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![Page 1: Solutions. Review of Properties of Water Is a polar molecule Has extensive hydrogen bonding Many of water’s unusual properties are due to hydrogen bonding.](https://reader035.fdocuments.us/reader035/viewer/2022062312/551b4e00550346d41a8b5e2d/html5/thumbnails/1.jpg)
SolutionsSolutions
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Review of Properties of WaterReview of Properties of Water
Is a polar moleculeHas extensive
hydrogen bondingMany of water’s
unusual properties are due to hydrogen bonding
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How aqueous solutions are formedHow aqueous solutions are formed
Solvation
The process by which cations and anions become surrounded by water molecules
Occurs at the surface of the solute
Solvation Process
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16.1 Solution Formation16.1 Solution Formation
The nature of the solvent and solute determine solution formations
“Like dissolves like”◦Polar dissolves polar/ionic◦Non-polar dissolves non-polar
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Rate of solution formationRate of solution formation
Temperature◦Kinetic energy of solvent & solute
Amount of surface area exposed to solvent◦Particle size◦Stirring
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Surface Area and Particle SizeSurface Area and Particle Size
6 m2 x 8 = 48 m2 24 m2
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SolubilitySolubility
Expresses the degree to which a substance dissolves
Usually expressed in g solute/100 g solvent
Examples◦Solubility of KNO3 is 85 g/100 g water at 20°C
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Important Factors Affecting Important Factors Affecting SolubilitySolubility
Temperature◦For most solid solutes, solubility increases with
increasing temperature◦↑ T → ↑ Solubility◦For gases, solubility decreases with increasing
temperature◦↑ T → ↓ Solubility
Pressure◦No effect on solubility of solids◦For gases, ↑ P → ↑ Solubility
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Solubility and TemperatureSolubility and Temperature
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Solubility and TemperatureSolubility and Temperature
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Types of solutionsTypes of solutions
Saturated◦Contain maximum amount of solute at a given
temperature◦Dissolved solute in equilibrium with undissolved◦All solutions are saturated solutions on a solubility
curveUnsaturated
◦Contain less than maximum solute◦No undissolved solute present
Supersaturated◦Contain more than the maximum amount of solute
at a given temperature◦How could this happen?
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Henry’s Law and Solubility of Henry’s Law and Solubility of GasesGases
At a given temperature, solubility of a gas is directly proportional to the partial pressure of the gas
2
2
1
1
P
S
P
SxPkS
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Saturated, Unsaturated and Saturated, Unsaturated and Supersaturated solutionsSupersaturated solutions
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16.2 Concentrations of Solutions16.2 Concentrations of Solutions
Concentration tells how much solute is dissolved in an amount of solution or solvent
Many ways of expressing concentrationMost common is molarity (M)Concentrated solutions have much soluteDilute solutions have little solute
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MolarityMolarity
Is the moles of solute per liter of solution
What is the molarity of a solution containing 0.9 g NaCl dissolved in 100 mL of solution?
L
mol
solution liters
solute molesM
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MolarityMolarity
To make a 0.5-molar (0.5M) solution, first add 0.5 mol of solute to a 1-L volumetric flask half filled with distilled water.
16.2
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MolarityMolarity
Swirl the flask carefully to dissolve the solute.
16.2
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MolarityMolarity
Fill the flask with water exactly to the 1-L mark.
16.2
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Molarity ProblemMolarity Problem
What mass of CaCl2 is needed to make 0.50 L of 2.5 M solution?
138.6 gExplain how to prepare the solution.
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Making DilutionsMaking Dilutions
The total number of moles of solute remains unchanged upon dilution, so you can write this equation.
M1 and V1 are the molarity and volume of the initial solution, and M2 and V2 are the molarity and volume of the diluted solution.
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Making DilutionsMaking Dilutions
Making a Dilute Solution
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Percent ConcentrationPercent Concentration
Sometimes concentration is expressed as a percent
Example: the label on a bottle of bleach reads 8.25% sodium hypchlorite (NaClO)
What does this mean?
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Percent ConcentrationPercent Concentration
Volume percent means
What is the V% when 15.0 mL ethanol is dissolved in 65.0 mL water?
18.8%, why not 23.1%
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Percent ConcentrationPercent Concentration
Mass percent means
What is the m% when 2.50 g of KCl is dissolved in 75.0 mL of water?
3.23%, why not 3.33%
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Colligative Properties of SolutionsColligative Properties of Solutions
Solutes change the properties of solventsColligative properties depend upon the
concentration of solute particles in solution
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Important colligative propertiesImportant colligative properties
Vapor pressure loweringBoiling point elevationFreezing point depression
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Vapor Pressure LoweringVapor Pressure Lowering
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Colligative Properties and Number Colligative Properties and Number of Solute Particlesof Solute Particles
Colligative properties depend on the total moles of solute particles and not upon their identity
1 mol glucose 1 mol glucose◦(= 1 mol particles)
1 mol NaCl 1 mol Na+ + 1 mol Cl- ◦(= 2 mol of particles)
1 CaCl2 1 Ca 2+ + 2 Cl-
◦(= 3 mol particles)
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Colligative Properties and Number Colligative Properties and Number of Solute Particlesof Solute Particles
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Changes in Pvap, bp, fp are Changes in Pvap, bp, fp are proportional to the number of solute proportional to the number of solute particles dissolved in the solventparticles dissolved in the solvent