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9. One source of error in this lab is the use of the ideal number 2 for i. The actual number is actually slightly less. Why might this be? If the number is slightly less, would your calculation for the molar mass be too high or too low based compared to using the number 2. Make sure you carefully explain your answer.

9. One source of error in this lab is the use of the ideal number 2 for i. The actual number is actually slightly less. Why might this be? If the number is slightly less, would your calculation for the molar mass be too high or too low based compared to using the number 2. Make sure you carefully explain your answer.

Chemistry
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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question 9 please!

8. The boiling point elevation can be calculated using the equation AT =K, x m xi, where AT is the change in boiling point, i is the number of ions in the solution per mole of dissolved Nacl (i = 2), m is the molality of the solution, and K, is the molal boiling point constant for water which is 0.51C/m. Using this equation and the data recorded in the data table, calculate the molar mass for NaCl and compare it with the actual value. Make sure to show a stepwise detailed calculation of how you get this number. AT =Kb x m x I Kb= 0.51C/m m= .6963 m I=2 0.51 x .6963 x 2 = .710°C 100 °C + .71 = 100.71 °C Therefore, the boiling point once elevated is 100.71 °C when elevated. And the boiling point is lower than the boiling point of the solution in the experiment. 9. One source of error in this lab is the use of the ideal number 2 for i. The actual number is actually slightly less. Why might this be? If the number is slightly less, would your calculation for the molar mass be too high or too low based compared to using the number 2. Make sure you carefully explain your answer.
Transcribed Image Text:8. The boiling point elevation can be calculated using the equation AT =K, x m xi, where AT is the change in boiling point, i is the number of ions in the solution per mole of dissolved Nacl (i = 2), m is the molality of the solution, and K, is the molal boiling point constant for water which is 0.51C/m. Using this equation and the data recorded in the data table, calculate the molar mass for NaCl and compare it with the actual value. Make sure to show a stepwise detailed calculation of how you get this number. AT =Kb x m x I Kb= 0.51C/m m= .6963 m I=2 0.51 x .6963 x 2 = .710°C 100 °C + .71 = 100.71 °C Therefore, the boiling point once elevated is 100.71 °C when elevated. And the boiling point is lower than the boiling point of the solution in the experiment. 9. One source of error in this lab is the use of the ideal number 2 for i. The actual number is actually slightly less. Why might this be? If the number is slightly less, would your calculation for the molar mass be too high or too low based compared to using the number 2. Make sure you carefully explain your answer.
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