Determining an Equilibrium Constant Using Spectrophotometry (5)

Determining an Equilibrium Constant Using Spectrophotometry (5)

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Unformatted text preview: Post-Laboratory Questions (Use the spaces provided for the answers and additional paper if necessary.) 1. Why didn’t you need to know the molar absorptivity of the equ' ibrium the calculations you did in this experiment? ixture or the path length for 2. For each determination of the absorbance approximately 5-mL of the solution was used. WWould have been the effect on your determination of the absorbance if samples of approxima ely 6-mL volumes had been used? Briefly explain. I OH MWM’: Ju-m Jam swam mm a! m «00th 0/149in J/MW MN m‘ AIM ,oanu ifQMMA/(W 54/041“ Mohav- - 3. Frank and Oswalt report a molar absorptivity of 470 What absorbance would you expect for a solution t path length is 1.00 cm? A-‘Ebc moi“ cm‘1 for the thiocyanatoiron(lII) ion. tis 1.0 x 10"‘M in thiocyanatoironflll) ion, if the / A? (CHOU emf" cm" )(Lombgfl I. 0W0 ' V Moi/1:) 4. At a given temperature, the equilibrium constant for the system studied in this experiment is 1.40 x102. Suppose 100.0 mi. of 2.00 x10‘3M KSCN was mixed with 100.0 ml of 2.00 x 10‘3M g Fe(N03)3. At equilibrium, what molar concentration of the thiocyanatoironflll) ion would you expect? 2:? ’ ‘ F " L )(Juat 0" 7 s K3 [HSCNZU 357’.) 5 It, 00000 f— ): {.oowo 3M .ZL ° 3‘ CN 3 ...~ 533 CR 3E5 MW‘XMoinfill-3e.£19-;J5 § KEFH‘KILN'J lir'r‘jmzfl \Lq X10"! :[ie 3.qu- Lgcwj .— (,1L)(9v00rro ->> ‘ L—r‘ ». . —-—-~-~~ 'll’w “0' a m/ 5, .2 a ~------~--- - \ WWW-3% ...
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