Chapter 18: Solution Chemistry (Also including some Ch. 17!)
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Transcript of Chapter 18: Solution Chemistry (Also including some Ch. 17!)
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Chapter 18: Solution Chemistry
(Also including some Ch. 17!)
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A few things you need to recall…
Ionic = metallic element + nonmetallic element Covalent = nonmetal + nonmetal
Polar Nonpolar
Examples:
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Solutions:
Aqueous Solutions: Water that contains a dissolved substance. Kool Aid Salt water Magnesium chloride solution Vinegar
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Solutions are made up of Solvents and Solutes:
Solute: The dissolving substance
Solvent: The medium in which a solute is dissolved.
Water is the mostcommon solvent
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Dissolving NaCl
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Dissolving Ionic Compounds
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A molecular look at dissolving an ionic compound in water
http://www.chem.umass.edu/~botch/Chem112S05/Chapters/Ch14/SolvationIons.jpg
Solvation: process that occurs when a compound is dissolved in water.
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Solute or Solvent?
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Oil/Water Activity
In your beaker add about 20 mL of oil to 20 mL of water.
Do the two substances mix? Add 4-5 drops of food coloring to the
beaker? What happens? Based on your experiment, does food
coloring have properties that are similar to water or similar to oil?
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Likes Dissolve Likes
Polar molecules dissolve in Polar solvents. Nonpolar solutes dissolve in nonpolar
solvents.
Ionic compounds and polar covalent compounds dissolve the best in water. Why?
Water is a polar compound
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Mixing Oil and Water
Vinegar (acetic acid)
Olive Oil
Polar
Non-Polar
Oil and vinegar are immiscible – they do not dissolve in each
other.
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Making Solutions
http://www.chem4kids.com/files/matter_solution.html
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Factors that affect dissolving rate
How do you make sugar dissolve faster in iced tea?
1) Stirring = Agitation Changes rate, but not how much dissolves.
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Factors that affect dissolving rate
Does sugar dissolve faster in hot tea or cold tea?
2)Temperature Kinetic Energy of water molecules increases;
more collisions with surface of sugar crystals
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Factors that affect dissolving rate
Does granular sugar or a sugar cube dissolve fastest?
3) Particle Size More solute is exposed to water, dissolves faster
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Homogeneous vs. Heterogeneous
Homogeneous = evenly mixed; same throughout
Heterogeneous = unevenly mixed; not the same throughout
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Solubility: How much dissolves?
Solubility: The amount of solute that will dissolve in a solvent at a given temperature. Very temperature dependent. Usually expressed in
g/100mL (or g/100g H2O)
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Examples:
Example #1: What is the solubility of sodium chloride at 70 °C?
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Example 2:
Example #2: At 25 °C, how many grams of potassium nitrate will dissolve in 200 mL water?
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Practical Applications
What are the optimum conditions to explode a can of coke on your little brother?
Why do divers have to worry about
how fast they return to the ocean
surface?
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Warm Up 12/02/08
1. How many moles are in 510 g of AgNO3?
2. List the 3 factors that affect how fast a substance dissolves.
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Types of Solutions:
Saturated Solution: Contains the max amount of solute at a given temperature. No more can be dissolved
Unsaturated: Contains less than max amount of solute
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Types of Solutions
Supersaturated: Solutions that hold more solute than possible.
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Real life supersaturation experience…
Rock Candy!
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Factors Affecting Solubility
Temperature Solids: More soluble in hot solvent Gases: More soluble in cold solvent
Pressure Gases: More soluble at high pressure
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Concentration of Solutions
Concentration is the amount of solute per amount of solvent.
To make Kool Aid:2 Scoops Kool Aid1 Quart Water
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Describing Solutions
Version 1: No Math! (Qualitative)
Dilute :Low
concentration of solute
Concentrated :High
concentration of solute
½ scoop Kool Aid2 Quarts Water
2 ½ scoop Kool Aid2 Quarts Water
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Common Chemistry Concentrations
Version 2 (MATH ) Molarity (M) Molality (m) Percent Composition
%m/%v %v/%v
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Molarity
http://www.cartage.org.lb/en/kids/science/Chemistry/math/pix/molarity.gif
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Example 1:
A solution has a volume of 2.0 L and contains 36.0 g of glucose (mm 180 g/mol). What is the molarity of the solution?
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Example 2:
How many moles of ammonium nitrate are in 335 mL of 0.425 M NH4NO3?
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Dilutions
Used when you want a less concentrated solution. Kool Aid Example:
Same number of moles of solute when you make a dilution:
M1 x V1 = M2 x V2
Initial MolarityOf Concentrated
SolutionInitial Volume Final Molarity
Of Dilute Sln
Final VolumeOf Dilute Sln
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Example 3
Explain how to prepare 25 L of a 0.10 M BaCl2 solution, starting with solid BaCl2.
Specify the volume of the solution above to get 0.020 mol of BaCl2.
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Example 3
How many mL of a stock solution (concentrated) of 4.00 molar potassium iodide would you need to prepare 250 mL of 0.760 M KI?
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Percent Compostion
%(m/v) = (mass solute (g)) ÷ (mL solution) 100%
%(v/v) = (volume solute) ÷ (L solution) 100%
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Example 4:
Determine the %(m/v) of a solution that is 20.0
g sugar in 401 mL solution.
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Parts per million (ppm)
ppm = (mass solute (g)) ÷ (mL solution) 1,000,000