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Putting it All Together!

Putting it All Together!. Physical Properties. Phases of Matter. Solids. SOLIDS : Retains a fixed volume Rigid particles are locked into place Not easily compressible Little free space between particles Does not flow easily Particles are tightly packed, usually in a regular pattern

maisie-barnett
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Putting it All Together!

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  1. Putting it All Together!

  2. Physical Properties Phases of Matter Solids • SOLIDS: • Retains a fixed volume • Rigid particles are locked into place • Not easily compressible • Little free space between particles • Does not flow easily • Particles are tightly packed, usually in a regular pattern • Solids vibrate (jiggle), but generally do not move from place to place

  3. Physical Properties Phases of Matter Solids Liquids • LIQUIDS: • Assumes the shape of the part of the container it occupies • Particles can move/slide past one another • Not easily compressible • Little free spaces between particles • Flows easily • Particles are close together with no regular arrangement • Particles vibrate, move about and slide past each other

  4. Physical Properties Phases of Matter Solids Liquids Gases • GASES: • Assumes the shape of the entire container • Particles can move past one another • Compressible • Lots of space between particles • Flows easily • Particles are well separated with no regular arrangement • Gas particles vibrate and move freely at high speeds

  5. Freezing Point Physical Properties Phases of Matter Solids Liquids Gases • Freezing Point: • Liquid  Solid • Liquid Water  Frozen Water

  6. Freezing Point Physical Properties Phases of Matter Solids Liquids Melting Point Gases • Melting Point: • Solid  Liquid • Frozen Water  Liquid Water

  7. Freezing Point Physical Properties Phases of Matter Solids Liquids Melting Point Gases Freezing Point and Melting Point occur at the same temperature! The substance is approaching from opposite ways!

  8. Solubility Curve for KNO3 50 45 40 35 30 g KNO3 / 100 g H2O 25 20 15 10 5 30 40 50 60 80 90 10 20 70 100 Temperature (oC) Physical Properties • Unsaturated Solutions: • More solute can be dissolved in solvent • Area underneath the curve Solubility UNSATURATED Unsaturated

  9. Solubility Curve for KNO3 50 45 40 35 30 g KNO3 / 100 g H2O 25 20 15 10 5 30 40 50 60 80 90 10 20 70 100 Temperature (oC) • Saturated Solutions: • Perfect ratio of solute to solvent • No more solute can be dissolved in the solvent Physical Properties Solubility SATURATED Unsaturated Saturated

  10. Solubility Curve for KNO3 50 45 40 35 30 g KNO3 / 100 g H2O 25 20 15 10 5 30 40 50 60 80 90 10 20 70 100 Temperature (oC) • Super Saturated Solutions: • More solute is in solution than the solvent can dissolve • Area above the curve Physical Properties Solubility SUPER SATURATED Super Saturated Unsaturated Saturated

  11. Freezing Point Physical Properties Phases of Matter Solids Liquids Melting Point Gases Solubility Concentration Super Saturated Unsaturated Saturated

  12. Freezing Point Physical Properties Phases of Matter Solids Liquids Melting Point Gases Solubility Concentration ppb ppm Molarity Super Saturated % Concentration Molality Unsaturated Saturated

  13. Molarity Molarity (M) = moles of solute liters of solution • The number of moles of solute in 1 liter Example: What is the molarity of a solution in which 58 g of NaCl are dissolved in in 1 L of solution? Step #1: Convert g NaCl to moles NaCl Step #2: Convert to Liters (if needed) Already in LITERS!! Step #3: Divide! Back to Chart

  14. Molality • The number of moles of solute per kilogram of solvent Molality = moles of solute kilograms of solvent Example: What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 kg of water? Step #1: Convert to moles ALREADY IN MOLES!!! Step #2: Convert to kilograms (1000g = 1kg) ALREADY IN KILOGRAMS Step #3: Divide! Back to Chart

  15. Percent Concentration • Percent of solute to solvent. Want the units in g/100ml water Example: You make a solution with 5.1 g of NaCl and mix it with 150 mL of water. What is the percent concentration of this solution? Mass of Solute: 5.1 g Volume of Solvent: 150 mL Back to Chart

  16. ppm • Parts per MILLION!! • Used to represent a very dilute solution (low concentration) mass solute X 106 = ppm mass H2O Example: Suppose a 155.3 g sample of pond water is found to have 1.7 x 10-4 g of Ca3(PO4)2. What is the concentration in ppm? Mass of Solute: 1.7 x 10-4g Mass of Solvent: 155.3 g (assume density of pond water=1) Back to Chart

  17. ppb • Parts per BILLION!!! • Used to represent an even diluter solution! mass solute X 109 = ppm mass H2O Example: Suppose a 155.3 g sample of pond water is found to have 1.7 x 10-4 g of Ca3(PO4)2. What is the concentration in ppb? Mass of Solute: 1.7 x 10-4g Mass of Solvent: 155.3 g (assume density of pond water=1) Back to Chart

  18. Freezing Point Physical Properties Phases of Matter Solids Liquids Melting Point Gases Solubility Concentration ppb ppm Molarity Super Saturated % Concentration Molality Unsaturated Saturated

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