The addition of hot nitric acid to CuS (s) will... Form NIS Oxidize sulfide to elemental sulfur Release nickel ions. Form toxic fumes of nitrous oxides and hydrogen chloride
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- Cerium(IV) is a strong oxidizing agent commonly used in redox titrations. Which of the following statemnt is/are NOT true for cerium(IV)? I.A Ce** standard solution is prepared using primary-standard-grade ammonium hexanitratocerate(IV), (NH4)2Ce(NO3); dissolved in hot hydrochloric acid solution. II. Ce** is yellow and Ce3* is colorless. The color change is abrupt enough that Ce** can serve as its own indicator. III. Ce**/Ce* exists in different formal potential in different acids due to the interaction of the anions part of the acid with Ce** IV. Analysis of many organic analyte such as alcohol, aldehydes can be determined using Ce**by an indirect method involving a technique of back titration of unreacted excess Ce*with standard iron Il titrant O a. 1,11,IV O b. 1, II, III O. I,II O d. II, II, IV O e. I, II, III, IVA basic lining is given to a furnace by using:(a) Calcined dolomite(b) Copper sulphate(c) Haematite(d) SilicaA sample of pyrolusite weighing 0.6000 g is dissolved in a solution containing 5.00mL of 6.00 N H2SO4 and 0.900 g of H2C2O4.2H2O. The excess oxalate then requires24.00 mL of KMnO4 solution for titration. If each mL of the KMnO4 will oxidize the Fe(II)in 0.03058 g FeSO4.7H2O, what is the oxidizing power of the sample in terms of MnO2?84.33%
- Thortveitite is a mineral that contains the silicate ion [Si2O7]6-. The structure of this ion is such that the each Si atom is bonded to three terminal oxygen atoms, and the seventh O atom forms a bridge between the two Si atoms:[O3Si-O-SiO3]6-A 0.8965 g sample is dissolved in HNO; and filtered. The aluminum is present in solution as AP. The solution is made basic with ammonium hydroxide, NH.OH, and the aluminum hydroxide, Al(OH): (FW 78.004), precipitates. This gel is filtered in a porous glass crucible, rinsed with dilute ammonium hydroxide, ignited, cooled in a desiccator, and weighed. The resulting alumina, Al:O: (FW 101.94), weighed 0.1605 g. Why is the solution filtered after acid dissolution? • Why rinse with ammonium hydroxide solution? • What chemical transformation takes place during ignition? (Show the balanced chemical equation) Why use a desiccator during cooling? • Calculate the weight percent Al (AW 26.9815) in the sample.(A) if both sentences are true, (B) if both sentences are false, (C) if the first sentence is true but the second is false, and (D) if the first sentence is false but the second is true. 1. In oxygen fixation, the alkaline-iodide-azide solution was used to acidify the solution. The brown hydrated precipitate that formed in the process of oxygen fixation was magnesium hydroxide. 2.Visual inspection is enough to determine if water is of appropriate quality. The standards for drinking water quality are typically set by governments or by international standards. 3.Deeper levels of water often do not reach 100% air saturation equilibrium because they are not shallow enough to be affected by the waves and photosynthesis at the surface. The dissolved oxygen content is an important index when considering its suitability for town supply. 4. The normality (N) of a solution is determined by multiplying the molarity of the solution by its volume. In the standardization of the sodium thiosulfate…
- What is the uses of the following minerals group? SulfidesA sample of pyrolusite weighing 0.6000 g is dissolved in a solution containing 5.00 mL of 6.00 N H2SO4 and 0.900 g of H2C2O4 .2H2O. The excess oxalate then requires 24.00 mL of KMnO4 solution for titration. If each mL of the KMnO4 will oxidize the Fe(II) in 0.03058 g FeSO4 .7H2O, what is the oxidizing power of the sample in terms of MnO2?In what kind of sulfur preparation is precipitated sulfur preferred? Why?
- Please compare the solubility of ferrihydrite (Fe(OH)3) and goethite (FeOOH), with dissolution reactions provided. FeOOHgoethite + 3 H+ à Fe3+ + 2 H2O Fe(OH)3(ferrihydrite) 3 H+ à Fe3+ + 3 H2OA 1.000-g sample of limestone gave a precipitate of Fe2O3 and Al2O3, weighing 0.0800 g. The precipitate of mixed oxides was fused with KHSO4, dissolved in sulfuric acid, and passed through a Jones reductor. The iron was titrated with 20.00 mL of 0.0100 N permanganate solution. Calculate the percentage of FeO and Al2O3 in the limestone (assume all iron present as FeO in the original sample)Silicate [SiO4] 4- and Phosphate [PO4]3- anions seem to be quite similar when briefly viewed. However, there are subtle differences that differintiate these two molecules. What is the electrostatic valency (or e.v. for short) bond strengths for the phosphate and silicate anions mentioned above? Given the electrosatic valency principal, what is the difference between these molecules relative to the structures for silicate and phosphate minerals? Lastly, I want you to calculate the value of e.v. for both molecules (phosphate and silicate). Remember, this is a three part question. If you do not answer completely you will not be given full credit for this assignment!!