QUESTION 1The actual freezing point of dodecanol is 23.9°C, and its freezing point constant is 2.9°C/m. If 1.20 g of an unknown solid (non-electrolyte) are dissolved in15.2 gof dodecanol producing a solution that freezes at 20.2°C, what is the molar mass of the unknown solid?QUESTION 2Would the calculated molar mass be higher, lower, or the same as the actual molar mass of the compound if the unknown contained an insoluble impurity?lower because the change in temperature observed will be higherhigher because the change in temperature observed will be lowersame because there is no effecthigher because the change in temperature observed will be higherO lower because the change in temperature observed will be lower

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QUESTION 1 The actual freezing point of dodecanol is 23.9°C, and its freezing point constant is 2.9°C/m. If 1.20 g of an unknown solid (non-electrolyte) are dissolved in 15.2 g of dodecanol producing a solution that freezes at 20.2°C, what is the molar mass of the unknown solid?

QUESTION 1 The actual freezing point of dodecanol is 23.9°C, and its freezing point constant is 2.9°C/m. If 1.20 g of an unknown solid (non-electrolyte) are dissolved in 15.2 g of dodecanol producing a solution that freezes at 20.2°C, what is the molar mass of the unknown solid?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 127QRT

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

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