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Solutions I

Solutions I. Characteristics. Solutions. Homogeneous mixture : has no visible boundaries because the components are mixed as individual atoms, ions, and molecules.

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Solutions I

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  1. Solutions I Characteristics CHM 1010 PGCC Barbara A. Gage

  2. Solutions • Homogeneous mixture : has no visible boundaries because the components are mixed as individual atoms, ions, and molecules. • Solution : A homogeneous mixture is also called a solution. Solutions in water are called aqueous solutions. Although we normally think of solutions as liquids, they can exist in all three physical states. CHM 1010 PGCC Barbara A. Gage

  3. Components… • Solute – substance that is dispersed or dissolved • Solvent – substance that facilitates the dispersing or dissolving • Entropy will generally make solution formation favorable! CHM 1010 PGCC Barbara A. Gage

  4. Solubility • Maximum amount of solute that dissolves in a given amount of solvent at a set temperature NH4Cl 37.2 g/100g H20 @20oC CHM 1010 PGCC Barbara A. Gage

  5. Factors Affecting Solubility • Nature of solute and solvent…IMFs “Like dissolves like” If the forces are similar the components will mix… CHM 1010 PGCC Barbara A. Gage

  6. Figure 13.1 The major types of intermolecular forces in solutions. CHM 1010 PGCC Barbara A. Gage

  7. water methanol A solution of methanol in water Figure 13.3 Like dissolves like: solubility of methanol in water. CHM 1010 PGCC Barbara A. Gage

  8. The dissolution of an ionic compound… Solvation Figure 4.2 CHM 1010 PGCC Barbara A. Gage

  9. Dissolution of a polar compound…Solvation The slightly charged ends of polar solute molecules are attracted to the polar ends of polar solvents. The molecules are surrounded by solute particles. The solute particles stay intact. CHM 1010 PGCC Barbara A. Gage

  10. To determine solubility, decide what the IMFs of the solute and solvent are first. CHM 1010 PGCC Barbara A. Gage

  11. PROBLEM: Predict which solvent will dissolve more of the given solute: PLAN: Consider the intermolecular forces which can exist between solute molecules and consider whether the solvent can provide such interactions and thereby substitute. (a) Methanol - NaCl is ionic and will form ion-dipoles with the -OH groups of both methanol and propanol. However, propanol is subject to the dispersion forces to a greater extent. (b) Water - Hexane has no dipoles to interact with the -OH groups in ethylene glycol. Water can H bond to the ethylene glycol. (c) Ethanol - Diethyl ether can interact through a dipole and dispersion forces. Ethanol can provide both while water would like to H bond. SAMPLE PROBLEM 13.1 Predicting Relative Solubilities of Substances (a) Sodium chloride in methanol (CH3OH) or in propanol (CH3CH2CH2OH) (b) Ethylene glycol (HOCH2CH2OH) in hexane (CH3CH2CH2CH2CH2CH3) or in water. (c) Diethyl ether (CH3CH2OCH2CH3) in water or in ethanol (CH3CH2OH) SOLUTION: CHM 1010 PGCC Barbara A. Gage

  12. Factors Affecting Solubility • Nature of solute and solvent…IMFs • Temperature As temperature increases, particle motions and interactions increase. CHM 1010 PGCC Barbara A. Gage

  13. Solubility Curves What is the general trend for solids? For gases? Why are they different? CHM 1010 PGCC Barbara A. Gage

  14. solute (aggregated) + heat solute (separated) DHsolute > 0 solvent (aggregated) + heat solvent (separated) DHsolvent > 0 solute (separated) + solvent (separated) solution + heat DHmix < 0 Heats of solution and solution cycles 1. Solute particles separate from each other - endothermic 2. Solvent particles separate from each other - endothermic 3. Solute and solvent particles mix - exothermic DHsoln = DHsolute + DHsolvent + DHmix CHM 1010 PGCC Barbara A. Gage

  15. Figure 13.4 Solution cycles and the enthalpy components of the heat of solution. Exothermic solution process Endothermic solution process CHM 1010 PGCC Barbara A. Gage

  16. Endo- and Exothermic Dissolvers • Endothermic dissolvers can be used to form chemical cold packs because the solvent (water) becomes cold as it provides energy for the dissolving process. • Exothermic dissolvers provide the basis for chemical hot packs since the energy released heats the solvent. CHM 1010 PGCC Barbara A. Gage

  17. Factors Affecting Solubility • Nature of solute and solvent…IMFs • Temperature • Molar Mass The larger the solute molecule the more solvent molecules are required to keep the solute in solution. Solvation shell of water molecules for Na+ (left) and a larger peptide (right) CHM 1010 PGCC Barbara A. Gage http://www.theochem.rub.de/~axel.kohlmeyer/research.html

  18. Factors Affecting Solubility • Temperature • Nature of solute and solvent…IMFs • Molar Mass The larger the molecule the more solvent molecules are required to keep the solute in solution. • Pressure (for gases only) CHM 1010 PGCC Barbara A. Gage

  19. The higher the pressure over the solution, the greater the solubility of the gas (Henry’s Law). The “bends”… CHM 1010 PGCC Barbara A. Gage

  20. Electrolytes • If a solute conducts electricity when dissolved it is called an electrolyte. • Solutes that dissolve but do not form ions form non-conducting solutions and are called non-electrolytes. • A solute that dissociates partially and conducts electricity on a limited basis is called a weak electrolyte. CHM 1010 PGCC Barbara A. Gage

  21. The electrical conductivity of ionic solutions. Figure 4.3 CHM 1010 PGCC Barbara A. Gage

  22. Colloids and Suspensions • When a solute is suspended in a solvent the result is a heterogeneous mixture that may appear homogeneous. Such mixtures are called colloids or colloidal suspensions. These generally do not settle in the short term. • Suspensions are heterogeneous mixtures that do settle in the short term. They require shaking before dispensing. CHM 1010 PGCC Barbara A. Gage

  23. Colloids and Suspensions • Both colloids and suspensions scatter light. A true solution will not scatter light because the dispersed solute particles are too small to affect the path of the light. Colloid True solution CHM 1010 PGCC Barbara A. Gage

  24. Types of Colloidal Suspensions CHM 1010 PGCC Barbara A. Gage

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