Chapter 11
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Transcript of Chapter 11
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Chapter 11
Water and Solutions
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Homework for Chap 11Homework for Chap 11
Read p 275 – 280; 283 - 293
Applying the Concepts # 1 - 21;
27 - 30, 32, 33, 37 - 49
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Properties of Water
• Aqueous solutions ≡ solids, liquids, or gasesdissolved in water
• Household water:
• Drinking/cooking 2 %• Washing dishes 6 %• Laundry 11%• Bathing 23%• Toilets 29%• Lawns/gardening 29%
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Fig. 11.2 (A) The water molecule is polar (It has a dipole)
H2O
Fig. 11.2 (B) Attractions between water molecules
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Ice is less dense than water
Water is a Unique Substance:
Fig. 11.3 The hexagonal structure of ice
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Maximum Density4 °C
Density of Water
Fig. 11.4 The density of water just above its freezing point
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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
Solution Solvent Solute
Soft drink (l)
Air (g)
Soft Solder (s)
H2O
N2
Pb
Sugar, CO2
O2, Ar, CH4
Sn
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Types of Solutions
• Unsaturated solution - can dissolve more solid
• Saturated solution – holds all the solid it can at agiven temperature
• Supersaturated solution – hold more solid that normal ata given temperature
There is a limit to how much solid can dissolve in a liquid
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Fig 11.9 Solubility change with temperature
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Fig 11.5 Structural formula of a soap molecule
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Fig 11.6 NaCl dissolving in water
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Hydration - process in which an ion is surrounded by water molecules arranged in a specific
manner.
NaClNaCl CHCH33OHOH
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NaClNaCl CHCH33OHOH
H2O is a polar molecule
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Electrolyte - a substance that, when dissolved in water, results in a solution that can conduct electricity.
Nonelectrolyte - a substance that, when dissolved, results in a solution that does not conduct electricity.
nonelectrolyte weak electrolyte strong electrolyte
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Electrolyte Properties
Figure 4.2
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Strong Electrolyte – 100% dissociation
NaCl (s) Na+ (aq) + Cl- (aq)H2O
Weak Electrolyte – not completely dissociated
CH3COOH CH3COO- (aq) + H+ (aq)
Conduct electricity in solution?
Cations (+) and Anions (-)
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Fig. 11.11 The reaction of water and hydrogen chloride
Hydronium ion
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Fig 11.13 Dissolving a mole of a compound in water
1 mole sucrose → 1 mole of molecules
1 mole NaCl → 2 moles of ions
1 mole CaCl2 → 3 moles of ions
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Strong Electrolytes Are…
Strong acids
Strong bases
Soluble ionic salts
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Acids
1. Have a sour taste. e.g., Vinegar, lemons, limes, sour milk
2. Cause litmus to change from blue to red.
4. Acid solutions conduct electricity.
3. Acids neutralize bases.
Fig 11.14 (A)
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1. Have a bitter taste. e.g., caffeine, walnuts, soap
3. Feel slippery. Many soaps contain bases.
Bases
5. Basic solutions conduct electricity.
2. Cause litmus to change from red to blue.
4. Bases neutralize acids.
Fig 11.14 (B)
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Based on powers of 10:
e.g., a soln with pH = 3 is 10 times moreacidic than a solution with pH = 4
How do we express the concentration
of an acid or a base?
pH scale – based on concentration of the
hydronium ion (H3O+)
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
acidic basicneutral
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Fig. 11.16 Common substances that are acidic
citric acidascorbic acid
acetic acid
carbonic acid
citric acidascorbic acid
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Table 11.5Approximate pH of some common substances
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Acids, Bases, and Salts
acid + base salt + water
HCl (aq) + NaOH (aq) NaCl (aq) + H2O
A Neutralization Reaction:
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