Using freezing point depression to find molecular weight freezing temperature of pure lauric acid (c°) 4384 freezing temperature of the benzoic acid-lauric acid mixture (c°) 3905 a calculate molality (m), in mol/kg, using the formula δt = k f m the kf value for lauric acid is 39°c•kg/mol. Freezing point depression experiment 19 note: you do not need to do a regular lab report and coversheetanswer all analysis questions and complete the graph purpose to determine the freezing points of pure lauric acid and a solution of camphor dissolved in lauric. This experiment will not use water and salt to observe the freezing point depression instead, lauric acid will be used as the solvent and benzoic acid will be the solute.
Learn freezing point depression with free interactive flashcards choose from 500 different sets of freezing point depression flashcards on quizlet. Where d t is the freezing point depression, k f is the freezing point depression constant for a particular solvent (39°c•kg/mol for lauric acid in this experiment ) and m is the molality of the solution (in mol solute/kg solvent. And lauric acid in the mixture and finding the freezing point depression, ∆t, the equations above can be used to find the formula weight of the unknown acid look up the melting point (freezing point) of pure lauric acid (also called dodecanoic acid.
Laboratory activity: notes teacher activity 2: the freezing point depression of lauric acid major chemical concept the major chemical concept is the freezing point depression due to a dissolved solute. Of pure lauric acid and that of the lauric acid-benzoic acid solution the freezing-point depression constant (k f ) for lauric acid is given (39˚c•kg/mol) the molality is determined by the freezing-point depression equation given above. In scientific laboratories, lauric acid is often used to investigate the molar mass of unknown substances via freezing-point depression in industry, lauric acid is used as an intermediate and as a surface active agent. Properties, benefits, and uses of lauric acid found in coconut oil and palm kernel oil, lauric acid is beneficial to our body read this nutrineat article to know about the properties, uses, and health benefits of lauric acid this technique is called freezing-point depression it is also used as a food shortening benefits lauric acid is.
The determination of the freezing point of lauric acid purpose the intention of this experiment was to quantitatively calculate the freezing point/melting point of lauric acid through melting and cooling the lauric acid and finding the freezing point on the graph of its temperature change over time. Where δt is the freezing point depression, k f is the freezing point depression constant for a particular solvent (39°c-kg/mol for lauric acid in this experiment 1), and m is the molality of the solution (in mol solute/kg solvent. Freezing point depression the freezing point of a solution is less than the freezing point of the pure solvent this means that a solution must be cooled to a lower temperature than the pure solvent in order for freezing to occur.
Where ∆t is the freezing point depression, kf is the freezing point depression constant for a particular solvent (39°c-kg/mol for lauric acid in this experiment 1 ), and m is the molality of the. Problem #11: when 200 grams of an unknown nonelectrolyte compound are dissolved in 5000 grams of benzene, the freezing point of the resulting solution is 377 °c the freezing point of pure benzene is 5444 °c and the k f for benzene is 512 °c/m. Queston 5: using your measured amounts of stearic acid and lauric acid for the second addition, calculate the colligative molality (m c) of the resulting solution, the freezing point depression (δ t f) this molality should cause and the theoretical freezing point of the solution enter your results in data table b.
Lauric acid is a saturated medium-chain fatty acid with a 12-carbon backbonelauric acid is found naturally in various plant and animal fats and oils, and is a major component of coconut oil and palm kernel oil. First they heated lauric acid to determine the temperature that the freezing point of the solvent is and then compared the temperature to that of the lauric acid/ benzoic acid solution they then took the change in temperature in order to determine the molality of the benzoic acid, which was calculated to be 1 mol/kg. Determination of molar mass by freezing-point depression is called the molal freezing-point depression constant lauric acid (the solvent in this experiment) has a reported kf = 39 °c g/mol = 39 °c/m determination of molar mass by freezing-point depression. Where ∆t is the freezing point depression, kf is the freezing point depression constant for a particular solvent (39°c • kg/mol for lauric acid in this experiment 1 ), and m is the molality of the.