c ondensed s tates chemistry spring 2015. a genda 3/2/15 hard boiled egg?? tests back? learning...
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![Page 1: C ONDENSED S TATES Chemistry Spring 2015. A GENDA 3/2/15 Hard Boiled Egg?? Tests Back? Learning Targets for Unit 3 Review from 1 st Semester Notes over](https://reader035.vdocuments.us/reader035/viewer/2022062409/5697c0271a28abf838cd61bb/html5/thumbnails/1.jpg)
CONDENSED STATESChemistry Spring 2015
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AGENDA 3/2/15
Hard Boiled Egg??
Tests Back?
Learning Targets for Unit 3 Review from 1st Semester
Notes over the review Topics
HW: Complete the Phase Change Graphic **Tomorrow TESTING DAY**
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ENERGY AND PHASES REVIEW
1. Potential vs Kinetic Ea. PE = stored energy
Breaking bonds increases PE Making bonds releases PEb. KE = E of motion KEgas > KEliquid > KEsolid
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ENERGY AND PHASES REVIEW
2. Exothermic vs Endothermica. Exothermic Gives off E (E is released to surroundings) Bond formation Gas liquid solid (“intermolecular force
formation”) Why? I am forming bond, making things more stable –
energy is released.
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ENERGY AND PHASES REVIEW
b. Endothermic Absorbs E (E taken from surroundings) Bonds breaking Solid liquid gas (“intermolecular force
breaking”) Why? Energy is needed to break bonds.
**BARF**Break, absorb, release, form
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ENERGY AND PHASES REVIEW
Solid
Liquid Gascondensation
evaporation
freezing
meltingsublimation
deposition
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ENERGY AND PHASES REVIEW
Inside Arrows: Exothermic (feels hot) Decreases PE Forming IM forces More order Particles closer
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ENERGY AND PHASES REVIEW
Outside Arrows Endothermic (feels cold) Increases PE Breaking IM forces Less order Particles spread out
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ENERGY AND PHASES REVIEW
3. Heat vs Temperaturea. Heat Form of energy Measured in Joules (J) kJ (1000 J) Flows from warmer object to colder object
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ENERGY AND PHASES REVIEW
b. Temperature Measure of average KE of particles How much particles are moving E given to particles increase motion
increase T Measuring Temperature
Celsius vs Kelvin2 different temperature scales
K is a more direct reflection of KE
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ENERGY AND PHASES REVIEW
Celsius (oC) Kelvin (K)
Absolute zero -273oC 0 K
Freezing point of water
0oC 273 K
Boiling point of water
100oC 373 K
Remember: K = C + 273
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AGENDA 3/4/15
Hand Back Unit 2 Tests 5 Minute Remediation
Notes on Solutions and Solubility Solubility Curves
Pre-Lab for Solubility Lab Tomorrow
HW: Complete Solubility Curve WS
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SOLUTIONS
SolutionsHomogeneous mixture is the
same throughoutStable won’t spontaneously
separateExamples: Kool-Aid, saltwater,
popMade of 2 parts:
Solute – chemical that is dissolved (Kool-Aid mix)
Solvent – chemical that does the dissolving (water)
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SOLUTIONS
Aqueous Solution – a solution where H2O is the solvent
Why do things dissolve?Molecule – Ion AttractionSimilar chemical structure
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SOLUTIONS
+ - +
+- -
-
+
++ - -
NaCl (s)
OH
H
O
HH
+H
H
H
H
H
H
O
O
O
OH
H
Na+ (aq)
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SOLUTIONS
+ - +
+- -
-
+
+- -
NaCl (s)
O
H
H
O
H
HH H
H
H
H HO
O
O
OH
H
Na+ (aq)
-
Cl- (aq)+
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SOLUTIONS
SolvationOccurs on the surface of a
solidMay be exothermic or
endothermicHeat of Solution – energy
change caused by dissolvingEx: acid in water is warm
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AGENDA 3/5/15
Finish notes on Solutions and Solubility
Solubility Lab of Ammonium Chloride Solubility Curves
Examples of Solubility Curves
Notes on Molarity Practice Problems
HW: Complete Solubility Lab
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WARM-UP
What is a solute?
What is a solvent?
What are three ways to dissolve solids faster?
Explain solvation to your partner.
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How do you get things to dissolve faster?
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SOLUTIONS
Factors that affect the rate of solvation:1. Stirring – fresh solvent is brought to surface of solute (faster)
2. Increase T – solvent molecules have more KE (faster)
3. Surface area – powder dissolves faster than a chunk
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SOLUTIONS
*LIKES DISSOLVE LIKES*
water & food coloring“miscible”2 substances are alike and will mix
water & oil“immiscible”2 substances are different and will not mix
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SOLUBILITY LAB
Safety: Do not reach over the hot plate
Tips: Heat the test tube in the water very gently Use the distilled water in the test tube only Use tap water in the beaker Make sure you know the amount of Ammonium
Chloride your group is responsible for.
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AGENDA 3/6/15 Wrap-Up Solubility Lab
What does it mean?
Notes on Solubility Curves Saturation/Super-Saturation
Practice Problems with Solubility
Notes on Molarity Practice Problems
HW: Complete Solubility WS
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SOLUBILITY LAB
What was the solubility of Ammonium chloride at 55 degrees C?
What would the solubility be at 85 degrees C?
What would the solubility be at 35 degrees C?
What does our best-fit line tell us about the solubility of Ammonium chloride?
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Solubility – the maximum amount of solute that can be dissolved in a given amount of solvent
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SOLUBILITY CURVES
Solid in Liquid Solutions - 3 “stages”1.Unsaturated
• Contains less than the maximum amount of solute
• All solute dissolves and there is room for more
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SOLUBILITY CURVES
2. Saturated maximum amount of solute is dissolved additional solute will not dissolve at that T depends on T occurs when rate of dissolving = rate of
crystallization
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SOLUBILITY
3. Supersaturated more solute dissolved than the solution
would normally hold can make by carefully cooling a saturated
solution unstable, wants to crystallize
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SOLUBILITY
= dissolving = crystallizing
Sugar cubedissolving in
H2O
Some dissolvesSome crystallizes
Equilibriumdissolving = crystallization
Solution is saturated!
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AGENDA 3/9/15
Review Solubility Check HW
Notes on Molarity
Practice Problems with Molarity
HW: Complete Molarity WS
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SOLUTIONS WARM-UP
Explain the following terms:
Unsaturated
Saturated
Supersaturated
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How do we measure the amount of solute in a solvent?
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Concentration – the amount of solute dissolved in a given amount of solvent
Dilute – small amount of solute (weak)Concentrated – a lot of solute (strong)
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MOLARITY
Molarity A unit of concentration # of moles of solute per 1 L of solution
Molarity (M) = moles of solute = mol Liters of solution L
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MOLARITY
Examples:
A salt solution has a volume of 152 mL and contains 0.90 mol NaCl. What is the molarity of the solution?
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MOLARITY
M = molL
152 mL = 0.152 L
M = 0.90 mol 0.152 L
= 5.9 M
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MOLARITY
A 3.0 L aqueous solution contains 45.0 g KI. What is the solution’s molarity?
45.0 g KI166.00 g KI
1 mol KI=0.271 mol KI
M = molL
M = 0.271 mol3.0 L
M = 0.090 M
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MOLARITY
How many moles of NaCl are in 1.5 L of a 3.0 M NaCl solution? What mass of salt is this?
M = molL
3.0 M = x mol 1.5 L
x = 4.5 mol
3.0 M(1.5 L) = x mol
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MOLARITY
4.5 mol NaCl58.44 g NaCl
1 mol NaCl=262.98 g NaCl
260 g NaCl
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AGENDA 3/10/15
Check Molarity HW Warm-Up
Notes on Dilution
Salt Lab
HW: Write-Up Lab
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WARM-UP
Example: A 500.00 mL solution of HCl contains 45.0 grams of the chemical. What is the molarity of this solution?
Ans: 2.47 M
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ANSWERS TO 1-5 ON SOLUTIONS PRACTICE
1. .901M2. 83.9 g KCl3. 6.09M4. 1.47 x 106 g KOH5. 20.5 M Pb in Sn
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DILUTIONS
Dilutions – making a less concentrated solution from a stock solution
soln of known concentration
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DILUTIONS
M=mol/L → M x L = mol
M1V1 = moles of solute before dilution
M2V2 = moles of solute after dilution
The moles of solute does not change during a dilution. You’re just adding more water.
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DILUTIONS
M1V1 = M2V2
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DILUTIONS
Examples:
How would you prepare 305 mL of 0.500 M AgCl from a 1.20 M stock solution?
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DILUTIONS
M1 = 1.20 M
V1 = ?
M2 = 0.500 M
V2 = 305 mL = 0.305 L
M1V1 = M2V2
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DILUTIONS
(1.20M)(V1) = (0.500M)(0.305L)
(1.20M)(V1) = 0.1525
1.20 1.20
V1 = 0.127 L
V1 = 127 mL127 mL of stock soln& 178 mL of H2O
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DILUTIONS
To prepare 1.00 L of 6.0 M HCl, what volume of concentrated (12.1 M) HCl must be used?
M1 = 12.1 M
V1 = ?
M2 = 6.0 M
V2 = 1.00 L
M1V1 = M2V2
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DILUTIONS
(12.1 M)(V1) = (6.0 M)(1.00 L)
(12.1 M)(V1) = 6.0
12.1 12.1
V1 = 0.496 L
V1 = 0.50 L500 mL of 12.1 M HClshould be addedto 500 mL of H2OV1 = 500 mL
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SALT SOLUTIONS LAB
Safety: Bunsen Burners: Keep your hair tied back
Tips: Have the fresh samples of water ready to go
while boiling the first solution and salt solutions.
Keep data on the back of the lab for easy reference.
Be sure to use distilled water, not tap water.
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AGENDA 3/11/15
1st Hour: Complete Lab, graph and conclusion
7th and 8th: Review Findings in the lab
Practice Dilution and Molarity calculations
HW: Finish any make-up work you have left
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SALT LAB WARM-UP
Answer these questions with your partner:
1. How did adding the salt to the water affect the boiling temperature of the water?
2. How did diluting the salt concentration affect the boiling temperature of the water?
3. Bonus question: Why would adding salt to pasta water make the pasta cook faster?
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CONCLUSION
Take time to write up your lab conclusion.
When you are complete turn in your lab and pick up the dilutions worksheet.
When finished with the dilutions worksheet, pick up the molarity and dilution worksheet.
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AGENDA 3/12/15
1st Hour: Collect Lab
Check Dilutions Hw
Notes on Evaporation and Boiling Boiling Demonstration
Colligative Properties
HW: Complete WS as study guide for Quiz
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SALT LAB WARM-UP
Answer these questions with your partner:
1. How did adding the salt to the water affect the boiling temperature of the water?
2. How did diluting the salt concentration affect the boiling temperature of the water?
3. Bonus question: Why would adding salt to pasta water make the pasta cook faster?
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PHASE CHANGE: EVAPORATION
Evaporation – Process of changing from l
g Occurs at any T Occurs at the surface of the
liquid
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PHASE CHANGE: EVAPORATION
Saturated air with vapor (“air is full”)
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PHASE CHANGE: EVAPORATION
Vapor PressureThe pressure (collisions) caused by the vapor
above a liquid in a sealed container of equilibrium
Caused by the collision of vapormolecules with the surface of theliquid
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PHASE CHANGE: EVAPORATION
VP depends on: T (as T ↑, evaporation ↑, vapor ↑ and VP ↑)
Because more molecules have the E to break free of the surface
T (as T ↓, evaporation ↓, vapor ↓ and VP ↓) Because fewer molecules have E to break free of
the surface
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PHASE CHANGES: BOILING Occurs when the VP of a liquid = the atm P
on it Vapor forming within the liquid, not at surface The pressure from the atmosphere would crush
bubbles
P inside = P outside
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PHASE CHANGE: BOILING
Boiling Point – T at which VP = atmospheric P Normal Boiling Point (NBP) = BP when P = 1 atm
P inside = P outside
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PHASE CHANGE: BOILING
Why would the vapor pressure need to be equal to or greater than the atmospheric pressure?
How could we increase the vapor pressure? Think how to increase the amount of vapor present in a liquid.
ANSWER: We heat it…vapor pressure is directly related to the temperature.
1 atm
.022 atm
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PHASE CHANGES
What if you’re not at 1 atm?
Pike’s Peak, CO CLC, IL
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PHASE CHANGES
1.05 atm (mine) 107oC
1.00 atm (IL) 100oC
0.894 atm (Denver) 94oC
Pike’s Peak 89oC
Mt. Everest 70oC
H2O VP = 0.022 atm
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PHASE CHANGES
Will foods cook faster in Denver?
No, because the BP is lower, water is cooler, cooking takes longer.
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What causes the boiling point and melting point to change when a salt is dissolved in it?
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COLLIGATIVE PROPERTIES
Properties that depend entirely on the number of particles dissolved in a given mass of solvent
Ex: Boiling point and melting point
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COLLIGATIVE PROPERTIES
Vapor Pressure Lowering Allows liquids to boil at temperatures lower than
their normal boiling point.
Vacuum Demo!!
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COLLIGATIVE PROPERTIESWhy?
Because vaporization occurs at the surface and the solute is in the way….so less vaporizes, therefore VP is lower.
*depends on the # of particles of solute
= solvent
= solute
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COLLIGATIVE PROPERTIES
2. Boiling Point Elevation – a solution boils at a higher T than a pure solvent (like our salt lab)
Why? Boiling occurs when VP = atm P Since VP is lowered by adding salt, more E must be
added to raise VP to atm P Proportional to # of particles
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COLLIGATIVE PROPERTIES
Example:
Salt in H2O for cooking pasta
H2O boils at a higher T, pasta cooks faster
H2O does not boil faster
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COLLIGATIVE PROPERTIES
3. Freezing Point Depression – a solution freezes at a lower T than a pure solvent
Why? Particles in liquid disrupt the orderly pattern
of solid crystal, bonds cannot form as easily Must get colder to solidify Proportional to the # of particles
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COLLIGATIVE PROPERTIESExample:
Melting Ice
Sand doesn’t melt ice NaCl dissolves, melts ice by
lowering fp AlCl3 better (more particles)
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AGENDA 3/13/15
Check Molarity and Dilutions HW
Last minute questions before quiz
Molarity and Dilutions Quiz
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AGENDA 3/16/15
Quizzes Tomorrow/Maybe Today
Back to Balancing Equations Equations in Solutions
Predicting States of matter
*** GRAB A WS FROM THE BACK TABLE***
HW: Ionic Equations
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04/21/23Free template from www.brainybetty.com 78
SOLUTIONS
+ - +
+- -
-
+
++ - -
NaCl (s)
OH
H
O
HH
+H
H
H
H
H
H
O
O
O
OH
H
Na+ (aq)
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AGENDA 3/17/15 ST. PATTY’S DAY!!
Review Quiz
Ionic Equation Review HW Check
Ionic Reaction Demo
Energy/Phases Review
HW: Energy and Ionic Equation Worksheet
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IONIC REACTIONS DEMO
I have a solution of lead (II) nitrate and lithium chloride.
Will a precipitate form?
If not, why not?
If yes, what is the precipitate that formed?
Write a complete balanced reaction including phases.
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IONIC REACTION DEMO
I have a solution of sodium hydroxide and a solution of hydrogen chloride.
Will a precipitate form?
If not, why not?
If yes, what is the precipitate that formed?
Write a complete balanced equation including phases.
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PHASE DIAGRAMS
Describe the conditions of T and P where each phase is most likely to exist
Gas High T, low P
Liquid middle
Solid Low T, high P
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PHASE DIAGRAMSPhase Diagram – shows the
relationship between the 3 phases in a sealed container
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PHASE DIAGRAMS Features: Lines of Equilibrium
On the lines, the substance exists in equilibrium between two states
At that T and P, both phases exist
1. s g2. s l3. l g
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PHASE DIAGRAMS
Features: Triple Point
One specific point at which all three phases exist in equilibrium in a sealed container
A
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PHASE DIAGRAMS Features: Critical Point
Point past which neither liquid nor gas truly exist
An intermediate fluid phase (plasma*)
B
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PHASE DIAGRAMS
Phase Diagram for H2O