An anion has an electrophoretic mobility of -2.50 cm2 /kV - min on a CE system containing a 30 cm long capillary with a detector located 25.0 cm from the point of injection. If the electroosmotic mobility of the buffer is 4.10 cm- /kV - min, and the applied voltage is 15.0 kV, what are the migration time (v) and the apparent mobility (Ha)?
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- 4. The molar absorptivities of the indicator weak acid HIn (K_{a} = 1.42 * 10 ^ - 5) and its conjugate base In at 570 were determined as epsilon(HIn) = 7120 and ε(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 and pH = 6.5 .4. The molar absorptivities of the indicator weak acid HIn (K₁ = 1.42 x 105) and its conjugate base In at 570 were determined as ε(HIn) = 7120 and ɛ(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 × 10%. (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 x 105 and pH = 6.5.WARIARTAM 2. 1.2589 g of a certain brand of milk powder required 25.89 mL of 0.01873M EDTA to titrate the calcium contained in the sample. (a) What is the percent calcium in the sample? (b) Would the true result be higher, lower, or not be affected if the milk powder sample has been slightly wet?
- Potentiometric titration A potentiometric titration of a 0.278 g sample of FeSO.7H,0 salt, in acidic medium, with a 0.011 M solution of potassium dichromate (K.Cr.0-) was conducted. The potential is measured with respect to a calomel electrode (Eadnd = 246 mV). The following graph represents the measured potential with respect to the volume of added dichromate. 700- 675 650 Calculate E for the half- 625 reaction: Fe" + e Fe (Show your work using Nemst equation). 600 > 575 550 Hint: Use the graph, to determine, appraximately, the equivalence point and mid-point of the titration 525 500 475 450 425 400 6 8 10 12 14 16 18 20 22 V (K>Cry0,) in ml. (Au) 3Complexometric titrations are generally conducted to determine divalent cations. The most important applications are the titration of calcium and magnesium with EDTA. (a) A supplement tablet containing about 300.00 mg of calcium ion was dissolved, filtered, and diluted to 100.00 ml volume. Several 2.00 ml samples of the total solution were titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 13.65 mL. Calculate the calcium content of the supplement tablet in mg units. (b) A sample of Epsom Salt of mass 0.7567 g was dissolved uniformly in distilled water in a 250.00 mL volumetric flask. Portions of the magnesium ion solution of volume 10.00 mL were titrated using a 0.01000 M solution of EDTA. The mean corrected titration volume was 12.25 ml. Calculate the percentage by mass (% w / w) of the magnesium in the Epsom Salt sample. (c) A 100.00 mL sample of tap water was titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 14.80 mL. Determine…A 10.0 mL solution of 0.050 M AgNO3 was titrated with 0.0250 M NaBr in the cell: S.C.E || titration solution | Ag(s) Find the cell voltage for 30.0 mL of titrant. (A) +0.093 V (B) -0.039 V (C) -0.093 V (D) +0.039 V
- Solutions of cobalt (II) ions have a magenta color with a molar absorptivity constant (e) value at 511 nm of 5.87 M-1cm-1. A 0.500 mL sample is transferred from a 50.0 mL stock solution of Co(NO3)2 and diluted with water to a final volume of 7.50 mL. The dilution had an absorbance value at 511 nm in a standard cuvette (1.00 cm light path) of 0.382. Calculate the mass of Co(NO3)2 contained in the original 50.0 mL stock solution.(a) For the precipitation reaction: A+ + B– AB(s)Calculate the value of the equilibrium constant for 99.99% conversion to AB atthe equivalence point, assuming that the analyte content is 5.00 mmole and thetotal volume at the equivalence point is 100.00 mL.(b) What factors affect end-point sharpness in a precipitation titration? Explain.(c) Explain briefly why silver nitrate is an important reagent used in precipitationtitrations.(d) Mohr Method, Volhard Method and Fajans Method are commonly used for thevolumetric analysis of chlorides. Distinguish the three methods in terms of thetitrants and indicators used, and how the titrations are carried out.Penicillin F is recovered from a dilute aqueous fermentation broth by extraction with amyl acetate, using 6.5 volumes of solvent per 100. volumes of the aqueous phase. At pH = 3.8 the distribution coefficient KD is 74. (a) What fraction of the penicillin would be recovered in a single ideal stage? (b) What would be the recovery with three-stage extraction using fresh solvent in both stages? (c) How many ideal stages would be needed to give the same recovery as in part (b) if a counterflow cascade were used with V/L = 0.065?
- A 2.50 mL aliquot of a solution that contains 3.85 ppm Fe(III) is treated with an appropriate excess of KSCN and diluted to 100.0 mL. What is the absorbance of the resulting solution at 580 nm in a 0.50 cm cell? (Molar absorptivity of Fe (SCN)2+is 7.0 x 105L mol-1cm-1). AW: K =39.098 S=32.08 C=12.011 N=14.007 Fe=55.845(b) An unknown solution containing 25.00 mL of Ni2+ in dilute HCI is treated with a known excess of 25.00 mL of 0.05382 M EDTA solution. The solution turns yellow when a few drops of indicator are added. The excess unreacted EDTA back titrated with 0.02299 M Zn²*, which requires 17.00 mL to reach the red end point. What is the molarity of Ni2+ in the unknown solution?) What amperage is required to plate out 0.250 mol Cr from a Cr3+ solution in a period of 8.00 h?