CH302 Chapter 17 Notes part1-2

CH302 Chapter 17 Notes part1-2 - CH302 Chapter 17:...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: 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 , F You should have covered this in CH301 in Chapter 5 (Daltons Law) Mole Fraction of A % = F A = __n A ____ n A + n B + ... 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! The volume of 100g of a solution is NOT 100ml!...
View Full Document

Page1 / 2

CH302 Chapter 17 Notes part1-2 - CH302 Chapter 17:...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online