The digestion of a 0.1387-g sample of a phosphorus containing compound in a mixture of HNO, and H2SO4 resulted in the formation of CO2, H20, and H 3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4);PO4 12M0O3. This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.1963 M NaOH. After the solution was boiled to remove the NH3, the excess NaOH was titrated with 17.55 mL of 0.1828 M HCI to a phenolphthalein end point. Calculate the percentage of phosphorus in the sample.

The digestion of a 0.1387-g sample of a phosphorus containing compound in a mixture of HNO, and H2SO4 resulted in the formation of CO2, H20, and H 3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4);PO4 12M0O3. This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.1963 M NaOH. After the solution was boiled to remove the NH3, the excess NaOH was titrated with 17.55 mL of 0.1828 M HCI to a phenolphthalein end point. Calculate the percentage of phosphorus in the sample.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

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Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.34QAP

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A mixture of xenon and ?uorine was heated. A sample of the white solid that formed reacted with hydrogen to yield 81 ml of xenon (at STP) and hydrogen ?uoride, which was collected in waiter, giving a solution of hydro?uoric acid. The hydro?uoric acid solution was titrated, and 68.43 mL of 0.3172 M sodium hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced Chemical equations for the reactions involving xenon.
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?
The digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the sample.
The mass of K3PO4 needed to prepare 250.0mL of an aqueous solution in which PO4-3 concentration is 0.0550M. The answer is ……………………… How many grams of silver sample is equal to 0.0417 mole of silver The answer is ……………………… When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of PbI2, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the recovered PbSO4 is found to have a mass of 0.0471g, what was the concentration of iodide ions in the original solution The answer is ……………………………… Express 96.342 m using 2 significant figures The answer is ………………………………. The oxidation number of sulfur in (Na2S2O5) is? The answer is ………………………………
What volume of 0.200 M NaOH is necessary to neutralize the solution produced by dissolving 2.00 g of PCl3 is an excess of water? Note that when H3PO3 is titrated under these conditions, only one proton of the acid molecule reacts.
A 9.12g of KClMgCl26H2O is to be dissolved to prepare a solution in sufficient water to give 1.500L. What is the molar analytical concentration of KClMgCl2 in this solution?
A sample of water in contact with solid Fe(OH)3 is found to have a pH of 7 .5. If no other dissolved solids are present in this water, what is the expected concentrated of Fe3+ in this sample?
A technician is setting up a laboratory to standardise ~0.0200 mol dm–3 KMnO4. What mass of Mohr’s salt [FeSO4(NH4)2SO4·6H2O] would the technician be required to weigh out to produce a 5.00 L solution of Mohr’s salt such that 25.0 cm3 aliquots of the salt would require a titre of 20.0 cm3 to standardise the KMnO4 solution?
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.
What weight of sample in gram containing 8.00 % Fe3O4 (MW= 231.53 g/mole) must be taken to obtain a precipitate of Fe (OH)3 (MW= 106.867 g/mol) that, when ignited to Fe2O3 (MW = 159.69 g/mole), weighs 150.0 mg
A 1.1324 g sample of magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe2+ and Fe3+. Nitric acid was added and the solution was boiled for a few minutes, which converted all of the iron to Fe3+. The Fe3+ was then precipitated as Fe2O3*xH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temp to give 0.5394 g of pure Fe2O3. What is the percent Fe and the percent Fe3O4 in the sample?
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