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Based on the information I was able to solve and provide, may I get help on #25 (Compare the actual to the theoretical). Ignore #26

Based on the information I was able to solve and provide, may I get help on #25 (Compare the actual to the theoretical). Ignore #26

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter13: Solutions And Their Behavior
Section: Chapter Questions
Problem 107SCQ
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Based on the information I was able to solve and provide, may I get help on #25 (Compare the actual to the theoretical). Ignore #26
Name Donovan Snider Part III: Salt solution 14. Prepare another tumbler of ice with distilled water. 15. Weigh out 10-15 g table salt. Record the mass of salt 16. Add the table salt to the beaker of ice water. Stir with the thermometer until the salt has all dissolved, and the temperature has stabilized. This will take many minutes. Add more ice as needed, so that there is always ice in the solution. Record the lowest temperature obtained-1.9 11.5 g. °C 17. Adjust the temperature based on your thermometer calibration. -2.7 °C 18. Let all the ice melt. Measure the volume of solution to the nearest 0.1 mL. 70 mL 19. Write the chemical formula for table salt. NaCS lisu, vour 20. Calculate the molar mass of table salt. NaCI Na =22.990 x1:22.99O CI=35.45 x1=35.45 hn e The we 38.44 g/mol) 21. Calculate the moles of salt in the mass of table salt that you used. Molar mass of Nacl=58.44g/mol Mass of table Salt 1.5 a O.19678303 mol Molar mass of NaCI 58.449/mol 22. Calculate the moles of particles (recall that the salt dissociates into ions in solution, so the number of moles of particles is greater than the moles of salt.) NaCI > Na + CI >0,19678303 mol +0.19678303 mol =0.39356605 mol
Transcribed Image Text:Name Donovan Snider Part III: Salt solution 14. Prepare another tumbler of ice with distilled water. 15. Weigh out 10-15 g table salt. Record the mass of salt 16. Add the table salt to the beaker of ice water. Stir with the thermometer until the salt has all dissolved, and the temperature has stabilized. This will take many minutes. Add more ice as needed, so that there is always ice in the solution. Record the lowest temperature obtained-1.9 11.5 g. °C 17. Adjust the temperature based on your thermometer calibration. -2.7 °C 18. Let all the ice melt. Measure the volume of solution to the nearest 0.1 mL. 70 mL 19. Write the chemical formula for table salt. NaCS lisu, vour 20. Calculate the molar mass of table salt. NaCI Na =22.990 x1:22.99O CI=35.45 x1=35.45 hn e The we 38.44 g/mol) 21. Calculate the moles of salt in the mass of table salt that you used. Molar mass of Nacl=58.44g/mol Mass of table Salt 1.5 a O.19678303 mol Molar mass of NaCI 58.449/mol 22. Calculate the moles of particles (recall that the salt dissociates into ions in solution, so the number of moles of particles is greater than the moles of salt.) NaCI > Na + CI >0,19678303 mol +0.19678303 mol =0.39356605 mol
Name Oonovan Snider 23. Calculate the kg of water in your solution. T ģliml x 70 ml= 10 g 70g-11.5g:58.5g 58.5gx Ikg 0.0585 ka L000g 24. Calculate the theoretical freezing point for your salt solution. 1.86°C hg o.19678303 mol 0.0585 kg 0,.39356605 mol mol 0.19678303 mol 1.86 x 3.36*29412.5°c TrO°C- 12.5°C 25. Compare the actual to the theoretical. g point or the De freeing pnt of water for mofour histe sion. D vent di =-12.5°c stutions in life, such as to keep the reservoir dingold winter weat r car from freezing 26. Discuss the two experiments, using at least four sentences. At a minimum, your discussion should address the following questions: Did the measured temperature match the expected temperature for each solution? If not, were both solutions off by a similar amount, and were they both either over or under? Or was one over and the other under? Discuss at least two sources of error in this experiment. Be specific (human error is vague. A specific source of error might be that you spilled some of the salt while pouring it into the solution, so that the full mass did not get added.) Yo rg yr ow You don't t lto des poin A
Transcribed Image Text:Name Oonovan Snider 23. Calculate the kg of water in your solution. T ģliml x 70 ml= 10 g 70g-11.5g:58.5g 58.5gx Ikg 0.0585 ka L000g 24. Calculate the theoretical freezing point for your salt solution. 1.86°C hg o.19678303 mol 0.0585 kg 0,.39356605 mol mol 0.19678303 mol 1.86 x 3.36*29412.5°c TrO°C- 12.5°C 25. Compare the actual to the theoretical. g point or the De freeing pnt of water for mofour histe sion. D vent di =-12.5°c stutions in life, such as to keep the reservoir dingold winter weat r car from freezing 26. Discuss the two experiments, using at least four sentences. At a minimum, your discussion should address the following questions: Did the measured temperature match the expected temperature for each solution? If not, were both solutions off by a similar amount, and were they both either over or under? Or was one over and the other under? Discuss at least two sources of error in this experiment. Be specific (human error is vague. A specific source of error might be that you spilled some of the salt while pouring it into the solution, so that the full mass did not get added.) Yo rg yr ow You don't t lto des poin A
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