RECALL TYPES OF MIXTURES: SUSPENSIONS COLLOIDS SOLUTIONS All
mixtures are physically combined and can be physically
separated.
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DEFINITION A solution is a homogeneous mixture of two or more
substance in a single physical state
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Solution a mixture of two or more substances that is identical
throughout can be physically separated composed of solutes and
solvents the substance in the smallest amount and the one that
dissolves in the solvent the substance in the larger amount that
dissolves the solute Colloids (milk, fog, jello) are considered
solutions Iced Tea Mix (solute) Water (solvent) Iced Tea (solution)
Salt water is considered a solution. How can it be physically
separated?
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Solutes Change Solvents The amount of solute in a solution
determines how much the physical properties of the solvent are
changed Examples: Lowering the Freezing Point The freezing point of
a liquid solvent decreases when a solute is dissolved in it. Ex.
Pure water freezes at 32 0 F (0 0 C), but when salt is dissolved in
it, the freezing point is lowered. This is why people use salt to
melt ice. Raising the Boiling Point The boiling point of a solution
is higher than the boiling point of the solvent. Therefore, a
solution can remain a liquid at a higher temperature than its pure
solvent. Ex. The boiling point of pure water is 212 0 F (100 0 C),
but when salt is dissolved in it, the boiling point is higher. This
is why it takes salt water longer to boil than fresh water.
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TYPES OF SOLUTIONS SOLUTESOLVENTEXAMPLE GAS Air
GASLIQUIDSeltzer (CO 2 ) LIQUID Antifreeze (ethyl glycol in water)
SOLIDLIQUIDSea water ( salt in water) GASSOLIDCharcoal filter
(poisonous gases in carbon) LIQUIDSOLIDDental filling (mercury in
silver) SOLID Sterling silver (copper in silver)
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SOLID SOLUTION Contain two or more metals called alloys Formed
by melting the components and mixing them together and allowing
them to cool Properties of alloys are different from the original
component metals
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TYPES OF ALLOYS ALLOYCOMPONENTUSES BabbittTin, antimony, copper
Bearings Bell metalCopper, tinBells Coinage metalsCopper, tin,
zincCoins 16 karat goldGold, copper, silverJewelry SterlingSilver,
copperJewelry, flatware NichromeNickel, iron, chromium, manganese
Heating elements
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Important terminologies: Soluble substance that dissolves
another substance Insoluble substance that does not dissolve
another substance
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Solutes Change Solvents The amount of solute in a solution
determines how much the physical properties of the solvent are
changed Examples: Lowering the Freezing Point The freezing point of
a liquid solvent decreases when a solute is dissolved in it. Ex.
Pure water freezes at 32 0 F (0 0 C), but when salt is dissolved in
it, the freezing point is lowered. This is why people use salt to
melt ice. Raising the Boiling Point The boiling point of a solution
is higher than the boiling point of the solvent. Therefore, a
solution can remain a liquid at a higher temperature than its pure
solvent. Ex. The boiling point of pure water is 212 0 F (100 0 C),
but when salt is dissolved in it, the boiling point is higher. This
is why it takes salt water longer to boil than fresh water.
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SOLUBILITY
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Solubility Solubility maximum grams of solute that will
dissolve in 100 g of solvent at a given temperature varies with
temp based on a saturated solution
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Solubility SATURATED SOLUTION no more solute dissolves
UNSATURATED SOLUTION more solute dissolves SUPERSATURATED SOLUTION
becomes unstable, crystals form increasing concentration
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Concentration the amount of solute dissolved in a solvent at a
given temperature described as unsaturated if it has a low
concentration of solute described as saturated if it has a high
concentration of solute described as supersaturated
ifsupersaturated contains more dissolved solute than normally
possible
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C.Determine if a solution is saturated, unsaturated, or
supersaturated. If the solubility for a given substance places it
anywhere on it's solubility curve it is saturated. If it lies above
the solubility curve, then it's supersaturated, If it lies below
the solubility curve it's an unsaturated solution. Remember though,
if the volume of water isn't 100 cm 3 to use a proportion first as
shown above.
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Temp. ( o C) Solubility (g/100 g H 2 O) KNO 3 (s) KCl (s) HCl
(g) SOLUBILITY CURVE Solubility how much solute dissolves in a
given amt. of solvent at a given temp. below Unsaturated: solution
could hold more solute; below line on Saturated: solution has just
right amt. of solute; on line Supersaturated: solution has too much
solute dissolved in it; above the line
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Solubility Table LeMay Jr, Beall, Robblee, Brower, Chemistry
Connections to Our Changing World, 1996, page 517 0 10 20 30 40 50
60 70 80 90 100 Solubility vs. Temperature for Solids Solubility
(grams of solute/100 g H 2 O) KI KCl 20 10 30 40 50 60 70 80 90 110
120 130 140 100 NaNO 3 KNO 3 HClNH 4 Cl NH 3 NaCl KClO 3 SO 2 shows
the dependence of solubility on temperature gases solids
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Solubility Solids are more soluble at... Solids are more
soluble at... high temperatures. Gases are more soluble at... low
temperatures & high pressures (Henrys Law). EX: nitrogen
narcosis, the bends, soda
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How to use a solubility graph? A.IDENTIFYING A SUBSTANCE (
given the solubility in g/100 cm 3 of water and the temperature)
Look for the intersection of the solubility and temperature.
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Example:What substance has a solubility of 90 g/100 cm 3 of
water at a temperature of 25C ?
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Example: What substance has a solubility of 200 g/100 cm 3 of
water at a temperature of 90C ?
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B.Look for the temperature or solubility Locate the solubility
curve needed and see for a given temperature, which solubility it
lines up with and visa versa.
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What is the solubility of potassium nitrate at 80C ?
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At what temperature will sodium nitrate have a solubility of 95
g/100 cm 3 ?
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At what temperature will potassium iodide have a solubility of
230 g/100 cm 3 ?
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What is the solubility of sodium chloride at 25C in 150 cm 3 of
water ? From the solubility graph we see that sodium chlorides
solubility is 36 g.
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Solubility in grams=unknown solubility in grams 100 cm 3 of
waterother volume of water ___36 grams____=unknown solubility in
grams 100 cm 3 of water150 cm 3 water Place this in the proportion
below and solve for the unknown solubility. Solve for the unknown
quantity by cross multiplying. The unknown solubility is 54 grams.
You can use this proportion to solve for the other volume of water
if you're given the other solubility.
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Solids and Gases dissolved in Liquids ToTo Sol. ToTo Solids
dissolved in liquids Gases dissolved in liquids As T o,
solubility
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How many additional grams of solute must be added in order to
make it saturated? From the graph you can see that the solubility
for potassium nitrate at 50C is 84 grams
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If there are already 30 grams of solute in the solution, all
you need to get to 84 grams is 54 more grams ( 84g-30g )
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Solubility Table LeMay Jr, Beall, Robblee, Brower, Chemistry
Connections to Our Changing World, 1996, page 517 shows the
dependence of solubility on temperature 0 10 20 30 40 50 60 70 80
90 100 Solubility vs. Temperature for Solids Solubility (grams of
solute/100 g H 2 O) KI KCl 20 10 30 40 50 60 70 80 90 110 120 130
140 100 NaNO 3 KNO 3 HClNH 4 Cl NH 3 NaCl KClO 3 SO 2 gases
solids
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Classify as unsaturated, saturated, or supersaturated. per 100
g H 2 O 80 g NaNO 3 @ 30 o C 60 g KCl @ 60 o C=saturated 50 g NH 3
@ 10 o C = unsaturated 70 g NH 4 Cl @ 70 o C =unsaturated
=supersaturated 0 10 20 30 40 50 60 70 80 90 100 Solubility vs.
Temperature for Solids Solubility (grams of solute/100 g H 2 O) KI
KCl 20 10 30 40 50 60 70 80 90 110 120 130 140 100 NaNO 3 KNO 3
HClNH 4 Cl NH 3 NaCl KClO 3 SO 2 gases solids
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So sat. pt. @ 40 o C for 500 g H 2 O = 5 x 66 g = 330 g 120 g
< 330 g unsaturated saturation point @ 40 o C for 100 g H 2 O =
66 g KNO 3 Per 500 g H 2 O, 120 g KNO 3 @ 40 o C Solubility vs.
Temperature for Solids Solubility (grams of solute/100 g H 2 O) KI
KCl 20 10 30 40 50 60 70 80 90 110 120 130 140 100 NaNO 3 KNO 3
HClNH 4 Cl NH 3 NaCl KClO 3 SO 2 gases solids 0 10 20 30 40 50 60
70 80 90 100
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(A) Per 100 g H 2 O, 100 g Unsaturated; all solute NaNO 3 @ 50
o C. dissolves; clear solution. (B) Cool solution (A) very
Supersaturated; extra slowly to 10 o C. solute remains in solution;
still clear. Describe each situation below. (C) Quench solution (A)
in Saturated; extra solute an ice bath to 10 o C. (20 g) cant
remain in solution, becomes visible.