You are studying the % CI in FeCl2. You have 5.53 g of Ferrous chloride (FeCl2) sample and after a lengthy process involving filtering you obtained 2.45 g of wet precipitate that was placed in the oven for 2 hours. After the heat treatment the mass of dry chloride precipitate was 0.273 g. Important information Molar Mass of Fe2+ = 55.85 g / mol Molar Mass of Cl = 35.45 g/mol Please answer the following four (4) questions: h 1. What is the proper gravimetric setup for this question? 2. What is the molar mass of the sample? 3. What is the mass of precipitate in mg? 4. What is % CI in FeCl₂?

You are studying the % CI in FeCl2. You have 5.53 g of Ferrous chloride (FeCl2) sample and after a lengthy process involving filtering you obtained 2.45 g of wet precipitate that was placed in the oven for 2 hours. After the heat treatment the mass of dry chloride precipitate was 0.273 g. Important information Molar Mass of Fe2+ = 55.85 g / mol Molar Mass of Cl = 35.45 g/mol Please answer the following four (4) questions: h 1. What is the proper gravimetric setup for this question? 2. What is the molar mass of the sample? 3. What is the mass of precipitate in mg? 4. What is % CI in FeCl₂?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter12: Gravimetric Methods Of Analysis

Section: Chapter Questions

Problem 12.19QAP

See similar textbooks

Similar questions

On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
What mass of HCl is contained in 45.0 mL of an aqueous HCl solution that has a density of 1.19 g cm-3 and contains 37.21% HCl by mass?
You want to prepare a 1.0 mol/kg solution of ethyleneglycol, C2H4(OH)2, in water. Calculate the mass of ethylene glycol you would need to mix with 950. g water.
A certain grade of steel is made by dissolving 5.0 g of carbon and 1.5 g of nickel per 100. g of molten iron. What is the mass percent of each component in the finished steel?
The substance KSCN is frequently used to test for iron in solution, because a distinctive red color forms when it is added to a solution of the Fe3+ cation. As a laboratory assistant, you are supposed to prepare 1.00 L of a 0.200 M KSCN solution. What mass, in grams, of KSCN do you need?