solutions chapter 13 5.0 chemistry. what is a solution solution: a homogeneous mixture of 2 or more...
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Solutions
Chapter 135.0 Chemistry
What is a solution
Solution: A homogeneous mixture of 2 or more substances in a single physical state.
Suspension: Particles are somewhat evenly dispersed, but will settle when at rest. (clay & water)
Colloid: Particle size between suspension and solution (milk)
Properties of Solutions
Small Particles
Evenly distributed particles
Particles do not separate when at rest.
Solubility: The ability to dissolve in another substance.
Properties of Solutions
Solute: substance that is dissolved
Solvent: Substance that does the dissolving
Solute
Solvent
Properties of Solutions
Soluble means something can be dissolved in something else.
Insoluble means something cannot be dissolved in something else.
Solid Solutions
Alloys: Solid solutions that contain 2 or more pure substance.
Advantages of alloys over pure metals: Stronger Cheaper Resistance from corrosion Lighter
Alloys
Gaseous Solutions
The properties of gaseous solutions depend on the properties of its components.
Ex. Air
Liquid Solutions
Miscible Liquids: 2 liquids that can mix together in any amount
Ex. Alcohol and water
Liquid Solutions
Immiscible Liquids: 2 liquids that cannot mix
Ex. Oil and Water
Other types of solutions
Aqueous Solutions: Solutions with water as the solvent.
Because water can dissolve so many things, it is called the universal solvent.
Electrolyte: A solution that conducts electricity
Tincture: Solutions with alcohol as the solvent.
Type of Solution Specific Solute Specific Solvent
Gas in Gas
Air O2 N2
Gas in Liquid
Soda CO2 H2OGas in Solid
catalytic converter hydrocarbons PtLiquid in Gas
fog H2O airLiquid in Liquid
Lemonade lemon juice waterLiquid in Solid
teeth fillings mercury silverSolid in Gas
smoke carbon airSolid in Liquid
Kool-Aid sugar waterSolid in Solid
steel carbon iron
IN
Concentration and Molarity
Concentration: Refers to the amount of solute per given amount of solvent.
Dilute Solutions – Has little solute
Concentrated Solutions – Has large amount of solute
Molarity
Molarity – Term used for concentration
Molarity = Moles of Solute
Liters of Solution
D. Molarity: (M)
Ex #1) What is the molarity of a solution formed by mixing 10.0 g of sulfuric acid with enough water to make 100.0 mL of solution?
moles of solutemolarity =
liters of solution
n mol = units =
V LM
2 410.0 g H SO 2 4
2 4
1 mol H SO
98 g H SO2 4 = 0.102 mol H SO
2
0.102 mol = 1.02
0.1000 L H OM M
Ex #2) How many grams of bromine are needed to prepare 0.500 L of a 0.0100 M solution of bromine in water?
2
n0.0100 = n = 0.00500 mol Br
0.500 LM
20.00500 mol Br 2160 g Br
1 mol Br2
2
= 0.800 g Br
Solubility and the Dissolving Process
Saturated: A solution is saturated if it contains as much solute as can possibly be dissolved under existing conditions of temperature and pressure.
Unsaturated: Has less than the maximum amount that can be dissolved.
Supersaturated: Has more than the maximum amount that can be dissolved.
Saturated vs. Unsaturated
Saturated vs. Unsaturated
Supersaturated
Dilutions
Formula for Dilutions: M1V1 = M2V2
How a solution forms Process of dissolving takes place at the
surface of the solute.
Dissolving Process
The interaction between the solute and solvent to allow ions to separate is called solvation. This interaction is called hydration when water is the solvent.
Dissolving Process
Energy is absorbed when the bonds break. (endo)
Energy is released when bonds form. (exo)
Solubility
Solubility is amount of solute that will dissolve in a specific solution under given conditions.
See solubility curves
Solubility Graph for NaNO3
0
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
So
lub
ilit
y (
g/1
00 g
wat
er )
Saturated sol’n
Supersaturated solution
Unsaturated solution
At 20 oC, a saturated solution contains how many grams of NaNO3 in 100 g of water?
What is the solubility at 70 oC? 135 g/100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30 oC?
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40 oC?
supersaturated
90 g
Factors that affect solubility
1) Nature of Solute and Solvent General rule: Like dissolves Like See example
2) Temperature As temperature increases, the solubility of
gases and liquids decrease.
Gases are less soluble at high temperatures than at low temperatures.
Pressure: As pressure increases, the solubility increases.
Factors Affecting the Rate of Dissolving
1) Surface Area 2) Stirring 3) Temperature
Altering these 3 factors will either increase the frequency of collisions or the energy of collisions between the solute and solvent.