The fat content of 10 g of commercial ice cream was determined by the Mojonnier method. The weights of the extracted fat after the second extraction and the third extraction were 1.30 and 1.36 g, respectively. How much of fat, as percentage of the total, was extracted during the third extraction?
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1)The fat content of 10 g of commercial ice cream was determined by the Mojonnier method. The weights of the extracted fat after the second extraction and the third extraction were 1.30 and 1.36 g, respectively. How much of fat, as percentage of the total, was extracted during the third extraction?
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- Weigh out accurately 9.99 g of copper(II) sulfate pentahydrate (CuSO4·5H2O) by taring using a clean and dry empty 250-ml beaker. 2. Add tap water to the beaker to reach the 50-mL mark on the side of the beaker. 3. Dissolve all the crystals of CuSO4·5H2O in the water using a clean glass rod for stirring. 4. Then using a glass funnel transfer all the blue solution to a 100-mL volumetric flask. Rinse the beaker with about 10 mL of water and transfer the solution to the volumetric flask. Repeat the rinsing of the beaker with another 10 mL of water and transfer the solution to the volumetric flask. This is called quantitative transfer of the solution. 5. Then add enough water to reach the calibration mark of the volumetric flask. (You will need to use a dropper to add the last few drops of water to ensure the meniscus is on the calibration mark). Close the volumetric flask with a stopper and mix the solution well (so that it is homogeneous). 6. You have now prepared a standard solution (or…3. Corev was synthesizing a chemical in the laboratory. He used different purification techniques to try to obtain a pure compound. The melting point of the pure compound is 65 degrees. When he tested his compound in the lab the melting point he obtained was 62-68 degrees. Is the product he synthesized pure? 4A company was low on copper metal and decided to use some chemical additives just this once to some copper wiring they were installing in a house. How will this impact the conductivity of the wiring?2. The goal behind suction filtration is to remove soluble impurities that are on the surface of the crystals. Therefore, why can't you simply use suction filtration instead of recrystallization to purify an impure solid?
- What are the types of gravimetric methods? Give an examples where each method is used in an analysis. What is particulate gravimetry? When do we use this technique?You were tasked to separate the components of a mixture containing silica, sodium chloride and charcoal. TNāCI dissolves in water while silica and charcoal are not water-soluble. Only charcoal dissolves in carbon disulfide. a. Write a short experimental procedure to carry out the separation of the mixture. b. Given the following data, determine the percentage of charcoal, sodium chloride and silica. Mass (g) Mass of beaker 100.000 Mass of beaker + mixture 110.000 mass of evaporating dish 62.000 mass of evaporating dish + solid after evaporation of water 65.000 Mass of beaker + charcoal + silica after evaporation of excess water 117.000 mass of beaker + silica after decanting dissolved charcoal and drying 113.545II. b) What is the difference between liquid-liquid, solid-liquid and solid-phase extraction? Complete the table below and sort the following examples in the correct column: Steeping tea, washing an organic phase (workup), brewing beer, chemical desalting of crude oil, activated carbon sugar decolorization. liquid-liquid solid-liquid solid-phase Phase that contains analyte before extraction? Phase that contains analyte after extraction? Example(s)
- what is the purpose of adding concentrated sulfuric acid to a product after distillation? Write the chemical equation to illustrate the role of sulfuric acid.a) Name the four main compositions of crude oil.b) Identify the process/reaction and draw the chemical structure for each below.i. ethene to polyetheneii. hexane to benzeneiii. octane to paraffin and olefiniv. heptane to 2,2 – dimethylpentaneA student prepared a compound. the melting point of the crude the product was 42 to 48 degree C. after purifying the solid for the first time, the melting point was 47 to 51 degree C. after another purification, the melting point was 50 to 53 degree C. at this stage, can the student confidently say the product has been completely purified? justify your answer
- 1. A stock solution of I2 is standardized using a 0.1430 g sample of pure ascorbic acid. The titration to the starch endpoint required 25.45 mL of the I2 solution. Calculate the molarity of the I2 solution. 2. A vitamin C tablet was divided into three equal mass portions. One portion was crushed into a fine powder, dissolved in water, and titrated with the standardized solution from question 2 (above). The titration to the endpoint required 27.60 mL of the I2 solution. Calculate the number of milligrams of vitamin C that are in the original tablet.Why is the percent recovery of the essential oil less than 100%? State at least two reasons that are inherent to the experiment as performed and are thus unavoidable.[4cde] c. Calculate for the mass of struvite that can be formed in the given urine sample. d. Given that the specific gravity of struvite is 1.7, determine if the amount of struvite in c can pass through the kidney. Note: less than 6mm diameter urolith can pass through the kidney. Assume that the urolith is spherically shaped. e. Using your answer in c, calculate for the number of phosphate ions in the sample.