem 208, Spring 2008 Problem Set 8 Due Friday, April 4, 2:00 PM 5. The Ksp for Cu(OI—I)2 is 1.6 x 1019. The complex CU(NH3)42+ is produced by mixing Cu2+ with ammonla: Cu2 (aq) + 4 NI-I3(aq) 4:. Cu(NH3)42+(aq) K = 1.0 x 1013 (a) Calculate the equilibrium constant for the following reaction: CU(OH)2(3) + 4NH3(aq) ¢> CutNH3)f*(aq) + 2 Oman» (b) Calculate the molar solubility of Cu(OH)2 in 3.0 M NH3(aq). ((3) Should Cu(OH)2(s) precipitate if 100.0 ml, of a 0.0010 M solution of Cu2+(aq) is added to 100.0 mL of a solution buffered at pH = 8.0? . . . . . . . .at pH = 6.0? Chem 208, Spring 2008 Problem Set 8 Due Friday, April 4, 2:00 PM 6. The active ingredient in aspirin is acetylsalicylic acid. The titration of a 2.51 gram sample of pure acetylsalicylic acid required 27.36 mi. of 0.5106 M NaOH to reach the equivalence point. Addition of 15.44 mL of 0.4524 M HCl to this titrated solution produced a solution with pH = 3.48. An aspirin tablet with a mass of 0.8238 gram was then titrated with 0.2820 M NaOH. The Equivalence point of this titration was reached after addition of l 1.26 mL of the NaOH. (a) Calculate the molecular mass of acetylsalicylic acid (it is a monoprotic acid). (b) Calculate Ka for acetylsalicylic acid. (c) Calculate the percent of the aspirin tablet that is filler and other inactive material, and not acetylsalicylic acid. ...
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This note was uploaded on 09/03/2008 for the course CHEM 2080 taught by Professor Davis,f during the Spring '07 term at Cornell University (Engineering School).

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C__DOCUME~1_NICHOL~1_LOCALS~1_Temp_plugtmp-9_ProblemSet_8_final

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