I. Making Solutions
A. Background
Definitions
Solution - homogeneous mixture of one or more substances
dissolved in another
Solute - the substances (solids or liquids) that are
dissolved
Solvent - the "dissolver" - a liquid, usually water
A. The procedure for making
solutions
Kitchen: Fruit Punch Lab:
50X Denhardt's Solution
Ingredients:
12 oz frozen pineapple juice 5 g Ficoll
20
oz frozen strawberries 5 g Polyvinylpyrrolidone
1
pint strawberry ice cream 5
g BSA (fraction V)
Chilled
lemon-lime soda Nuclease-free
water
Preparation:
1. Combine each in turn, Stir w/heating, dissolving
blending
until smooth: each
solute completely in turn:
pineapple
juice concentrate Ficoll
strawberries PVPP
ice
cream BSA
2. Pour into chilled punch bowl Transfer to graduated cylinder
3. Add soda to 2 quarts Bring to 500mL with water
4. Top with ice
cream Filter through a 0.22 mm filter
5. Serve in punch cups. Store in 50mL
pre-sterilized tubes.
B. Many recipes for lab solutions do NOT give amounts
but instead give concentrations:
Amounts: Concentrations: (amount
per volume)
5g g/L
(mg/ml)
500mL %
M (mM)
2. Making solutions to
concentration
a. Molarity - number of moles of solute dissolved per
liter of solution (moles/L)
Review:
1 mole of any element
contains 6.02 x 1023 atoms
*the
weight of 1 mole of an element is its gram atomic weight
Ex. 1 mole of C weighs 12.0g
Compounds
are atoms of 2 or more elements bonded together
1 mole of a compound contains
6.02 x 1023 molecules
*the weight of 1 mole of a compound
is its gram formula weight (FW) or gram molecular weight (MW)
Ex. 1mole of Na2SO4
is 142.04g:
2 Na
atoms = 2 x 22.99g = 45.98g
1 S
atom = 1 x 32.06g = 32.06g
4 O
atoms = 4 x 16.00g = 64.00g
142.04g
A
1 molar (1M) solution of a compound contains 1 mole of that compound
dissolved in 1 L of total solution.
Ex. 1M Na2SO4 = 1mole or 142.04g
of Na2SO4 in 1L of solution
Ex. 1mM Na2SO4 = 1mmole (10-3M)
or 0.14204g of Na2SO4 in 1L of solution
Ex. 1mM Na2SO4 =
1mmole (10-6M) or 0.000142g of Na2SO4
in 1L of solution
Making
1L of 1M Na2SO4 -
MW = 142.04g/mol
Making
100mL of 1M Na2SO4
Making
100 mL of 10mM Na2SO4
b. Weight per Volume - solute
expressed as weight, solvent as volume
Ex. 2mg/mL proteinase K
each
mL solution contains 2 mg Proteinase K
You want to make 50 mL of
Proteinase K solution at a concentration of 2 mg/mL
You know the concentration
and volume of solution you want, you need to figure out the amount of solute
needed:
c. Percent - amount of solute
in 100 units of total solution
What is 2% milk?
2g of milk solids per 100mL
of milk
a weight per volume
expression (w/v)
i. Weight per volume
Ex. 20g NaCl in 100mL total
solution is a 20% (w/v) solution
ii. Volume percent
Ex. 100mL of methanol in
1000mL of total solution is a 10% (v/v) solution
2. Preparing dilute solutions
from concentrated solutions
Directions for making orange juice from concentrate:
Add 1 can concentrated orange
juice to 3 cans cold water.
How can we express the
concentration of our “drinkable” orange juice?
How can we express the
concentration of our concentrated orange juice?
ConcentrationStock
x VolumeStock = ConcentrationFinal x VolumeFinal
C1V1 =
C2V2
C1 = initial concentration
of stock solution
V1 = volume of
stock solution required
C2 = final
concentration desired
V2 = final volume
desired
Want to prepare 500mL of 1X
TBE from a 5X stock
C1V1 =
C2V2
What is known?
What is the unknown?
Want to prepare 100 mL of 1M Tris
from a 2M Tris stock solution.
C1V1 =
C2V2
What is known?
What is the unknown?
3. Preparing solutions with
more than one solute
preparing without stocks
preparing with stock
solutions - use the C1V1 = C2V2 equation
for each solute