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- The concentration of ammonia (17.031 g/mol) can be determined through back titration. After addition of 10.00 mmol of HCI into a sample of NH, solution, back-titration with Na.CO, revealed that 5.00 mmol of HCI remained. What would be the concentration in %w/v of ammonia if the 10.00 mL of the sample was analyzed?

- The concentration of ammonia (17.031 g/mol) can be determined through back titration. After addition of 10.00 mmol of HCI into a sample of NH, solution, back-titration with Na.CO, revealed that 5.00 mmol of HCI remained. What would be the concentration in %w/v of ammonia if the 10.00 mL of the sample was analyzed?

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ISBN:9781305957404
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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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A. The concentration of ammonia (17.031 g/mol) can be determined through back titration. After addition of 10.00 mmol of HCl into a sample of NH3 solution, back-titration with Na.CO. revealed that 5.00 mmol of HCl remained. What would be the concentration in %w/v of ammonia if the 10.00 mL of the sample was analyzed? B. In order for all of the analyte to be consumed completely, an excess of a reagent has to be added. If 10.00 mL of a 0.1000 M HCI is needed in the back titration, what volume of a 0.5000 M NaOH should be added to a sample that contains 2.000 mmol of aspirin?
Transcribed Image Text:A. The concentration of ammonia (17.031 g/mol) can be determined through back titration. After addition of 10.00 mmol of HCl into a sample of NH3 solution, back-titration with Na.CO. revealed that 5.00 mmol of HCl remained. What would be the concentration in %w/v of ammonia if the 10.00 mL of the sample was analyzed? B. In order for all of the analyte to be consumed completely, an excess of a reagent has to be added. If 10.00 mL of a 0.1000 M HCI is needed in the back titration, what volume of a 0.5000 M NaOH should be added to a sample that contains 2.000 mmol of aspirin?
1. True of False: During back titration of aspirin, a more dilute than usual NaOH solution was used, while back-titration of the unreacted base and the rest of the experiment followed the usual procedure. Under this condition, the calculated amount of analyte will be higher expected because the amount of aspirin consumed by NaOH will be lower. 2. Identify two among the following situations that can most likely be the cause. In an experiment to determine the content of acetylsalicylic acid in an aspirin tablet, the result showed that the calculated mass of acetylsalicylic acid was much higher than the indicated amount in the packaging. Choices: a. Aspirin was not completely hydrolyzed. b. Tablet contained other acids that can be neutralized by a base. c. Molar mass of salicylic acid was used instead of acetylsalicylic in the calculations. d. Mass of the tablet recorded included the packaging. e. After grinding, some of the pulverized tablet was not transferred to the flask. f. The unreacted base was over titrated during back titration.
Transcribed Image Text:1. True of False: During back titration of aspirin, a more dilute than usual NaOH solution was used, while back-titration of the unreacted base and the rest of the experiment followed the usual procedure. Under this condition, the calculated amount of analyte will be higher expected because the amount of aspirin consumed by NaOH will be lower. 2. Identify two among the following situations that can most likely be the cause. In an experiment to determine the content of acetylsalicylic acid in an aspirin tablet, the result showed that the calculated mass of acetylsalicylic acid was much higher than the indicated amount in the packaging. Choices: a. Aspirin was not completely hydrolyzed. b. Tablet contained other acids that can be neutralized by a base. c. Molar mass of salicylic acid was used instead of acetylsalicylic in the calculations. d. Mass of the tablet recorded included the packaging. e. After grinding, some of the pulverized tablet was not transferred to the flask. f. The unreacted base was over titrated during back titration.
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