Flashcards in Chp. 13.4- Concentration Terms Deck (15)
amt. (mol) of solute / volume (L) of solution
amt. (mol) of solute / mass (kg) of solvent
Parts of mass
mass of solute / mass of solution
Parts by volume
volume of solute / volume of solution
Mole fraction (X)
amt. (mol) of solute / [amt. (mol) of solute + amt. (mol) of solvent]
Sample Prob. 13.3. What is the molality of a solution prepared by dissolving 32.0 g of CaCl2 in 271 g of H20?
1.06 m CaCl2
Mass % = mass of solute / mass of solution * 100
mass of solute / mass of solution * 100
volume of solute / volume of solution * 100
Mole fraction (X) =
amt. (mol)of solute / [amt. (mol) of solute + amt. (mol) of solvent]
Find the conc. of calcium ion (in ppm) in a 3.50-g pill that contains 40.5 mg of Ca2+.
1.16x10^4 ppm Ca2+
The label on a 0.750-L bottle of Italian chianti indicates "11.5% alcohol by volume". How many liters of alcohol does the bottle of wine contain?
A sample of rubbing alcohol contains 142 g of isopropyl alcohol (C3H7OH) and 58 g of H20. What are the mole fractions of alcohol and water?
X_C3H7OH = 0.423
X_H20 = 0.577
If you were to make a 0.800m aqueous solution of glucose, what would be its boiling point and freezing point? (K_b = 0.51C/molarity, K_f=1.86C/molarity)
T_b = 100.41C
T_f = -1.49C
The higher the molality, the _______ the freezing point.
(Adding solute to a solvent will essentially dilute the solvent molecules, and according to Raoult's law, this leads to a decrease in vapor pressure.