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Solutions

Solutions. Chapters 13 & 14. What is a solution?. Homogeneous mixture Solute – what gets dissolved Solvent – what does the dissolving Suspensions – solute particles are so big they settle out (must be shaken) Colloid – solute particles are large, but do not settle

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Solutions

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  1. Solutions Chapters 13 & 14

  2. What is a solution? • Homogeneous mixture • Solute – what gets dissolved • Solvent – what does the dissolving • Suspensions – solute particles are so big they settle out (must be shaken) • Colloid – solute particles are large, but do not settle • Refer to table 13-1 for solution types (p. 396)

  3. Electrolytes • Solutions that conduct electricity • Solutes must ionize (break apart into ions when dissolved) ex. NaCl • Neutral solutes are nonelectrolytes, ex. sugar

  4. The solution process • Heat, motion, size of solute – help solid dissolve in a liquid (think kool-aid) • Lack of heat, lack of motion and increase in pressure – help gas dissolve in a liquid (think soda pop)

  5. Saturation • Saturated – solution contains the most solute it can hold at a particular temperature • Unsaturated – solution can hold more solute • Supersaturated – solution is heated, maximum solute is dissolved and then solution is cooled so that excess solute remains dissolved

  6. Dissolving Rules • Like dissolves like • Polar solvents will ONLY dissolve polar solutes • Nonpolar solvents will ONLY dissolve nonpolar solutes

  7. Molarity • Number of moles of solute per liter of solvent (mol/L) • Need to know molar mass of solute and amount of solvent in liters • Convert mass of solute to moles of solute using molar mass. Then divide by volume amount.

  8. Example You have 3.50 L of solution that contains 90.0 g of NaCl. What is the molarity?

  9. Example You need to make 500. mL of 4.00 molar H2SO4. How much sulfuric acid do you need?

  10. Dissociation • When an ionic compound is dissolved it separates into ions • Remember an ionic compound is made of a metal bonded to a nonmetal CaCl2 Ca+2 + 2Cl- 

  11. Precipitates • Insoluble solid that is formed when two liquids react in a double replacement reaction • Solubility rules on p. 427 (do not need to memorize, but do need to know how to use)

  12. Net Ionic Equations (NH4)2S + Cd(NO3)2 2 NH4NO3 + CdS 2 NH4+ + S-2 + Cd+2 + 2 NO3-  2 NH4+ + 2 NO3- + CdS S-2 + Cd+2  CdS Spectator Ions: NH4+ & NO3-

  13. Colligative Properties • Properties that depend on the amount of solute present • Dissolved solutes lower the freezing point and raise the boiling point of water

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