Boiling Point Elevation/Freezing Point DepressionAT = m KWhere:AT = T(solution) - T(pure solvent) *m = (# moles solute / Kg solvent)Kb = boiling point elevation constant.Kf = freezing point depression constant.K₁ and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations thatfollow.SolventWaterEthanolChloroformBenzeneDiethyl etherFormulaH₂OCH3CH₂OHCHCI 3C6H6CH3CH₂CH₂CH3Kb (°C/ m) Kf (°C / m)0.5121.223.672.532.02-1.86-1.99-5.12*Please note that AT as defined above will be a negative number for freezing point depression. Therefore, Kf must alsobe given as a negative number. The freezing point of ethanol CH3CH₂OH is -117.30°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves inethanol is chlorophyll.If 13.92 grams of chlorophyll, C55H72MgN405 (893.5 g/mol), are dissolved in 186.9 grams of ethanol …..The molality of the solution isThe freezing point of the solution ism.°C.

Given mass of chlorophyll = 13.92 g Molar mass of chlorophyll = 893.5 g/mol Mass of ethanol =…

The freezing point of ethanol CH3CH₂OH is -117.30°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is chlorophyll. If 13.92 grams of chlorophyll, C55H72MgN4O5 (893.5 g/mol), are dissolved in 186.9 grams of ethanol ... The molality of the solution is The freezing point of the solution is m. °C.

The freezing point of ethanol CH3CH₂OH is -117.30°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is chlorophyll. If 13.92 grams of chlorophyll, C55H72MgN4O5 (893.5 g/mol), are dissolved in 186.9 grams of ethanol ... The molality of the solution is The freezing point of the solution is m. °C.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 74AP

See similar textbooks

Similar questions

A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
A water solution of sodium hypochlorite (NaOCl) is used as laundry bleach. The concentration of sodium hypochlorite is 0.75 m. Express this concentration as a mole fraction.
A gaseous solute dissolves in water. The solution process has H=15 kJ. Its solubility at 22C and 6.00 atm is 0.0300 M. Would you expect the solubility to be greater or less at (a) 22C and 1 atm? (a) 18C and 6 atm? (a) 15C and 10 atm? (a) 35C and 3 atm?
You dissolve 1.0 mol of urea (H2NCONH2) in 270 g of water. The mole fraction of urea is (a) 3710 3 (b) 0.063 (c) 16 (d) 1.0 and its molality is (a) 1.0 (b) 3.7 (c) 0.063 (d) 0.27
From the data presented in Figure 12.11, determine which has the more positive enthalpy of solution: NaCl or NH4Cl. Explain.
The Henry's law constant for the solubility of helium gas in water is 3.8104M/atm at 25C. (a) Express the constant for the solubility of helium gas in M/mm Hg. (b) If the partial pressure of He at 25C is 293 mm Hg, what is the concentration of dissolved He in mol/L at 25C? (c) What volume of helium gas can be dissolved in 10.00 L of water at 293 mm Hg and 25C? (Ignore the partial pressure of water.)
Create a flow diagram, similar to those used in the example problems of this chapter, that outlines the determination of the molar mass of a compound from freezing-point depression measurements. Clearly indicate the data needed for this determination.
The Henry's law constant for the solubility of radon in water at is 9.57106 M/mm Hg. Radon is present with other gases in a sample taken from an aquifer at 30C. Radon has a mole fraction of 2.7106 in the gaseous mixture. The gaseous mixture is shaken with water at a total pressure of 28 atm. Calculate the concentration of radon in the water. Express your answers using the following concentration units. (a) molarity (b) ppm (Assume that the water sample has a density of 1.00 g/mL.)
6-21 Are mixtures of gases true solutions or heterogeneous mixtures? Explain.
An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25 C. (a) What is the average molar mass of starch? (The result is an average because not all starch molecules are identical.) (b) What is the freezing point of the solution? Would it be easy to determine the molecular weight of starch by measuring the freezing point depression? (Assume that the molarity and molality are the same for this solution.)
Situation 2: 0.9% (w/v) sodium chloride (MW = 58.44 g/mol) solution (Normal Saline Solution) has an osmotic pressure of 3.91 atm at 25°C:
Freezing point for molar mass. Do not round mid equation because Aleks flags it. Round at the end to appropriate sig figs