2.5 g sample of impure mercury (II) oxide, in excess of potassium iodide is being resolved. HgO(k) +4I^- + H2O ------>> Hg(l4)^-2+ 2OH^- Calculate the percentage of HgO in the sample, since 45 mL of 0.2 M HCl is consumed in the titration of the hydroxide formed. (MaHgO=216.59g/mol
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- The arsenic in a 1.22-g sample of a pesticide was converted toAsO43- by suitable chemical treatment. It was then titratedusing Ag+ to form Ag3AsO4 as a precipitate. (a) What is theoxidation state of As in AsO43-? (b) Name Ag3AsO4 by analogyto the corresponding compound containing phosphorusin place of arsenic. (c) If it took 25.0 mL of 0.102 M Ag+to reach the equivalence point in this titration, what is themass percentage of arsenic in the pesticide?The level of dissolved oxygen in a water sample can be determined by the Winkler method. In a typical analysis, a 100.0-mL sample is made basic, and treated with a solution of MnSO4, resulting in the formation of MnO2. An excess of KI is added, and the solution is acidified, resulting in the formation of Mn2+ and I2. The liberated I2 is titrated with a solution of 0.00870 M Na2S2O3, requiring 8.90 mL to reach the starch indicator end point. Calculate the concentration of dissolved oxygen as parts per million of O2.calculate the mass of Sn when 50 mL of a sample containing Sn2+ is titrated with 42.00 mL of 0.0150M MnO4- to reach endpoint
- 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 weight percent by volume of NaOCl in the sample.(MaNaOC:74,4 g/mol)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 mgA solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 785 mL. Calculate b) the weight/volume percentage of K3Fe(CN)6, the number of millimoles of K+ in 35.0 mL of this solution, and the ppm of Fe(CN)63-
- 0.2219 g of pure iron wire was dissolved in acid nd iron reduced to+2 state. Then the solution required 34 65ml of cerium(4) in a titration . Calculate molar concentration of ce4+???The purity of a pharmaceutical preparation of sulfanildamide (C6H4N2O2S), is prolonged oxidizing the sulfur in the sample to SO2 and bubbling this SO2 through a solution of H2O2 which converts it to H2SO4. The acid is titrated with a standard solution of NaOH (0.1251 M) until the end point with bromothymol blue, which changes color when both protons of the acid sulfuric have been neutralized. Calculate the purity of the preparation in % by weight given that a sample of 0.5136 g required 50.00 mL of the NaOH solutionIf 1.000 ml. of a solution of KMn04 is equiva- lent to 0.1000 millimole of NaCHO2 (sodium formate) in the fol- lowing titration: 3CHO2- + 2MnO- + H2O -> 3CO2 + 2MnO2 + 5OH-, what is the value of the KMnO4 in terms of grams of CaO in the volumetric method for calcium in which that element is precipitated as CaC2 4 .H2O and the precipitate is filtered, dis- solved in dilute H2S04 , and the oxalate titrated with permanganate?
- 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 ………………………………3 L contaminated air 50 mL 0.0116 M in an air pollution analysisCarbon dioxide (CO2) BaCO3 is passed through Ba (OH) 2 solution.is precipitated as. Excess of base, next to phenol phthalate (f.f.) indicatorIt is titrated with 23.6 mL of 0.0108 M HCl. CO2 in this air sampleCalculate its concentration in ppm. (Density of CO2Take it as 1.98 g / L. C = 12, O = 16 g / mol).A 20 mL volume of 0.015 M KIO3 containing an excess of KI, is added to a 0.312 g sample of a Real Lemon solution containing vitamin C. The Yellow-brown solution, caused by excess I2 is titrated to a colorless starch endpoint with 11.3 mL pf 0.106M Na2S2O3. Question: Calculate the percent by mass of Vitamin C in the Real Lemon Sample