To find the Ce content, a 5.23 g solid were dissolved and treated with excess iodate to precipitate Ce(I03)4. The precipitate was collected, washed well, dried, and ignited to produce 0.235 g of CeO2 (172.114 g/mol). What was the mass of Ce (140.116 g/mol) in the original solid? Express your final answer in 4 decimal places. *

To find the Ce content, a 5.23 g solid were dissolved and treated with excess iodate to precipitate Ce(I03)4. The precipitate was collected, washed well, dried, and ignited to produce 0.235 g of CeO2 (172.114 g/mol). What was the mass of Ce (140.116 g/mol) in the original solid? Express your final answer in 4 decimal places. *

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.74QE: Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman...

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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?
148. Addition of 50.00 mL of 2.238 m H2SO4 (solution density = 1.1243 g/mL) to 50.00 mL of 2.238 M BaCl2 gives a white precipitate. (a) What is the mass of the precipitate in grams? (b) If you filter the mixture and add more H2SO4 solution to the filtrate, would you obtain more precipitate? Explain.
Calculate the weight of pure sodium carbonate that is necessary to prepare 2.806 L of 0.223 N Na2CO3 (105.99 g/mol) from the primary-standard solid. Assume the solution is to be used for titrations in which the reaction is: CO32- + 2H+ ----> H2O + CO2 Express you answers in 3 decimal places
A solution of HClO4 was standardized by dissolving 0.4008 g ofprimary-standard-grade HgO in a solution of KBr: HgO(s) + 4Br- + H2O → HgBr4 2- + 2OH- The liberated OH2 consumed 43.75 mL of the acid. Calculate themolar concentration of the HClO4.
A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.
To determine the amount of magnetite, Fe3O4 in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl to obtain a mixture of Fe2 + and Fe3 +. After HNO3 is added to oxidize Fe2 + to Fe3 + and diluted with water, Fe3 + is precipitated as Fe (OH) 3 by adding NH3. 0.8525 g of pure Fe2O3 is obtained by filtering, rinsing and burning the precipitate. Calculate the percentage of Fe3O4% in the sample. (Fe = 55,847g / mol, O = 15,999g / mol)
In one trial of Part B of the experiment 0.108 g of a solid mixture of NaCl and NaNO3 was dissolved in 100 mL of water with K2CrO4 indicator. A mass of 4.35 g of 1.70% AgNO3 solution was required to fully consume all of the chloride in the mixture. What was the mass percentage of NaCl in the original solid mixture? Enter your answer to the nearest tenth of a percent; do not include the percent symbol.
25 mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL solution taken from here and the I2 released is titrated with 35.5 mL of 0.0409 M NaS2O3. Accordingly, calculate the weight percent by volume of NaOCl in the sample. (Ma(NaOC:74,4 g/mol)
Sodium carbonate is a reagent that may be used to standardizeacids in the same way. In such standardization it was found that a 0.432-g sample ofsodium carbonate required 22.3 mL of a sulfuric acid solution to reach the end point forthe reaction.Na2CO3(aq) + H2SO4(aq) -----> H2O(l) + CO2(g) + Na2SO4(aq)What is the molarity of the H2SO4?
please help me The aluminum in a 1.200g sample of impure ammonium aluminum sulfate was precipitatedwith aqueous ammonia as the hydrous Al2O3 · XH2O. The precipitate was filtered and ignitedat 100°C to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysisin terms of % Al.
When a Vitamin C (ascorbic acid; MM = 176.12 g mol-1) tablet is crushed, dissolved and titrated with 0.0340 M KIO3(aq) to a purple/blue endpoint (given by a starch indicator), the volume of KIO3 used is 29.80 mL. If 60 mg of ascorbic acid is the recommended dietary allowance (i.e., 100% of the RDA), then what is the % RDA for the Vitamin C in the tablet? KIO3(aq) + 5 KI + 6 H+ → 3 I2(aq) + 3 H2O I2 (aq) + ascorbic acid → 2 I- + dehydroascorbic acid
25 mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL solution taken from here, and the released I2 is titrated with 35.5 mL of 0.0409 M NaS2O3. Accordingly, calculate the percent by volume of NaOCl in the sample (MaNaOC: 74.4 g/mol)A. 10.50%B. 15.75%C. 5.25%D. 20.85%