Data 1. Mass of empty flask 31.38 2. Description of extracted caffeine: Include physical state (solid, liquid, gas) and color. liquid and the COlor is browN. 3. Mass of flask containing caffeine 81.42 6. Calculations and Conclusions 4. Mass of caffeine extracted 0.04 40 mg 40 5. Actual amount of caffeine in coffee sample The coffee was prepared by the stockroom manager. According to the recipe used, the coffee had a caffeine concentration of 1 mg/mL. Calculate the actual amount of caffeine in the coffee mg sample you used for the extraction. Show work here:

Data 1. Mass of empty flask 31.38 2. Description of extracted caffeine: Include physical state (solid, liquid, gas) and color. liquid and the COlor is browN. 3. Mass of flask containing caffeine 81.42 6. Calculations and Conclusions 4. Mass of caffeine extracted 0.04 40 mg 40 5. Actual amount of caffeine in coffee sample The coffee was prepared by the stockroom manager. According to the recipe used, the coffee had a caffeine concentration of 1 mg/mL. Calculate the actual amount of caffeine in the coffee mg sample you used for the extraction. Show work here:

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.11QAP

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A 1.59g sample containning KI was analyzed gravimetrically and .0538g of barium iodate was recovered. Express the results of this analysis as percent potassium iodide.
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.
An experiment was performed to look at how density changes when t he ratio of water and ethanol was changed. The following data was obtained: % Mass Ethano1.00 2.50 3.50 4.00 6.00 7.50 9.50 Density, g/mL0.9963 0.9936 0.9918 0.9910 0.9878 0.9855 0.9826 Use Excel or a similar spreadsheet program to plot these six data points and answer the following questions . a.What is the independent variable? b.What is the dependent variable? c.What is the equation of the best-‐fit line? d.What is the value of the coefficient of determination? e. According to the best-‐fit line, what should the density of pure water be (i.e. what is the density when % mass ethanol = 0.00)?
The mass of a beaker is 5.333 g. After 5.00 mL of a concentrated hydrochloric acid solution is pipetted into the beaker, the combined mass of the beaker and the hydrochloric acid sample is 11.229 g. From the data, what is the measured density of the hydrochloric acid solution?
The mass of a beaker is 8.342 grams. After 3.00 mL of an organic liquid is pipetted into the beaker, the combined mass of the beaker and the organic liquid is 10.697 grams. From the data, what is the measured density of the organic liquid ?
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.
Convert 450 m2/kg into cm2/g. Need detailed explanation for solution.
Given the following data for Mass of test tube and stearic acid = 14.17 gMass of test tube = 11.40 gFreezing point of strearic acid = 69.59o CMass of weighing paper + naphthalene =1.230 gMass of weighing paper = 0.920 gFreezing point solution = 64.00o CKf = 4.5o C/m Determine the following1. mass of stearic acid in g (2 decimal places); 2.77g2. mass of naphthalene in g (2 decimal places); 0.31g3. freezing point depression (2 decimal places); 3.93oC4. molality of solution (3 significant figures); _____5. moles of naphthalene (3 significant figures); _____6. molar mass of naphthalene, experimentally (3 significant figures); _____7. % error if theoretical molar mass of naphthalene is 128.17 g/ mole, USE ABSOLUTE VALUE (3 significant figure); _____
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he Don Juan Pond in Antarctica has one of the highest salt concentrations of any natural body of water on Earth. Even though it is in one of the coldest places on the planet, it almost never freezes due to this high salt content. The density of the pond water averages 1.3 g/mL. a.) Calculate the mass (in grams) of 1 gallon of water from the Don Juan Pond. b.) The dissolved salts are dominated by calcium chloride and the pond water is 44% salt by mass. What is the mass (in grams) of the salt in 1 gallon of the pond water? c.) If the salt is all CaCl2, what would be the molarity of the pond water?
The mass is 82.03g show work using dimensional analysis
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