4. Calculate the molecular and Empirical formula of the compound following compositions; Cr = 26.52%, S= 24.52% and O= 48.96% with molecular mass having the of 2.96 amu.
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Determine the empirical and molecular formula of the following compounds.
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- When titrated in neutral solution with 0.05000 N I2, a mixture of As2O3, As2O5, and inert material requires 20.10 ml. The resulting solution is then acidified, and excess KI is added. The liberated I2 requires 29.92 ml of 0.1500 N NaS2O3 . Calculate the sum of the weights of As2O3 and As2O5 in the sample.Pyrolusite (MnO2) is dissolved in hydrochloric acid:MnO2 + HCl → MnCl2 + H2O + Cl2The chloride was passed into potassium iodide solution where it liberated iodine:Cl2 + KI → KCl + I2The iodine liberated was estimated by adding sodium thiosulfate, the reaction beingI2 + Na2S2O3 → NaI + Na2S4O6If 5.6 g of crystallized sodium thiosulfate, Na2S2O3 5H2O ,were used up, how many grams of manganese were present?MW (g/mole): I =126.9; Mn =54.94; Cl = 35.45; K = 39.09; Na = 23; S = 32How much CaCO3 (in grams) would you need to produce theoretically 500 g of baghdadite, via solid-state sintering, assuming the CaCO3 is the sole source of Ca2+? (nearest whole number) *note that ths solid-state sintering method mix material in stoichiometric ratios. A. 365 gB. 146 gC. 150 gD. 122 g
- 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.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.Suppose you reacted 0.500 g of Mg powder mixed with several acid-inactive substances and obtained 246 ml of hydrogen gas under S.T.P. conditions.What percentage by weight of the model is magnesium?
- The mercury in a 0.8142-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5 Hg 2+ + 2 H5IO6 ---> Hg5(IO6)2 (s) + 10 H + The precipitate (MW = 1448.8 g/mol) was filtered, washed free of precipitating agent, dried, and weighed, and 0.4114 g was recovered. Calculate the a) % Hg (200.6 g/mol) b) % Hg2Cl2 (472.1 g/mol)Use the following atomic masses (in g/mol):Mg = 24.31; O = 16; Ca = 40.08; C = 12.01; Na = 23; H = 1; N = 14.01; S = 32.06; Cl = 35.45; 2.) Limestone consists chiefly of mineral calcite (CaCO3). The carbonate content of 0.5413g of powdered limestone was measured by suspending the powder in water, adding 10mL of 1.392M HCl and heating to dissolve the solid and expel CO2. The excess acid required 39.96mL of 0.1004M NaOH for complete titration to a phenolphthalein end point. Find the % wt of calcite in limestone.A516.7 mg sample containing a mixture of K2SO, and (NH4)2S0, was dissolved in water and treated with BaCl2,precipitating the S042- as BaSO4. The resulting precipitate was isolated by filtration, rinsed free of impurities, and dried to a constant weight, yielding 863.5 mg of BaSO4. What is the %w/w K2SO4 in the sample?
- A sample known to consist of NaOH orNaHCO3, or Na2CO3 or possible compatible mixtures of these, together with inert matter. With methyl orange, a 1.10 g sample requires 31.40 mL of HCl (of which 1.00 mL ≈ 0.0140 g CaO). With phenolphthalein, the same weight of sample requires 13.30 mL of the acid. Calculate the percentage of inert matter in the sample.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?The use of silica to form slag in the production of phospho-rus from phosphate rock was introduced by Robert Boyle morethan 300 years ago. When fluorapatite [Ca₅(PO₄)₃F] is used inphosphorus production, most of the fluorine atoms appear in theslag, but some end up in toxic and corrosive SiF₄ (g).(a) If 15% by mass of the fluorine in 100. kg of Ca₅(PO₄)₃F forms SiF₄, what volume of this gas is collected at 1.00 atm andthe industrial furnace temperature of 1450.°C?(b) In some facilities, the SiF₄ is used to produce sodium hexa-fluorosilicate (Na₄SiF₆) which is sold for water fluoridation: 2SiF₄(g)+Na₂CO₃(s)+H₂O(l) →Na₂SiF₆(aq)+SiO₂(s)+CO₂(g)+2HF(aq) How many cubic meters of drinking water can be fluoridated toa level of 1.0 ppm of Fusing the SiF₄ produced in part (a)?