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- Discuss three practical applications of solvent extraction in analytical chemistry.An impure sample of calcium carbonate with a mass of 7.95 g was reacted with 50.00 cm3 of 1.00 mol dm hydrochloric acid (an excess). The resulling solution was transferred to a volumetric flask and titrated with 11.10cm3 of 0.300 mol dm-3 sodium hydroxide solution. Determine the percentage purity by mass of the calcium carbonate sample.CaCO3 + HCl -> CaCl2 + H2O + CO2 HCl + NaOH -> NaCl +H2O a. Determine how many moles of hydrochloric acid were used.b. Determine how many moles of excess HCI was titratedc. Determine how much in moles calcium carbonate present in the sample.d. Calculate the mass of calcium carbonate presente. Determine the percentwge calcium carbonate is in the sample.Provide a complete and detailed separation scheme for the following compounds, you have the following chemicals: 1.0M NaOH, 1.0M HCl, THF, H2O. Consider you have any standard glassware and a separatory funnel.
- 1. The surface of silica gel has a structure shown in the diagram below : OH OH OH -0- Si- 0 Si Si – 0- main body of silica structure Suppose you used a plate coated with silica gel, with propanone, CH;COCH;, as the solvent for thin layer chromatography. Suppose also that the mixture you were trying to identify contained A compound, P, which could form strong hydrogen bonds. A compound, Q, which formed hydrogen bonds, but not as strongly as P. A compound, R, which was polar, relying on dispersion forces and dipole-dipole interactions for its intermolecular attractions. Describe and explain what the chromatogram would probably look like.What is precipitation from homogeneous solution; what are the benefits of this method.Describe liquid-liquid extraction. Provide at least one application for liquid-liquid extraction in industry
- In an experiment to determine the concentration of H2SO4 in a brand of toilet cleanser, 10.0 cm3 of the cleanser was first diluted to 250.0 cm3 with distilled water. 25.0 cm3 of the diluted cleanser were titrated with 0.320 mol dm–3 NaOH solution, using methyl orange as indicator.If 29.2 cm3 of NaOH solution is used, what is the concentration of H2SO4 in the undiluted toilet cleanser?a. 2.30 mol dm–3b. 4.60 mol dm–3 c. 9.20 mol dm–3 d. 11.50 mol dm–3(a) In 20 or less of yourown words define the term “leachate”and describe how it forms. (b) Previous records had shown that to prevent acute toxicity to organisms, the maximum mass of CdSO4 that should be allowed into the landfill was determined to be 0.1 kg. This was calculated using a standard concentration of Cd in mg/L where the volume of the leachate pond was used as 500 000L. (i) Provide the name of the CdSO4 compound. State the oxidation number of Cd in this compound (ii) You need to ensure that the concentration used to determine the mass of Cd allowed in the landfill, meets the current regulatory standard. Assuming that previous calculations determined that all of the CdSO4 would be deposited in the leachate pond, what standard concentration of Cd in mg/L was used to determine the maximum mass of allowable CdSO4?Chemistry A young adult (60 kg body weight) drinks two beers of 12 oz. each, over a period of 10 minutes. Assuming instantaneous dilution of alcohol in the total body water after finishing the beers, (Alcohol content in beer is 6 %; density of alcohol is 0.9 g /mL.; 1 oz. = 30 mL.; 80% proof = 40% v/v alcohol; elimination rate is about 10 mL/hour (zero order) (b) one hour after drinking the beers. Assuming that the plasma level of 100 mg /dL is the index of intoxication, was legally drunk this person?
- Caustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?(b) Suppose the laboratory Technician carried out the same titration experiment in which he/she recorded an average volume of 20 cm³ of the dilute hydrochloric acid (HC) by titrating with 0.05 mol dm³ and 25 cm³ of potassium hydroxide (KOH). Calculate the concentration of hydrochloric acid from the Technician's experiment.3. A sealed glass vial is prepared with 4 mL of air and 36 mL of water. Trichloroethylene (TCE) is added to the water to create an initial aqueous phase concentration of 100 ppb (a) (b) After the system equilibrates, what will the concentration of TCE be in the aqueous phase (in µg/L)? Determine the % mass partitioning of TCE between the water and the air when equilibrium is established. (c) If a quantity of TCE is accidentally spilled into a well-mixed river, where would you expect most of the TCE to end up in the short term - in the air or in the water? Explain.