solubility and concentration chemistry mrs. coyle
TRANSCRIPT
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Solubility and Concentration
ChemistryMrs. Coyle
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Part I Solubility:
The ability of a solute to dissolve in a solvent.
Expressed as g solute/100g H2O
or g solute/100mL H2O
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Soluble
• Soluble: a solute that has appreciable solubility.
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Miscible
Substances that dissolve in each other.
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Solubility Curves
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Precipitate: solute that comes out of solution.
•
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Types of Solutions
Saturated contains the maximum amount of solute that can be dissolved at the given conditions of T and P.
Unsaturated contains less than the saturated amount of solute.
Supersaturated contains more than the saturated amount of solute by dissolving at higher temp and then cooling.
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A supersaturated solution crystallizes after a seed crystal is introduced.
http://www.chem.ufl.edu/~itl/2045/change/C12F11.GIF
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Rates of Solution
Does every candy you eat take the same time to dissolve?
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Factors affecting the rate of dissolving:
Surface Area
Stirring
Temperature (average kinetic energy)
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Factors Affecting Solubility
Temperature (affects solid, liquid and gaseous solutes)
Pressure (affects gaseous solutes)
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Effect of temperature on solubility of gases.
Example:Compare the amount of oxygen dissolved in the waters of the arctic ocean
to the amount of oxygen dissolved in warm tropical waters.
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Effect of temperature on solubility of solids. Example:
Can you dissolve more sugar in warm water or in cold water?
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Solubility Curves
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Effect of Pressure on solubility of solids. Negligible.
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Effect of Pressure on solubility of gases. Henry’s Law: the amount of gas dissolved in
a solution is directly proportional to the pressure of the gas above the solution.
The higher the pressure the higher the solubility of the gas.
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Effect of Pressure on solubility of gases.
http://www.chem.ufl.edu/~itl/2045/lectures/lec_i.html
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Example
An unopened bottle of soda has a pressure of 5atm above the liquid, so the concentration of CO2 in the soda is high.
Compare that to a pressure of 1 atm above the liquid when the bottle has been opened.
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Part II Concentration: A measure of the amount of solute dissolved in
the solution. Molarity (M) Molality (m) Mole Fraction (x) Percent by Mass (%)
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Part II
Concentration
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Molarity
• A unit of concentration of a solution expressed in moles solute per liter of solution. (Note: 1L = 1 dm3)
Molarity (M) =Moles of Solute
Liters of Solution
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Why Molarity ?
http://www.chem.ucla.edu/~gchemlab/volumetric_soln_conc.jpg
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Steps involved in the preparation of a standard aqueous solution
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Process of making 500 mL of a1.00 M acetic acid solution
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Ex. 1 Molarity
What is the molarity of a solution of 8g NaOH in 100mL of solution?
Answer: 2M NaOH
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Ex. 2 Molarity
How many grams of NaOH are contained in 2L of a 3M NaOH solution?
Answer: 240g NaOH
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Making Dilutions
Moles Solute=M1V1=M2V2
M molarity V volume
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Ex. 3 Dilutions
How many milliliters of 2.00M MgSO4 solution must be diluted with water to prepare 100.00 mL of 0.400M MgSO4?
Answer: 20.0mL
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Percent by Mass
% by mass= Mass of solute x 100 % Mass of solution
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Percent by Volume
% by volume= Volume of solute x 100 % Volume of solution
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Part III Molality and Mole Fraction
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Molality
Moles of Solute per kilogram of Solvent
Molality (m) = moles solute kg solvent
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Mole Fraction
xsolute = Moles of solute Moles of solution
xsolvent = Moles of solvent Moles of solution
xsolute + xsolvent= 1