0.004 C8H7NO3, 15mL ethanol, 0.002mol NaBH4 was used. HCl was used to acidify. It was then extracted with ether. Then it was dried and a mass of 0.32g was obtained. What is the balanced equation of this synthesis, and what is the limiting reagent?
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0.004 C8H7NO3, 15mL ethanol, 0.002mol NaBH4 was used. HCl was used to acidify. It was then extracted with ether. Then it was dried and a mass of 0.32g was obtained. What is the balanced equation of this synthesis, and what is the limiting reagent?
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- To prepare a very dilute solution of K2Cr2O7 (294.18 g/mol), 0.661 g of K2Cr2O7 was transferred to a 250.0-mL volumetric flask and adding water to the mark. A sample of this solution of volume 1.000 mL was then transferred to a 500.0-mL volumetric flask and diluted to the mark with water. Subsequently, 10.0 mL of the diluted solution was transferred to a 250.0-mL flask and diluted to the mark with water. What is the final concentration of K2Cr2O7 in this last solution?Calcium peroxytoctahydrate is synthesized according to the following reaction. During the synthesis based on 3.5 g calcium carbonate, 7.5 mL of 18% HCl with a density of 1.19 and 5.5 mL of 25% NH3 with a density of 0.91 were used, and further hydrogen peroxide and excess water were added to the medium. Since 2.35 g of calcium peroxytoctahydrate is obtained in this way, what is the% yield of the experiment? (HCl: 36.5 g/mol; NH3: 17 g/mol; CaCO3: 100 g/mol; CaO2.8H2O: 216 g/mol) CaCO3 + 2HCl 2NH3 + H2O2 + 7H2O → CaO2.8H2O + CO2 + 2NH4+ + 2 Cl-A 244.5-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4.7H20. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (CaP2O7). The mass of CaP2O, obtained is 0.0419 g. Give the calcium content of the ground water in parts per million (to three significant figures).
- By pipet, 5.00 mLmL of a 0.823 MM stock solution of potassium permanganate (KMnO4) was transferred to a 50.00-mL volumetric flask and diluted to the calibration mark. Determine the molarity of the resulting solution.Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) What is the %m/m of the solution? Final answer must be rounded off to 1 decimal place, and shall NOT have any unit.By pipet, 19.00 mL of a 0.823 M stock solution of potassium permanganate (KMnO4) was transferred to a 50.00-mL volumetric flask and diluted to the calibration mark. Determine the molarity of the resulting solution.
- A quantitative analysis for ethanol, C2H6O, can be accomplished by a redox back titration.Ethanol is oxidized to acetic acid, C2H4O2, using excess dichromate, Cr2O72–, which is reduced toCr3+. The excess dichromate is titrated with Fe2+, giving Cr3+ and Fe3+ as products. In a typicalanalysis, a 5.00-mL sample of a brandy is diluted to 500 mL in a volumetric flask. A 10.00-mLsample is taken and the ethanol is removed by distillation and collected in 50.00 mL of anacidified solution of 0.0200 M K2Cr2O7. A back titration of the unreacted Cr2O72–requires 21.48mL of 0.1014 M Fe2+. Calculate the %w/v ethanol in the brandyA student carried out an experiment trying to prepare tetra-methyl-ammonium tri-iodide.The student weighed 1.13 g tetra-methyl-ammonium iodide into a beaker containing 25 mL ethanol, and then added 1.57 g of iodine. The mixture was heated gently, whilst stirring, on a hotplate until tetra-methyl-ammonium iodide, a white powder, was completely dissolved. After the mixture was allowed to cool down to room temperature, the mixture was further cooled on ice. After filtration on a Buechner funnel, washing with diethyl ether and leaving it under vacuum suction for a couple of minutes, the student recovered the product and weighed it. The mass of the obtained tetra-methyl-ammonium triiodide was 1.62 g.What is the yield of the reaction in percent [%]? For the calculation, assume that the product is completely dry and pure, so there are no impurities like side-products, unreacted educts, or solvent residues.Zinc and magnesium react with hydrochloric acid to produce the metal chlorides and hydrogen gas. A 10.00 gram smaple of a mixture of Zn and Mg was with the stoichiometric quanitity of HCl. The reaction mixture was then reacted with 156 mL of 3.00M silver nitrate to produce the maximum quantity of silver chloride. First determine the % magnesium in the mixture- then, if 76.0 mL of HCl was added, what was the molarity of the HCl?
- The aluminum in a 1.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysis in terms of %NH4Al(So4)2 %Al2O3 %Al25.0mL of a 0.515 M K2S solution is mixed with 30.0 mL of 0.833 M HNO3 acid solution to give the following reaction: K2S(aq) + 2HNO3(aq) → 2KNO3(aq) + H2S(g) H2S is an unwanted by-product in a pulp and paper industry. To capture H2S gas, it is bubbled through a NaOH solution to produce Na2S with a yield of 94%. H2S(g) + 2NaOH (aq) → Na2S (aq) + 2H2O(l) The mass of H2S(g) that was processed (in kg) if 10.76 kg of Na2S was collected isCalculate the limiting and excess reagent of 3I2 + 6KOH → 5KI + KIO3 + 3H2O with solutions. 950g=I2, 1500g=KOH
