properties of solutions
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Properties of Solutions. Solutions. Solutions are homogeneous mixtures of two or more pure substances. In a solution, the solute is dispersed uniformly throughout the solvent . Solutions. - PowerPoint PPT PresentationTRANSCRIPT
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Properties of Solutions
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Solutions
• Solutions are homogeneous mixtures of two or more pure substances.
• In a solution, the solute is dispersed uniformly throughout the solvent.
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Solutions
The intermolecular forces between solute and solvent particles must be strong enough to compete with those between solute particles and those between solvent particles.
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How Does a Solution Form?
As a solution forms, the solvent pulls solute particles apart and surrounds, or solvates, them.
Dissolution of an ionic solid in water.
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How Does a Solution Form?
If an ionic salt is soluble in water, it is because the ion-dipole interactions are strong enough to overcome the lattice energy of the salt crystal.
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Energy Changes in Solution
• Simply put, three processes affect the energetics of solution:– separation of solute
particles,– separation of solvent
particles,– new interactions between
solute and solvent.
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Endothermic vs. Exothermic
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Instant Ice Pack
Ammonium nitrate instant ice pack are often used to treat athletic injuries.
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Student, Beware!
Just because a substance disappears when it comes in contact with a solvent, it doesn’t mean the substance dissolved.
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Student, Beware!
• Dissolution is a physical change — you can get back the original solute by evaporating the solvent.
• If you can’t, the substance didn’t dissolve, it reacted.
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Factors Affecting Solubility
• Chemists use the axiom “like dissolves like."– Polar substances tend to
dissolve in polar solvents.
– Nonpolar substances tend to dissolve in nonpolar solvents.
Nonpolar liquids tend to be insoluble in polar liquids.
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Factors Affecting Solubility
The more similar the intermolecular attractions, the more likely one substance is to be soluble in another.
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Factors Affecting Solubility
Glucose (which has hydrogen bonding) is very soluble in water, while cyclohexane (which only has dispersion forces) is not.
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Factors Affecting Solubility
• Vitamin A is soluble in nonpolar compounds (like fats).
• Vitamin C is soluble in water.
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Gases in Solution
• The solubility of liquids and solids does not change appreciably with pressure.
• The solubility of a gas in a liquid is directly proportional to its pressure.
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Henry’s Law
Sg = kPg where• Sg is the solubility of the
gas,• k is the Henry’s Law
constant for that gas in that solvent, and
• Pg is the partial pressure of the gas above the liquid.
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Temperature
Generally, the solubility of solid solutes in liquid solvents increases with increasing temperature.
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Temperature
• The opposite is true of gases.– Carbonated soft drinks
are more “bubbly” if stored in the refrigerator.
– Warm lakes have less O2 dissolved in them than cool lakes.
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Colligative Properties
• Changes in colligative properties depend only on the number of solute particles present, not on the identity of the solute particles.
• Among colligative properties are– Vapor pressure lowering – Boiling point elevation– Melting point depression– Osmotic pressure
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1- Vapor-Pressure Lowering
Because of solute-solvent intermolecular attraction, higher concentrations of nonvolatile solutes make it harder for solvent to escape to the vapor phase.
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Vapor Pressure
Therefore, the vapor pressure of a solution is lower than that of the pure solvent.
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Raoult’s Law
PA = XAPA
where– XA is the mole fraction of compound A, and
– PA is the normal vapor pressure of A at that temperature.
NOTE: This is one of those times when you want to make sure you have the vapor pressure of the solvent.
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Glycerin (C3H8O3) is a nonvolatile nonelectrolyte with a density of 1.26 g/mL at 25 °C. Calculate the vapor pressure at 25 °C of a solution made by adding 50.0 mL of glycerin to 500.0 mL of water. The vapor pressure of pure water at 25 °C is 23.8 torr, and its density is 1.00 g/mL.
The vapor pressure of the solution has been lowered by 0.6 torr relative to that of pure water.
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2- Boiling Point Elevation• The change in boiling point is proportional to the
molality of the solution:Tb = Kb m
where Kb is the molal boiling point elevation constant, a property of the solvent.
Tb is added to the normal boiling point of the solvent.
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3- Freezing Point Depression
Tb is subtracted from the normal boiling point of the solvent.
• The change in freezing point can be found similarly:Tf = Kf m
• Here Kf is the molal freezing point depression constant of the solvent.
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Boiling Point Elevation and Freezing Point Depression
Note that in both equations, T does not depend on what the solute is, but only on how many particles are dissolved.
Tb = Kb m
Tf = Kf m
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Automotive antifreeze consists of ethylene glycol, CH2(OH)CH2(OH), a nonvolatile nonelectrolyte. Calculate the boiling point and freezing point of a 25.0 mass % solution of ethylene glycol in water.
Moles of ethylene glycol = 250 g/62.1 g mol-1 = 4.03 mol
4.03 mol0.75 Kg
Molality = = 5.37 m
Tb = Kb m = (0.51 oC/m)(5.73 m) = 2.7 oC
Tf = Kf m = (1.86 oC/m)(5.73 m) = 10.0 oC
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Freezing point = (normal fp of solvent) - Tf
= 0 oC - 10 oC = -10 oC
Boling point = (normal bp of solvent) + Tb = 100 oC + 2.7 oC = 102.7 oC
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4- Osmotic Pressure
Osmosis• Some substances form semipermeable
membranes, allowing some smaller particles to pass through, but blocking other larger particles.
• In biological systems, most semipermeable membranes allow water to pass through, but solutes are not free to do so.
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Osmosis
In osmosis, there is net movement of solvent from the area of higher solvent concentration (lower solute concentration) to the are of lower solvent concentration (higher solute concentration).
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Osmotic Pressure
The pressure required to stop osmosis, known as osmotic pressure, , is
nV = ( )RT = MRT
where M is the molarity of the solution.
If the osmotic pressure is the same on both sides of a membrane (i.e., the concentrations are the same), the solutions are isotonic.
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The average osmotic pressure of blood is 7.7 atm at 25 °C. What molarity of glucose (C6H12O6) will be isotonic with blood?
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Using Colligative Properties to Determine Molar Mass
1. A 7.85 g sample of a compound with the empirical formula C5H4 is dissolved in 301 g of benzene. The freezing point of the solution is 1.05° C below that of pure benzene. What are the molar mass and molecular formula of this compound?
2. A solution is prepared by dissolving 35.0 g of hemoglobin (Hb) in enough water to make up 1 L in volume. If the osmotic pressure of the solution is found to be 10.0 mmHg at 25° C, calculate the molar mass of hemoglobin.
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Colligative Properties of Electrolytes
Since these properties depend on the number of particles dissolved, solutions of electrolytes (which dissociate in solution) should show greater changes than those of nonelectrolytes.
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Colligative Properties of Electrolytes
However, a 1M solution of NaCl does not show twice the change in freezing point that a 1M solution of methanol does.
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van’t Hoff Factor
One mole of NaCl in water does not really give rise to two moles of ions.
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van’t Hoff Factor
Some Na+ and Cl- reassociate for a short time and form of ion pairs.
so the true concentration of particles is somewhat less than two times the concentration of NaCl.
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van’t Hoff Factor
• Reassociation is more likely at higher concentration.
• Therefore, the number of particles present is concentration-dependent.
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van’t Hoff Factor
• We modify the previous equations by multiplying by the van’t Hoff factor, i.
Tf = Kf m i Tf = Kf m i = iMRT
The vant’t Hoff Factor of 0.100 m for Electrolyte Solutions at 25° CElectrolyte i (Measured) i (Calculated)Sucrose 1.0 1NaCl 1.87 2K2SO4 2.32 3MgSO4 1.21 2
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How to Calculate van’t Hoff factor i
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The osmotic pressure of a 0.010 M potassium iodide (KI) solution at 25 °C is 0.465 atm. Calculate the van’t Hoff factor for KI at this concentration.
Measured Osmotic pressure (π) is 0.465 atm
Calculated Osmotic pressure (π) :π = MRT = 0.010 X 0.0821 X 298 = 0.245 atm