CHEM 230 W16 PREP Final Exam KEYp114a) Carbonated water is prepared by cooling water to 8.0oC and pressurizing water with a PCO2of 8.3 bar. I wanted to find the solubility of CO2at this temperature, but I could not find a value for kH(the Henry's law constant) at 8.0oC. However, I found the mole fraction of CO2in water water to be 0.002771 at 8.0oC when the partial pressure of CO2was 8.3 bar. What is the solubility (molarity) of carbon dioxide under these conditions given a solution density of 0.997g/mL?pick100 moles total:0.002771 =molCO2mol total=mol CO21000.2771molCO244gCO21molCO2"#$%&'=12.19gCO2100−0.2771=99.723molH2O18gH2O1molH2O"#$%&'=1795gH2OTotal g=12.19+1795=1807.1gtotal1mLsolution0.997g total"#$%&'1L1000mL"#$%&'=1.812LM=molCO2Lsolution"#$%&'=0.2771mol1.812L"#$%&'=0.153MCO2b) Based on the solubility that you found in part a, what is kHfor CO2in water at 8oC?[CO2(aq) ]M0.153s=kHPCO20.153molL=kH(8.3bar)0.0184molLbar=kHkHmol/(L bar)0.0184If the CO2(g)above the water is removed and replaced by air (N2(g)and O2(g)) at a pressure of 8.3bar, how will each of the following quantities change as the system goes to equilibrium? Circle one answer in each box.c) The [O2]aqwill: increase decrease stay the samed) The partial pressure of CO2(g)will: increase decrease stay the same15555-3 mistake plugging in or math-3 per math/transcription0.355 = 4 pts total-5 per conceptual mistke
CHEM 230 W16 PREP Final Exam KEYp215) Three different bases are titrated with 0.1M HCl as described below. Compare the titrations and select the one that best matches the description in parts a-d. Check one column for each row.10 mL, 0.2 M NH2OHpKb= 7.9710 mL, 0.2 M NH2NH2pKb= 5.7710 mL, 0.2 M CH3NH3pKb= 3.44b) highestvolume of 0.1 M HCl to reach the stoichiometric pointAll are the samec) lowestpH @ 1/2 stoichiometric pointd) highestpH at the stoichiometric pointXXX2016) a) What is the minimum number of grams of Pb(NO3)2(MW= 331.21) that must be added to 100 mL of 5.4x10-4M Na2SO4in order to observe a precipitate? (KspPbSO4= 2.53x10-8)PbSO4(s)--> Pb+2(aq)+ SO42-(aq)Ksp= 2.53x10-8Ksp=[Pb2+][SO4−2]2.53x10−8=[Pb2+](5.4x10−4)4.68x10−5=[Pb2+]4.68x10−5molPb+2L0.1L#$%&'(1molPb(NO3)21molPb+2#$%&'(331.21gPb(NO3)21moPb(NO3)2#$%&'(=1.552x10−3gPb(NO3)2g1.552x10-31020For a saturated aqueous solution of PbSO4, describe the response to each of the following stresses.b) adding PbSO4(s): PbSO4(s)will: dissolve precipitate neither cannot determinec) adding NaNO3(s): PbSO4(s)will: dissolve precipitate neither cannot determined) adding NaNO3(aq): PbSO4(s)will: dissolve precipitate neither cannot determinee) adding Pb(NO3)2(aq): PbSO4(s)will: dissolve precipitate neither cannot determine(Circle one answer in each box.)a) highestinitial pHX3 pts Ksp4 pts [Pb+2]3 pts conversion to g
CHEM 230 W16 PREP Final Exam KEYp3Ti(s)Cl2(g)TiCl4(l)ΔHof(kJ/mol)Som (J/K mol)30.7223.07-804.16221.930a) Write out the balanced chemical equation for the formation of TiCl4(l).