SOLUTIONS Chapter 16 Test Monday 8/09/04 What is a solution? Any substance – solid, gas, or liquid...
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Transcript of SOLUTIONS Chapter 16 Test Monday 8/09/04 What is a solution? Any substance – solid, gas, or liquid...
What is a solution?
Any substance – solid, gas, or liquid – that is evenly dispersed throughout another substance – solid, gas, or liquid – is a solution.
Solutions are homogeneous mixtures.
Examples of solutions: Air, 14K gold, sea water
SOLVENT: The substance that is the dissolving medium
SOLUTE: The substance dissolved in the solvent
These are relative terms. The substance you have more of in a solution is the solvent. Ex. CH3CH2OH
The process of Solvation
How can water molecules break the ionic bonds in a crystal of potassium permanganate (KMnO4) to dissolve it?
HH
O
KPermanganate
ion
HH
O
At the surface of the crystal the water molecules becomes associated with the ions in the crystal.
A group of water molecules will surround each ion and isolate it from its neighbors.
These ions are said to be HYDRATED
This process of dissolving a solute in a solvent is called SOLVATION.
Dissociation
The process of decomposition of a crystal into hydrated ions is called DISSOCIATION.
Example
NaCl(s) Na+(aq) + Cl– (aq)
The symbol (aq) means that the ions are hydrated.
Molecular Solvation
Solvation can also occur between polar solute molecules and polar solvent molecules.
Example: methanol CH3OH.
Is methanol capable or forming a hydrogen bond?
The polar ends of the solute molecules are attracted to the oppositely charged polar regions of the solvent molecules.
In some cases the geometry and attraction between polar molecules cause that when two volumes are added the total volume is less than the one expected.
Ex. H2O and CH3CH2OH
Miscibility
Two substances are said to be miscible when there is no limit to the solubility of one substance into the other
When polar and non-polar substances are mixed, they show very little attraction for each other. Solvation does not occur. Ex: oil and water.
Two liquids that do not mix are called immiscible
Solutions
Solutions are transparent. You can see through them.
The mixture remains stable and does not separate after standing for any period of time.
The particles are so small they cannot be separated by normal filtration.
Colloids
Colloids are mixtures with particle sizes that consist of clumps of molecules. The particles have dimensions between 2 to 1000 nanometers.
The colloid looks homogeneous to the naked eye. Fog and milk are examples of colloids.
Colloids frequently appear "murky" or "opaque". The particles are large enough to scatter light.
Colloids generally do not separate on standing. They are not separated by filtration.
Suspensions
Suspensions are mixtures with particles that have diameters greater than 1000 nm. They are are visible to the naked eye. Ex: Blood
Suspensions are "murky" or "opaque". They do not transmit light. Suspensions separate on standing. The mixture of particles can be separated by filtration.
Examples of matter in solution
gas in gas: air ( N2, O2 , Ar, CO2 , etc)
gas in liquid: soda pop (CO2 in water)
liquid in liquid: gasoline (hydrocarbons)
solid in liquid: sea water (dissolved salts)
gas in solid: H2 in palladium
liquid in solid: dental amalgams ( Hg in Ag)
solid in solid: alloys ( brass, (Cu/Zn))
Like dissolves like
Generally two polar molecules are soluble in each other. Ex. Water and alcohol.
Many non-polar molecules will dissolve in non-polar solvents. Ex. Iodine will dissolve in mineral oil.
The rule of thumb is: like dissolves like
Solubility
SATURATED: A solution that cannot dissolve any more solute at a given T.UNSATURATED: A solution that can dissolve more soluteSOLUBILITY: Is the amount of solute needed to make a saturated solution at a given T.SUPERSATURATED: A solution that contains more solute that it would normally holds at a given T.
Solubility is the amount of substance needed to make a saturated solution at a given temperature.
It is usually given in grams of the solute per 100 g of water.
It depends on the solute and solvent.
The word soluble is not a precise term because solubilities vary greatly. It is commonly used for solubilities greater than 0.1 mol per liter of solution.
Factors affecting solubility
TEMPERATURE
For many substances solubility increases with temperature.
The solubility of a gas decreases as the temperature increases.
Factors affecting solubility
PRESSURE
The solubility of a gas depends on the pressure.
The higher the pressure the higher the solubility.
Henry’s Law
How does oxygen partial pressure affect dissolved oxygen levels?
Oxygen in water obeys Henry's law; the solubility is roughly proportional to the partial pressure of oxygen in the air:
pO2 = KO2 xO2
PO2 = partial pressured of the gas
KO2 = Henry constant for water
XO2 = Mole fraction of O2 in a saturated solution
Which pair forms a precipitate?
KI(aq) + Pb(NO3)2(aq) ----> KNO3 + PbI2
1. KNO3
2. PbI2
3. Neither pair forms a ppt.
Identify the spectator ion(s)
Fe(s) + Cu2+(aq) + SO42-+(aq) Cu(s) + Fe2+(aq) + SO4
2-
(aq)
1. Cu(s)
2. Cu2+
3. Fe2+
4. SO42-
5. None are spectator ions.
Acid – Base reaction
When an acid and a base react, a salt and water are formed
Reaction of sodium hydroxide and hydrochloric acid
NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l)
Base Acid Salt Water
Net Ionic: OH–(aq) + H+(aq) H2O(l)
Reaction of a metal and H+ ion
Metals more active than hydrogen react with H+ ions in solution to form metallic ions and hydrogen gas.
Reaction of zinc and hydrochloric acid
Zn(s) + 2 HCl(aq) ZnCl2(s) + H2(g)
Net ionic:
Zn(s) + 2H+(aq) Zn2+(aq) + H2(g)
Rxn of an acid and a carbonate
When carbonic acid is form in a reaction it decomposes into CO2 and H2O.
This is an important reaction in living organisms
Reaction of Na2CO3 and HCl
Na2CO3(aq) + 2HCl(aq) 2NaCl(aq) + H2CO3(aq)
===========
H2CO3(aq) CO2(g) + H2O(l)