Solutions

_______________ 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 ______ dissolved in _______ In other types Solute is substance in ___________ amount ______ is the substance that was a different phase than the resulting solution

Similar Mixtures ___________ Homogenous appearance Medium particle size Particles will not settle Particles will disperse light (tyndall effect) For example: Foam, fog, milk ____________ Heterogeneous appearance Large particle size Particles will settle over time For example: Italian salad dressing

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 ___________ and ____________ solutions Really a question of _______________ dissolves

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

Gas-Liquid Solutions Solubility ______________ with higher partial pressures of the gas over a liquid Solubility _____________ with increasing temperature

Liquid-Liquid Solutions Some liquids are ______________ 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

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

Solid-Liquid Solution _________________ Compound broken into ions when dissolves Solution can carry electrical current _________________ IMF’s (but not molecules) are broken when dissolves No electrical current can be carried

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

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

V’ant Hoff Factor Represented by ____ Equals the number of particles created from each solute when dissolved Nonelectrolytes ________ C 12 H 22 O 12 (s)  C 12 H 22 O 12 (aq) * _______________ Electrolytes ________________ from ionization or dissociation NaCl (s)  Na + (aq) + Cl - (aq) * _________________ MgCl 2 (s)  Mg +2 (aq) + Cl - (aq) * _________________

Solvation Process of ____________ Also called hydration when solvent in _________ 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

Saturation An amount of solvent can only hold a certain amount of solute Amount depends on ______________ Amount also depends on ________________ Usually ____________ temperature _____________ 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

Solubility Curves Graph depicting the solubility of substances at different temperatures

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 %

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

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

ppm, ppb, and ppt Mass/Volume Used for very __________ solutions ppm = parts per million one part solute in a million parts solution Roughly equal to one person in a large city ppb = parts per billion one part solute in a billion parts solution Roughly equal to one person in India ppt = parts per trillion One part solute in a trillion parts solution Not exact terms but we will use ppm = 1 mg/L ppb = 1  g/L ppt = 1 ng/L

Mole Fraction Mol/Mol Equation Mole Fraction (  ) = moles of component / moles of all components No units All of the mole fractions of a solution add up to ________

Mass Percent Mass/Mass Equation Mass Percent = (mass of solute/ mass of solution) x 100

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

Vapor Pressure Vapor pressure of solvent in solution is _______ than vapor pressure of pure solvent Equation P solv =  solv P° solv P solv = pressure of solvent vapor over solution  solv = mole fraction of solvent in solution P° solv = pressure of solvent vapor over pure solvent

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 °C kg/mol

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

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

Osmotic Pressure Pressure that must be applied in order to stop __________

Osmosis Movement of water from an area of ____________ concentration to an area of ______________ concentration Occurs across semipermeable membranes (cell membranes)

Calculating Osmotic Pressure  = iMRT  = osmotic pressure (will have pressure units) i = V’ant Hoff factor M = Molarity of solution R = gas constant ( atm L mol -1 K -1 ) T = temperature in K