Boiling Point Elevation
{"Image DocumentName": "Boiling Point Elevation", "Image ImageDescription": "For nonelectrolytes, \u0394Tb = Kbm. where: \u0394Tb is the boiling point elevation of the solvent. m is the molal concentration of the solution. Kb is the molal boiling point elevation constant (see Table 5, pg. 500). The units for this constant are 0C/m. Note: Every solute has a different Kb. Kb is the difference between the boiling points between a 1 m solution and a pure solvent. Like vapor pressure lowering, boiling point elevation is a colligative property. The value of the boiling point elevation is directly proportional to the solutions, solute molality, the greater the number of solute particles in the solution, the greater the boiling point elevation.", "Image XResolution": "37", "Image YResolution": "37", "Image ResolutionUnit": "Pixels/Centimeter", "Image Software": "SlidePlayer", "Image YCbCrPositioning": "Centered"}