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1 16.3 Colligative of Solutions > 16.3 Colligative of Solutions > CHEMISTRY & YOU Chapter 16 Solutions 16.1 of Solutions 16.2 Concentrations of Solutions 16.3 Colligative of Solutions 16.4 Calculations Involving Colligative Why do you need salt to make ice cream? Ice-cream makers know that if you add rock salt to ice, the mixture freezes at a few degrees below 0 C Colligative of Solutions > Describing Colligative 16.3 Colligative of Solutions > Describing Colligative Describing Colligative What are three colligative properties of solutions? Tea is not the same as pure water. Some of these differences in properties have little to do with the specific identity of the solute. Instead, they depend upon the mere presence of solute particles in the solution Colligative of Solutions > Describing Colligative 16.3 Colligative of Solutions > Describing Colligative A colligative property is a property of solutions that depends only upon the number of solute particles, not upon their identity. Three important colligative properties of solutions are vapor-pressure lowering freezing-point depression boiling-point elevation 5 6 1
2 16.3 Colligative of Solutions > Describing Colligative Vapor pressure is the pressure exerted by a vapor that is in dynamic equilibrium with its liquid in a closed system Colligative of Solutions > Describing Colligative Vapor pressure is the pressure exerted by a vapor that is in dynamic equilibrium with its liquid in a closed system. A solution that contains a solute that is nonvolatile (not easily vaporized) always has a lower vapor pressure than the pure solvent Colligative of Solutions > Describing Colligative 16.3 Colligative of Solutions > Describing Colligative Higher vapor pressure Lower vapor pressure Pure solvent Solvent particle Equilibrium is established between the liquid and vapor in a pure solvent. Solution containing nonvolatile solute Solute particle In a solution, solute particles reduce the number of solvent particles able to escape the liquid. Equilibrium is established at a lower vapor pressure Colligative of Solutions > Describing Colligative 16.3 Colligative of Solutions > Describing Colligative Three moles of sodium chloride dissolved in water produce 6 mol of particles because each formula unit of NaCl dissociates into two ions. 11 Three moles of calcium chloride dissolved in water produce 9 mol of particles because each formula unit of CaCl 2 dissociates into three ions. 12 2
3 16.3 Colligative of Solutions > Describing Colligative 16.3 Colligative of Solutions > Describing Colligative The decrease in a solution s vapor pressure is proportional to the number of particles the solute makes in solution. Three moles of glucose dissolved in water produce 3 mol of particles because glucose does not dissociate Colligative of Solutions > Describing Colligative Colligative of Solutions > Describing Colligative Which solution has the lowest vapor pressure? Which solution has the lowest vapor pressure? The vapor-pressure lowering caused by 0.1 mol of NaCl in 1000 g of water is twice that caused by 0.1 mol of glucose in the same quantity of water Colligative of Solutions > Describing Colligative Colligative of Solutions > Describing Colligative Which solution has the lowest vapor pressure? When a substance freezes, the particles of the solid take on an orderly pattern. In the same way, 0.1 mol of CaCl2 in 1000 g of water produces three times the vapor-pressure lowering as 0.1 mol of glucose in the same quantity of water
4 16.3 Colligative of Solutions > Describing Colligative When a substance freezes, the particles of the solid take on an orderly pattern. The presence of a solute in water disrupts the formation of this pattern Colligative of Solutions > Describing Colligative When a substance freezes, the particles of the solid take on an orderly pattern. The presence of a solute in water disrupts the formation of this pattern. As a result, more kinetic energy must be withdrawn from a solution than from the pure solvent to cause the solution to solidify Colligative of Solutions > Describing Colligative The freezing point of a solution is lower than the freezing point of the pure solvent Colligative of Solutions > Describing Colligative The freezing point of a solution is lower than the freezing point of the pure solvent. The difference in temperature between the freezing point of a solution and the freezing point of the pure solvent is called the freezing-point depression Colligative of Solutions > Describing Colligative Freezing-point depression is another colligative property. The magnitude of the freezing-point depression is proportional to the number of solute particles dissolved in the solvent and does not depend upon their identity Colligative of Solutions > Describing Colligative The freezing-point depression of aqueous solutions plays an important role in helping keep travelers safe in cold, icy weather
5 16.3 Colligative of Solutions > Describing Colligative The freezing-point depression of aqueous solutions plays an important role in helping keep travelers safe in cold, icy weather. The truck spreads a layer of salt on the icy road to make the ice melt. The melted ice forms a solution with a lower freezing point than that of pure water Colligative of Solutions > Describing Colligative The boiling point of a substance is the temperature at which the vapor pressure of the liquid phase equals atmospheric pressure Colligative of Solutions > Describing Colligative The boiling point of a substance is the temperature at which the vapor pressure of the liquid phase equals atmospheric pressure. Adding a nonvolatile solute to a liquid solvent decreases the vapor pressure of the solvent Colligative of Solutions > Describing Colligative The boiling point of a substance is the temperature at which the vapor pressure of the liquid phase equals the atmospheric pressure. Adding a nonvolatile solute to a liquid solvent decreases the vapor pressure of the solvent. Because of the decrease in vapor pressure, additional kinetic energy must be added to raise the vapor pressure of the liquid phase of the solution to atmospheric pressure and initiate boiling Colligative of Solutions > Describing Colligative The boiling point of a solution is higher than the boiling point of the pure solvent Colligative of Solutions > Describing Colligative The boiling point of a solution is higher than the boiling point of the pure solvent. The difference in temperature between the boiling point of a solution and the boiling point of the pure solvent is the boiling-point elevation
6 16.3 Colligative of Solutions > Describing Colligative The fluid circulating through a car s cooling system is a solution of water and ethylene glycol, or antifreeze. The antifreeze doesn t just lower the freezing point of the water in the cooling system. It also elevates the boiling point, which helps protect the engine from overheating in the summer Colligative of Solutions > Describing Colligative Boiling-point elevation is a colligative property; it depends on the concentration of particles, not on their identity Colligative of Solutions > Describing Colligative 16.3 Colligative of Solutions > CHEMISTRY & YOU Boiling-point elevation is a colligative property; it depends on the concentration of particles, not on their identity. The magnitude of the boiling-point elevation is proportional to the number of solute particles dissolved in the solvent. The boiling point of water increases by C for every mole of particles that the solute forms when dissolved in 1000 g of water. Solutes other than NaCl could be used to produce the same freezingpoint depression in an ice-cream machine. What factors do you think make NaCl a good choice? Colligative of Solutions > CHEMISTRY & YOU 16.3 Colligative of Solutions > Solutes other than NaCl could be used to produce the same freezingpoint depression in an ice-cream machine. What factors do you think make NaCl a good choice? NaCl, or rock salt, is readily available, inexpensive, and nontoxic. It is an ionic compound. It produces twice the freezing-point depression of a molecular solid such as sucrose, or table sugar. You have 500 ml of 1M solutions of NaCl, Na 2 SO 4, Na 3 PO 4, and Al 2 (SO 4 ) 3. Which solution will have the highest boiling point? A. NaCl(aq) B. Na 2 SO 4 (aq) C. Na 3 PO 4 (aq) D. Al 2 (SO 4 ) 3 (aq)
7 16.3 Colligative of Solutions > 16.3 Colligative of Solutions > Key Concepts You have 500 ml of 1M solutions of NaCl, Na 2 SO 4, Na 3 PO 4, and Al 2 (SO 4 ) 3. Which solution will have the highest boiling point? A. NaCl(aq) B. Na 2 SO 4 (aq) C. Na 3 PO 4 (aq) D. Al 2 (SO 4 ) 3 (aq) Colligative properties of solutions include vapor-pressure lowering, freezing-point depression, and boiling-point elevation Colligative of Solutions > Glossary Terms 16.3 Colligative of Solutions > Glossary Terms colligative property: a property of a solution that depends only upon the number of solute particles, and not upon their identities; boilingpoint elevation, freezing-point depression, and vapor-pressure lowering are colligative properties freezing-point depression: the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent boiling-point elevation: the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent Colligative of Solutions > BIG IDEA 16.3 Colligative of Solutions > The Mole and Quantifying Matter Solubility, miscibility, concentration, and colligative properties are used to describe and characterize solutions. END OF
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