Which of the following is a proper practice in transferring a certain volume of a liquid reagent from its reagent bottle to your own container? * Hold the reagent bottle in such a way that the palm of your hand covers the label of the reagent bottle. Use a clean and dry pipet or a graduated cylinder to measure the right amount of volume you need, then proceed to transfer the liquid to your container. If the reagent bottle comes with a dropper, use the dropper to get the right amount of liquid you need while making sure that after using the dropper, it is then placed directly at the back of the bottle. all choices are correct

Which of the following is a proper practice in transferring a certain volume of a liquid reagent from its reagent bottle to your own container? * Hold the reagent bottle in such a way that the palm of your hand covers the label of the reagent bottle. Use a clean and dry pipet or a graduated cylinder to measure the right amount of volume you need, then proceed to transfer the liquid to your container. If the reagent bottle comes with a dropper, use the dropper to get the right amount of liquid you need while making sure that after using the dropper, it is then placed directly at the back of the bottle. all choices are correct

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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drc%3D0&gi=24758088ctgl=18dnb 06 What is the molarity of a solution prepared by dissolving 213.6 grams of Fe(OH)3 in enough water to produce a total volume of 1.5 L? Round your answer to 1 decimal place. Your Answer: Answer units D Add attachments to support your work
DATA: Mass of potassium nitrate mass of test tube and potassium nitrate mass of test tube mass of potassium nitrate Volume of water taken Buret readings: Final gaml Initial Volume 4.97 added Temperature at which crystals appear Total volume of water in tube ML 1st addition 2nd addition 7.09ml 12.1ml 2.12 mal 7.09 ml 12.1ml 53.85839 43.9740g 9.9131 water. Record all data in the 4.97 9.98 15.78 4.97 9.98 3rd addition 17.9 ml 21.1ml 78.8 Temperature of water when volume is measured Density of water at when volume is measured (from reference) 0.970 Trial | || 52.0 39.1 21.4°C 15,18 4th addition 18.98 17.9ml ||| 28.2 18.98 IV 2
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Below is a picture of a 10-fold dilution series. What is the dilution factor of tube # 3? Write as both a fraction and scientific notation. i mL EC 9 mL 9 mL 9 mL HIO 9 mL ecterial Sampie TLbe #1 Tube e2 Tube #3 Tube #4
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Data obtained: Chips # of extractions Chips' weight (g) Fat weight (g) Regular 3 20.043 6.745 3 20.187 6.438 3 20.198 7.451 Low fat 3 19.456 3.982 3 20.072 4.547 3 20.192 4.589 Mass percent is a method of expressing the concentration of a substance in a mixture or element in a compound. It is calculated as the mass of the component divided by the total mass of the mixture and then multiplied by 100 to get the percent. The formula is: mass % of component= (mass of component / total mass) x 100% 1) Reproduce the following table, and use the data to determine the mass % of fat in the chips for each trial. 2) Show one example calculation. Chips Trial % by mass of fat Regular 1 2 3 Lowfat 1 2 3
Q) A student misreads the directions and adds 4.0 g of benzoic acid instead of 0.4 g. What do you expect to happen? Would the experiment still be valid? Explain your reasoning. Pure Lauric Acid Lauric Acid + 0.4 g Benzoic Acid Lauric Acid + 0.5 g Benzoic Acid Mass of Lauric Acid 3.03g 3.00g 3.00g Mass of Benzoic Acid 0 g 0.40g 0.50g Freezing Point 43’C 39’C 38’C Freezing Point Depression * 4’C 5’C Molality of Benzoic Acid in Lauric Acid* 1.026 mol/kg 1.282 mol/kg Moles of Benzoic Acid * 0.003 moles 0.004 moles Experimental Molar Mass of Benzoic Acid * 133.3g/mol 125 g/mol Average Molar Mass * 129.15g/mol Percent Error * 5.75%
1. A student weighs an empty special round bottom flask and stopper. He finds the mass to be 56.972 g. He then adds about 5 mL of an unknown liquid and heats the flask in a boiling water bath at 100°C. He allows all the liquid to vaporized and then removes the flask from the bath, stoppers it, and lets it cool. Upon cooling, he briefly removes the stopper, then replaces it and weighs the flask and condensed vapor, obtaining a mass of 57.917 g. The volume of the flask is known to be 240.2 mL. The barometric pressure in the laboratory that day is 743 mm Hg. What was the pressure of the vapor in the flask in atm? O 0.9776 atm 0.98 atm 0.978 atm 0.977 atm
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Assume that the mass of impure acetanilide is 1.748 g. and the mass of recrystallized acetanilide is 1.272 g. Calculate the percent recovery. Calculate your answer to 2 decimal places. Remember the units!
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