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Mixtures can be _ homogenous _ or __ heterogeneous __

Mixtures can be _ homogenous _ or __ heterogeneous __. A True Solution is __ homogenous ___ does not__ settle ____ out, is __ clear__ can_not ___ be filtered out. ( ex. Salt in water ) NaCl ( aq ) , air.

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Mixtures can be _ homogenous _ or __ heterogeneous __

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  1. Mixtures can be _homogenous_ or __heterogeneous__ A True Solution is __homogenous___does not__settle____ out, is __clear__ can_not___ be filtered out. (ex. Salt in water) NaCl(aq), air

  2. A suspension is __hetergeneous______ and __settles_____ __out__ over time (ex muddy water, Italian salad dressing)

  3. SOLUTION: any MIXTURE THAT’S homogeneous on a microscopic LEVEL Ex: Air: A gas solution ALLOY: a metal solution

  4. Metals arrange in an alternating pattern with Sea of mobile valence electrons gluing them together. Examples:brass (zinc + Copper) steel(iron + carbon)

  5. Characteristics of Solutions • Homogeneous mixtures (aq) • Clear • can have color or colorless • Do not settle upon standing • Cannot be separated by filter

  6. How to separate a solution • Evaorate • Chromatography: Separate particles in a soln by charge or mass. Water moves up the paper to separate out the colors charge or mass. • Distillation: separated by different boiling points. Ex water and alcohol (80c bpt of alcohol vs 100c bpt water)

  7. There are 2 Parts to a Solution 1.Solute:substance that are dissolved in a soln; usually a solid and a lesser quantity. 2. Solvent: The substance doing the dissolving. Usually a liquid and a greater quantity. Aqueous=H2O is the solvent Tincture= alcohol is the solvent

  8. HOW TO CHANGE THE RATE OF; OR SPEED UP THE DISSOLVING PROCESS 1.stir/shake the mixture. It brings fresh solute and solvent together. 2. Break Up up the mixture into smaller pieces greater surface area means faster dissolution. 3. Heat speeds up the rate of dissolution.

  9. Solubility • Solubility: a measure of how much solute will dissolve in a certain amount of solvent@ a given temperature. • soluble: will dissolve (miscible ex alcohol and water) • Insoluble: will not dissolve (immiscible ex oil and water) • Concentration: ratio of the amount of solute per amount of solvent

  10. TO INCREASE THE SOLUBILITY OF A SOLUTE IN A SOLVENT; HOW MUCH NOT HOW FAST • Nature OF SOLUTE AND SOLVENT, IONIC dissolves better in water “likes dissolve likes” 2. Heat USUALLY INCREASES SOLUBILITY EXCEPT IN THE CASE OF Gases (Heat decreases the solubility of a gas ex. Pop goes flat when warm) 3. Pressure: increases the solubility of a gas in a liquid. WHAT HAPPENS WHEN IONIC SUBSTANCES DISSOLVE IN WATER? ION-MOLECULE ATTRACTION.

  11. solubility & dissolving: “LIKES DISSOLVE LIKES” POLAR DISSOLVES(WATER) • Polar with polar(Ex sugar in water) 2. Ionic with Polar(Ex NaCl in water) NONPOLAR DISSOLVES(CARBON TETRACHLORIDE CCl4 • Nonpolar dissolves nonpolar (fats/grease/oils) Summary:

  12. Solubility Table F • Tells us what substances are soluble or Insoluble

  13. Match up the correct terms with definitions: 1.______solvent A. An example is muddy water 2._____tincture B. the substance that does the dissolving 3._____solution C. A sol in which alcohol is the solvent 4.______alloy D. the substance being dissolved 5._____solute E. homogeneous, clear and cannot be filtered 6. _____suspension F. this does not settle because particles are charged 7.______collid G. A sol which metals are made 8._______aqueous 9______. Miscible H. pour the liquid off leaving settled solids behind 10._____distillation I. separate particles by charges or mass 11._______decant J. cannot dissolved when mixed K. to purify at different boiling points 12.______chromatography L. soluble or they dissolve into each other 13._______immiscible M. liquid on the top is called this 14._______capillary action N. water is the solvent

  14. Concentration Parts per million Table T ppm=mass of solute x 1,000,000 mass of soln Ex 300.og of drinking water is found to have 38mg of lead. What’s the parts per million?

  15. 1. 0.003g of helium gas is dissolved in 200.0g water. What’s the ppm?

  16. 2. 365g of water has 23mg Au. What’s the ppm?

  17. 3. A 650.0g sample of hard water contains 101mg Ca. What’s the ppm?

  18. % mass or volume Table T %mass=mass of part x 100 mass of whole %volume= volume of part x 100 volume of whole

  19. Ex 30.g of phenolphthalein are added to 120g of water. Whats the % by mass?

  20. 1. 34 mL of alcohol is added to 179mL of water, What’s the % by volume?

  21. 2. 48.7 g of alcohol is added to 100.0mL of cold water what’s the %volume?

  22. Molarity Table T M=moles of solute liter of solution Unit is M not m

  23. Ex What is the molarity of an H2SO4 solution if 0.25L of the solution contains 0.75 moles of H2SO4?

  24. 1. What is the total number of moles of the solute H2SO4 needed to prepare 5.0L of a 2.0M solution of H2SO4 ?

  25. 2. What volume of a 2.0M solution is needed to provide 0.50 MolNaOH?

  26. 3. What is the molarity of a solution that has 85.0g of KCl in 400.0mL of solution?

  27. 4. What is the molarity of a solution that contains 40.g of NaOH in 0.50L of solution?

  28. 5 How much HCl must be added to 200.mL to make 4.6M solution?

  29. 6. How much KOH must be added to 3.5L to make 0.01M solution?

  30. Colligative Properties-depends on concentration or the # of particles of the solute. It raisesthe boiling point of a substance and lowers the freezing point of a substance Ex: adding a solute to solvent, such as ethylene glycol, antifreeze to a car radiator, does what to its boiling point?_____freezingpoint?_____ The amount or moles of particles in the solution is a direct relationship to the amount that the boiling point is raised and the freezing point lowered ex more particles means more effect

  31. Ex. Sugar molecules are molecular they do not come apart in water. Therefore 1 mole of sugar molecules= 1 mole of particles in solution(C12H22O11) 1 mole NaCl (ionic, salt) in water comes apart into 2 moles of pieces and therefore affects fpt and bpt twice as much 1 mole CaCl2(ionic salt) in water comes apart into 3 pieces and therefore 1 mole of it gives 3 Moles of pieces in solution. It affects the fpt and bpt by 3 times that of sugar!!!!!

  32. Which freezes at the lowest temp? • 1 mole of sugar in 500g water • 1 mole of sugar in 1000g water • 2 mole of sugar in 500g water • 2 mole of sugar in 1000g water Which has the highest bpt? a. NaCl B.C6H12O6 C. AgNO3 D. KF

  33. Practice quiz 1.A solute= copper (II) sulfate solvent=water 1b. Solute= water solvent=alcohol 2. Method to separate crude oil is fractional distillation 3. Miscible means? Soluble; two liquids mix. Ex alcohol & water 4 Speed up rate: heat, stir, increase surface area 5. Nature solute/solvent, heat, pressure (gases only)

  34. 6. Calcium carbonate=i silver chloride=I lithium bromide =s 7. A us b. us/sat c. ss 8. Increase pressure, decrease temp 9. .023g x 1,000,000=26.4ppm~26ppm 870 • 43g x 100 = 22.279~22% 193 • M=3.7=.627~ .63M 5.9

  35. 12 42g/58g=.72moles M= .72/.392=1.83M~1.8M 13. .25=x 3.2 x=.8~.80moles x 58g=46.4g~46g 14. 4.7=2.8 x x=.5957~.60L

  36. p.128 Reviewbook 24. moles= 116 KF=39+19+58 58 moles=2 M= 2/1.00=2 25. M=.75/.25 =3.0 26. M=moles of solute/L soln 2.0=moles 5.0 moles=10

  37. 27.M=mol/L 2.0=.50 x 2.0x=.50 X=.25L

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