12. Recall that the freezing point is depressed by -1.86 °C per mole of solute per kg of water. Calculate the theoretical freezing point of the mixture you created.
12. Recall that the freezing point is depressed by -1.86 °C per mole of solute per kg of water. Calculate the theoretical freezing point of the mixture you created.
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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need help with #12
Transcribed Image Text:Imass of isopropanol (C3H§O).
C =12.011 amu x3=36.033 amu
H=1,008 annu x 8=8.064 amo
= 60.096glmol
O= 15,999 amu x 1=15.999 amu
9. Calculate the number of moles of isopropanol added to your ice solution. Pure
isopropanol is 16.64 M.
Molarity (o. of moles x I000)
volume of solution
no. of moles :(molaritysvol of sol.)/1000>C16.64 Mx 70 ml000
El.165 moles
10. Calculate the volume of water in your melted ice and isopropanol solution.
Volume after ice melted - volume of Isopropanol
70-50=(20ml
11. Calculate the mass of water in the solution. (Recall that 1.0 mL of pure water has a mass
of 1.0 g) Convert your answer to kg.
Volume of isopropanol:50 m!
Total volume of liquid in tumbler: 7oml
Volume of uwater = 70-50 ml=20ml
20.0ml-20.0g → 20.og
* 1 ha .02 ka
12. Recall that the freezing point is depressed by -1.86 °C per mole of solute per kg of water.
Calculate the theoretical freezing point of the mixture you created.
13. Compare the actual to the theoretical.
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