The phosphorus in a 0.2091-g sample was precipitated as the slightly soluble (NH4)3PO4 -12M0O3. This precipitate was filtered, washed, and then redissolved in acid. Treatment of the resulting solution with an excess of Pb* resulted in the formation of 0.2922 g of PBM0O4 (367.14 g/mol). Express the results of this analysis in terms of percent P205 (141.94 g/mol). Show your solution. O A. 2.251 % B. 1.257 % O C. 5.215 % D. 2.154 %

The phosphorus in a 0.2091-g sample was precipitated as the slightly soluble (NH4)3PO4 -12M0O3. This precipitate was filtered, washed, and then redissolved in acid. Treatment of the resulting solution with an excess of Pb* resulted in the formation of 0.2922 g of PBM0O4 (367.14 g/mol). Express the results of this analysis in terms of percent P205 (141.94 g/mol). Show your solution. O A. 2.251 % B. 1.257 % O C. 5.215 % D. 2.154 %

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter12: Gravimetric Methods Of Analysis

Section: Chapter Questions

Problem 12.29QAP

See similar textbooks

Similar questions

Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60 C), filtering to remove insoluble impurities, cooling to 0 C to precipitate solid NaHCO3, and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 C is 164 g/L. Its solubility in cold water of 0 C is 69 g/L. What is the percent yield of NaHCO3 when ills purified by this method?
When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
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?
68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?
A 300.0-g sample of a solid is made up of a uniform mixture of NaNO3, MgCl2, and BaCl2. A 100.0-g sample of the mixture is dissolved in water and treated with an excess of KOH. The precipitate from the reaction has a mass of 13.47 g. The remaining 200.0-g sample is also dissolved in water and treated with an aqueous solution of AgNO3. The resulting precipitate has a mass of 195.8 g. What are the masses of NaNO3, MgCl2, and BaCl2 in the 300.0-g sample?
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
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)
The mercury in a 1.1113-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5Hg2+ + 2H5IO6 → Hg5(IO6)2 + 10H+ The precipitate was filtered, washed free of precipitating agent, dried, and weighed, and 0.4733 g was recovered. Calculate the percentage of Hg2Cl2 in the sample. _______%
An analyst was assigned to work a sample with minerals. This iron-containing sample was analyzed by dissolving a 1.3142g sample in concentrated HCl. The resulting solution was diluted with water and iron (III) was precipitated as the hydrated oxide Fe2O3 xH2O by the addition of HN3. After filtration and washing, the residue was calcined at high temperature to produce 0.5488g of pure Fe2O3 (159.69g / mol). Determine the following:a) the% Fe (55.847 g / mol) and the% Fe3O4 (231.54 g / mol) in the sample.
A water sample known to contain lead (MM: 207.2) and silver (MM: 107.9) was analyzed to determine its lead and silver content. A 10.00-mL aliquot (portion) of the water sample was chemically treated to convert all lead to Pb2* and silver to Ag* then added with slight excess of HCI to precipitate them as chlorides (MM PbCI2: 278.1; AgCI: 143.3). After thorough washing and drying, 0.0620 g of the precipitate was recovered. Simultaneously, another 10.00-mL portion of the water sample was subjected to electrogravimetry. Lead was deposited as PO (MM: 223.2) while silver was deposited as metal on the surface of a platinum electrode. The deposited material weighed 0.0467 g. Calculate %Pb and %Ag (by volume) in the water sample.

SEE MORE QUESTIONS

Recommended textbooks for you

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

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

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

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

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry