1. A given grain sample was found to contain 8.65 percent moisture. A 5.2146 g as received sample was placed into a crucible (28.5033 g, tare). The ashed crucible weighed 28.5939 g. Calculate the percent ash on: a) as-received (net-weight basis)
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Kindly answer both with complete solutions. Thank you! Pls skip if unsure or not willing to answer both since online references were not accurate.
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- Given the following data forMass of test tube, beaker and cyclohexane = 100.17 gMass of test tube and beaker = 84.07 gFreezing point of cyclohexane = 6.59 oCMass of weighing paper + naphthalene =1.080 gMass of weighing paper = 0.928 gFreezing point solution = 5.11oCKf = 20.8oC/mDetermine the followinga. mass of cyclohexane in g (2 decimal places); _____b. mass of naphthalene in g (4 decimal places); _____c. freezing point depression (2 decimal places); _____d. molality of solution (3 significant figures); _____e. moles of naphthalene (3 significant figures); _____f. molar mass of naphthalene, experimentally (3 significant figures); _____g. % error if theoretical molar mass of naphthalene is 128.17 g/ mole, USE ABSOLUTE VALUE (3 significant figure); ____using exactly 5.00 mL of 0.0400 M stock CuSO4 solution. Add 100 mL of water. Data for Part IMass of empty dish: 32.470 g empty dishVolume of 0.0400 M solution: 5.00 mL CuSO4 solution.Mass of dish and 0.0400 M solution: 37.497 g dish and solutionMass of dish and CuSO4 solid: 32.503 g dish and CuSO4 solidCalculations for Part I1. Calculate the mass of solution? 5.027 g 2. Calculate the mass of solid CuSO4 dissolved in the solution? 0.033 g 3. Calculate the number of moles of solid CuSO4 dissolved in the solution? 2.07 x 10-4 mol4. Calculate the mass of water evaporated from the solution? 0.0414 M5. Calculate the density of solution, (g solution/mL solution)?6. Calculate the % by mass, CuSO4 in solution (100 x g CuSO4/g solution)?7. Calculate the molality of solution (moles CuSO4/kg solvent)?8. Calculate the molarity of solution (moles CuSO4/L solution)?9. Given that the true molarity is 0.0400 M, calculate the percent error…using exactly 5.00 mL of 0.0400 M stock CuSO4 solution. Add 100 mL of water. Data for Part IMass of empty dish: 32.470 g empty dishVolume of 0.0400 M solution: 5.00 mL CuSO4 solution.Mass of dish and 0.0400 M solution: 37.497 g dish and solutionMass of dish and CuSO4 solid: 32.503 g dish and CuSO4 solidCalculations for Part I1. Calculate the mass of solution2. Calculate the mass of solid CuSO4 dissolved in the solution.3. Calculate the number of moles of solid CuSO4 dissolved in the solution.4. Calculate the mass of water evaporated from the solution.5. Calculate the density of solution, (g solution/mL solution).6. Calculate the % by mass, CuSO4 in solution (100 x g CuSO4/g solution).7. Calculate the molality of solution (moles CuSO4/kg solvent).8. Calculate the molarity of solution (moles CuSO4/L solution).9. Given that the true molarity is 0.0400 M, calculate the percent error of your result.
- A beaker containing the sample was weighed using the analytical balance and obtained a weight of 15.4g. What is the actul weight of the sample, if the weight of the empty beaker was recorded at 9.4g?Medicare does not cover the cost of this prescription medicine, which currently averages $297.78 per kilogram. The theoretical yield for the pure barium sulfate you were transferring was 500.00kg. You spilled 27.45 kg. What is the % yield of the transfer that you need to report? And also determine the consumer price of the spilled barium sulfate.Calculate the suspended solids in mg/L given the following data: Weight of crucible: 21.0256 g, Weight of crucible and dry solids: 21.0301 g, Weight of crucible and ash: 21.0263 g, and Volume of sample filtered: 50 mL. Answer should have 2 significant figures.
- Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.The mass of preheated crucible with cover was 12.1125 g. After the hydrate sample was added, the weight increased to 13.1533 g. After heating the crucible for three times in order to remove hydrate water and bring it to the constant weight the lowest of the three mass measurements was 12.9971 g. 1)What is the mass percent of water in the hydrate? Please report your answer with the correct number of significant figures but without "%" (Canvas will not let you to enter units in this problem). 2) What is the theoretical mass % of water in the hydrate if the salt is BaCl2 x 2H2O? Make sure you use enough significant figures for the atomic weights of the elements and round your answer to 3 decimals. 3) What is the mass of the hydrate placed in the crucible? 4) What is the mass of the anhydrous salt?-If ethanol (S.G. = 0.790) were used rather than water in measuring the density of the irregular objects, how would that have affected the result? Explain. -When you were measuring the volume of the irregular solid you were told to stir to eliminate bubbles. If the bubbles were not eliminated, how would that affect the density? Explain. -Suppose the density of 65.0 mL of some liquid was found to be 0.748 g/mL. What would be the specific gravity of 45.0 mL of this liquid?
- A student decided to undertake a balance calibration exercise during a lab session involving burette calibration. He found the apparent weight of calcium carbonate in air to be 100 grams and density to be 1.33g/mL. Assume that the standard steel weight used in the calibration has a density of 8.0g/mL and air has a density of 0.0012g/mL. What would be the true mass of the calcium carbonate sample?A method to determine an antibiotic was developed and validated in a pharmaceutical company. The method allows analysis of 100 mg tablets containing 7.5 mg of the antibiotic. According to the validation data, the confidence limits are 7.50 mg± 0.04mg. How many samples will need to be analyzed for an analyst to ensure that the content of the antibiotic in a macerated sample of that drug is 7.50 mg ± 0.03 mg with 95% reliability when analyzing 100 mg of the macerated sample?The mass is 82.03g show work using dimensional analysis