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I need to figure out how to calculate the molar mass of this unknown acid by titration , and give some errors why the ideal molar mass was not obtained? Mass of acid used: 2.4060 grams Buret initial volume : 0.00mL End volume of buret: 99.4 mL [NaOH]=0.1501M unknown #122 : molar mass 152.15 g.mol for error analysis

I need to figure out how to calculate the molar mass of this unknown acid by titration , and give some errors why the ideal molar mass was not obtained? Mass of acid used: 2.4060 grams Buret initial volume : 0.00mL End volume of buret: 99.4 mL [NaOH]=0.1501M unknown #122 : molar mass 152.15 g.mol for error analysis

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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I need to figure out how to calculate the molar mass of this unknown acid by titration , and give some errors why the ideal molar mass was not obtained?

Mass of acid used: 2.4060 grams

Buret initial volume : 0.00mL

End volume of buret: 99.4 mL

[NaOH]=0.1501M

unknown #122 : molar mass 152.15 g.mol for error analysis

Experiment 1 Part B, Molar Mass of an Unknown Acid 1. Weigh a weighing boat and record its mass. Your unknown acid is in plastic sample bag. Write your description of the sample including unknown number in your notebook. Your instructor will direct you to the mass of the unknown acid that you need to weigh within +/- 0.005 grams of the sample size. Transfer sample to 250 mL Erlenmeyer flask. Add about 50 mL of deionized water and 2-3 drops of phenolphthalein to the sample in the flask. The acid may be relatively insoluble, so don't worry if it doesn't all dissolve at first. 0.4M 2. Fill the buret with the previously standardized sodium hydroxide solution (make sure you note the concentration and write it in your notebook for use in the calculations section of your report) and record the level of the liquid in the buret to 0.01 mL. C. 3. Titrate the acid to the end point. As the acid is neutralized by the base, it will tend to dissolve in the solution. If your unknown is so insoluble that the phenolphthalein color persists before all the solid dissolves, add about 25 mL of ethanol to the solution to increase the solubility. [This procedure does not affect the results of the titration, only insures that all the unknown solid acid is dissolved in the solution where it can react with the sodium hydroxide.] Then continue the titration. Record the volume of liquid in the buret at the end point. 4. Prepare a second sample of your unknown and titrate as before.o du Note: Waste instructions will be given by your instructor 0.17
Transcribed Image Text:Experiment 1 Part B, Molar Mass of an Unknown Acid 1. Weigh a weighing boat and record its mass. Your unknown acid is in plastic sample bag. Write your description of the sample including unknown number in your notebook. Your instructor will direct you to the mass of the unknown acid that you need to weigh within +/- 0.005 grams of the sample size. Transfer sample to 250 mL Erlenmeyer flask. Add about 50 mL of deionized water and 2-3 drops of phenolphthalein to the sample in the flask. The acid may be relatively insoluble, so don't worry if it doesn't all dissolve at first. 0.4M 2. Fill the buret with the previously standardized sodium hydroxide solution (make sure you note the concentration and write it in your notebook for use in the calculations section of your report) and record the level of the liquid in the buret to 0.01 mL. C. 3. Titrate the acid to the end point. As the acid is neutralized by the base, it will tend to dissolve in the solution. If your unknown is so insoluble that the phenolphthalein color persists before all the solid dissolves, add about 25 mL of ethanol to the solution to increase the solubility. [This procedure does not affect the results of the titration, only insures that all the unknown solid acid is dissolved in the solution where it can react with the sodium hydroxide.] Then continue the titration. Record the volume of liquid in the buret at the end point. 4. Prepare a second sample of your unknown and titrate as before.o du Note: Waste instructions will be given by your instructor 0.17
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