Unit 4 Review - Unit 4 notes PDF

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Unit 4 notes...

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Solutions and Solubility Solution: 2+ substances in a homogenous mixture Homogenous Mixture: Cannot see individual parts Solute: Smaller amount Solvent: Larger amount Miscible: two liquids that dissolve in each other. “Mixable” Immiscible: two liquids that do not dissolve in each other Amalgam: Liquid dissolves in solid Alloy: Solid dissolves in solid Solubility: Ability of a substance to dissolve Saturation: Maximum amount of solute that can dissolve in solvent is reached (saturation point). Unsaturated Solutions: Solution has not reached saturation point. Factors Affecting Solubility ➢ Temperature: Higher energy of particles leads to more interaction ➢ Agitation: Stirring solution allows more interaction ➢ Particle Size: Smaller pieces increases surface area for more interactions Why do some things dissolve? ➢ Depends on attractive forces of the solute. Larger ionic charges lead to greater attractions. Ex. PO43- vs. Cl➢ Attractive forces of the solvent ➢ Attractive forces between solute and solvent. Ex. water is a good solvent as it is polar. So ionic compounds can dissolve as they are attracted to different ends of water. ➢ General Rule: “ Like dissolves like” ○ Polar dissolves in polar. Nonpolar in nonpolar. Acids and bases: ➢ Acids break down to form H+ , bases break down to form OH- ➢ Acid is a proton donor, base is a proton acceptor. ➢ Strong acids/bases have complete dissociation, weak acids/bases have partial....