1. The total mass of water in each sample equals the mass of ice plus the mass of water added from the graduated cylinder. Determine this total mass from data in Table 10.4. Record the total mass of the water sample in Table 10.5 2 Calculate and record the mass of the sodium chloride solute sample used 3. One mole of sodium chloride weighs 58.5 g. Use this value and the sodium chloride sample mass to calculate the number of moles of sodium chloride in the sample (Equation 10.4). Record the result in Table 10.5 1 mol NaCI 585g Naci (Eq. 10.4) moles NaCl mass NaCl x
1. The total mass of water in each sample equals the mass of ice plus the mass of water added from the graduated cylinder. Determine this total mass from data in Table 10.4. Record the total mass of the water sample in Table 10.5 2 Calculate and record the mass of the sodium chloride solute sample used 3. One mole of sodium chloride weighs 58.5 g. Use this value and the sodium chloride sample mass to calculate the number of moles of sodium chloride in the sample (Equation 10.4). Record the result in Table 10.5 1 mol NaCI 585g Naci (Eq. 10.4) moles NaCl mass NaCl x
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter15: Solutions
Section: Chapter Questions
Problem 55A
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Table 10.4 (data) | ||
B. Freezing-Point Depression | Sodium Chloride Solute | Ethylene Glycol Solute |
Mass of beaker + ice + water | 111.438 g | 112.337 g |
Freezing point of pure wate | 58.650 g | 53.263 g |
Mass of sample + container | 0 C | 0 C |
Mass of empty container | 7.686 g | 33.185 g |
Freezing point of solution | 2.676 g | 28.524 g |
Table 10.5 (report) | Sodium Chloride Solute | Ethylene Glycol Solute |
Total water mass | ||
Mass of solute | ||
Moles of solute | ||
?t f | ||
Water mass in kg | ||
Solution molality | ||
K f |
Use Equation to complete table 10.5 from the attached picture.
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