SOLUBILITY 13.3
IONIC COMPOUNDS <ul><li>When ionic compounds dissolve in water they: </li></ul><ul><ul><li>Break down into single molecule...
Dissociation <ul><li>This occurs because ions have charged particles. </li></ul><ul><ul><li>water is polar </li></ul></ul>...
POLARITY <ul><li>Water is polar because it has a positive and a negative side. </li></ul><ul><li>Some substances are nonpo...
LIKES DISSOLVE LIKES POLAR DISSOLVES IN POLAR NONPOLAR DISSOLVES IN NONPOLAR
Solubility <ul><li>How much of a substance will dissolve in a given amount of water. </li></ul><ul><li>Will it dissolve? <...
States of Solubility <ul><ul><li>Unsaturated:  When a solvent holds less solute than it normally could at a given temperat...
SOLIDS VS. GASES <ul><li>Solids </li></ul><ul><ul><li>solubility increases as temp. increases </li></ul></ul><ul><ul><li>s...
Reading a Solubility Curve: Above line = supersaturated On the line = saturated Below the line = unsaturated
KCl To make a saturated solution of KCl at 60ºC, how much would I add  to 100 ml of water? 46g
KNO 3 At what temperature will 80g of KNO 3  dissolve in 100ml of water to make  a saturated solution? 48ºC
NH 4 Cl What kind of a solution would 75g of NH 4 Cl  dissolved in 100 ml of water at 55ºC be? Point falls above the line ...
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13.3 solubility

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Transcript of "13.3 solubility"

  1. 1. SOLUBILITY 13.3
  2. 2. IONIC COMPOUNDS <ul><li>When ionic compounds dissolve in water they: </li></ul><ul><ul><li>Break down into single molecules. </li></ul></ul><ul><ul><li>Break down into their ions. </li></ul></ul>Na Cl water Na Cl + - this is called dissociation
  3. 3. Dissociation <ul><li>This occurs because ions have charged particles. </li></ul><ul><ul><li>water is polar </li></ul></ul><ul><ul><li>it has a + and - pole </li></ul></ul>+ -
  4. 4. POLARITY <ul><li>Water is polar because it has a positive and a negative side. </li></ul><ul><li>Some substances are nonpolar. </li></ul><ul><ul><li>no charges or poles </li></ul></ul><ul><ul><li>example: oil </li></ul></ul>
  5. 5. LIKES DISSOLVE LIKES POLAR DISSOLVES IN POLAR NONPOLAR DISSOLVES IN NONPOLAR
  6. 6. Solubility <ul><li>How much of a substance will dissolve in a given amount of water. </li></ul><ul><li>Will it dissolve? </li></ul><ul><li>SOLUBLE: substance will dissolve . </li></ul><ul><li>INSOLUBLE: substance will not dissolve. </li></ul>
  7. 7. States of Solubility <ul><ul><li>Unsaturated: When a solvent holds less solute than it normally could at a given temperature. </li></ul></ul><ul><ul><li>Saturated: When a solvent holds as much solute as it normally could at a given temperature. </li></ul></ul><ul><ul><li>Supersaturated: When a solvent is holding more solute than it would at a given temperature. </li></ul></ul>
  8. 8. SOLIDS VS. GASES <ul><li>Solids </li></ul><ul><ul><li>solubility increases as temp. increases </li></ul></ul><ul><ul><li>solubility decreases as temp. decreases </li></ul></ul><ul><li>Gases </li></ul><ul><ul><li>solubility increases as temp. decreases </li></ul></ul><ul><ul><li>solubility decreases as temp. increases </li></ul></ul>
  9. 9. Reading a Solubility Curve: Above line = supersaturated On the line = saturated Below the line = unsaturated
  10. 10. KCl To make a saturated solution of KCl at 60ºC, how much would I add to 100 ml of water? 46g
  11. 11. KNO 3 At what temperature will 80g of KNO 3 dissolve in 100ml of water to make a saturated solution? 48ºC
  12. 12. NH 4 Cl What kind of a solution would 75g of NH 4 Cl dissolved in 100 ml of water at 55ºC be? Point falls above the line supersaturated

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