Chapter 13.2 : The Solution Process
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1) Three factors that affect the rate of dissolution of a solid in a liquid are increasing the surface area of the solute, agitating the solution, and heating the solvent. 2) There are three types of solutions: saturated contains the maximum amount of dissolved solute, unsaturated contains less than saturated, and supersaturated contains more than saturated. 3) Whether a substance dissolves depends on if it is polar or nonpolar - polar substances dissolve in polar solvents and nonpolar dissolve in nonpolar.
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Solution chemistry notes
This document provides information on solution chemistry and concepts including:
- Definitions of key terms like solution, solute, and solvent
- The process of dissolution where solvent molecules pull apart solute molecules
- How saturated, supersaturated and concentrated solutions are classified
- Factors that influence solubility like temperature, pressure and nature of solute
- Colligative properties of solutions like vapor pressure lowering, freezing point depression and boiling point elevation that depend on amount of solute.
- Equations to calculate values like molarity, molality and mole fraction in solutions.
Properties of solutions
1) Solutions are homogeneous mixtures of two or more substances, where the solute is dispersed uniformly throughout the solvent.
2) For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome those within the pure substances.
3) The energetics of dissolving involves breaking interactions within the pure substances and forming new interactions between solute and solvent particles. Even endothermic processes can occur spontaneously if they increase the disorder or entropy of the system.
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- The process of dissolving a solute involves the solute and solvent particles separating and the solvent surrounding and solvating the solute particles. This process can be endothermic or exothermic.
- Solubility depends on properties of the solute and solvent as well as temperature and pressure. Solubility curves show how solubility changes with temperature. Saturation occurs when a solution contains the maximum amount of solute possible.
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This document provides information on solution chemistry and concepts including:
- Definitions of key terms like solution, solute, and solvent
- The process of dissolution where solvent molecules pull apart solute molecules
- How saturated, supersaturated and concentrated solutions are classified
- Factors that influence solubility like temperature, pressure and nature of solute
- Colligative properties of solutions like vapor pressure lowering, freezing point depression and boiling point elevation that depend on amount of solute.
- Equations to calculate values like molarity, molality and mole fraction in solutions.
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* Given: 0.85 g of gas dissolves in 1 L of water at 4 atm
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* P2 = 1 atm
* S1 = 0.85 g
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Chapter 13.2 : The Solution Process
- 1. The solution process Chapter 13.2 Objectives : List and explain three factors that affect the rate at which a solid solute dissolves in a liquid solvent. Explain solution equilibrium, and distinguish among saturated, unsaturated, and supersaturated solutions. Explain the meaning of “like dissolves like” in terms of polar and nonpolar substances. List the three interactions that contribute to the heat of solution, and explain what causes dissolution to be exothermic or endothermic. Compare the effects of temperature and pressure on solubility.
- 2. Factors Affecting the Rate of Dissolution Increasing the surface area of the solute Sugar cube will dissolve slower than ground up sugar Agitating a solution Stir your iced tea and the sugar will dissolve faster. Heating a Solvent Sugar dissolves faster in hot tea
- 3. Solubility Solution equilibrium Physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates. Saturated solution Solution that contains the maximum amount of dissolved solute Example: At 20oC, 35.9 g of NaCl is the maximum amount that will dissolve in 100. g of water Unsaturated solution Solution that contains less solute than a saturated solution under existing conditions
- 4. Supersaturated solutions Solution that contains more dissolved solute than a saturated solution contains under the same conditions. Disturbing solution will cause rapid crystallization Video demonstration 1 Video demonstration 2 Solvent : water Solute : glucose
- 5. Solute-Solvent Interactions “Like dissolves Like” Polar will dissolve polar Nonpolar will dissolve nonpolar Polar will NOT dissolve in nonpolar Dissolving ionic compounds in aqueous solutions Hydration : solution process with water as the solvent CuSO4•5H2O - hydrate Crystalline compounds that incorporate water molecules
- 6. Nonpolar solvents Carbon tetrachloride and toluene Substances similar to oil Liquid solutes and solvents Immiscible LIQUID solutes and solvents that are not soluble in each other Example: oil and vinegar Miscible Liquids that dissolve freely in one another in any proportions Ethanol and water
- 7. Effects of Pressure on Solubility Increase in pressure – increases gas solubilities in liquids gas + solvent solution Henry’s Law Solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid. Effervescence Rapid escape of a gas from a liquid in which it is dissolved Mentos demo
- 8. Effects of Temperature on Solubility For gaseoussolutes Increase in temperature Decrease in solubility For solid solutes Increase in temperature Increase in solubility