1. Account for the fact that for all transition metals, Ti to Cu, the +2 oxidation state is known but the highest oxidation state decreases from Mn(VII) to Cu(III). Use a sketch of the RDF to help illustrate your answer.
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- 1. When Pearl added (NH4)2CO3 solution to an unknown salt solution in basic conditions, the solution remained clear and colorless. Which of the following is the metal ion present in the salt solution?a.Ca2+b.K+c.Sr2+d.Ba2+2. The unknown salt solution assigned to Hayoung produced a white precipitate with (NH4)2CO3 (in basic conditions), and the resulting precipitate is soluble in 6 M CH3COOH. Then, she added 3 drops of 1 M K2CrO4 to a portion of the original salt solution, and a yellow precipitate was observed. What is the identity of the yellow precipitate? a.Na2CrO4 b.BaCrO4 c.CaCrO4 d.(NH4)2CrO4The amount of Fe in a 0.4891-g sample of an ore is determined by titrating with K2Cr207. After dissolving the sample in HCI, the iron is brought into a +2 oxidation state using a Jones reductor. Titration to the diphenylamine sulfonic acid end point requires 36.92 mL of 0.02153 M K2Cr207. Report the ore's iron content as %w/w Fe203. In this problem, which is the indicator ? Fe2+ Fe203 HCI K2Cr207 diphenylamine sulfonic acidUse the data provided for stock concentration and mass to calculate the concentrations of each solution. Solution A) A stock solution of 0.0100 M solution of K3[Fe(CN)6] is provided. Calculate the volume of the stock solution needed to prepare 100.0 ml of .00200 M K3[Fe(CN)6]. Deionized water should be used to dilute the solution. Solution B) Calculate the volume of solution A needed to prepare 50.0 ml of .0010 M K3[Fe(CN)6]. Deionized water should be used to dilute this solution.
- The amount of Fe in a 0.4891-g sample of an ore is determined by titrating with K2Cr207. After dissolving the sample in HCI, the iron is brought into a +2 oxidation state using a Jones reductor. Titration to the diphenylamine sulfonic acid end point requires 36.92 mL of 0.02153 M K2Cr207. Report the ore's iron content as %w/w Fe203. In this problem, which is the titrant? K2Cr207 diphenylamine sulfonic acid Fe203 HCI Fe2+6. A mixture contains at least one of the ions in the silver group (Ag*, Hg²*, Pb²+). Read the following procedure and determine which ions are present. Cold 6M HCl was added to the mixture producing a white precipitate. Hot water was then added and the solution was stirred, and the supernatant decanted to isolate a white precipitate after centrifugation. Sulfuric acid was added to one portion of the supernatant and potassium chromate was added to a second portion of the supernatant, but no precipitates formed. The isolated white precipitate was mixed well with 4 drops of concentrated ammonia. The resulting solution was centrifuged. The supernatant was decanted to show the presence of a grayish-black precipitate. To the supernatant, concentrated nitric acid was added dropwise until blue litmus paper added turned red and a white precipitate was present.1. Give the electron configuration (in t2g and eg forms) for Ti(III), Mn(II), and Ni(II) ions in: a) Octahedral (high spin) b) Tetrahedral crystal fields
- 1. The general formula for the copper ammine complex is [Cu(NH3)x]SO4•H2O. Calculate the formula weight for several values of x. (Include a short discussion on what you think reasonable values for x might be.) 2.You will need to prepare approximately 6 g of the copper ammine product. Estimate how much CuSO4•5H2O you should start with to prepare approximately 6 g of the copper ammine complex. 3.Calculate how many grams of CuSO4•5H2O are required to prepare a 0.05 M solution in a 100 mL volumetric flask. This solution will serve as a stock solution from which you’ll prepare your standards. 4.Show the equation needed to calculate the volume of 0.05 M stock solution needed to prepare a set of diluted solutions in a 10 mL volumetric flask. 5.Rearrange the equation from (4) to show how you can calculate the actual concentration of each standard, given the actual volume of stock solution delivered. 6.Show how you will calculate the ratio of ammine to copper (the value of x in the formula…A concentrated ammonia solution is added to a 0.010 M Ni(No3)2 to solution. Given the equilibrium concentration of ammonia [NH3] to is 0.20 M, determine the nickel (II) ion concentration. The formation constant Kf of the complex Ni(NH3)6^2+ + is 1.2 x 10^9. Assume the volume change from the addition of ammonia solution is negligible.[No^2+]=Using crystal field theory, draw an electron box energy level diagram for the valence d orbitals on the iron atom in a a [Fe(CO)]²+ complex. Your diagram should show the relative energy of each orbital, and the number of electrons in each orbital. Note: to make your diagram easier to read, label the d orbitals with just the subscript. For example, label the d2 orbital with just 2². Energy |
- 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, IVThe Kf (complex formation constant) of [Ag(en)₂*] > is 5.0x107. The standard reduction potential Eº Ag+/Ag is +0.800 V. • What is the Eº Ag(en)2*/Ag--the standard reduction potential of the silver complex to Agº at 298.15 K? • Use F= 96485 units, R= 8.3145 J/mol K. • Write answer in 2 (Two) significant figures. example if answer is -0.22334 V then you should write -0.22Calculate the concentration of [Ag(S2O3)2]3- in a solution which contains 8.5E-6 M Ag+ ions and twice that molar concentration of thiosulfate ions at equilibrium? The Kf for [Ag(S2O3)2]3- is 4.7 x 1013. Your answer should have 2 sig figs.