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5A: Solutions and Molarity Chapter 15

5A: Solutions and Molarity Chapter 15. Mixtures. Mechanical Mixtures. Suspension. Solutions. Colloids. How can we separate mixtures?. 1. 2. 15.1 - Solubility A. Key Definitions 1. A solution is –

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5A: Solutions and Molarity Chapter 15

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  1. 5A: Solutions and MolarityChapter 15

  2. Mixtures Mechanical Mixtures Suspension Solutions Colloids

  3. How can we separate mixtures? 1. 2.

  4. 15.1 - Solubility A. Key Definitions 1. A solution is – 2. The part of a solution present in the largest amount is the _______________. 3. Other substances in a solution are known as ___________________. 4. ________________ solutions are solutions where water is the solvent.

  5. Ionic Solutes in Water

  6. Dissociation of Ions • Strong Electrolytes • Weak Electrolytes • Nonelectrolytes

  7. Solubility Guidelines for Aqueous Solutions

  8. Colligative Properties • Properties that depend on the number of solute particles. • Freezing Point Depression • Melting Point Elevation • Lowering of Vapor Pressure • Osmotic Pressure

  9. Boiling Point Elevation and Freezing Point Depression In Terms of KMT When a “non-volatile” solute (ie. Salt) is dissolved in a solvent, the salt interferes with the movements of the solvent particles. That results in lowering the Freezing point and elevating the boiling point. For example, water boils at 100oC and freezes at 0oC. If you dissolve salt in the water, the boiling point will increase to over 100oC and it will freeze at a temp below 0oC.

  10. Lowering Vapor Pressure

  11. Boiling Point ElevationFreezing Point Depression(Honors) Tb = Kb·m Kb for water = 0.512°C/m Tf = Kf·m Kf for water = 1.86°C/m DT = b.p. elevation or f.p. depression K = molality b.p. elevation or f.p. depression constant m = molality of solution =

  12. Example: Calculate the boiling point of a solution of 1.9 mol of sugar (C12H22O11) dissolved in 400 g of water. Tb = Kb·m Kb for water = 0.512 oC/m

  13. Example 2: Calculate the freezing point of a solution of 56g NaCldissolved in 325 g of water. Tf = Kf·m Kf for water = 1.86°C/m

  14. Molecular Solutes in Water

  15. Does H2O Dissolve Everything? • Polar vs. Nonpolar Solvents • Organic vs. Inorganic Solvents

  16. 15.2 - Solution Composition: An Introduction A. Key Terms 1. When a solution has as much solute as it can hold at that temperature it is _____________________. 2. A solution that has not reached the limit of solute that will dissolve in it is said to be ____________________. 3. A solution that contains more of the solute than could be dissolved by the solvent under normal circumstances is said to be ______________________. 4. “Strong” solutions are known as ___________________. 5. “Weak” solutions are ___________________.

  17. 15.3 - Solution Composition: Mass Percent A. Mass Percent is – Example – Practice – p. 475 (15,17)

  18. 15.4 - Solution Composition: Molarity A. Molarity is – Examples – Practice – p. 475 (33, 35, 43, 45)

  19. Solution Concentration • The concentration of a solution may differ from the concentration of solute particles.

  20. 15.5 - Dilution Dilution is – To calculate the new molarity, or volume, of a solution after it has been diluted you can use the equation : Examples – Practice – p.477 (55, 56)

  21. Aqueous Reactions • Precipitation Reactions • Molecular Equation • Complete Ionic Equation • Net Ionic Equation

  22. Example • K2CrO4 (aq) + Ba(NO3)2 (aq)→

  23. 15.6 - Stoichiometry of Solution Reactions • Remember – in the middle of every stoichiometry reaction is Moles … so the question is…how can you get moles of a substance out of a volume and concentration of a solution for that substance? • See Steps for problem solving on 465. • Examples (Self Check 15.8 on 476) – • Practice – p477 (63-65)

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