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Chapter 16: Solutions
Concentration formulas
Freezing pt. depression
Boiling pt. elevation
Ch. 16
Making a solution
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Concentration formulas
_____________ __________
Equation M = mole of solute . Liter of solution
m = mole of solute . kilogram of solvent
Effects Depends on temp. Does not depend on temp.
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How do you make a solution?
• _________: process of surrounding solute particles with solvent particles to form a solution
• Heat of solution: overall energy change that occurs during the solution formation process
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Speed of dissolving• Solution formation depends on how much
solute will dissolve in solvent.
Affect on dissolving
1__________________
2 __________
3 __________
Stir/agitate Solute dissolves faster
Increase temp Solute dissolves faster
Increase surface area Solute dissolves faster
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Su
rfac
e ar
ea
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Solubility – amount of solute that dissolves in solvent at a given _____________________________
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Varying solubility of solution
1 _________ solution
2 ___________ Solution
3___________
_____ solution
Less solute than saturated solution
Contains maximum amount of solute at given temp and pressure
Contains more solute than it can theoretically hold at given temp. and pressure
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Factors affecting solubility
Simulation: Solubility and temp
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Factors affecting solubility
1Temper-
ature
• Increase temp
• __________solubility of solids
• Allows supersaturated soln. to be made
• _________ solubility of gases
• Crystallization of supersaturated soln. initiated by • ____________ • If container is scratched
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Factors affecting solubility
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Factors affecting solubility
2 Pressure
• Negligible for solubility of L and S
• Increase pressure gas increase solubility gas
• _______________
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Section 2 Concentrations of Solutions
Objective:
Using Molarity (M)
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1. Mass of solute in grams
2. Amount of solute in ____
3. Volume of solute in __
4. Molar concentration, __
Change to moles!!
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1. What is the molarity of a solution prepared by dissolving 37.94 g of potassium hydroxide in some water and then diluting the solution to a volume of 500.0 mL?
Given:
Unknown:
Don’t forget to
use moles!
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2. Determine the molarity of a solution prepared by dissolving 141.6 g of citric acid, C3H5O(COOH)3 in water and then diluting the resulting solution to 3500.0 mL.
Given:
Unknown:
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3. What is the molarity of a salt solution made by dissolving 280.0 mg of NaCl in 2.00 mL of water?
Given:
Unknown:
mg… tricky?How do you get grams?
Here’s a hint: 1g = 1000 mg
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4. What is the molarity of a solution that contains 390.0 g of acetic acid, HC2H3O2, dissolved in enough acetone to make 1000.0 mL of solution?
Given:
Unknown:
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5. An analytical chemist wants to make 750.0 mL of a 6.00 M solution of sodium hydroxide. What mass of NaOH will the chemist need to make this solution?
Given:
Unknown:
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6. What mass of glucose, C6H12O6 would be required to prepare 5.000x103 L of a 0.215 M solution?
Given:
Unknown:
Can you figure this
out?
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7. A solution has a volume of 2.0 L and contains 36.0 g of glucose (C6H12O6). If the molar mass of glucose is 180 g/mol. What is the molarity of the solution?
Given:
Unknown:
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8. A solution has a volume of 250 mL and contains 0.70 mol NaCl. What is its molarity?
This is
CAKE!
Given:
Unknown:
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Making Dilutions
• M1 V1 = M2 V2
•Question If you have 6M HCl acid, you want 500ml of 2M HCl acid, How can you prepare this?
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Section 3: Colligative properties
• Property that depends on amount of solute in solution, and not on identity of solution.
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Freezing point (FP)• Solute disrupts formation of orderly pattern; as a
result, more kinetic energy must be withdrawn from a solution to cause solidification.
* Solution that contains a solute has a ____________ than the pure solvent
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Boiling point (BP)
• Since adding a solute to a solvent decreases VP, additional kinetic energy must be added to raise VP and initiate boiling.
* Solution that contains a solute has __________ than the pure solvent
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Factors affecting Colligative Properties
1. Increase amt. of solute, increase magnitude…
a. VP lowering
b. FP depression
~1 mol solute lowers FP by 1.86°C
c. BP elevation
~ 1 mole solute increases BP by 0.512°C
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2. Solutes that dissociate have greater effects than nondissociating (nonpolar) solutes
Factors affecting Colligative Properties
3 particles 6 particles 9 particles
Affect colligative property least
Affect colligative property most
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Calculations with Colligative properties
• Freezing pt. depression (FP dep) – difference in temperature between FP of
solution and FP of pure solvent
ΔTf = (Kf)(m)
FP dep. example problems
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FP dep example 1: What is the freezing point depression (ΔTf) of a 0.100 m solution made with water?
ΔTf = (Kf)(m)
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FP dep. Example 2: A solution made with ethanol is made to lower the freezing point by 6.10˚C. What is the molality of the solution?
ΔTf = (Kf)(m)
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Calculations with Colligative properties
• Boiling point elevation (BP elev.)– difference in temp between BP of a solution
and BP of pure solvent
ΔTb = (Kb)(m)
BP dep. example problems
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BP elev. Example 1: What molality of NaCl solution would have to be used raise the boiling point of water by 2.00˚C?
ΔTb = (Kb)(m)
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BP elev. Example 2: Determine BP elevation (ΔTb) of a 0.857 m CaCl2 solution?
ΔTb = (Kb)(m)