Download - Standard 6: Solutions chapter 16
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Standard 6: Solutionschapter 16
ChemistryMs. Siddall
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Standard 6a: solution definitions• Solution: a homogeneous mixture of 2 or
more substances in the same physical state.
• Properties:
– Particles are small
– Particles are evenly mixed
– Particles will not separate• Examples:
– air (nitrogen & oxygen)
– Gatorade (water, sugar, etc)
– NaCl(aq) (salt & water)
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Summary 1
• Is muddy water a solution? Why/why not?
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• Solute: substance that is dissolved e.x. sugar
• Solvent: does the dissolving e.x. water
• Concentration: The amount of solute in a given amount of solvent e.x. [HCl]
• (aq) = aqueous = A solution where water is the solvent
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Summary 2
Consider lemonade.
1. What is the solvent?
2. What are the solutes?
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• Solvent: H2O molecules with dipole
• Solute: Ionic crystal lattice
Standard 6b: Dissolving Process
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• Polar H2O molecules surround positive and negative ions and break apart crystal lattice
• Water molecules move away (diffusion) so the process is repeated
Show animation
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Summary 3
Explain how water dissolves ionic compounds
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• It takes energy to break bonds
NaCl(s)
NaCl(aq)en
erg
y
Energy needed to overcome
lattice energyEnergy
released during
dissolvingDissolving
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Summary 4
Does the energy diagram for dissolving NaCl represent anendothermic or exothermic process? Explain your answer.
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Saturated solution: A solvent can not dissolve any more solute
• A saturated solution is at equilibrium. Particles are dissolving and precipitating at the same rateNaCl(s) Na+
(aq) + Cl-(aq)
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Summary 5
Does the dissolving process stop at equilibrium? Explain why/why not.
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• Some factors affect solubility (how much solute is dissolved)
• Some factors affect rate (how fast solute is dissolved)
• Some factors affect rate and solubility
Standard 6c: Factors that affect the dissolving process
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Standard 6c: Factors that affect the dissolving process
Factors affecting how much solute is dissolved
1. Type of solvent / solute
• Polar solvents dissolve polar & ionic solutes
• Non-polar solvents dissolve non-polar & covalent solutes
e.x oil and water do not mix
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Summary 6
Is oil a polar compound or a non polar compound? How do you know?
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2. Temperature• For solids: Temperature solubility
Temperature increases kinetic energy of solvent particles therefore more solute can be dissolved
• For gases: Temperature solubility Temperature increases the kinetic energy of solute particles therefore more particles escape from solution
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Summary 7
Why does the solubility of gas in solution decrease with increasing temperature?
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Solubility of solids & gases
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3. Pressure (Gasses Only!)
• Increasing pressure forces more gas into solution
• Pressure solubility • Pressure solubility
High pressure
low pressure
solution
air
Gas
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Summary 8
Does the concentration of carbon dioxide in your soda increase or decrease when you open the bottle? Why?
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Factors that affect the rate of solubility (how quickly something dissolves)
1. Temperature:
• T rate • T rate • Increasing temperature increases kinetic
energy = increased motion = increased diffusion
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2. Surface Area (particle size):
• S.A. (particle size ) rate • S.A. (particle size ) rate • Increasing surface area increases
opportunity for interaction between solute and solvent
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3. Stirring:
• stirring rate • stirring rate • Stirring increases particle motion so more
particles can be dissolved at the surface of the solid
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Summary 9
1. Name one factor that affects only solubility
2.Name one factor that affects only rate
3.Name one factor that affects rate and solubility
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Standard 6d: calculations• Molarity (mol/L)Molarity = Moles solute Liters solution • Grams per Liter (g/L)
= Grams solute
Liters solution
• Percent Composition (%)
grams solute x 100%
grams solution• Parts Per Million (ppm)
grams solute x 106
grams solution
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Summary 10
A solution contains 80g of NaOH in 500ml of solution. Calculate:
1.‘grams per liter’2. Molarity3. percent composition for the solution
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• Using ‘Parts per Million’ (ppm)• Usually used to measure solutions
containing a small amount of solute • e.x air quality or drinking water quality
– Air contains about 1ppm CO2 (Every 1million grams of air contains 1g CO2)
• smaller concentrations are measured in ppb(parts per billion)– Drinking water usually contains ≤ 0.5 ppb lead
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Summary 11
Which solution has the highest concentration of fluoride ions?a) 10 ppm F-
b) 100 ppm F-
c) 10 ppb F-
d) 100 ppb F-
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• Example: What is the concentration (ppm) of a 1L solution containing 5mg arsenic?
(The density of aqueous solutions = 1g/ml)
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Standard 6e: effect of solute on freezing and boiling point.
Molality (m) = moles solute Kg
solvent
e.x. what is the molality of a solution made by dissolving 180g sugar (C6H12O6) in 500g water?
180g sugar
500g water 180g sugar
1 mol sugar 1000g
1 kg= 2m
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Summary 18
what is the molality of a solution made by dissolving 92g ethanol (C2H6O) in 200g water?
92g ethanol
200g water 46g ethanol
1 mol ethanol 1000g
1 kg= 20m
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Freezing point depression and boiling point elevation: adding solute to a solvent lowers the freezing point and raises the boiling point of the solvent.
• Solute particles disrupt crystallization and evaporation.
• The change in freezing point or boiling point is directly proportional to the molality of solute particles.
• A solute that produces more ions in solution has the greatest effect.
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Summary 19
Explain why it takes more energy to boil water when it has more solute particles dissolved in solution.
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3m sugar
3 moles NaCl produces 6m of solute particles
3moles CaCl2 produces 9m of solute particles
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Summary 19
Which will affect the boiling point of solution more? WHY?
a) 1m NaClb) 1m CaCl2c) 1m AlCl3
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6f: Chromatography and distillation.
Chromatography: the separation of solution into individual substances using differences in polarity.
e.x. DNA analysis
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Distillation: separation of solutions into individual substances using differences in physical properties (boiling point)
e.x. salt water can be purified by distillation
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Summary 20
Why is it possible to separate alcohols by distillation?