c) An impure sample of Na3PO3 weighing 0.1392 g was dissolved in 25 mL of water. A solution containing 50 mL of 3% w/v mercury(II) chloride, 20 mL of 10% w/v sodium acetate and 5 mL of glacial acetic acid was then prepared. The solution containing the phosphite was added dropwise to the second solution, oxidizing PO3³ to PO4³ and precipitating Hg2Cl2. After digesting, filtering, and rinsing, the precipitated Hg2Cl₂ was found to weigh 0.4320 g. What is the purity of the original sample as %w/w Na3PO3

c) An impure sample of Na3PO3 weighing 0.1392 g was dissolved in 25 mL of water. A solution containing 50 mL of 3% w/v mercury(II) chloride, 20 mL of 10% w/v sodium acetate and 5 mL of glacial acetic acid was then prepared. The solution containing the phosphite was added dropwise to the second solution, oxidizing PO3³ to PO4³ and precipitating Hg2Cl2. After digesting, filtering, and rinsing, the precipitated Hg2Cl₂ was found to weigh 0.4320 g. What is the purity of the original sample as %w/w Na3PO3

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter4: Calculations Used In Analytical Chemistry

Section: Chapter Questions

Problem 4.32QAP

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An impure sample of Na3PO3 weighing 0.1392 g was dissolved in 25 mL of water. A solution containing 50 mL of 3% w/v mercury(II) chloride, 20 mL of 10% w/v sodium acetate, and 5 mL of glacial acetic acid was then prepared. The solution containing the phosphite was added dropwise to the second solution, oxidizing PO3^3– to PO4^3– and precipitating Hg2Cl2. After digesting, filtering, and rinsing, the precipitated Hg2Cl2 was found to weigh 0.4320 g. Report the purity of the original sample as %w/w Na3PO3. Moles Na3PO3 = moles Hg2Cl2
A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe2O3 (aq) to elemental iron: I. Enough sulfur trioxide gas was bubbled to Fe2O3 aqueous suspension to completely yield ferric sulfate. II. Then, 5.00 M nitric acid was added to ferric sulfate yielding an aqueous solution of ferric nitrate. III. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron ----- a. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, l, g).(CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express final answers in 3 significant figures. c. High-concentration HCl is supposed to be added at the last part of the procedure. Briefly state its purpose.
An exhausted zeolite softener was regenerated by passing 100 litres, of NaCl. Solution containing 150 gm per lit. of NaCl. How many lit. of a sample of H2O of hardness 300 ppm can be softened by this softener? (Given at wts. for C = 12, O = 16, Na = 23, CI = 35.5, Ca = 40).
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?
An impure sample of Na3PO3 weighing 0.1 g is dissolved in 35 mL of water. A solution containing 45 mL of 3% w/v HgCl2, 30 mL of 10% w/v sodium acetate, and 10 mL of glacial acetic acid is then prepared. After digesting, filtering, and rinsing the precipitate, 0.2857 g of Hg2Cl2 is obtained. Report the purity of the original sample as % w/w Na3PO3.
what wt. of limestone containing 9.57% Mg must be taken for analysis in order to precipitate of 0.551g Mg2P2O7? how many grams of Na2SO4 are required to ppte Ag2SO4 from 2.000t of AgNO3? a sample of magnetite (impure Fe3O4) weighing 0.5000g is fused with oxidizing flux and the ferric compound formed is eventually precipitated as ferric hydroxide and ignited to ferric oxide which weighs 0.4980calculate %Fe & %Fe2O3
A sample of an iron ore was prepared for Fe3+ analysis as following: 3.4g of the sample was added anddissolved in acid environment then diluted to 250 mL using volumetric flask. After that, 10 mL of the resultingsolution was transferred by pipet to a 50-mL volumetric flask and continue to be diluted. The scientists foundout that this solution gives the concentration of Fe3+ as 2.3 mg/L. Find the weight percentage of Fe3+ in theoriginal sample.
Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)
The chief chemist of the Brite-Metal Electroplating Co. isrequired to certify that the rinse solutions that are discharged from the company’s tin-plating process into the municipal sewer system contain no more than 10 ppm (parts per million) by mass of Sn2+. The chemist devises the following analytical procedure to determine the concentration. At regular intervals, a 100-mL (100-g) sample is withdrawn from the waste stream and acidified to pH = 1.0. A starch solution and 10 mL of 0.10 M potassium iodide are added, and a 25.0-mA current is passed through the solution between platinum electrodes. Iodine appears as a product of electrolysis at the anode when the oxidation of Sn2+ to Sn4+ is practically complete and signals its presence with the deep blue color of a complex formed with starch. What is the maximum duration of electrolysis to the appearance of the blue color that ensures that the concentration of Sn2+does not exceed 10 ppm?
Six iron tablets containing FeSO4.7H2O were dissolved in 100-ml of 0.1M HNO3 with gentle heating. All of the Fe2+ is converted to Fe3+ by the strong oxidizing conditions. After the solution had cooled to room temperature , 2.5-ml of 35wt% NH4OH was added. The precipitate Fe2O3-xH2O that was filtered weighed 0.345g. Thermogravimetric analysis of the crude product showed a 10.5% weight loss . A. How many waters of hydration were in the precipitate B. How much iron is present in each tablet
Given the solubility of ferrihydrite (Fe(OH)3) and goethite (FeOOH), with dissolution reactions shown below: [1] Fe(OH)3 3 H+ à Fe3+ + 3 H2O Ksp = 8.4 x 10^4 ∆ Gr0 = -28 KJ/mol Solubility of Fe(OH3) = 7.468 [2] FeOOH + 3 H+ à Fe3+ + 2 H2O Ksp = 8.8 x 10^-2 ∆ Gr0 = 6 KJ/mol Solubility of FeOOH = 0.353 QUESTION: [A] How much Fe3+ from ferrihydrite would dissolve at pH 2 ? [B] How much Fe3+ from ferrihydrite would dissolve at pH 7 ? [C] How much Fe3+ from goethite would dissolve at pH 2 ? [D] How much Fe3+ from goethite would dissolve at pH 7 ?
A sample of feldspar weighing 1.500g is decomposed, and eventually there is obtained a mixture of KCl and NaCl weighing 0.1801 g. These chlorides are dissolved in H2O, a 50-mL pipetful of 0.08333 N AGNO3 is added, and the precipitate is filtered off. The filtrate requires 16.47 mL of 0.1000N KCNS, with ferric alum as indicator. Calculate the percentage of K2O in the silicate.