viii CONTENTS.
meafldiremeiit of the relatiye osmotic preararefl in different aolations, 35. Taminann*B meaBorements, 37. Further experiments on osmotic pressure, 38.
CHAPTER IV.
Vapour Preasore of Solutions.
Vapour pressure of a solution, 39. Connection between vapour pressure and osmotio pressure, 39. ReUitive lowering of vapour pressure, 41. Vapour pressure of solutions in ether, 43. Higher concentrations, 44. Aqueous solutions, 45.
CHAPTER V.
Boiling Point and Freezing Point of Solutions.
Calculation of the boiling point of a solution, 47. Freezing point of solutions, 49. Experimental determination of the freezing point, 51. Experi- mental determination of the boiling point, 52. Advantages of the freezing point method, 53. Connection between depression of vapour pressure and depression of freezing point, 54. Connection between o6motici.pressure of a solution and its freezing point and vapour pressure, 55. Molecular lowering of the freezing point, 56. Molecule complexes, 58. Dissociation of electrolytes, 59. Range of validity of van't }Ioff*s law, 60. Alloys, 61. Solid solutions, 63. Experimental results on the rise of boiling point, 63. Comparison between the various methods for determining the molecular weight, 65. Review of the results obtained, 66.
CHAPTER VI.
General Conditions of Eqailibrium.
Chemical reactions, 69. Chemical equilibrium, 70. The phase rule of Gibbs, 73. Osmotic work, 75. Henry's law, 77. Distribution law, 80. Kinetic considerations, 82. Depression of solubility, 83. Homogeneous equilibrium, 84. Clapeyron's formula, 90. Change of solubility with temperature, 91. Change of homogeneous equilibrium with temperature, 93. Maxima and minima in equilibria, 96. Influence of pressure, 98.
��CHAPTER VII. Velocity of Reaction.
Formation of the state of equilibrium, 100. Inversion of cane sugar, 100. Saponification of an ester, 102. Velocity in heterogeneous systems, 103. Influence of temperature, 104. Velocity of reaction and osmotio pressure, 107. Action of neutral salts, 109.
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