QUESTION 21 What is the mechanism involved upon observation of the blue-black color in lodometry? complexation between the ferric ions and analyte back-titration has been performed adsorption of molecular iodine in the helical structure of amylose formation of starch-iodo complex
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- Answer the following :(i) What is the role of cryolite in the metallurgy of aluminium?(ii) Difference between roasting and calcination.(iii) What is meant by the term ‘chromatography’?b. Given that the cuvette path length was 1.17 cm, use the slope of this line to calculate the molar absorptivity of the cobalt complex at this wavelength. (Assume Beer’s law is obeyed.) c. An unknown cobalt sample was treated as follows: 40.8 mg of the unknown was dissolved in solvent to prepare 50.00 mL of solution in a volumetric flask. 4.00 mL of this solution was treated with thiocyanate, and diluted to a final volume of 50.00 mL. A sample of this final solution was placed in the same cuvette as the standards, and showed an absorbance of 0.38 at 625 nm. Determine the percentage of cobalt in the original unknown, given that the atomic mass of cobalt is 58.933 g/mol.Find the isoelectric and zwitter ion of lysine, show the steps
- Use the following information to answer the question. Molar absorptivity data for the cobalt and nickel complexes with 2,3-quinoxalinedithiol are ϵCo = 36400 and ϵNi = 5520 at 510 nm and ϵCo = 1240 and ϵ Ni = 17500 at 656 nm. A 0.457-g sample was dissolved and diluted to 200.0 mL. A 25.0-mL aliquot was treated to eliminate interferences; after addition of 2,3-quinoxalinedithiol, the volume was adjusted to 50.0 mL. This solution had an absorbance of 0.970 at 510 nm and 0.393 at 656 nm in a 1.00-cm cell. (a) Calculate the concentration of cobalt (in ppm) in the initial solution prepared by dissolving the sample. (b) Calculate the concentration of nickel (in ppm) in the initial solution prepared by dissolving the sample.A 50.0-mL solution containing Ni21 and Zn21 was treated with 25.0 mL of 0.045 2 M EDTA to bind all the metal. The excess unreacted EDTA required 12.4 mL of 0.012 3 M Mg21 for complete reaction. An excess of the reagent2,3-dimercapto-1-propanol was then added to displace the EDTA from zinc. Another 29.2 mL of Mg21 were required for reaction with the liberated EDTA. Calculate the molarities of Ni21 and Zn21 in the original solution.The potassium ion in 250 ml of a water sample was first precipitated as potassium tetraphenylborate: K +(aq) + (C6H5)B- (aq)- KB(C6H5)4 (s). washed, dried and dissolved in an organic solvent. treatment of the organic solution with an excess of aqueous solution of the Hg(ii)-edta complex generated the following reaction: 4HgY2- (aq) +KB(C6H5)4(s) + 4H2O ➜H3BO3, (aq) +4C6H5Hg+(aq) + 4HY3- (aq) + K+ (aq) + OH -(aq) The released edta (in the form of HY3-) was fully titrated with 28.73 ml of 0.04xy mol/l zncl2 solution. Determine the concentration in mg/l of potassium in the water sample. xy is 11
- What transition (d–d charge transfer) is responsible for the dark blue color of [Cu(phen)2]BF4? Why does the dissolution [Cu(phen)2]BF4 of in dichloromethane (DCM) result in a dark orange solution? Justify your answer.Calmagite is often used as a substitute for Eriochrome Black T as indicatorin the determination of Ca. List down two main advantages of calmagite overEriochrome Black T.You wish to measure the iron content of the well water on the new property you are about to buy. You prepare a reference standard Fe3+ solution with a concentration of 5.74×10−4 M. You treat 14.0 mL of this reference with HNO3 and excess KSCN to form a red complex and dilute the reference to 60.0 mL. The diluted reference is placed in a cell with a 1.00‑cm light path. You then take 30.0 mL of the well water, treat with HNO3 and excess KSCN, and dilute to 100.0 mL. This diluted sample is placed in a variable pathlength cell. The absorbance of the reference and the sample solutions match when the pathlength is 1.76 cm. What is the concentration of iron in the well water? For each solution, the zero is set with a blank.
- You wish to measure the iron content of the well water on the new property you are about to buy. You prepare a reference standard Fe3+ solution with a concentration of 5.53×10−4 M. You treat 10.0 mL of this reference with HNO3 and excess KSCN to form a red complex and dilute the reference to 45.0 mL. The diluted reference is placed in a cell with a 1.00‑cm light path. You then take 20.0 mL of the well water, treat with HNO3 and excess KSCN, and dilute to 100.0 mL. This diluted sample is placed in a variable pathlength cell. The absorbance of the reference and the sample solutions match when the pathlength is 3.25cm. What is the concentration of iron in the well water? For each solution, the zero is set with a blank.What is the mechanism involved upon observation of the blue-black color in Iodometry? complexation between the ferric ions and analyte adsorption of molecular iodine in the helical structure of amylose formation of starch-iodo complex back-titration has been performedyou've been tasked to compound 30 grams of a 0.5% Zinc oxide ointment. you have a stock preparation of zinc oxide 5% strength to mix with petrolatum to dilute the ordered strength. In what (parts) ratio could this be compounded?