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8. A solution containing 1.00 g of an unknown nonelectrolyte liquid and 9.00 g water has a freezing point of -3.33 °C. The Kr= 1.86 °C/m for water. Calculate the molar mass of the unknown liquid in g/mol.

8. A solution containing 1.00 g of an unknown nonelectrolyte liquid and 9.00 g water has a freezing point of -3.33 °C. The Kr= 1.86 °C/m for water. Calculate the molar mass of the unknown liquid in g/mol.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
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 71GQ: An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25...
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Please explain 8. How can I find molar mass?

6. What mass of NaCl is dissolved in 200 g of water in a 0.100 m solution? the free2ing point of solution is lower than the true. This means that The ATF will we high and the molar mass Of solute would be loww. would the calculated molar mass of the solute have been too high or too low? Bxplam In having the T reezrng point of solution is lowerr than the tue. This means tha he Ale wl we high and the mofan ma ss of solute would be Tow. Freezing Point read incorrectly; that means that the 6. What mass of NaCl is dissolved in 200 g of water in a 0.100 m solution? %3D 258.449 x .02=1.1698 う58.44g 200g. Thg = 0.akg 0.akg mol = (aa)(.100) 1000g mol Mass of Nacl= 19 mol = o02 %3D Mass = moles × Molar mass %3D 1. Calculate the molalities of some commercial reagents from the following data: HCl(aq) 36.465 NH3(aq) 17.03 Formula weight (g/mol) Density of solution (g/mL) Weight % Molarity 1.19 0.90 37.2 28.0 12.1 14.8 M= mol Kg sofvent 8. A solution containing 1.00 g of an unknown nonelectrolyte liquid and 9.00 g water has a freezing point of -3.33 °C. The Kf= 1.86 °C/m for water. Calculate the molar mass of the unknown liquid in g/mol.
Transcribed Image Text:6. What mass of NaCl is dissolved in 200 g of water in a 0.100 m solution? the free2ing point of solution is lower than the true. This means that The ATF will we high and the molar mass Of solute would be loww. would the calculated molar mass of the solute have been too high or too low? Bxplam In having the T reezrng point of solution is lowerr than the tue. This means tha he Ale wl we high and the mofan ma ss of solute would be Tow. Freezing Point read incorrectly; that means that the 6. What mass of NaCl is dissolved in 200 g of water in a 0.100 m solution? %3D 258.449 x .02=1.1698 う58.44g 200g. Thg = 0.akg 0.akg mol = (aa)(.100) 1000g mol Mass of Nacl= 19 mol = o02 %3D Mass = moles × Molar mass %3D 1. Calculate the molalities of some commercial reagents from the following data: HCl(aq) 36.465 NH3(aq) 17.03 Formula weight (g/mol) Density of solution (g/mL) Weight % Molarity 1.19 0.90 37.2 28.0 12.1 14.8 M= mol Kg sofvent 8. A solution containing 1.00 g of an unknown nonelectrolyte liquid and 9.00 g water has a freezing point of -3.33 °C. The Kf= 1.86 °C/m for water. Calculate the molar mass of the unknown liquid in g/mol.
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