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# General College Chemistry II CHE 152

Monroe Community College

GPA 3.9

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This 17 page Study Guide was uploaded by Dr. Golda Donnelly on Thursday October 15, 2015. The Study Guide belongs to CHE 152 at Monroe Community College taught by Sherman Henzel in Fall. Since its upload, it has received 51 views. For similar materials see /class/223550/che-152-monroe-community-college in Chemistry at Monroe Community College.

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Date Created: 10/15/15

Equilibrium Problems CHE 152 Sherman Henzel ICE Tables To ICE or not to ICE that is the question ICE tables are used when initial I concentrations are given If only equilibrium concentrations are given then ICE tables are not employed ICE problems include pH determination of weak acids and bases equilibrium concentrations K determinations reacting species such as buffer reactions and salts that can form a precipitate titrations of weak acids and based solubility problems and precipitation problems Examples 1 Determine the pH of a solution that is 01500 M in HC2H302 01500 M HC2H3O2 is an initial concentration and an ICE table is employed answer pH 279 Similar problems Chapter 18 pages 11 12 15 and 17 2 An organic acid HOrg MW 32500 gmol is soluble in water to the extent of 158 g HOrgL Ifthe pH ofa 5000 mL HOrg solution has a pH of 4821 what is the K21 for this acid HOrg H20 Org39 H3O The pH is measured at equilibrium but the solubility of the acid is an initial concentration and an ICE table is employed answer Ka 470 X 10398 Similar problems Chapter 18 pages 13 and 14 3 Calculate the pH ofa solution that is 01250 M in hydroxylamine 01250 M hydroxylamine is an initial concentration and an ICE table is employed answer pH 953 Similar problems Chapter 18 page 18 4 Calculate the pH ofa solution that is 01150 M in NaOCl 01150 M NaOCl is an initial concentration and an ICE table is employed answer pH 1030 Similar problems Chapter 18 pages 20 21 29 30 and 31 Equilibrium Problems page 2 5 Calculate the HZSe HS39e S39Ze and H301e in a solution that is 01750 M in HZS 01750 M HZS is an initial concentration and an ICE table is employed answer HZS 01750 M HS39 14 XlO394 M H3O 14 X 104 M S39Z 10 X 103914 Similar problems Chapter 18 pages 23 and 24 6 Determine the pH in a solution that is 01500 M in HNO2 and 01250 M in HCl 01250 M 01500 M HNO2 and 01250 M HCl are both initial concentrations and an ICE table is employed answer pH 090 Similar problems Chapter 19 page 2 7 Calculate the pH ofa solution that is 05000 M in HC2H3O2 and 02500 M in NaC2H302 05000 M HC2H3O2 and 02500 M NaC2H3O2 are both initial concentrations and an ICE table is employed answer pH 446 Similar problems Chapter 19 page 3 8 Calculate the pH ofa buffer that is 01025 M in HONH2 and 02000 M HONH3C1 01025 M HONH2 and 02000 M HONH3C1 are both initial concentrations and an ICE table is employed answer pH 567 Similar problems Chapter 19 pages 5 and 8 bottom 9 What is the effect of adding 001000 moles of NaOH to 100 L ofthe buffer in problem 8 above 001000 M NaOH a strong base will react with the conjugate acid of the buffer and an ICE table is employed answer ApH 006 pH units Similar problems Chapter 19 pages6 7 8 9 and 10 Equilibrium Problems page 3 10 5000 mL of 02000 M HC2H3O2 are titrated with 04000 M NaOH Calculate the pH after 1500 mL of NaOH are added Weak acid or weak base titrations require an ICE table from the initial addition of titrant until the equivalence point Post equivalence an ICE table is not required answer pH 494 Similar problems Chapter 19 pages 21 to 29 11 Calculate the solubility of AgCl in water Solubility problems employ ICE tables answer S 13 X 10395 M Similar problems Chapter 19 page 38 12 Calculate the solubility of CaF2 in a solution that is 001500 M in NaF Solubility problem 001500 M NaF is an initial concentration employs ICE table answer S 24 X 10395 M Similar problems Chapter 19 pages 42 and 43 13 A 1500 mL sample of 001500 M AgNO3 is added to 2000 mL of 002500 M KI Will AgI precipitate Will the precipitation of Ag be complete AgNO3 and KI can react to form a precipitate and ICICE table is employed answer Ag 11 X 103914 M ppt is complete Similar problems Chapter 19 pages 46 and 47 14 Calculate the solubility of Ang03 in a solution buffered to a pH of 300 Solubility problems employ ICE tables answer S 0029 M Similar problems Chapter 19 pages 52 and 53 15 What is the molar solubility of AgCl in 01015 M NH3 Solubility problems employ ICE tables answer S 49 X 10393 M Similar problems Chapter 19 pages 60 and 61 Equilibrium Problems page 4 16 What is the solubility of FeS in 1050 M HCl Solubility problems employ ICE tables answer S 0521 M Similar problems Chapter 19 pages 66 and 67 No ICE Tables ICE tables are not employed when equilibrium E concentrations are given NonICE problems include pH determination of strong buffer preparation titrations of strong acids and bases post equivalence point for weak acid and base titrations KSp determination calculation of Q ion separation by precipitation and preventing precipitation 17 Calculate the H301 OH39 and CI in 5000 mL ofa solution that is 01115 M in HCl Strong acid does not employ and ICE table answer H3O N03 01115 M OH39 90 X 103914 M Similar problems Chapter 18 pages 7 and 8 18 What mass ofNaNO2 must be added to 2500 mL of 0350 M HNO2 in order to produce a buffer with a pH of 350 Buffer preparation involves all concentrations at equilibrium and does not employ ICE tables answer 97 f NaNO2 Similar problems Chapter 19 page 4 19 Describe the preparation of 2500 mL ofa buffer with a pH of 5000 from 01500 M HC2H3O2 and 02000 M NaC2H302 Buffer preparation involves all concentrations at equilibrium and does not employ ICE tables answer Mix 108 mL of0 1500 M HC2H3O2 with 142 mL of 02000 M NaC2H302 Similar problems Chapter 19 pages 12 and 13 Equilibrium Problems page 5 20 2500 mL of 01500 M HCl are titrated with 03000 M NaOH Calculate the pH after 750 mL of NaOH are added Strong acid and strong base titrations do not employ an ICE table answer pH 134 Similar problems Chapter 19 pages 15 to 20 21 5000 mL of 02000 M HC2H3O2 are titrated with 04000 M NaOH Calculate the pH after 3000 mL of NaOH are added Weak acid strong base tirations post equivalence point do not employ ICE tables answer pH 1240 Similar problems Chapter 19 pages 25 and 29 22 A 1250 mL sample is removed from a water solution saturated with CaOH2 at 250 0C The water is completely evaporated from the solution and a deposit of 01030 g of CaOH2 is obtained Calculate the KSp of CaOH2 at 250 0C In a saturated solution all concentrations are at equilibrium and an ICE table is not employed answer KSp 5502 X 10396 Similar problems Chapter 19 page 36 23 It is desired to separate Ba from Ag by the slow addition of SO 39 to a solution in which the concentration of Ba2 is 0002500 M and the concentration of Ag is 00001250 M a Which ion will precipitate first and at what SOZ39 b What will be the concentration of the first ion to precipitate when the second ion just begins to precipitate c Is the separation effective Separation problems involve equilibrium concentrations and ICE stables are not employed answer a Ba will precipitate first when SO 39 44 X 10398 M b Ba2 12 x 1013 M c Yes Similar problems Chapter 19 pages 40 and 41 Equilibrium Problems page 6 24 Eight drops of 001500 M NaCl are added to 1750 mL of 0007500 M AgNO3 Will AgCl precipitate 20 drops equal 1 mL Determination of Q does not employ an ICE table answer Q gt KSp therefore AgCl s will form Similar porblem Chapter 19 page 44 and 45 25 What concentration of C2H5NH must be maintained in order to prevent the precipitation of MgOH2 in a solution that is 001250 M in MgNO32 and 0003500 M in CZHSNHZ Preventing precipitation problems do not require an ICE table answer 0041 M Similar problems Chapter 19 page 51 26 What is the minimum concentration of NH3 required to prevent AgCl from precipitating in a solution that is 00002500 M in AgNO3 and 000009500 M in NaCl Preventing precipitation problems do not require an ICE table answer 00034 M Similar problems Chapter 19 pages 58 and 59 Equilibrium Problems page 7 Equilibrium Problems Key CHE152 Sherman Henzel ICE Tables Examples 1 Determine the pH of a solution that is 01500 M in HC2H302 HC2H3O2 H20 C2H3O393 H3O I 01500 0 0 C X X X EX 01500 X X X E m01500 C2H30H30 X2 174x10 5 X000162 01500 HC2H302 H3O 000162 M pH 279 2 An organic acid HOrg MW 32500 gmol is soluble in water to the eXtent of 158 g HOrgL Ifthe pH ofa 5000 mL HOrg solution has a pH of 4821 what is the K21 for this acid HOrg H20 Org39 H3O 7 158 g HOrg lmol HOrg 000486 mol HOrg L 32500 g HOrg L Horgh pH 4821 H301E 151x105 M HOrg H20 Org39 H301 I 000486 0 0 C X X X EX 000486X X X E 000485 151 X 10395 151X10395 75 2 KaJOIg H3o 12151x10 470X10s HOrg 000485 Equilibrium Problems Key page 8 3 Calculate the pH ofa solution that is 01250 M in hydroxylamine HONH2 H20 HONH OH39 I 01250 0 0 C X X X EX 01250 X X X E m01250 HONHg OH Kb 91X10 9 X34X10 5 HONHZ 01250 OH39 34 X 10395 M pOH 447 pH 953 4 Calculate the pH ofa solution that is 01150 M in NaOCl OCl39 H20 HOCl OH39 1 01150 0 0 C X X X EX 01150 X X X E m01150 HOCl OH K 100 10 14 b H7 w X 78 339x10 7 0C1 Ka 295x10 X2 339X10 7X 2197 X 10 4 01150 OH39 197 x104 M pOH 370 pH 1030 page 9 Equilibrium Problems Key 5 Calculate the HZSe HS39e S39Ze and H3Oe in a solution that is 01750 M in HZS HZS H20 HS39 H3O 1 01750 0 0 C X X X EX 01750 X X X E m0l750 HS H 0 X2 K21 ML1x10 7 x14x101 H28 01750 HZS 01750 M HS39 14 X10394 M H3O 14 X 10394M HS39 H20 S392 H3O I 14X10394 0 14X10394 C X X X EX 14X10394X X 14X10394 X E m14X104 m14X10394 32 Ho x14x104 Ka210x10 74X10X10 14S39Z10X103914M HS 14 X 10 6 Determine the pH in a solution that is 01500 M in HNO2 and 01250 M in HCl HNO2 H20 NO392 H3O 1 01500 0 01250 C X X X EX 01250 X X X E m01500 m01250 NO H 0 01250X aM513X104 X616X104 HNOZ 01500 H301 01250 M pH 090 Equilibrium Problems Key page 10 7 Calculate the pH ofa solution that is 05000 M in HC2H3O2 and 02500 M in NaC2H302 S110 m HC2H302 H20 C2H3O393 H30 05000 02500 0 39X X x 05000 x 02500 x x m05000 m02500 W 174 x1075 x 348 x1075 HC2H3OZ 05000 H301 348 x 105 M pH 446 8 Calculate the pH ofa buffer that is 01025 M in HONH2 and 02000 M HONH3C1 HONH2 H20 HONH OH39 I 01025 02000 0 C X X X EX 01025 X 02000 X X E m01025 m02000 b H gli l 91 x 1079 06210 20 x 47 x1079 OH39 47 X 10399 M pOH 833 pH 567 9 What is the effect of adding 001000 moles of NaOH to 100 L ofthe buffer in problem 8 above HONH OH39 HONH2 H20 1 02000 001000 01025 C 001000 001000 001000 1 01900 0 01125 C X X X Ex 01900x x 01125 x E m01900 m01125 b HONHOH7 91x10 9 0391900X x 54 x1079 HONHZ 01125 OH39 54 x109 M pOH 827 pH 573 ApH 573 567 006 pH units Equilibrium Problems Key page 11 10 5000 mL of 02000 M HC2H3O2 are titrated with 04000 M NaOH Calculate the pH after 1500 mL of NaOH are added 02000 M 5000 mL HC2H3OZ X 01538M 1 6500 mL 04000 M 1500 L OH x m 009231 M 1 6500 mL HC2H302 OH39 C2H3O393 H20 I 01538 009231 0 C 009231 009231 00923l I 00615 0 009231 C X X X Ex 00615 X 009231 X E 00615 m009231 7 714 K HC2H3OZOH Ka 100 x 10 00615X X Z 863 X 1010 b C2H30 Ka 174x10 5 009231 OH39 863 x 103910 M pOH 906 pH 494 11 Calculate the solubility of AgCl in water AgCl s Ag Cl39 0 p 1 x O a o x mm KSp AgCl39 18 X 103910 X2 X 13 X 10395 S13X10395M Equilibrium Problems Key page 12 12 Calculate the solubility of CaF2 in a solution that is 001500 M in NaF CaF2 s Ca2 2F39 1 0 001500 C X 2X EX X 001500 2X E m001500 Ksp 02mm2 53 x109 0015002 x x 24 x105 s 24 x 105 M 13 A 1500 mL sample of 001500 M AgNO3 is added to 2000 mL of 002500 M KI Will AgI precipitate Will the precipitation of Ag be complete 001500 molAgNO3 1molAg 1500mL X X 20006429 MAg L 1mol AgNO3 3500 mL 002500 molKI lmol 1 2000mL 2001429M1 L lmolKI 3500 mL Q Ag1 0006429 x 001429 92 x 105 Q gt Ksp ppt will form AgI s Ag I39 I 0006429 001429 C 0006429 0006429 I 0 000786 C X X Ex x 000786 x E m000786 Ksp AgI39 85 X 103917 000786X X 11 X 103914 Ag 11 X 103914 M ppt is complete Equilibrium Problems Key page 13 14 Calculate the solubility of AgZCO3 in a solution buffered to a pH of 300 AgZCO3 S 2 Ag CO2 Ksp 81 x 103912 co2 H30 HCO H20 lKaz 156 X 1039 18 X1010 HCO 1 H3 Hzco3 4 H20 1Ka1 142 x107 24 x106 Ag2C03 s 2 H30 2 Ag H2C03 2 H20 K 81 x 103912 X18 x1010 x 24 x106 35 x105 pH 300 H201 10 x103 M Ag2C03 s 2 H30 2 Ag HZCO 2 H20 1 10 X 10393 0 0 C 2 2 EX 2X X E 10 X 103 K Ag2HZSO3 35 x105 2X2 2 4Xg 6 x 044 H301 10x10 10x10 S 044 M 15 What is the molar solubility of AgCl in 01015 M NH3 AgC1s Ag C139 KSp 18 X 103910 Ag 2 NH3 AgNH3 Kf 16 X 107 AgCl s 2 NH3 AgNH3 Cl39 K 18 x1010 X16 x107 00029 AgCl s 2 NH3 AgNH3 C139 I 01015 0 0 C 2X 2 2 EX 01015 2X X X K 2 AgltNH3gt1CI 1 2 00029 2 x2 NH32 01015 2x2 I X2 X 000029 0053 X 49 X 10 3 01015 2X2 01015 2X S 49X10393M Equilibrium Problems Key page 14 16 What is the solubility of FeS in 1050 M HCl FeS s Fe 8239 KSp 6 X 103918 s2 H3 Hs H20 K 1Ka2 110 x 1014 10 x1014 HS39 H30st H20 K 1Ka2 111x107 91 x 106 FeS s2H3 Fe2st K6X103918X10X1014X91X106546X103 FeS s 2 H30 Fe st 2 H20 I 1050 0 0 C 2X X X EX 1050 2X X X 2 2 K Fe Wis 5 x103 X 2 H301 1050 2x 2 J5 x103 X 7 x101x 05 46 1050 2x2 39 1050 2x 21 s 0521 M NonICE Tables Examples 17 Calculate the H301 OH39 and NO in 5000 mL of a solution that is 01115 M in HNO3 HNO3 H20 a H3O NO H3OOH39 100 X 1039 01115OH39 100 X 1039 OH39 90 X 103914 M H301 N05 01115 M OH39 90 X 103914 M 18 What mass ofNaNO2 must be added to 2500 mL of 0350 M HNO2 in order to produce a buffer with a pH of 350 pH 350 H30 32 x104 M 7 7 74 a zwzjlg X1074 ZWJNOE 056M HNOZ 0350 056 mol NaNO2 68996 g NaNO2 02500 L 97 g NaNO2 L 1 mol NaNO2 1 Equilibrium Problems Key page 15 19 Describe the preparation of 2500 mL ofa buffer with a pH of 5000 from 01500 M HC2H3O2 and 02000 M NaC2H302 K C2H301H30l 2174 X1075 Cszogl 100 X1075 Cszogl a HCHO HCHO HCHO 232 232 232 2174 Let X mL 0fHC2H3O2 and y mL 0fNaC2H302 X y 2500 X 2500 y yO2000 2500 yO2000 2500 y0 1500 2500 y0 1500 39 2500 02000y 652 0261y y 142 X 2500 142 108 MiX 108 mL of 0 1500 M HC2H302 with 142 mL of 02000 M NaC2H302 20 2500 mL of 01500 M HCl are titrated with 03000 M NaOH Calculate the pH after 750 mL of NaOH are added H301 01500MX M01154 M 3250mL OH O3000 M x M 00692 M 3250mL H3O 01154 M 00692 M 00462 M pH 134 21 5000 mL of 02000 M HC2H3O2 are titrated with 04000 M NaOH Calculate the pH after 3000 mL of NaOH are added 5000mL HC2H3OZ O2OOOMX 01250M 8000 mL OH 04000 MX W 01500 M 8000 mL OH39 01500 M 01250 M 00250M pOH 160 pH 1240 Equilibrium Problems Key page 16 22 A 1250 mL sample is removed from a water solution saturated with CaOH2 at 250 0C The water is completely evaporated from the solution and a deposit of 01030 g of CaOH2 is obtained Calculate the KSp of CaOH2 at 250 0C 01030 g CaOH2 1 mol CaOH2 X 0001390m01CaOH2 1 74093 g CaOH2 2 000139Om01CaOH2 1m01 Ca X 1 OOHIZMCah 1 lmolCaOH2 01250 L 0001390 molCaOH2 2molOH 1 2002224MOH 1 lmolCaOH2 01250 L KSp Ca2OH392 001112 X 0022242 5502 X 10396 23 It is desired to separate Ba2 from Ag by the slow addition of 80239 to a solution in which the concentration of Ba2 is 0002500 M and the concentration of Ag is 00001250 M a Which ion will precipitate first and at what 80239 b What will be the concentration of the first ion to precipitate when the second ion just begins to precipitate c Is the separation effective BaSO4 s Ba2 30339 KP 11 x 103910 AgZSO4 s 2 Ag so Ksp 14 x 105 a Ksp Ba2soi 11 x 1010 0002500 s03 s03 44 x 108 M Ksp Ag2SOi39 14 x 10395 000012502 30139 S01 896 M Ba will precipitate first when 80239 44 X 10398 M b 3212 896 11 x 1010 Ba2 12 x 1013 M c Yes Equilibrium Problems Key page 17 24 Eight drops of 001500 M NaCl are added to 1750 mL of 0007500 M AgNO3 Will AgCl precipitate 20 drops equal 1 mL g x lmL 040 mL 1 20 d 001500 mol NaCl 040 mL 1mol Cl 2 34 X105 M Cl L 1754 mL 1mol 0007500 mol AgNO3 1750 mL 1mol Ag 2 0007483 M Ag L 1754 mL 1molAgNO3 Q AgC139 34 X 10395 X 0007483 26 X 10397 Q gt KSp therefore AgCl s will form 25 What concentration of C2H5NH must be maintained in order to prevent the precipitation of MgOH2 in a solution that is 001250 M in MgNO32 and 0003500 M in CZHSNHZ Ksp Mg20H392 18 x 103911 001250OH392 OH39 38 x105 M Kb CszNHUiOH 44 X101 CZHSNH 38 x105 C H NH 0041M CZHSNHZ 0003500 2 5 3 26 What is the minimum concentration of NH3 required to prevent AgCl from precipitating in a solution that is 00002500 M in AgNO3 and 000009500 M in NaCl Ksp AgC139 18 x 1010 Ag000009500 Ag 19 x 106 M A NH Kf g 32216X107 000062500 2 AgNH3 19x10 NH3 NH329X10 3M 00002500 mol Ag 2 mol NH3 L 1mol Ag 00005000 M NH3 NH3 00029 M 00005000 M 00034 M

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