Difference between revisions of "Krafft Points, Critical Micelle Concentrations, Surface Tension, and Solubilizing Power of Aqueous Solutions of Fluorinated Surfactants"
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To measure Krafft Point and CMC: Krafft point was determined by the abrupt increase in the electrical conductivity of as a function of temperature | To measure Krafft Point and CMC: Krafft point was determined by the abrupt increase in the electrical conductivity of as a function of temperature | ||
| − | Surface Tension Measurements: [(described in another paper)][http://pubs.acs.org/doi/pdf/10.1021/j100650a021] | + | Surface Tension Measurements: [(described in another paper)][http://pubs.acs.org/doi/pdf/10.1021/j100650a021] |
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| + | A drop-weight method was used to measure surface tension. This method involves obtaining an image of a drop and comparing its shape and size to theoretical profiles. Once <math>\beta</math> and b have been determined from shape and size comparisons, the surface tension is calculated from: | ||
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| + | [[Image:eqn.png]] | ||
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| + | The reason this is a viable method is, the shape of an axisymmetric pendant or sessile drop (see figure below) is only dependent on the Bond number (a measure of the relative importance of gravity to surface tension in determining the shape of the drop). For drops with Bond numbers near zero, surface tension dominates and the drop is close to a sphere in shape. For drops with larger Bond numbers, the drop becomes increasingly deformed by gravity. | ||
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| + | [[Image:bubble.png]] | ||
==Results== | ==Results== | ||
Revision as of 03:57, 26 October 2011
Contents
Krafft Points, Critical Micelle Concentrations, Surface Tension, and Solubilizing Power of Aqueous Solutions of Fluorinated Surfactants
Authors: Hironobu and Kozo Shinoba
Journal: The Journal of Physical Chemistry, Vol. 80, No. 22, 1976, p2468-2470
Introduction
This paper discusses the Krafft points, critical micelle concentrations (cmc), surface tension above the cmc, and solubilizing power in aqueous solutions of perfluoroalkane carboxylates as functions of fluorocarbon chain length.
The surface tension of these types of solutions is lower than that for ordinary surfactants. Fluorinated surfactants are very stable and have special industrial uses. The longer chain surfactants are more surface active and have high solubilization at low concentrations (compared to shorter chain surfactants). However, the Krafft point increases with increasing hydrophobic chain length. The Krafft point is the point above which ionic surfactants form micelles (and therefore dissolve well). Before this paper was published, it was shown that the kinds of [gegenions][1] affect the Krafft point. This paper outlines some results on the effect of the kinds of gegenions and chain length of surfactant on the Krafft point, surface tension, cmc, and solubilizing power in aqueous solutions of these perfluoroalkane carboxylates.
Experimental Method
Solutions of perfluoroalkane carboxylates with hydrocarbons of varying lengths were created.
To measure Krafft Point and CMC: Krafft point was determined by the abrupt increase in the electrical conductivity of as a function of temperature
Surface Tension Measurements: [(described in another paper)][2]
A drop-weight method was used to measure surface tension. This method involves obtaining an image of a drop and comparing its shape and size to theoretical profiles. Once <math>\beta</math> and b have been determined from shape and size comparisons, the surface tension is calculated from:
The reason this is a viable method is, the shape of an axisymmetric pendant or sessile drop (see figure below) is only dependent on the Bond number (a measure of the relative importance of gravity to surface tension in determining the shape of the drop). For drops with Bond numbers near zero, surface tension dominates and the drop is close to a sphere in shape. For drops with larger Bond numbers, the drop becomes increasingly deformed by gravity.
Results
Surfactants form micelles above the Krafft point and the solubility of surfactants in water increases drastically. Therefore, solubilization occurs above the Krafft point. CMC: measured by the electrical conductivity-concentration curve at constant temperature
