A measure of how much a gas, liquid, or solid becomes dissolved in a liquid.

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SOLUBILITY
A measure of how much a gas, liquid, or solid
becomes dissolved in a liquid.
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MTBE Methyl Tertiary Butyl Ether
A liquid that is very soluble in gasoline and
used to get more complete combustion of
gasoline. Unfortunately, also soluble in water.
42 g per liter. Can be tasted at 0.0001 g / liter
Over 20,000 of these storage tanks are estimated
to be leaking in Virginia
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Salt (NaCl) is very soluble in water. 350
g/liter. However, if water evaporates, there will
be too much salt for the water to hold in
solution. The salt begins to form crystals.
A lake near Death Valley is supersaturated with
salt causing the salt to crystallize out.
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Once a year the company who owns the lakes lets
visitors into the area to collect salt crystals.
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These are some of the salt crystals collected.
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Applications of Solubility Knowledge
Cleaning
Separation (purifying)
Detection Identification
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Like dissolves like

• To dissolve grease, use something that is also
  greasy or oily.

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Water the Universal Solvent

• One side of water is negatively charged because
  the oxygen atom keeps the shared electrons longer
  than the hydrogen atoms. As a result theoxygen
  side is negatively chargedand the hydrogen side
  of water is positively charged.

O
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Water the Universal Solvent

• Like a magnet that pulls on things that are
  magnetic, water pulls on things that are
  electrically charged. Magnets have north south
  poles, water has positive and negative poles and
  thus called a polar solvent.
• Since unlike charges attract, the negative end of
  water will be attracted to the positive sodium
  ion. The positive end of water will be attracted
  to the negative chloride ion.
• Since water is always in motion, it will pull on
  the ionic compound and move the ions away from
  each other. This dissolves the ionic compound.

Cl-
Na
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Wax does not repel water

• Weve heard that wax or oils repel water. But
  that isnt true. Water is so attracted to other
  water molecules that anything between them is
  squeezed out of the way.

Oildroplet
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Water is always trying to pull itself into a
tight ball as long as there is nothing nearby
that has a charge on it. Therefore, this surface
is not repelling water its simply not
attracting it and keeping water from doing what
it does naturally.
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We see the same effect on waxy leaves.
Water pulls on itself so much that it forms a
skin. Its called surface tension.
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We are lucky that water has this strong
attraction force otherwise wed never see
raindrops. The water would just breakup into a
mist as it fell. Very few liquids would remain
as drops if they fell from a large height.
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Soaps Detergents

• Soaps and detergents are chains that have one end
  that is like oil and has no charge and the other
  end is charged.

Oildroplet
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Acetone
O
CH3-C-CH3

• Solvent for fats, oils, waxes, resins, rubber,
  plastics, varnishes, nail polish remover,
  solvent for adhesives printing inks,
• Antiseptic solutions--to facilitate penetration
• The evaporation rate of acetone makes it quite
  useful for cleaning and drying. It dissolves
  water so you can wash away water allowing items
  to dry faster.

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Concentration of solutions
Approximate
Quantitative
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Approximate Descriptions of Concentration
Unsaturated
Dilute
Concentrated
Saturated
Supersaturated
Alum
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This reference book indicates the solubility of
many inorganic and organic compounds.
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Approximate
Guess what these abbreviations stand for. Click
on them for answer.
water
alcohol
ether
acetone
benzene
Next Slide
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ether
very soluble in Ethanol
slightly soluble in benzene
soluble in water
chloroform
Try to guess what these abbreviations mean and
then click on them for answers.
Chemical Abstracts Service
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Quantitative Measurement of Concentrations
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Mass/Volume (w/v)
These can be easily turned into Mass/Volume
Percent (w/v)
Na3P
Saturated solutions
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Mass/Volume Percent (w/v)
0.14 grams per 100 cc.
Many products list the concentration of their
ingredients. Fluoride is the active ingredient.
Na2PO3F Apparently F replaces one of the
oxygens, and since F has 7 electrons then the
phosphate is -2 instead of -3. Na2PO3F Mol Wt
144. 1.06 if stated as wt/vol of Na2PO3F
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0.243 grams NaF per 100 cc.
0.15 grams Fluoride ion per 100 cc.
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Insecticides are often dissolved in solvents.
Their concentrations are usually given as sample
weight divided by solvent weight converted to
percent.
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For every 100 grams, how much of it is Diazinon?
Mass Percent (w/w)
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Mass/Volume Percent (w/v)
100100
5mg1mL
g 100 mL
.001milli
0.5
Two ways of showing concentration are given.
Lets turn 5mg per mL into 0.5 to see they are
the same.
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Mass/Volume Percent (w/v)
1 1g/100mL 0.2 0.2g/100mL 0.20.2g/100mL
0.2g 15mL .03 grams 100mL
To calculate the grams of glycerin in this bottle
use dimensional analysis.
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Mass/Volume Percent (w/v)
0.1 0.1
This lists the ingredients of Dextrose 5. It
says 50 grams in 1,000 mL of water. The
dimensional analysis above shows how 50g per
1000mL can be converted to 5 (w/v)
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Calculate Mass/Volume Percent (w/v)
Find grams per mL (divide 39g by 355mL)
Multiply by 100 to get grams per 100mL
Calculate the percent (w/v) of sugar.
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½ of proof
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Parts per million (ppm)
4 4 grams/ 100 ml x 25 ml 1 gram Chlorine
1 g per 10 liters ? 1 g per 10 kg ? 1 g per
10,000 g 1g x 100 100 g
or 100 ppm10,000g x 100 1,000,000 g
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• Ionic Breeze complies with U.S. requirements for
  low ozone emission (less than 50 parts per
  billion)

O.S.H.A. 24 hour exposure limit, 0.05 PPM, Parts
Per Million
The product lists 50 parts per billion (ppb)
concentration of ozone. OSHA, however, lists the
level as 0.05 ppm. Lets convert the ppm to ppb
to better compare these values.
After multiplying by 1000 we find the 0.05 ppm is
the same as 50 ppb.
0.05 1000 50 1,000,000
1000 1,000,000,000
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Quantitative Measurement of Concentrations
Mass Percent (w/w)
solid mixtures/ solids in solvents
Mass/Volume (w/v)
mg/mL, g/Liter
Medical solutions g/100mL or g/100cc
Mass/Volume Percent (w/v)
Volume Percent (v/v)
Liquid in liquid, liquors
Parts per million (ppm)mg/liter (if water) wt or
vol
Trace amounts in water or air
Molarity (M)(mol/liter)
Chemistry reagents
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You want to neutralize 360 grams NaOH How many
grams of HCl is needed?
Reactants
Products

• Weight

• Weight

Chemical reaction
NaOH(aq) HCl(aq) ? NaCl(aq) HOH(l)
9
360 g NaOH moles NaOH
mole g
1 40
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You want to neutralize 360 grams NaOH How many
grams of HCl is needed?
Reactants
Products

• Weight

• Weight

Chemical reaction
9 moles
9 moles
NaOH(aq) HCl(aq) ? NaCl(aq) HOH(l)
328.5
9 moles HCl grams HCl
g mole
36.5 1
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Art of Counting Without Counting
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Products
Reactants
Molarity M

• Weight
• Volume
• Concentration

• Weight
• Volume
• Concentration

1 moleLiter
1 M
If you had half a liter of 1M NaOH, how much 1M
HCl is needed to neutralized it.
Convert volume Conc.to moles
For NaOH, 40 grams in one liter makes 1 M.
Convert moles to Volume
Chemical reaction
NaOH(aq) HCl(aq) ? NaCl(aq) HOH(l)
1 M
1 M
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• Ingredients Aspirin 325 mg, sodium bicarbonate
  1700 mg, citric acid 1000 mg.

• Reactions go faster if the reactants are well
  mixed. Dissolving them first in water and then
  mixing them makes the reaction go faster.

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Why are chemicals or drugs dissolved in water?
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Concentration based on Moles per Liter

• This bottle of Sodium Phosphate lists the
  concentration as 0.1 M. How many moles of sodium
  phosphate are there in one liter of this
  solution?
• How many moles of sodium phosphate in 3 liters?
• How many moles in 0.1 liters?

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• Weve used silver nitrate to test for chloride
  ion (Cl-) in a few lab experiments.
• Ag Cl- ? AgCl(s)
• Silver nitrate dissolved in water is a convenient
  way to add a small amount of silver nitrate to
  something else to see if a reaction occurs with
  either the silver or the nitrate.
• If this bottle is 250 mL, how many moles of
  silver nitrate does it contain?

250mL x 0.001 milli
0.250 L
0.25L x 0.2 moles 1 Liter
0.05 moles
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• Weve used silver nitrate to test for chloride
  ion (Cl-) in a few lab experiments.
• Ag Cl- ? AgCl(s)
• A salt solution is 0.2 M NaCl. How much of this
  salt solution is needed to precipitate all of the
  Ag from this one liter bottle?
• What if the NaCl solution was 0.4 molar? How
  much would be needed?

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Lets say the left bottle is 4 liters. How many
moles of sodium arsenate are in a full bottle?
How much sodium arsenate would you weigh out to
make up 4 liters of this 0.1M solution?
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