8. Identify X, and justify your choice using chemical equations where relevant. (5 A) Manganese is a transition metal that can display a range of oxidation states: Mn²+, Mn³+, Mn4*, Mn6+ and Mn7+ are all known. Here, manganese is in a hydrated compound with the element X. Element X will precipitate out of the solution as part of an ionic compound if a suitable cation is added. Conduct an investigation to identify the element X, given the formula MnX. 4H₂O (note that the quantity of X is not specified in the formula).

8. Identify X, and justify your choice using chemical equations where relevant. (5 A) Manganese is a transition metal that can display a range of oxidation states: Mn²+, Mn³+, Mn4*, Mn6+ and Mn7+ are all known. Here, manganese is in a hydrated compound with the element X. Element X will precipitate out of the solution as part of an ionic compound if a suitable cation is added. Conduct an investigation to identify the element X, given the formula MnX. 4H₂O (note that the quantity of X is not specified in the formula).

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 105AE: Chlorisondamine chloride (C14H20Cl6N2) is a drug used in the treatment of hypertension. A 1.28-g...

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Triiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: IO3(aq) + I(aq) I3(aq) Triiodide ion concentration is determined by titration with a sodium thiosulfate (Na2S2O3) solution. The products are iodide ion and tetrathionate ion (S4O6). a. Balance the equation for the reaction of IO3 with I ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HQ required to convert all of the IO3 ions to I ions? c. Write and balance the equation for the reaction of S2O32 with I3 in acidic solution. d. A 25.00-mL sample of a 0.0100 M solution of KIO. is reacted with an excess of KI. It requires 32.04 mL of Na2S2O3 solution to titrate the I3 ions present. What is the molarity of the Na2S2O3 solution? e. How would you prepare 500.0 mL of the KIO3 solution in part d using solid KIO3?
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Chlorisondamine chloride (C14H20Cl6N2) is a drug used in the treatment of hypertension. A 1.28-g sample of a medication containing the drug was treated to destroy the organic material and to release all the chlorine as chloride ion. When the filtered solution containing chloride ion was treated with an excess of silver nitrate, 0.104 g silver chloride was recovered. Calculate the mass percent of chlorisondamine chloride in the medication, assuming the drug is the only source of chloride.
A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to precipitate all of the iodide ion as silver iodide, AgI. If 1.545 g of the soluble iodide gave 2.185 g of silver iodide, how many grams of iodine are in the sample of soluble iodide? What is the mass percentage of iodine, I, in the compound?
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