LecturePLUS Timberlake1 The Atom Atomic Number and Mass Number Isotopes.
LecturePLUS Timberlake1 Chapter 6.2 Dissolving and Solubility.
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Transcript of LecturePLUS Timberlake1 Chapter 6.2 Dissolving and Solubility.
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LecturePLUS Timberlake 1
Chapter 6.2
•Dissolving and Solubility
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LecturePLUS Timberlake 2
Making process of dissolving FASTER!
• Many of same things that make chemical reactions go faster –
• But DISSOLVING IS A PHYSICAL CHANGE, NOT A CHEMICAL CHANGE.
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LecturePLUS Timberlake 3
Faster dissolving
• When a chunk of something dissolves, you are just pulling it apart into smaller bits (even down to individual molecules or ions)
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LecturePLUS Timberlake 4
Faster dissolving
• heat
• stirring
• shaking
• smaller chunks (larger surface area)
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LecturePLUS Timberlake 5
In a solution, the solute moleculesare randomly distributed amongthe solvent molecules
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LecturePLUS Timberlake 6
Figure 15.1: Dissolving of solid sodium chloride.
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LecturePLUS Timberlake 7
• The solvent is the substance that dissolves the solute to make a solution.
• The solute is the substance that dissolves in a solution.
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LecturePLUS Timberlake 8
Why is water such a great dissolver (solvent) for other
substances?
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LecturePLUS Timberlake 9
Water is polar...
It has a slightly negative “side” by the oxygen atom, and slightly
positive “side” by the hydrogens.
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LecturePLUS Timberlake 10
Water can dissolve ionic compounds, and covalent compounds that are polar (have “slightly negative”
and “slightly positive” parts).
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LecturePLUS Timberlake 11
The interaction of polar water molecules with ions
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LecturePLUS Timberlake 12
Representation of the polar hydrogen chloride molecule
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LecturePLUS Timberlake 13
Chlorine hogs the electron blanket, leavinghydrogen partially, but positively, exposed
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LecturePLUS Timberlake 14
Figure 15.3: The ethanol molecule contains a polar O—
H bond.
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LecturePLUS Timberlake 15
Figure 15.3: The polar water molecule interacts strongly with the polar O—H bond in ethanol.
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LecturePLUS Timberlake 16
Soap
• The nonpolar side of a soap molecule is “attached” (attracted to) nonpolar grease and oil, the polar side hangs on to the water, and the dirt slips off your hands and is pulled down the drain, trapped, along with the water molecules, by that pesky soap molecule!
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LecturePLUS Timberlake 17
(a) non-polar gasoline and non-polar oil mix (b) polar vinegar and nonpolar oil do not mix (c) polar water and polar ethyl alcohol mix
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LecturePLUS Timberlake 18
Figure 15.6: An oil layer floating on water.
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LecturePLUS Timberlake 19
For a more detailed explanation of why polar and nonpolar materials can’t
dissolve each other:
• http://www.knoxnews.com/kns/science/article/0,1406,KNS_9116_1971484,00.html
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LecturePLUS Timberlake 20
Saturated and Unsaturated
A saturated solution contains the maximum
amount of solute that can dissolve.
Undissolved solute remains.
An unsaturated solution does not contain all
the solute that could dissolve
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LecturePLUS Timberlake 21
Supersaturated Solutions
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LecturePLUS Timberlake 22
To see more of this supersaturation experiment:
• http://www.csudh.edu/oliver/demos/supersat/supersat.htm
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LecturePLUS Timberlake 23
To see more exciting supersaturation stuff, go to:
• Crystallization from Supersaturated Solutions of Sodium Acetate
• Note, you may need to hit “refresh” to get demonstration started and restarted.
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LecturePLUS Timberlake 24
Solubility
The maximum amount of solute that can dissolve in a specific amount of solvent usually 100 g.
g of solute
100 g water
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LecturePLUS Timberlake 25
Molarity
• Concentration unit of a solution that expresses moles of solute dissolved per liter of solution.
• To make a 1 molar solution of a substance, put 1 mole of stuff into a container and add solvent (usually water) up to the “1 liter” mark.
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LecturePLUS Timberlake 26
Not this type of Mole
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LecturePLUS Timberlake 27
Or this type of Mole
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LecturePLUS Timberlake 28
Mole• 6.02 x 1023 is a mole -
602,000,000,000,000,000,000• If you counted paper at the rate of one sheet
per second it would take you 19,089,294,774,226,281 years to count a mole of paper.
• It is a big number because atoms are small.
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LecturePLUS Timberlake 29
• A mole of sugar weighs about one half pound but contains how many molecules of sugar?
• 602,000,000,000,000,000,000• 6.02 x 1023 molecules.
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LecturePLUS Timberlake 30
Temperature and Solubility of Solids
Temperature Solubility (g/100 g H2O)
KCl(s) NaNO3(s) 0° 27.6 74 20°C 34.0 88 50°C 42.6 114100°C 57.6 182
Does the solubility of solids seem to increase or decrease with an increase in the temperature?
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LecturePLUS Timberlake 31
A. Why would a bottle of carbonated drink
possibly burst (explode) when it is left out
in the hot sun ?
B. Why would fish die in water that gets too warm?
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LecturePLUS Timberlake 32
Solutions
A. Gas in the bottle builds up as the gas becomes less soluble in water at high temperatures, which may cause the bottle to explode.
B. Because O2 gas is less soluble in warm
water, the fish may not obtain the needed
amount of O2 for their survival.