properties of solutions

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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 Presentation

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Page 1: Properties of Solutions

Properties of Solutions

Page 2: 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.

Page 3: Properties of Solutions

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.

Page 4: Properties of Solutions

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.

Page 5: Properties of Solutions

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.

Page 6: Properties of Solutions

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.

Page 7: Properties of Solutions

Endothermic vs. Exothermic

Page 8: Properties of Solutions

Instant Ice Pack

Ammonium nitrate instant ice pack are often used to treat athletic injuries.

Page 9: Properties of Solutions

Student, Beware!

Just because a substance disappears when it comes in contact with a solvent, it doesn’t mean the substance dissolved.

Page 10: Properties of Solutions

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.

Page 11: Properties of Solutions

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.

Page 12: Properties of Solutions

Factors Affecting Solubility

The more similar the intermolecular attractions, the more likely one substance is to be soluble in another.

Page 13: Properties of Solutions

Factors Affecting Solubility

Glucose (which has hydrogen bonding) is very soluble in water, while cyclohexane (which only has dispersion forces) is not.

Page 14: Properties of Solutions

Factors Affecting Solubility

• Vitamin A is soluble in nonpolar compounds (like fats).

• Vitamin C is soluble in water.

Page 15: Properties of Solutions

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.

Page 16: Properties of Solutions

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.

Page 17: Properties of Solutions

Temperature

Generally, the solubility of solid solutes in liquid solvents increases with increasing temperature.

Page 18: Properties of Solutions

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.

Page 19: Properties of Solutions

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

Page 20: Properties of Solutions

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.

Page 21: Properties of Solutions

Vapor Pressure

Therefore, the vapor pressure of a solution is lower than that of the pure solvent.

Page 22: Properties of Solutions

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.

Page 23: Properties of Solutions

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.

Page 24: Properties of Solutions

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.

Page 25: Properties of Solutions

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.

Page 26: Properties of Solutions

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

Page 27: Properties of Solutions

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

Page 28: Properties of Solutions

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

Page 29: Properties of Solutions

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.

Page 30: Properties of Solutions

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).

Page 31: Properties of Solutions

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.

Page 32: Properties of Solutions

The average osmotic pressure of blood is 7.7 atm at 25 °C. What molarity of glucose (C6H12O6) will be isotonic with blood?

Page 33: Properties of Solutions

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.

Page 34: Properties of Solutions

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.

Page 35: Properties of Solutions

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.

Page 36: Properties of Solutions

van’t Hoff Factor

One mole of NaCl in water does not really give rise to two moles of ions.

Page 37: Properties of Solutions

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.

Page 38: Properties of Solutions

van’t Hoff Factor

• Reassociation is more likely at higher concentration.

• Therefore, the number of particles present is concentration-dependent.

Page 39: Properties of Solutions

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

Page 40: Properties of Solutions

How to Calculate van’t Hoff factor i

Page 41: Properties of Solutions

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