1. Solutions

2. ____________ mixtures Occur in each state of matter Gas mixed in gas (_______) Gas mixed in liquid (__________________) Liquid mixed in liquid (______________) Solid mixed in liquid (____________) Solid mixed in solid (___________________________) Composed of a solute mixed with solvent Terms used most commonly with solids dissolved in liquids In other types Solute is substance in _____________ amount Solute is the substance that was a different _____ than the resulting solution

3. Similar Mixtures Colloids ____________ appearance ____________ particle size Particles will not settle Particles will disperse light (tyndall effect) For example: Foam, fog, milk Suspensions __________ appearance ________ particle size Particles will settle over time For example: Italian salad dressing

4. Solubility Ability of a substance to dissolve within another substance Depends on ____________ being used Usually ______ dissolves _______ We often mean the solubility in __________ solutions Really only in question for liquid-liquid and solid-liquid solutions Really a question of _____________ dissolves

5. Gas-Gas Solutions Mix freely with each other Each gas acts on its own

6. Gas-Liquid Solutions Solubility ___________ with higher partial pressures of the gas over a liquid Solubility ___________ with increasing temperature

7. Liquid-Liquid Solutions Some liquids are immiscible Insoluble in each other Due to polarity of liquids (usually non-polar with polar) Miscible liquids Usually like with like Polar with polar Non-polar with non-polar

8. Solid-Solid Solutions Alloys ALLOYCOMPONENT METALS Bronzecopper, tin Brasscopper, zinc Steeliron, carbon, (various other metals) Sterling Silversilver, nickel, copper 14K Goldgold, copper, antimony Pewtertin, copper, antimony Soldertin, lead

9. Solid-Liquid Solution Electrolytes Compound broken into _____ when dissolves Solution can carry electrical current Nonelectrolytes IMF’s (but not molecules) are broken when dissolves No electrical current can be carried

10. Dissolving Nonelectrolytes Non-polar molecules Soluble in non-polar solvents Insoluble in polar solvents Polar molecules (or molecules with polar sections) Soluble in polar solvents Insoluble in non-polar solvents Do not break apart ____ mole of solid solute creates ____ mole of particles in solution

11. Dissolving Electrolytes Ionization Breaks a covalently bonded compound into ions Ions spread throughout solutions Dissociation Breaks ions in ionic bond apart Ions spread throughout solution Both processes create more particles in solution than were present in the solid solute

12. V’ant Hoff Factor Represented by ___ Equals the number of particles created from each solute when dissolved Nonelectrolytes i = ____ C 12 H 22 O 12 (s)  C 12 H 22 O 12 (aq) * 1 particle i = ___ Electrolytes i = # of ions created from ionization or dissociation NaCl (s)  Na + (aq) + Cl - (aq) * 2 particles i = ___ MgCl 2 (s)  Mg +2 (aq) + 2 Cl - (aq) * 3 particles i = ___

13. Solvation Process of ___________ Also called hydration when solvent is _________ Bonds or IMF’s between particles must be broken Energy is absorbed Solvent particles surround the solute particles and form new bonds or IMF’s Energy is released

14. Saturation An amount of solvent can only hold a certain amount of solute Amount depends on ________ Amount also depends on _____________ Usually increasing temperature increases solubility ______________ solution Amount of solute is below the amount that the solvent can hold _____________ solution Amount of solute is at the amount that the solvent can hold _______________ solution Amount of solute is above the amount that the solvent can hold Not common, made by carefully cooling a saturated solution

15. Solubility Curves Graph depicting the solubility of substances at different temperatures

16. Concentrations of Solutions Comparison of amount of solute in a solvent _______________ Dilute- small amount of solute compared to solvent Concentrated- large amount of solute ___________ Molarity Molality ppm, ppb, ppt Mole fraction Mass %

17. Molarity Mole/Volume Equation Molarity (M) = moles of solute / liters of solution (not solvent) * Amount must be in ________ * Volume must be in __________ Changes with temperature

18. Molality Mole/Mass Equation Molality (m) = moles of solute / mass of solvent * Amount must be in __________ * Mass must be in ____________ Does not change with temperature

19. Colligative Properties Properties of solutions that depend on the ________ of solute particles not the _________ of the solute Shift in Points Freezing point _________- solution freezes at a lower temperature than the pure solvent Boiling point ________- solution boils at a higher temperaure than the pure solvent Vapor Pressure Osmotic Pressure

20. Vapor Pressure Vapor pressure of solvent in solution is lower than vapor pressure of pure solvent

22. Variables in Point Shifts m- Molality of solution i- V’ant Hoff factor Constants K f Specific to solvent Shows the affect of solute on that solvent’s freezing point K f for water is 1.86 °C kg/mol K b Specific to solvent Shows the affect of solute on that solvent’s boiling point K b for water is 0.512 °C kg/mol

23. Freezing Point Depression Equation Δ T f = iK f m Gives change in freezing point Must subtract from pure solvent’s freezing point to find solution’s freezing point

24. Boiling Point Elevation Equation Δ T b = iK b m Gives change in boiling point Must add to pure solvent’s boiling point to find solution’s boiling point