Molality (m) 
nsolute
msolvent( kg )
Molarity ( M ) 
M 1V1  M 2V2
nsolute
Vsol'n ( L )
Dilutions:
Mole fraction of A 
moles of component A
(moles of component A + moles of component B)
moles of component B
(moles of component A + moles of component B)
Percent by Volume (v/v) =
V
Percent (v / v)  solute  100%
Vsol'n
Mole fraction of B 
Percent by Mass / Volume (m/v) =
Percent (m / v) 
msolute( g )
Vsol'n ( mL)
 100%
Percent by Mass (m/m) =
Percent (m / m) 
msolute
100%
msol'n
Parts Per Million (ppm) =
mcomponent
msolution
mcomponent
msolution
 10 6
Parts Per Billion (ppb) =
 10
9
1. What is the molarity of a 5.00 liter
solution that was made with 10.0 moles of
KBr ?
2. Calculate the molarity of the solution when
95.5 g of CaCl2, calcium chloride, is dissolved
in enough water to make 1.25 L of solution.
3. How many grams of ammonia are present in
5.0 L of a 0.050 M solution?
Molality (m)
moles of solute
m =
mass of solvent (kg)
Find the molality of the following solutions:
1) a solution is made by adding 83 grams of
sodium hydroxide to 750 mL of water.
2) a solution that contains .500 mol HC2H3O2 in
0.125 kg H2O.
3) a solution that contains 63.0 g HNO3 in 0.500 kg
H2O.
4. Dissolve 82.0 g of ethylene glycol in 250. g
of H2O. Calculate molality and % by mass of
ethylene glycol.
5. Calculate the molality of a 60.5% by
mass of nitric acid (HNO3) solution.
6. Find the molality of a 50.0 g NaCl
dissolved in 50.0 ml of water.