1 / 30

Solutions

Solutions. 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 (_________________________)

driscoll-mooney
Download Presentation

Solutions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Solutions

  2. 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

  3. 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

  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 ___________ and ____________ 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 ______________ • 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

  9. 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

  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 _______ 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

  12. V’ant Hoff Factor • Represented by ____ • Equals the number of particles created from each solute when dissolved • Nonelectrolytes ________ • C12H22O12(s)  C12H22O12 (aq) * _______________ • Electrolytes ________________ from ionization or dissociation • NaCl (s) Na+(aq) + Cl-(aq) * _________________ • MgCl2 (s) Mg+2(aq) + Cl-(aq) * _________________

  13. 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

  14. 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

  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. 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

  20. 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 ________

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

  22. 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

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

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

  25. Freezing Point Depression • Equation • ΔTf = iKfm • Gives change in freezing point • Must subtract from pure solvent’s freezing point to find solution’s freezing point

  26. Boiling Point Elevation • Equation • ΔTb = iKbm • Gives change in boiling point • Must add to pure solvent’s boiling point to find solution’s boiling point

  27. Osmotic Pressure • Pressure that must be applied in order to stop __________

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

  29. Calculating Osmotic Pressure •  = iMRT •  = osmotic pressure (will have pressure units) • i = V’ant Hoff factor • M = Molarity of solution • R = gas constant (0.08206 atm L mol-1 K-1) • T = temperature in K

More Related