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find FT-IR of Hexammine chromium(III) nitrate
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- 5. The detection limits reported for Aluminum with ICP-AES and GFAAS are 2 ppb and 5 pg, respectively. If we assume a 20-µL sample volume is used with the GFAAS determination, which method has the better (i.e., lower) detection limit? (I am expecting a calculation here.)You were calculating the concentration of EDTA (MW 372.24 g/mol; Q = 98.45%). You weighed out 8.6731 g of dried EDTA into a 450.13 mL clean volumetric flask. You showed your lab instructor your calculated EDTA concentration of (no units in standard notation with proper number of significant figures) A M. You prepared your limestone sample (1.7737 g) by dissolving it in HCI, gently heating and then filling to the line in the 450.13 mL volumetric flask. You lab partner used a 12.55 mL volumetric pipette for the limestone sample, and from the titration you recorded 25.60 mL (wine colour). 25.63 mL (purple colour), 25.67 mL (blue colour), 25.72 ml (blue colour). The P/F ratio for this calculation is (in standard notation and to the proper number of significant figures) and the % Mg in the limestone sample is (answer in standard notation with no units to the proper number of significant figures) %.A 100.0-mL sample of spring water was treated to convert any iron present to Fe2+.Titration with 35.00-mLof 0.002345 M K2Cr2O7 resulted in the reaction6Fe2+ + Cr2O72- + 14H+ 6Fe3+ 1 2Cr3+ + 7H2OThe excess K2Cr2O7 was back-titrated with 8.32 mL of 0.00897 M Fe2+ solution.Calculate the concentration of iron in the sample in parts per million.
- Chromel is an alloy composed of nickel, iron, and chromium. A 0.6418-g sample was dissolved and diluted to 250.0 mL. When a 50.00-mL aliquot of 0.05173 M EDTA was mixed with an equal volume of the diluted sample, all three ions were chelated, and a 5.27-mL back-titration with 0.06139 M copper(II) was required. The chromium in a second 50.0-mL aliquot was masked through the addition of hexamethylenetetramine; titration of the Fe and Ni required 35.81 mL of 0.05173 M EDTA. Iron and chromium were masked with pyrophosphate in a third 50.0-mL aliquot, and the nickel was titrated with 25.77 mL of the EDTA solution. Calculate the percentages of nickel, chromium, and iron in the alloy. Percentage of nickel = % Percentage of iron = Percentage of chromium = % %3 In EDTA titrations, why does the pH of the solution need to be controlled?Determine the percentage of iron in a sample of limonite from the following data:weight of sample = 0.5000g volume of KMNO4 added 50.0mL ; 1.00mL Kmno4 = 0.0005507 g fevolume of FeSO4 used for back titration 8.00mL ; 1.00mL FeSO4= 0.008950 g FeOMW: Fe= 55.85 FeO= 71.84
- 30.0 ml solution of I was treated with 50.0 mL of 0.365 M AgNO. Agl (s) was filtered off, and the filtrate (plus Fe3+) was titrated with 0.287 M KSCN. When 37.60 mL had been added, the solution turned red. How many milligrams of I were in the original solution? (Given At. Mass of lodine = 126.9)The standard calibration curve for absorbance vs. [Cu- yielded a straight line with an equation y = 57.48(x) + 0.000481. The absorbance of the solution of CuC,H,O, was equal to 0.177. Calculate concentration of [Cu"). 3.10x 103 O 3.11x 102 10.1x 10-2 5.05 x 10-29.00 mL of 6.00 x 103 M Fe(NO3)3 (6.00 times 10 to the minus 3rd power M Fe (NO3)3) is added to 5.00 mL of 6.00 x 10-3 M KSCN (6.00 times 10 to the minus 3rd power M KSCN) along with 4.00 mL of water. The concentration of [F e(SCN)2*] was found to be 1.00 x 10-4 M (1.00 times 10 to the minus 4th power M) at equilibrium. How many moles of SCN" (SCN minus) are present in the solution at equilibrium? Express your answer as a decimal number (no exponents). Your Answer: Answer units
- Calcium in powdered milk is determined by dry ashing a 1.46g sample and then titrating the calcium with EDTA solution, 12.1mL being required. The EDTA was standardized by titrating 10.4mL of a Zn solution prepared by dissolving 0.634g Zn metal in acid and diluting to 1L (10.83mL EDTA required for titration). What is the concentration (ppm) of calcium in the powdered milk?2) A 100.0-mL sample of spring water was treated to convert any iron present to Fe2*. Addition of 25.00 mb. of 0.008 M K2Cr207 resulted in the reaction 6F22+ + Cr2O72- + 14H*2 6FE3+ + 2Cr3+ + 14H2O The excess K2C12O7 was back-titrated with 8.53 ml of 0.00949 M Fe2* şolution. Calculate the molar concentration of iron in the sample.Question 3, In the Spectrophotometric determination of Iron experiment, the calibration curve is plotted as absorbance vs. concentration (unit: mol/L). The curve is a straight line written as y=(5.0000x10^0)x-0.0235. The path length of the cuvette used in the lab is 1.0 cm. What is the molar extinction coefficient of the tris(phenanthroline) iron(II) in L/(mol*cm)? *Provide your answer with 5 significant figures. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: Answer x10
