Ch. 8 Solutions, Acids, & Bases
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Transcript of Ch. 8 Solutions, Acids, & Bases
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Ch. 8Solutions, Acids, & Bases
I. How Solutions Form Definitions Types of Solutions Dissolving Rate of Dissolving
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A. DefinitionsSolution – a mixture that has the same
composition throughout the mixture; a homogeneous mixture.
Solvent – what the solute is dissolved in (in greater quantity)
Solute - substance being dissolved (in lesser quantity)
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A. Definitions
Solute - KMnO4 Solvent - H2O
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SolutionsSolution – a mixture that has the same
composition throughout the mix.Remember the difference between a
mixture and a compound.• Compounds have a fixed composition
throughout.• Mixtures can have a variable
composition throughout.
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Solubility – The maximum amount of solute that can be dissolved in the solvent at a given temperature.
A. Definitions
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B. Types of SolutionsSaturated solutions – maximum amount of solute at a given temperature.
Unsaturated solutions – less than the maximum amount of solute at a given temperature.
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Supersaturated solutions – more than the maximum amount of solute at a given temperature; unstable.
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B. Types of Solutions
SATURATED SOLUTION
no more solute dissolves
UNSATURATED SOLUTIONmore solute dissolves
SUPERSATURATED SOLUTION
becomes unstable, crystals form
concentration
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C. Dissolving
Solvation• occurs at the surface of the solute• solvent particles surround solute
particles (+/- attraction)• solute particles are pulled into solution
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D. Rate of Dissolving
Solids dissolve faster...• more stirring
• small particle size(increased surface area)
• high temperature
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Rate of DissolvingTo increase rate of dissolving of SOLIDS: Heat it
Crush it
Stir it
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D. Rate of Dissolving
Gases dissolve faster...• no shaking or stirring
• high pressure
• low temperature
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To make a gas dissolve more quickly in a liquid: •Cool it
• Increase the pressure of the gas
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Ch. 8Solutions, Acids, & Bases
II. Concentration & Solubility
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A. Concentration
% by Volume• usually liquid in liquid• Ex: 10% juice = 10mL juice + 90mL water
% by Mass• usually solid in liquid• Ex: 20% NaCl = 20g NaCl + 80g water
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A. Concentration
Concentrated solution • large amount of solute
Dilute solution • small amount of solute
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B. Solubility
Solubility• maximum grams of solute that will
dissolve in 100 g of solvent at a given temperature
• varies with temperature• based on a saturated solution
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B. Solubility
Solids are more soluble at...• high temperatures
Gases are more soluble at...• low temperatures• high pressures
(Henry’s Law)
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C. Solubility Charts Reading Solubility Charts• If the number in the problem is EQUAL to
the value on the chart the solution is considered SATURATED
• If the number in the problem is LESS than the value on the chart the solution is considered UNSATURATED
• If the number in the problem is MORE than the value on the chart the solution is considered SUPER SATURATED
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C. Solubility Charts Solubility of Compounds in g/100g of Water at various Temperatures
Compound 0◦ C 20◦ C 60◦ C 100◦ C
Ammonium chloride 29.4 37.2 55.3 77.3Copper(II) sulfate 23.1 32.0 61.8 114Lead(II)chloride 0.67 1.0 1.94 3.2Potassium bromide 53.6 65.3 85.5 104Sodium chlorate 79.6 95.9 137 204
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Chart
1) How would you classify a solution of 65.3g of potassium bromide at 20ºC? _________
2) How would you classify a solution of 65.3g of potassium bromide at 60ºC? ____________
3) How would you classify a solution of 65.3g of potassium bromide at 0ºC? ______________
4) How would you classify a solution of 37g of ammonium chloride at 20ºC? ___________
5) How would you classify a solution of 2.5 g of lead (II) chloride at 20ºC? ______________
Answer Questions on your paper
Saturated
Unsaturated
Supersaturated
Unsaturated
Supersaturated
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D. Solubility Graphs
Solubility Curve• shows the
dependence of solubility on temperature
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Graph
6) How would you classify a solution of 80g of HCl at 20ºC? ____________
7) How would you classify a solution of 30g of KNO3 at 20ºC? __________
8) How would you classify a solution of 39g of NaCl at 100ºC? ________
9) How would you classify a solution of 80g of NaNO3 at 30ºC? __________
10)How would you classify a solution of 40g of KClO3 at 80ºC? __________
Supersaturated
Unsaturated
Saturated
Unsaturated
Unsaturated
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11)How many grams of solute would you need to form a saturated solution of NH4Cl at 50ºC? _____
12)How would you classify a solution of 20g of SO2 at 0ºC? ___________
13)How much KI would you need to form a saturated solution at 10ºC? _____
14)Which solid decreases in solubility as the temperature increases? _______
50 g
Unsaturated
135 g
Na2SO4