ch302 notes ch17.1 - CH302 Chapter 17: PROPERTIES OF...

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CH302 Chapter 17: PROPERTIES OF SOLUTIONS Part 1 SOLUTION: Homogeneous mixture comprising : The SOLUTE: the smaller amount: that which is itself dissolved The SOLVENT: the larger amount: that which does the dissolving Ch. 17 will discuss AQUEOUS solutions Other solutions exist: See Table 17.1 CONCENTRATION MEASUREMENTS : Mass Percent: (also known as weight percent ) = grams of solute x 100% grams of solution Mole Fraction , χ You should have covered this in CH301 in Chapter 5 (Dalton’s Law) Mole Fraction of A % = χ A = __n A ____ n A + n B + . .. Molality, m: = moles of solute kilograms of solvent DO NOT GET THIS CONFUSED WITH MOLARITY, M! MOLARITY = __moles of solute ____ LITERs OF SOLUTION!! Concentration example: Calculate the molality and the molarity of an aqueous solution that is 10.0% by mass glucose, C 6 H 12 O 6 . Then calculate the mole fraction of glucose and water. The density of the solution is 1.04 g/mL. MM C 6 H 12 O 6 = 180 g/mol Important points to note when working with molarity and weight percent: Weight Percent: The volume of 100g of a solution is NOT 100ml! Only pure water has a density of 1g/ml or, i.e. 1kg/L
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This note was uploaded on 05/01/2009 for the course CH 52410 taught by Professor Sutcliffe during the Spring '09 term at University of Texas at Austin.

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ch302 notes ch17.1 - CH302 Chapter 17: PROPERTIES OF...

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