3. In a freezing point experiment using acetic acid as a solvent the following values were obtained: Tr (acetic acid) = 16.1°C Tr (with 1.60 g of solute in 10.00 mL of acetic acid) = -2.5°C Use this data to calculate the molecular mass of the solute. (Acetic acid: Kr=3.9 °C-kg/mol; D=1.05 g/mL)

3. In a freezing point experiment using acetic acid as a solvent the following values were obtained: Tr (acetic acid) = 16.1°C Tr (with 1.60 g of solute in 10.00 mL of acetic acid) = -2.5°C Use this data to calculate the molecular mass of the solute. (Acetic acid: Kr=3.9 °C-kg/mol; D=1.05 g/mL)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 68QAP: Consider two solutions at a certain temperature. Solution X has a nonelectrolyte as a solute and an...

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Concept explainers

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.

Question

2. Calculate the expected osmotic pressure for a solution prepared from 82.0 g of KBr and 125 g of
water at 20.0°C. (Density of this solution is 1.375 g/mL)
82.0 g KBv. Imolker = 0.689 moles HBr
119gKBr
K: 39.10
8=79.90
1198/mal
π = iMRT
200+273.15=2
3. In a freezing point experiment using acetic acid as a solvent the following values were obtained:
Tr (acetic acid) = 16.1°C
Tr (with 1.60 g of solute in 10.00 mL of acetic acid) = -2.5°C
Use this data to calculate the molecular mass of the solute. (Acetic acid: Kr=3.9 °C-kg/mol; D=1.05 g/mL)
4. Calculate the mole fraction of solvent in a NaC₂H302 (sodium acetate) in an aqueous solution that
has a freezing point of -4.40 °C. Use the theoretical van't hoff factor.

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