solubility notes
DESCRIPTION
Solubility Notes. Chemistry 5/5/14. Drill. Use the table from pg. 10 to give the amount of substances that will dissolve in 100 g of H 2 O: NH 3 at 10°C and 80°C Why does solubility of NH 3 decrease at higher temperatures? KCl at 10°C and 70°C - PowerPoint PPT PresentationTRANSCRIPT
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Solubility Notes
Chemistry 5/5/14
+DrillUse the table from pg. 10 to give the
amount of substances that will dissolve in 100 g of H2O: NH3 at 10°C and 80°C
Why does solubility of NH3 decrease at higher temperatures?
KCl at 10°C and 70°C If 50 g of KCl were dissolved in 100 g of
water, and it was cooled to 50°C, what kind of solution would you have?
HW: Back of pg. 5 (Cross out “Henry’s Law” and #9)
+Objectives
IWBAT List factors that increase rate of solution. List factors that increase degree of solubility. Explain dissolution of a solid in a liquid. Define suspension, colloid, and emulsion.
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Substances with similar bonds dissolve into each other. Polar & Polar
Water and Isopropanol (Rubbing Alcohol) Polar & Ionic
Water and most Salts (NaCl, CaCl2, KI, etc.) Nonpolar & Nonpolar
Nail Polish and Nail Polish Remover Oil Paint and Terpentine
Why doesn’t oil dissolve in H2O?
Oils are non-polar molecules.
Water is a polar molecule.
Molecules with unlike bonds do not dissolve into each other.
Oil - No charge on the molecule
Water -Separation of
Charge
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Animation of Salt Dissolving
Describe NaCl dissolving in H2O
Water is a dipole.
NaCl dissociates into Na+ ions and Cl- ions.
The - end of the H2O molecule is attracted to the Na+ ion in the salt crystal and pulls it into the water.
The + end of the water is attracted to the Cl- ion.
http://nobel.scas.bcit.ca/chem0010/unit9/9.4_solubilityionic.htm
http://nobel.scas.bcit.ca/chem0010/unit9/9.4_solubilityionic.htm
+YOU ANSWER
What are the different ways to buy juice?
If you watered down a drink, what would you be doing?
+ Dilution and Solutions
Dilute vs. Concentrated: Dilute – small amount of solute, large amount of
solvent Concentrated – small amount of solvent, large
amount of solute
Molarity -- the measurement of the number of moles of solute per liter of solvent M = n / V M -- molarity n -- number of moles V -- total volume of solution
+Mixtures that are like Solutions, but aren’t Solutions!
Suspension Mixture where particles eventually settle
to the bottom Particles are MUCH bigger than a solution.
They may be visible ex. Chocolate is suspended in hot
chocolate or chocolate milk ex. Tiny particles of dirt (silt) are
suspended in river or pond water
+Like Solutions, but not, cont.
Colloid Mixture containing particles of a size between
suspension and true solution The particles are not actually dissolved, but
also not as large as a suspension’s particles. Particles remain dispersed (do not settle out),
but not dissolved: may appear cloudy: ex. fog, aerosols,
smoke, plain milk may appear as something between two
phases: ex. Jell-o
Suspension, Colloid, Solution (L to R)
Notice that the particles have settled out of the Suspension
A Colloid’s particles reflect light
A Solution’s particles DON’T reflect light - looks clear!
http://dl.clackamas.cc.or.us/ch105-03/similar.htm
+Like Solutions, but not, cont.
Emulsions Colloidal dispersions of liquid in liquid Tiny particles of one liquid dispersed in
another liquid, but NOT dissolved. These are held together by an emulsifier:
An emulsifier causes two immiscible liquids to mix because one end is polar and one is nonpolar.
ex. egg in mayonnaise, soap in soapy water
Soap Molecule
Soap molecules immersed in grease stain
Nonpolar molecule of grease
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The End!
How many solutions do you think you encounter on a daily basis?