properties, concentrations, and dilutions. solute and solvent solute is the substance being...
TRANSCRIPT
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Properties, Concentrations, and Dilutions
CHAPTER 16: SOLUTIONS
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Solute and Solvent
Solute is the substance being dissolved.
Solvent is the substance doing the dissolving.
Example: Salt and Water. We dissolve salt in water.
Therefore, the salt is the solute and the water is the solvent.
Why is water called the universal solvent?
REVIEW
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Forming a Solution• The composition (what they are made out of) of the
solvent and solute determine whether a substance will dissolve.
How FAST will the substance dissolve?• This depends on three things:• 1. Stirring: Increase of decrease rate?• 2. Temperature: Increase or decrease rate?• 3. Particle Size: The more surface area exposed, the
faster it will dissolve.
PART 1: PROPERTIES OF SOLUTIONS
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What amount of a substance will dissolve?
Particles move from a solid into a solution. But how much can be dissolved?
Solubility describes the amount of substance that can be dissolved by a certain quantity of a solvent at a certain temp and pressure until the
solution becomes saturated.
PART 2: SOLUBILITY
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Different Types of Solutions:
• Saturated Solution: The maximum amount of solute that can be dissolved at a specific temp and pressure.
• Unsaturated Solution: A solution that contains less solute than required to be a saturated solution and a certain temp and pressure.
• Supersaturated Solution: contains more solute than it can theoretically hold at a given temperature.
• Miscible Solution: when two liquids will dissolve into one another. There is no separation.
• Immiscible: liquids that are not soluble in each other. You can tell if it is immiscible by observing layers.
SOLUBILITY
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SOLUBILITY
Miscible Immiscible
Oil and Water
Water and Acetone
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SOLUTIONS
Supersaturated Solution
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Learn how to make your own rock candy using Chemistry at home.
(AKA Crystal Meth… Not really. Just kidding.)
GOOD NEWS: BREAKING BAD FANS
http://video.about.com/chemistry/How-to-Make-Rock-Candy.htm
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What do YOU think?What type of solution is being utilized?
How are they making that solution?
ROCK CANDY EXPLAINED
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• 1. Temperature: Solubility of MOST substances increases as temperature increases.
• You can dissolve more solute in the solvent as you increase the temperature. Think about how we made our rock candy.
• EXCEPTION: Gas solubility increases as temperature decreases.
FACTORS THAT AFFECT SOLUBILITY
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• 2. Pressure: Changes in pressure doesn’t affect the solubility of solids and liquids, but it greatly influences the solubility of gases.
• As pressure increases, the solubility of gases also increases. Use Henry’s Law for calculations.
• S = solubility• P = pressure• Directly Proportional
FACTORS THAT AFFECT SOLUBILITY
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How would I describe solubility in terms of UNITS?
Solubility is usually expressed in grams of solute per 100g of solvent.
• Example: 36g of sodium chloride in 100g of water at 25 degC.
• Examples in terms of saturation: If 36g of NaCl is added to 100g water, it will dissolve completely, but if I added 1 more gram of NaCl, only 0.2g of that will dissolve. Therefore, 36.2g of NaCl in 100g of water is a SATURATED solution.
• How would I make it super saturated??
SOLUBILITY OF SOLUTIONS
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Concentration: a measure of the amount of solute that is dissolved in a given quantity of solvent.
Dilute Solution: a weak concentration. Contains small amount of solute.
Concentrated Solution: strong concentration. Contains a large amount of solute.
PART 3: CONCENTRATIONS
DiluteConcentrated
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MOLARITY
Moles of solute dissolved in 1 Liter of solution.
CONCENTRATIONS
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LET’S MAKE A SOLUTION
Let’s determine the molarity of a solution that we
make. Let’s start with 10
grams of sodium chloride and
add it to a 1-L volumetric flask half filled with distilled water.
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LETS MAKE A SOLUTION
Swirl the flask carefully to dissolve the solute.
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LETS MAKE A SOLUTION
Fill the flask with water exactly to the 1-L mark.
What is the concentration of the solution in molarity?
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Answer: 0.171M
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This will work with ANY volumetric flask. Big or small. We can then calculate the molarity
(concentration) of our solution.
LETS MAKE A SOLUTION
• How do we convert mL to L?
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Find the number of moles of solute in a solution…
WHAT IF YOU KNOW THE MOLARITY?
• We can also convert moles to grams.
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Diluting a solution reduces the number of moles per unit volume. The number of moles of solute remains unchanged.
Dilution equation:
DILUTIONS
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DILUTIONS
To prepare 100 ml of MgSO4 from a stock solution of 0.171M NaCl, a student first measures 10 mL of the stock solution with a 10-mL pipet.
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DILUTIONS
She then transfers the 10 mL to a 100-mL volumetric flask.
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DILUTIONS
Finally, she carefully adds water to the mark to make 100 mL of solution. What is the final concentration?
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Use M1 x V1 = M2 x V2
Answer: 0.0171
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Some volume measuring devices…
BuretGraduated Cylinder
Volumetric FlaskGlass Pipets
TO MEASURE VOLUME
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DILUTION CALCULATION
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These are not as common as molarity, but are used sometimes.
Percent by volume:
Percent by mass:
PERCENT CONCENTRATIONS OF SOLUTIONS
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Percent by volume: (volume/volume)
PERCENT CONCENTRATION CALCULATIONS
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Percent by mass: (mass/mass)• Suppose you want to make a 2000g
solution that has a 2.8% (m/m) concentration of glucose in water.
• How many grams of glucose should you use?
PERCENT CONCENTRATION CALCULATIONS
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Page 499# 42, 44, 46, 48, 49a, 51, 52, 53a,b, 54a,
55a
CLASS WORK