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Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 Chapter 12 12-1 (a) A colloidal precipitate consists of solid particles with dimensions that are less than 10-4 cm. A crystalline precipitate consists of solid particles with dimensions that at least 10-4 cm or greater. As a consequence, crystalline precipitates settle rapidly, whereas colloidal precipitates remain suspended in solution unless caused to agglomerate. (b) In gravimetric precipitation, the analyte is converted to a sparing soluble precipitate, which is then filtered, washed free of impurities, and then converted into a product of known composition by suitable heat treatment. In gravimetric volatilization, the analyte is separated from other sample constituents by converting it to a gas of known composition. (c) Precipitation is the process by which a solid phase forms and is carried out of solution when the solubility product of a chemical species is exceeded. Coprecipitation is a process in which normally soluble compounds are carried out of solution by precipitate formation. (d) Coagulation, or agglomeration, is the process by which colloidal particles coalesce to form larger aggregates. Peptization refers to the process by which a coagulated colloid reverts to its original dispersed state. Heating, stirring and adding an electrolyte can coagulate colloidal suspensions. Washing the coagulated colloid with water often removes sufficient electrolyte to permit the re-establishment of repulsive forces that favor return to the colloidal state. (e) Occlusion is a type of coprecipitation in which a compound is trapped within a pocket formed during rapid crystal formation. Mixed-crystal formation is also a type of coprecipitation in which a contaminant ion replaces an ion in the crystal lattice. Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 (f) Nucleation is a process in which a minimum number of atoms, ions or molecules associate to give a stable solid. Particle growth is a process by which growth continues on existing nuclei. Precipitation by nucleation results in a large number of small particles. Precipitation by particle growth results in a smaller number of large particles. 12-2 (a) Digestion is a process in which a precipitate is heated in the presence of the solution from which it was formed (the mother liquor). Digestion improves the purity and filterability of the precipitate. (b) Adsorption is the process by which ions are retained on the surface of a solid. (c) In reprecipitation, the filtered solid precipitate is redissolved and reprecipitated. Because the concentration of the impurity in the new solution is lower, the second precipitate contains less coprecipitated impurity. (d) Precipitation from a homogeneous solution is a technique by which a precipitating agent is generated in a solution of the analyte by a slow chemical reaction. Local reagent excess does not occur and the resultant solid product is better suited for analysis than precipitate formed by direct addition of precipitating reagent. (e) The counter-ion layer describes a layer of solution containing sufficient excess negative ions that surrounds a charged particle. This counter-ion layer balances the surface charge on the particle. (f) Mother liquor is the solution from which a precipitate is formed. (g) Supersaturation describes an unstable state in which a solution contains higher solute concentration than a saturated solution. Supersaturation is relieved by precipitation of excess solute. Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-3 A chelating agent is an organic compound that contains two or more electron-donor groups located in such a configuration that five- or six-membered rings are formed when the donor groups complex a cation. 12-4 Relative supersaturation can be regulated through control of reagent concentration, temperature and the rate at which reagents are combined. 12-5 (a) There is positive charge on the surface of the coagulated colloidal particles. (b) The positive charge arises from adsorbed Ag+ ions. (c) -3NO ions make up the counter-ion layer. 12-6 SHCONHCHOHCSNHCH 223243 ++ ←→ The slow hydrolysis of thioacetamide can be used to generate a source of hydrogen sulfide gas. Hydrogen sulfide gas is then involved in the equilibria below: −+ ← →− −+ ← → ++ ++ 2 32 322 SOHOHHS HSOHOHSH The S2- generated can then be used to precipitate Ni2+ in the form of NiS. 12-7 Peptization is the process by which a coagulated colloid returns to its original dispersed state as a consequence of a decrease in the electrolyte concentration of the solution in contact with the precipitate. Peptization can be avoided by washing the coagulated colloid with an electrolyte solution rather than pure water. Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-8 Chloroplatinic acid, H2PtCl6, forms the precipitate K2PtCl6 when mixed with K+ but does not form analogous precipitates with Li+ and Na+. Thus, chloroplatinic acid can be used to separate K+ from a mixture containing Li+ and Na+. 12-9 Note: M stands for molar or atomic mass in the equations below: (a) 4 2 BaSO SO 42 BaSOmassSOmass M M×= (b) 722 OPMg Mg 722 2 OPMgmassMgmass M M×= (c) 32OIn In 32 2OInmassInmass M M×= (d) 62PtClK K 62 2PtClKmassKmass M M×= (e) 22 )SCN(Cu Cu 22 2)SCN(CumassCumass M M×= (f) 43 2 OMn MnCl 432 3 OMnmassMnClmass M M×= (g) 2 43 PbO OPb 243 3 PbOmassOPbmass M M×= (h) 52 1122 OP OPU 521122 OPmassOPUmass M M×= (i) 32 2742 OB OH10OBNa 322722 2 OBmassOH10OBNamass M M ⋅×=⋅ (j) OH6)OHC()UO(NaZn ONa 29232322 2923232 2 2 OH6)OHC()UO(NaZnmassONamass ⋅ ×⋅= M M Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-10 %59.60%100 sampleimpureg2500.0 mole KClg55.74 AgClmole1 KClmole1 g32.143 AgClmole1AgClg2912.0 mole g55.74 mole g32.143 KClAgCl =× ⎟⎠ ⎞⎜⎝ ⎛×⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛×⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛× == MM 12-11 mole g15.237 mole g96.101 24432 )SO(AlNHOAl == MM (a) 244 244 244 244 3 244 3 32 244 32 32 32 )SO(AlNH%102%100 g910.0 )SO(AlNHmole )SO(AlNHg15.237)SO(AlNHmole10925.3 )SO(AlNHmole10925.3 OAlmole )SO(AlNHmole2 OAlg96.101 OAlmole1OAlg2001.0 =× ×× ×=×× − − (b) 3232 OAl%0.22%100sampleimpureg910.0 OAlg2001.0 =× (c) Al%6.11%100 sampleimpureg910.0 mole Alg981.26Almole10925.3 mole10925.3)SO(AlNHmole.noAlmole.no 2 3 244 =× ×× ×== − − 12-12 23 23 23 24 23 24 24 24 )IO(Cug828.0 )IO(Cumole1 )IO(Cug35.413 OH5CuSOmole1 )IO(Cumole1 OH5CuSOg67.249 OH5CuSOmole1OH5CuSOg500.0 =× ⋅×⋅ ⋅×⋅ Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-13 3 3 3 23 3 24 23 24 24 24 KIOg342.0 KIOmole1 KIOg214 )IO(Cumole1 KIOmole2 OH5CuSOmole1 )IO(Cumole1 OH5CuSOg67.249 OH5CuSOmole1OH5CuSOg2000.0 =×× ⋅×⋅ ⋅×⋅ 12-14 (Note: In the first printing of the text, the answer in the back of the book was in error.) AgIg178.0 AgImole AgIg773.234AgImole1057.7 AgImole1057.7 AlImole1 AgImole3 AlIg770.407 AlImole1AlI201.0sampleg512.0AgImole.no 4 4 33 3 3 =×× ×=×××= − − 12-15 The precipitate V2O5·2UO3 gives the greatest mass from a given quantity of uranium. 12-16 322332 AlCl2OH3CO3HCl6)CO(Al +++ ←→ Al%60.2%100 sampleimpureg8102.0 Alg02105.0 Alg02105.0 Almole Alg98.26 )CO(Almole1 Almole2 COmole3)CO(Almole1 COg01.44 COmole1COg0515.0 3322 332 2 2 2 =× = ×××× 12-17 42 CdSOO2CdS ← →+ mole1061.5 CdSOmole1 CdSmole1 g47.208 CdSOmole1CdSOg117.0CdSOmole.noCdSmole.no 4 4 4 44 −×= ××== Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 The number moles H2S is equal to number moles CdS. SH%025.0%100 sampleimpureg0.75 SHg0191.0 g0191.0 SHmole1 SHg08.34mole1061.5SHmass 2 2 2 24 2 =× =××= − 12-18 C%23.17%100 sampleg2121.0 Cmole1 Cg011.12 BaCOmole1 Cmole1 g34.197 BaCOmole1BaCOg6006.0 3 3 3 =× ××× 12-19 5914 5914 59145914 ClHC%589.1 %100 sampleg000.5 ClHCmole1 ClHCg72.354 AgClmoles5 ClHCmole1 g37.143 AgClmole1AgClg1606.0 = × ××× 12-20 (Note: In the first printing of the text, the answer in the back of the book was in error.) 22 22 22 2 2223 23 265 2 265 265 265 2 ClHg%16.41%100 sampleg8142.0 ClHgmole1 ClHgg09.472 Hgmole2 ClHgmole1Hgmol104198.1 Hgmol104198.1 )IO(Hgmole1 Hgmole5 )IO(Hgg75.1448 )IO(Hgmole1)IO(Hgg4114.0 Hgmol =× ⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛ ××× ×=×× = + +− +− + + Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-21 KI%12.2 %100 sampleimpureg97.1 mole KIg00.166 )IO(Bamole1 KImole2 g13.487 )IO(Bamole1)IO(Bag0612.0 mole g00.166 mole g13.487 23 23 23 KI)IO(Ba 23 = × ⎟⎠ ⎞⎜⎝ ⎛×⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛×⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛× == MM 12-22 3 33 PtNH NH%74.38%100 sampleimpureg2115.0 mole NHg0306.17 Ptmole1 NHmole2 g08.195 Ptmole1Ptg4693.0 mole g08.195 mole g0306.17 3 =× ⎟⎠ ⎞⎜⎝ ⎛×⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛×⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛× == MM 12-23 3 33 2 2 3 32 22 AlClMnO AlCl%24.26 %100 sampleimpureg1402.1 mole AlClg34.133 Clmole3 AlClmole1 MnOmole1 Clmole2MnOmol10366.3 mol10366.3 g94.86 MnOmole1)MnOg3521.0g6447.0(MnOmol mole g34.133 mole g94.86 32 = × ⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛ ⎟⎠ ⎞⎜⎝ ⎛×⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛×⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛×× ×=⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛×−= == − − MM Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-24 Let Sw = mass of sample in grams sampleg412.0 %20 %100 mole SOg064.96SOmole1057.8 samplegS SO%20%100 samplegS mole SOg064.96SOmole1057.8 SOmole1057.8 BaSOmole1 SOmole1 g39.233 BaSOmole1BaSOg200.0 mole/g064.96mole/g39.233 2 42 4 4 w 2 4 w 2 42 4 4 2 4 4 4 2 44 4 SOBaSO 244 = ××× = == ×× ×=×× == − −− − − −− −− − −MM The maximum precipitate weight expected given this sample weight, 4 4 2 4 4 2 4 2 4 BaSOg550.0 mole1 BaSOg39.233 SOg1 BaSOmole1 g064.96 SOmole1 sampleg100 SOg55sampleg412.0 = ×××× − −− 12-25 Let Sw = mass of sample in grams. The higher percentage of Ni in the alloy sample is selected because this corresponds to maximum amount expected precipitate. sampleg102.0 %35 %100 mole Nig693.58Nimole1006.6 samplegS Ni%35%100 samplegS mole Nig693.58Nimole1006.6 Nimole1006.6 )NOHHC(Nimole1 Nimole1 g92.288 )NOHHC(Nimole1)NOHHC(Nig175.0 mole/g693.58mole/g92.288 4 w w 4 4 2264 2264 2264 Ni)NOHHC(Ni 2264 = ××× = == ×× ×= ×× == − − − MM Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-26 Let Sw = mass of sample in grams (a) sampleg239.0 %68 %100ZrClg16259.0samplegS ZrCl%68%100 samplegS mole1 ZrClg03.233 AgClmole4 ZrClmole1 g32.143 AgClmole1AgClg400.0 mole/g03.233mole/g32.143 4 w 4 w 44 ZrClAgCl 4 =×= =× ××× == MM (b) AgClg494.0 mole1 AgClg32.143 ZrClmole1 AgClmole4 g03.233 ZrClmole1 sampleg100 ZrClg84sampleg239.0 4 44 =×××× (c) g406.0 %40 %100ZrClg16259.0samplegS %40 samplegS %100ZrClg16259.0ZrCl% 4 w w 4 4 =×= =×= Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-27 A B C D 1 Problem 12-27 2 3 Coefficient Matrix Constant Matrix 4 1.823 1.578 1.505 5 1 1 0.872 6 7 Inverse Matrix Solution Matrix 8 4.0816327 -6.4408200 0.526465306 9 -4.0816300 7.4408160 0.345534694 10 11 Mass of Sample % KBr % NaBr 12 0.872 39.6 60.4 13 14 Spreadsheet Documentation 15 A8:B8=MINVERSE(A4:B5) 16 D8:D9=MMULT(A8:B9,D4:D5) 17 C12=100*D9/A12 18 D12=100*D8/A12 12-28 A B C D 1 Problem 12-28 2 3 Coefficient Matrix Constant Matrix 4 1 1 0.443 5 1 0.6104698 0.3181 6 7 Inverse Matrix Solution Matrix 8 -1.5671952 2.5671952 0.122357321 9 2.5671952 -2.5671952 0.320642679 10 11 Mass of Sample Mass AgCl % Cl % I 12 0.6407 0.1223573 4.72 27.05 13 14 Spreadsheet Documentation 15 A8:B8=MINVERSE(A4:B5) 16 D8:D9=MMULT(A8:B9,D4:D5) 17 B12=D4-D9 18 C12=100*D9/A12 19 D12=100*D8/A12 Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-29 52 5252 4 4 4 4 44 44 OPPbMoO OP%089.2 %100 sampleg1969.0 mole1 OPg94.141 Pmole2 OPmole1 PbMoOmoles12 Pmole1PbMoOmol109565.6 PbMoOmol109565.6 g14.367 PbMoOmole1PbMoOg2554.0PbMoOmol mole/g94.141mole/g14.367 524 = × ⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛ ×××× ×=×= == − − MM 12-30 2 2 2 33 2 3232 33 3232 COKMgCOCO COg498.0 mole1 COg010.44mole0113.0COmass mole0113.01046.41076.6COmole g21.138 COKmole1 sampleg100 COKg42sampleg500.1 g31.84 MgCOmole1 sampleg100 MgCOg38sampleg500.1 COKmoleMgCOmoleCOmole mole/g21.138mole/g31.84mole/g010.44 3232 =×= =×+×= ⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛ ×× +⎟⎟⎠ ⎞ ⎜⎜⎝ ⎛ ××= += === −− MMM 12-31 AgClmole1022804.3 OH6MgClmole1 AgClmoles2OH6MgClmole1061402.1 AgClmole1013268.4 g32.143 AgClmole1AgClg5923.0 OH6MgClmole1061402.1 OPMgmole1 OH6MgClmoles2 g55.222 OPMgmole1OPMgg1796.0 mole/g32.203mole/g44.58mole/g55.222 3 22 22 3 3 22 3 722 22722 722 OH6MgClNaClOPMg 22722 −− − − • ×=⋅×•× ×=× ⋅× =⋅×× === MMM Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 OH6MgCl%69.47 %100 sampleg881.6 mL0.50 mL0.500 mole1 OH6MgClg32.203OH6MgClmole1061402.1 NaClmole100464.9 AgClmole1 NaClmole1AgClmole)10228.31013268.4( 22 22 22 3 433 ⋅= × ×⋅×•× ×=××−× − −−− NaCl%68.7%100 sampleg881.6 mL0.50 mL0.500 mole1 NaClg44.58NaClmole100464.9 4 =× ××× − 12-32 ,reagentlimitingtheisIOBecause IOmole10516.1 NaIOmole1 IOmole1 g89.197 NaIOmole1NaIOg300.0 Bamole10188.8 OH2BaClmole1 Bamole1 g26.244 OH2BaClmole1OH2BaClg200.0 mole/g13.487mole/g89.197mole/g26.244 3 3 3 3 33 3 24 22 2 22 22 )IO(BaNaIOOH2BaCl 23322 − −− − +− + ⋅ ×=×× ×= ⋅× ⋅×⋅ === MMM (a) 23 234 23 4 3 23 )IO(Bag369.0 mole1 )IO(Bag13.487mole10580.7)IO(Bamass mole10580.7 2 mole10516.1)IO(Bamoles =××= ×=×= − − − (b) ( ) OH2BaClg0149.0 mole1 OH2BaClg26.244OH2BaClmole1008.6OH2BaClmass mole10080.6mole)10580.7()10188.8(remainingOH2BaClmole 22 22 22 5 22 544 22 ⋅= ⋅×⋅×=⋅ ×=×−×=⋅ − −−− Fundamentals of Analytical Chemistry: 8th ed. Chapter 12 12-33 ,reagentlimitingtheisAgBecause CrOAgg5125.0 mole1 CrOAgg730.331 CrOKmole1 CrOAgmole1 g190.194 CrOKmole1CrOKg300.0 CrOAgg4882.0 mole1 CrOAgg730.331 AgNOmole2 CrOAgmole1 g873.169 AgNOmole1AgNOg500.0 mole/g190.194mole/g730.331mole/g873.169 42 42 42 4242 42 42 42 3 423 3 CrOKCrOAgAgNO42423 + = ××× = ××× === MMM (a) 4242 CrOAgg488.0CrOAgmass = (b) ( ) 42 42 42 5 42 533 42 CrOKg0142.0 mole1 CrOKg190.194CrOKmole10331.7CrOKmass mole10331.7mole)10472.1()10545.1(remainingCrOKmole = ××= ×=×−×= − −−−
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