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SOLUTION CHEMISTRY

SOLUTION CHEMISTRY. PROPERTIES OF WATER. Water’s unique role in chemical and biological systems. Hydrogen Bonding. Water is polar! . Cohesion / Surface Tension. Properties of Water. Continued . . . Universal Solvent. Adhesion Density (Liquid & Solid States).

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SOLUTION CHEMISTRY

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  1. SOLUTION CHEMISTRY

  2. PROPERTIES OF WATER Water’s unique role in chemical and biological systems Hydrogen Bonding • Water is polar! Cohesion/ Surface Tension

  3. Properties of Water Continued . . . Universal Solvent Adhesion Density (Liquid & Solid States) The empty space between the Molecules lowers the overall mass For a given volume

  4. SOLUTIONS: Mixtures with properties throughout

  5. Solutions . . . Facts to remember • Substances that are capable of being dissolved are • called ________________________ . Substances that are incapable of being dissolved are called ____________________ • Dissolving medium in a solution is called the ______________ , and the substance being dissolved is called the _________________________ • NOT ALL SOLUTIONS ARE LIQUIDS • _________________________________ liquids are able to freely dissolve in one another • _____________________ liquids are not soluble in each other and form layers based on their _________________ immiscible and miscible are for _________________ solutions only soluble insoluble solvent solute Miscible immiscible densities liquid

  6. “Like Dissolves Like” polar Non-polar • Polar & Ionic solutes dissolve in __________ solvents. • Non-polar solutes dissolve in _____________ • Rate of Dissolution – How quick a solute dissolves • Solubility – amount of solute that dissolves at a specific temperature

  7. Solubility & Concentration Level of concentration gdsdf • Unsaturated . . . • Solution contains less dissolved solute than the maximum amount at a given temperature • *More can be dissolved* • Saturated . . . • Solution contains the maximum amount of dissolved solute at a given temperature • No more can be dissolved • Supersaturated . . . • Solution contains more than the maximum amount of solute at a given temperature. • Unstable – if disturbed, the excess solute will crystallize out of solution

  8. Solubility Curves Shows the dependence of solubility on temperature. Questions from page 3 of your video notes Any amount of solute below the line indicates the solution is unsaturated at a certain temperature. Any amount of solute above the line in which all of the solute has dissolved shows the solution is supersaturated If the amount of solute is above the line but has not all dissolved, the solution is saturated and the extra grams of solute have precipitated (settled) to the bottom. (# of grams precipitated = total # grams in solution - # of grams of a saturated solution at that temperature

  9. Electrolytes and Dissociation Many people know me as containing “electrolytes”… that just means I contain dissolved, dissociated ions! • A substance that dissolves in water to make a solution that can conduct electrical current • A. Any soluble, ionic compound is an electrolyte • B. Some highly polar covalent molecules, such as strong acids, are also electrolytes. • Questions to consider . . . • Is the substance ionic? (Metal bonded to a non-metal, or contains a polyatomic ion) • Is the substance soluble in water? (Can it be dissolved in water) • CaCl2 • H2SO4 • NaOH

  10. Dissociation Continued . . . Li3PO4 BaSO4 **Remember that the substance must be ionic AND soluble in Order for it to be considered an electrolyte.

  11. MOLARITY _________________ is the measure of the amount of solute in a given amount of solvent or solution. **As you increase molarity, the solution is more CONCENTRATED……low molarity means you have a dilute solution, and high molarity means you have a CONCENTRATED solution

  12. Molarity Examples

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