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Solutions

Solutions. Definitions. Solution: homogeneous mixture of 2 or more substances in a single physical state Solute: the substance dissolved in the solution Solvent: the substance the solute is dissolved in. General Properties of Solutions. 1. solute particles in solutions are very small

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Solutions

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  1. Solutions

  2. Definitions • Solution: homogeneous mixture of 2 or more substances in a single physical state • Solute: the substance dissolved in the solution • Solvent: the substance the solute is dissolved in

  3. General Properties of Solutions • 1. solute particles in solutions are very small • 2. solute particles are evenly distributed throughout the solution • 3. particles in a solution will not separate under normal conditions

  4. Types of Solutions • Aqueous solutions: solutions with water as the solvent. • Electrolyte solutions: aqueous solutions of ionic compounds. Ionic compounds dissociate allowing for the solution to conduct an electrical charge • Nonelectrolyte solutions: aqueous solutions of molecular compounds. The solute does not dissociate.

  5. Solution Formation • When ionic compounds dissolve in water, they dissociate NaCl --> Na+ + Cl- • Each component has an attraction to a certain part of the water molecules

  6. Solubility Rules • Used to predict the solubility of ionic compounds. • Not all ionic compounds are soluble in water. • Some only dissolve partially and some not at all.

  7. Solubility Rules

  8. Precipitation reactions

  9. Precipitation Reactions • Generally reactants are soluble ionic compounds dissolved in water. • When mixed, one of the possible cations joins with one of the anions to produce a compound that is insoluble. • The insoluble compound falls out of solution as a precipitate.

  10. A solution of silver nitrate is reacted with a solution of potassium chloride. Write the complete balanced chemical equation with notations for state of matter. • Write the equation for the reaction of lead (II) nitrate with ammonium sulfide.

  11. Net Ionic Equations • Removes unused ions (spectator ions) from an equation. • Simpler form of a reaction • Examples: write net ionic equations for previous slide examples.

  12. Solution Concentration

  13. Mols of solute Liters of Solution M = Molarity (M) • Most common expression of solution concentration

  14. What is the molarity of a solution formed by mixing 38 grams of potassium hydroxide in enough water to make 250 mL of solution?

  15. If I have a 2.5 M sulfuric acid solution, how many liters of solution will be needed to obtain 70 grams of sulfuric acid? How many milliliters?

  16. Solution stoichiometry

  17. 37 mL of a 0.45 M silver nitrate solution are reacted with 3 grams of copper. What mass of silver will be produced from the reaction?

  18. 18 mL of 1.39M sodium iodide is combined with 83 mL of 0.25 M lead (II) nitrate. • Will a reaction occur? • If a reaction occurs, what mass of precipitate should be produced?

  19. What volume of 0.750 M Pb(NO3)2, in milliliters, is required to react completely with 1 L of 2.25 M NaCl?

  20. Changing the Concentration of a Solution (Diluting) M1V1 = M2V2

  21. What volume of 18 M sulfuric acid is needed to create 6 Liters of 3.25 M sulfuric acid?

  22. Describe how you would prepare 400 mL of a 3.75 M solution of nitric acid if given a supply of 14.3 M nitric acid.

  23. Describe how to prepare 500 mL of a 0.8 M solution of sodium hydroxide when provided with solid sodium hydroxide and distilled water.

  24. Saturation • Saturated: solution contains all possible solute under current conditions • Unsaturated: more solute can be dissolved • Supersaturated: solution contains solute past the saturation point for the current conditions

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