MISSED THIS? Watch KCV Colligative Properties Read Section 14.6. You can click on the Review link to access the section in your e Text. An aqueous solution containing 36.7 g of an unknown molecular (non-electrolyte) compound in 141.6 g of water was found to have a freezing point of -1.2 °C. Calculate the molar mass of the unknown compound (Use Kf 1.86 °C/m) Express your answer using two significant figures. IVE ΑΣΦΑ M Submit = Request Answer ? g/mol

MISSED THIS? Watch KCV Colligative Properties Read Section 14.6. You can click on the Review link to access the section in your e Text. An aqueous solution containing 36.7 g of an unknown molecular (non-electrolyte) compound in 141.6 g of water was found to have a freezing point of -1.2 °C. Calculate the molar mass of the unknown compound (Use Kf 1.86 °C/m) Express your answer using two significant figures. IVE ΑΣΦΑ M Submit = Request Answer ? g/mol

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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If 11.2 g of naphthalene, C 10H 8 (Molar mass= 128 g/mol), is dissolved in 107.8 g of chloroform, CHCI 3 (Molar mass = 118 g/mol), what is the molality of the solution? 0.0875 m 12.4 m 0.811 m 0.0941 m 0.0969 m
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When 4.18 g of a certain molecular compound X are dissolved in 45.0 g of benzene (C6H6), the freezing point of the solution is measured to be 4.9 °C. Calculate the molar mass of X. If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. □□ 品 5
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1. Suppose that you add 27.5 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 oC/m. With the added solute, you find that there is a freezing point depression of 3.58 oC compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound? 2. What is the freezing point (in degrees Celcius) of 3.70 kg of water if it contains 187.4 g of CaBr2? The freezing point depression constant for water is 1.86 oC/m and the molar mass of CaBr2 is 199.89 g/mol. 3. What mass, in grams, of NaCl needs to be added to 1.6 kg of water in order to create a solution with a freezing point of -5.6 °C? The freezing point depression constant of water is 1.86 ºC/m.
Suppose a group of students tell you that they added solid sodium chloride NaCls to 35 mL of deionized water and they did not record how many grams of NaCl they added but they got a freezing point depression of 1.25°C. Calculate how many grams of NaCl the students added. The pure freezing point of water is 0.00°C and the freezing point depression constant (K) of water is 1.858 °C/m. Remember that NaCl is a solid salt and an ionic compound therefore it contributes a negligible amount to the overall additive volume and keep track of its van't Hoff factor. The density of water at 20°C is 0.9982 g/mL.