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Chapter 11

Water and Solutions. Chapter 11. Homework for Chap 11 Read p 299 – 305; 307 - 319 Applying the Concepts # 1 – 9; 12 – 21; 27, 29, 30, 32, 33, 37 - 49. Properties of Water. Aqueous solutions ≡ solids, liquids, or gases dissolved in water Household water:

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Chapter 11

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  1. Water and Solutions Chapter 11

  2. Homework for Chap 11 Read p 299 – 305; 307 - 319 Applying the Concepts # 1 – 9; 12 – 21; 27, 29, 30, 32, 33, 37 - 49

  3. Properties of Water • Aqueous solutions ≡ solids, liquids, or gases • dissolved in water • Household water: • Drinking/cooking 2 % • Washing dishes 6 % • Laundry 11% • Bathing 23% • Toilets 29% • Lawns/gardening 29%

  4. Fig. 11.2 (A) The water molecule is polar (It has a dipole) H2O Fig. 11.2 (B) Attractions between water molecules

  5. Ice is less dense than water Fig. 11.3 The hexagonal structure of ice Water is a Unique Substance:

  6. Maximum Density 4 °C Fig. 11.4 The density of water just above its freezing point Density of Water

  7. Solution Solvent Solute Solution - a homogenous mixture of 2 or more substances Solute - the substance(s) present in the smaller amount(s) Solvent - the substance present in the larger amount Soft drink (l) H2O Sugar, CO2 Air (g) N2 O2, Ar, CH4 Pb Sn Soft Solder (s)

  8. Types of Solutions There is a limit to how much solid can dissolve in a liquid • Unsaturated solution - can dissolve more solid • Saturated solution – holds all the solid it can at a • given temperature • Supersaturated solution – hold more solid that normal at • a given temperature

  9. Fig 11.9 Solubility change with temperature

  10. Fig 11.5 Structural formula of a soap molecule

  11. Fig 11.6 NaCl dissolving in water

  12. nonelectrolyte strong electrolyte Electrolyte - a substance that, when dissolved in water, forms a solution that can conduct electricity. Nonelectrolyte - a substance that, when dissolved, forms a solution that does not conduct electricity.

  13. Fig 11.13 Dissolving a mole of a compound in water 1 mole sucrose → 1 mole of molecules 1 mole CaCl2 → 3 moles of ions 1 mole NaCl → 2 moles of ions

  14. Fig. 11.11 The reaction of water and hydrogen chloride Hydronium ion

  15. Acids • Have a sour taste. e.g., Vinegar, lemons, limes, sour milk • Cause litmus to change from blue to red. 3. Acids neutralize bases. 4. Acid solutions conduct electricity. Fig 11.14 (A)

  16. Bases 1. Have a bitter taste. e.g., caffeine, walnuts, soap 2. Cause litmus to change from red to blue. 3. Feel slippery. Many soaps contain bases. 4. Bases neutralize acids. 5. Basic solutions conduct electricity. Fig 11.14 (B)

  17. How do we express the concentration of an acid or a base? pH scale – based on concentration of the hydronium ion (H3O+) acidic neutral basic 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Based on powers of 10: e.g., a soln with pH = 3 is 10 times more acidic than a solution with pH = 4

  18. Fig. 11.16 Common substances that are acidic

  19. Table 11.5Approximate pH of some common substances

  20. acid + base salt + water HCl (aq) + NaOH (aq) NaCl (aq) + H2O Acids, Bases, and Salts A Neutralization Reaction:

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