Which of the following statements is TRUE about elimination tests for anions? of Select one: SCN' in the presence of acidified Fe(NO3)3 and toluene will| result to the formation of a blood-red organic layer. Addition of Ba(NO3)2 to the anion test solutions will provide positive results for CO3², PO4³, and NO3" In the elimination tests that involve toluene, the aqueous layer is on top of the organic layer.

Which of the following statements is TRUE about elimination tests for anions? of Select one: SCN' in the presence of acidified Fe(NO3)3 and toluene will| result to the formation of a blood-red organic layer. Addition of Ba(NO3)2 to the anion test solutions will provide positive results for CO3², PO4³, and NO3" In the elimination tests that involve toluene, the aqueous layer is on top of the organic layer.

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter14: Applications Of Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 14.22QAP: Mixing the chelating reagent B with Ni(II) forms the highly colored NiB22+, whose solutions obey...

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A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br-50.00 mL remaining solution was analyzed for its Br- content by potentiometry using a metallic electrode of the second kind. a) Write the cell notation of the potentiometric set-up with SCE as the reference electrode. b) Write the Nernst equation that describes the indicator electrode set-up. Ecell recorded in running the solution using the potentiometric set-up was Ecell = 0.0286 V. (E0Ag/AgBr = 0.095 V) c) Compute for Eind. d) Compute pBr in the 50.00 mL aliquot. e) Compute for % NaBr ( in the potentiometric technique).
2. A sample of material contains for its active components NaOH, NazCO3, NaHCO3, or compatible mixtures of these. Two samples, each weighing 1.000 g, are dissolved in H20. To one sample phenolphthalein is added and the solution is titrated cold with 1.038 N acid, of which 17.96 mL is required. The other sample is titrated cold, with methyl orange as indicator, and 21.17 mL of the same acid is required. What alkalis are present, and what is the percentage of each in the original sample?
A 0.703 g sample of a commercial detergent was red-calcined to destroy its components. organic. Treatment of the residue with hot HCl gave phosphorus in solution as H3PO4. the phosphate was precipitated as MgNH4PO4-6H2O by the addition of Mg + 2 or followed by aqueous NH3. The precipitate was filtered, washed, and converted to Mg2P2O7 by calcination at 1000 C. The residue weighed 0.432 g. Calculate the percentage of phosphorus in the sample.
Consider an F M solution of Fe2(SO4)3. Besides H+ and OH−, the known species are Fe3+, Fe(OH)2+, Fe(OH)2+, Fe2(OH)24+, FeSO4+, SO42−, and HSO4−. a) Write the charge balance equation for this solution. b) Which species must be an ion pair, and which comes from acid hydrolysis of Fe3+? Write the balanced acid hydrolysis reaction for the hexa-aquo complex of Fe3+ and report its pKa c) Write two mass balance equations for this solution, one for total iron and one for total sulfate. [How do you think you should handle the species that includes two iron atoms?] Give numerical values for these equations in terms of F.
Mention 3 typical organic complexing agents in the environment and describe in which environments (in the widest sense) they are found and which elements are particularly taken up.
Mixing the chelating reagent B with Ni(II) forms the highly colored NiB22+, whose solutions obey Beer’s lawat 395 nm overa wide range. Provided the analytical concentration of the chelating reagent exceeds that of Ni(II) by a factor of 5 (or more), the cation exists, within the limits of observation, entirely in the form of the complex. Use the accompanying data to evaluate the formation constant Kf for the process Ni2++2BNiB22+
Write equations to demonstrate the stepwise reaction of Cd(H2O)42+ in an aqueous solution of KI to form CdI42-. Showthat Kf(overall) = Kf1 x Kf2 x Kf3 x Kf4.
If PbCl2 was not completely removed by hot water from the first group precipitate, what will become of it when the residue is treated with NH4OH?
An unknown salt X reacts with hot conc. H2SO4 to produce a brown coloured gas which intensifies on addition on copper turnings. On adding dilute ferrous sulphate solution to an aqueous solution of X and then carefully adding conc. H2SO4along the sides of the test tube, a brown complex Y is formed at the interface between the solution and H2SO4. Identify X andY and write the chemical equation involved in the reaction.
You have been sent to India to investigate the occurence of goiter disease attributed to iodine deficency. As part of of your investigation, you must make field measurements of traces of Iodide(I-) in groundwater. The procedure is to oxidize I- to I2 and convert the I2 into an intensely colored complex with the dye brilliant green in the organic solvent toluene. a) A 3.15x10^-6 M solution of the colored complex exhibited an absorbance of 0.267 at 635nm in a 1.00cm cuvet. A blank solution made from distilled water in place of groundwater had an absorbance of 0.019. Find the molar absroptivity of the colored complex. b)The absorbance of an unknown solution prepared from ground water was 0.175. Find the concentration of the unknown.
From the structure of EDTA (and knowing that it is ethylene diamine tetraacetic acid) explain why the EDTA ismuch more soluble after the addition of the basic ammonia buffer. Is there a chemical reaction that isresponsible for this solubility change? If so explain what the reaction is and how it would be responsiblefor the increased solubility of EDTA in water.
A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br-Nickel ion required 11.70 mL of 0.002146 M EDTAWhat is the percentage of NaBr (102.894) in the 1.000 g sample?