Orthophosphate (PO4) in river sediment sample is determined by weighing ammonium phosphomolybdate, (NH4)PO412M0O3. 1.1682 g of precipitate were obtained from a 0.2711 g sample. [P = 30.97; PO4 = 94.97; P2O5 = 141.95; p.molybdate = 1876.5] i) Calculate the GF involving the analyte and precipitate.
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![(a)
Orthophosphate (PO4) in river sediment sample is determined by weighing
ammonium phosphomolybdate, (NH4)PO412M0O3. 1.1682 g of precipitate were
obtained from a 0.2711 g sample.
[P = 30.97; PO4 = 94.97; P2Os = 141.95; p.molybdate = 1876.5]
i)
Calculate the GF involving the analyte and precipitate.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F527c049b-edde-4315-a244-72d7a410fc36%2F99bfc2a2-91fd-4a7d-b6c2-3bc0a4d5c386%2F6502gkp_processed.jpeg&w=3840&q=75)
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- 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?The arsenic in a 1.203-g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and 40.00 mL of 0.05871 M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and in the washings from the precipitate was titrated with 9.63 mL of 0.1000 M KSCN, and the reaction was. Find the percentage of As2O3 in the sample.The arsenic in a 1.010 g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and exactly 40.00 mL of 0.06222M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag in the filtrate and in the washings from theprecipitate was titrated with 10.76 mL of 0.1000MKSCN; the reaction wasAg+ + SCN-→ AgSCN(s) Calculate the percent AsO3 in the sample.
- Write the balance equation of aqueous Pb(ClO3)2 with NaI. Include phases.What wt of magnetite should be taken for analysis in order that after converting to a precipitate of Fe2O3.xH2O, the percentage of Fe3O4 in the sample can be found by multiplying the wt in grams of the ignited precipitate (Fe2O3) by 100.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 ………………………………
- 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.One litre of a saturated aqueous solution of Ag2SO4 (MW = 311.79 g mol- 1) at 25 °C is evaporated to dryness. 4.844 g of Ag2SO4 residue was produced. What is the solubility product (Ksp)?A 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.
- The arsenic in a 1.223-g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, as 40.00 mL 0.07891 M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and washings from the precipitate was titrated with 11.27 mL of 0.1000 M KSCN; the reaction was Ag+ + SCN- → AgSCN(s) Calculate the percent As2O3 in the sample.The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?A solution was prepared by dissolving 514 mg of K3Fe(CN)6 in sufficient water to give 758 ml of solution. Cal a. The molar analytical concentration of K3Fe(CN)6 b. pK