Hello I am stuck in my laboratory, I already did the whole procedure, I am in the last step (# 9) but I can't understand that I have what data I have to put in the test data (Theoretical solubility of NaCl, Temperature, Source) could you explain that data I must put, here is all my lab Thank you very much. Test Data: Mass of empty 250-mL beaker: 100.7 gMass of 250-mL beaker and saturated NaCl solution :106.4 gTemperature of saturated NaCl solution: 24.1°CMass of 250-mL beaker and NaCl residue (1st weighing): 102.7 gMass of 250-mL beaker and NaCl residue (2nd weighing): 102.2 gMass of 250 mL beaker and NaCl residue (3rd weighing): 101.9 g (Use the lowest mass for calculations)This part 7.Theoretical solubility of NaCl ?????(a)Temperature ??????(b)Source ???? Note: Wait until the beaker has cooled to room temperature beforeweighing.Place the beaker with the NaCl residue on the trivet or hot pad and allowit to cool to room temperature. Determine its mass and record it in thetest data section of the lab report. Heat the beaker again for a fewminutes. Repeat the process of allowing it to cool to room temperature,determining its mass, and recording its mass. Repeat the process a thirdtime if the masses are not constant.8.*Take a photo of the beaker with the NaCl residue and submit thelabeled picture with your lab report. Remember to follow theinstructions in the syllabus for submitting a photo.9.Look up the solubility of NaCl and find the value that corresponds to thetemperature of your saturated solution in step 3. Record this value andthe source where you obtained the solubility information in the test datasection of the lab report.Caleulations:

Answered: Hello I am stuck in my laboratory, I…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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Hello I am stuck in my laboratory, I already did the whole procedure, I am in the last step (# 9) but I can't understand that I have what data I have to put in the test data (Theoretical solubility of NaCl, Temperature, Source) could you explain that data I must put, here is all my lab Thank you very much.

Test Data:

Mass of empty 250-mL beaker: 100.7 g
Mass of 250-mL beaker and saturated NaCl solution :106.4 g
Temperature of saturated NaCl solution: 24.1°C
Mass of 250-mL beaker and NaCl residue (1^st weighing): 102.7 g
Mass of 250-mL beaker and NaCl residue (2^nd weighing): 102.2 g
Mass of 250 mL beaker and NaCl residue (3^rd weighing): 101.9 g

(Use the lowest mass for calculations)

This part

7.Theoretical solubility of NaCl ?????

(a)Temperature ??????

(b)Source ????

Note: Wait until the beaker has cooled to room temperature before
weighing.
Place the beaker with the NaCl residue on the trivet or hot pad and allow
it to cool to room temperature. Determine its mass and record it in the
test data section of the lab report. Heat the beaker again for a few
minutes. Repeat the process of allowing it to cool to room temperature,
determining its mass, and recording its mass. Repeat the process a third
time if the masses are not constant.
8.
*Take a photo of the beaker with the NaCl residue and submit the
labeled picture with your lab report. Remember to follow the
instructions in the syllabus for submitting a photo.
9.
Look up the solubility of NaCl and find the value that corresponds to the
temperature of your saturated solution in step 3. Record this value and
the source where you obtained the solubility information in the test data
section of the lab report.
Caleulations:

Expert Solution

Step 1

Given,

Mass of empty beaker is $100.7 g$

Mass of empty beaker and $NaCl$ solution is $106.4 g$

Calculate the mass of $NaCl$ solution as follows:

$\begin{array}{rcl} Mass of NaCl solution & = & mass of empty beaker and NaCl solution - mass of empty beaker \\ = & 106.4 g - 100.7 g \\ = & 5.7 g \end{array}$

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