TOPICS TO BE COVERED 1. WHAT ARE SOLUTIONS? 2. · PDF fileobjective: measuring solubility. 3....
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Transcript of TOPICS TO BE COVERED 1. WHAT ARE SOLUTIONS? 2. · PDF fileobjective: measuring solubility. 3....
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TOPICS TO BE COVERED
1. WHAT ARE SOLUTIONS?
2. SOLVENTS AND SOLUTES
3. SOLUBILITY AND ITS FACTORS
4. CONCENTRATIONS
5. SOLUTION STOICHIOMETRY
6. COLLIGATIVE PROPERTIES
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SOLUTIONSCHEMICALS + WATER
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1. WHAT ARE SOLUTIONSOBJECTIVE: WHAT ARE THEY?
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SOLUTIONS
• IMPORTANCE OF STUDYING SOLUTIONS
• BECAUSE MANY REACTIONS TAKE PLACE IN
SOLUTIONS
• BECAUSE MIXING REACTANTS IN SOLID FORM
OFTEN DO NOT RESULT IN REACTIONS.
• REACTIONS REQUIRE COLLISIONS AT THE
ATOMIC/MOLECULAR LEVEL, AND IN THE
SOLID STATE, THIS DOES NOT OCCUR AT
A SIGNIFICANT RATE.
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1. WHAT ARE SOLUTIONS?
SOLUTIONS ARE…
HOMOGENOUS MIXTURES
• HOMOGENOUS VS. HETEROGENEOUS
• MIXTURE VS. COMPOUND
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1. WHAT ARE SOLUTIONS
Does not always involve liquids
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1. WHAT ARE SOLUTIONS
SOLVENT- PRESENT IN GREATER AMOUNT
- DOES THE “DISSOLVING”
WATER IS THE UNIVERSAL
SOLVENT
SOLUTE- PRESENT IN LESSER AMOUNT
- IS THE ONE “DISSOLVED”
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1. WHAT ARE SOLUTIONS
IF A SOLUTION IS A MIXTURE, DO
THE SOLUTES AND THE SOLVENTS
CHEMICALLY REACT
OR PHYSICALLY MIX?
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2. SOLUBILITYOBJECTIVE: IF SOMETHING DOES OR DOES NOT DISSOLVE
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2. SOLUBILITY
Why do some things dissolve
while others do not?
What does it mean for something
to “dissolve?”
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2. SOLUBILITY
What does it mean for
something to “dissolve?”
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dissociation
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2. SOLUBILITY
Why do some things dissolve
while others do not?
“Like dissolves Like”
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2. SOLUBILITY
“Like dissolves Like”
Polar Solvent will dissolve…
Non-Polar Solvent will dissolve
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2. SOLUBILITY
Miscible vs. Immiscible
Miscible = dissolves
Immiscible = does NOT dissolve
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2. SOLUBILITY
How much of some thing can be
dissolved?
SolubilityTHE MAXIMUM AMOUNT OF A SOLUTE THAT CAN DISSOLVE
AT A SPECIFIED TEMPERATURE AND PRESSURE
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2. SOLUBILITY
Increasing/Decreasing Solubility
1. Temperature
2. Pressure
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SO AS
TEMPERATURE
_______,
SOLUBILITY
______
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2. SOLUBILITY
Increasing/Decreasing
Solubility
with Temperature
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Unsaturated Solutions
more solute can be
dissolved
no heat necessary
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Saturated Solutions
no more solute can
be
dissolvedno heat necessary
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Super-Saturated
Solutions
more solute than
normal
heat necessary
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Super-Saturated
Solutions
Rock Candy
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SOLUBILITY OF GASES
AS TEMPERATURE _____ THE
SOLUBILITY OF GAS _______.
SO TEMPERATURE AND SOLUBILITY
OF A GAS HAVE A(N) ____.
RECALLING HEAT AS KINETIC
ENERGY, WE CAN EXPLAIN THIS
BY…
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SOLUBILITY OF SOLIDS
SOLUBILITY OF GASES
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SUMMARY & REVIEW
1. EXPLAIN WHY THERE MIGHT BE MORE MINERAL FORMATION
SURROUNDING THERMAL SPRINGS THAN COOL MOUNTAIN
SPRINGS.
2. WHY DOES WARM SODA “FLATTEN” QUICKER THAN COLD
SODA?
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3. CONCENTRATIONSOBJECTIVE: MEASURING SOLUBILITY
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3. CONCENTRATIONS
concentration =
how much solute in the solution
2 methods
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3. CONCENTRATIONS
Molarity MOLALITY
Symbol
Formula
Units
Example
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3. CONCENTRATIONS
Molarity MOLALITY
Symbol M
Formula M = mol
L
Units mol = mol of SOLUTE
L = liters of solution
Example 5 M, or 5 molar
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3. CONCENTRATIONS
1.23 mol of HCl in solution
With volume of 5.00 L.
What is molartiy?
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3. CONCENTRATIONS
3.45 M solution of AgCl is
made with 2. 45 mol of AgCl.
What is volume?
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3. CONCENTRATIONS
3.45 M solution of AgCl is
made with 2.45 L.
What is mol of AgCl?
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3. CONCENTRATIONS
Precipitate = a solid that forms
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3. CONCENTRATIONS
0.125 L of 0.100 M HCl is
added to Zn. What mass of
ZnCl2 is formed?
Zn + 2HCl → ZnCl2 + H2
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3. CONCENTRATIONS
11.0 g of Cu are needed. What
volume of a 0.500 M solution of
CuSO4 is needed to result in 11.0 g
of copper?
CuSO4+ Fe Cu + FeSO4
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Ba(NO3)2(aq) + Na2SO4(aq) Ba(SO4)(s) + 2NaNO3(aq)
25mL of 0.5M Ba(NO3)2 solution is
combined with excess Na2SO4. How
many grams of precipitate formed?
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Pb(NO3)2(aq) + 2NaCl(aq) PbCl2(s) + 2NaNO3(aq)
• How many grams of precipitate would form if
30mL of a 0.25M Pb(NO3)2 solution was added to
20mL of a 0.50M NaCl solution?
• How many moles of the excess reactant are left
over after the reaction?
• What is the molarity of the excess reactant after
the reaction?
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CaCl2(aq) + 2NH4OH(aq) Ca(OH)2(s) + 2NH4Cl(aq)
What volume of a 0.2M NH4OH solution
would be required to precipitate all of the
Ca2+ ions in 50mL of a 0.15M CaCl2
solution?
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• SOLUBILITY OF GASES
• HENRY’S LAW
• IF THE SOLUBILITY OF A GAS IN WATER IS
0.77G/L AT 350KPA OF PRESSURE, WHAT
IS ITS SOLUBILITY, IN UNITS OF
GRAMS/LITER, AT 100KPA?
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• SOLUBILITY OF GASES
• HENRY’S LAW
• A GAS HAS A SOLUBILITY OF 3.6G/L AT A
PRESSURE OF 100KPA. WHAT PRESSURE IS
NEEDED TO PRODUCE AN AQUEOUS
SOLUTION CONTAINING 9.5G/L OF THE
SAME GAS?
• THE SOLUBILITY OF METHANE IN WATER AT
100KPA IS 0.026G/L, WHAT WILL THE
SOLUBILITY BE AT A PRESSURE OF 180KPA?
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• SOLUBILITY OF LIQUIDS
• LIKE DISSOLVES LIKE
• MISCIBLE
• NON-POLAR AND NON-POLAR =
MISCIBLE
• POLAR + POLAR = MISCIBLE
• IMMISCIBLE
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• PERCENT SOLUTIONS
• SIMILAR TO PPM
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• PERCENT SOLUTIONS
• WHAT IS THE PERCENT BY VOLUME OF
ETHANOL (C2H6O) WHEN 75ML OF ETHANOL
IS DILUTED TO A VOLUME OF 250ML WITH
WATER?
• A SOLUTION CONTAINS 2.7G OF CUSO4 IN
75ML OF SOLUTION. WHAT IS THE PERCENT
BY MASS OF THE SOLUTION?
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• CONCENTRATION OF IONS
• CALCULATE THE NUMBER OF MOLES OF CL- IN
2.75 L OF 1.0X10-3M ZNCL2
• HOW MANY GRAMS OF SULFATE ION ARE
PRESENT IN 500ML OF A 2M AL2(SO4)3
SOLUTION?
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5. COLLIGATIVE PROPERTIESOBJECTIVE: HOW ADDING THINGS TO WATER
CHANGES WATER
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5. COLLIGATIVE PROPERTIES
MAIN IDEA:
The properties of a solution are different
from those of a pure solvent.
When you add things, like solutes, to
water, it changes the properties of
the water!
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SOME OF THESE DIFFERENCES ARE DUE TO THE
PRESENCE OF SOLUTE PARTICLES IN THE
SOLUTION.
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5. COLLIGATIVE PROPERTIES
COLLIGATIVE PROPERTIES =
A PROPERTY OF A SOLUTION THAT
DEPENDS ON THE
CONCENTRATION OF THE SOLUTE
PARTICLES.
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5. COLLIGATIVE PROPERTIES
COLLIGATIVE PROPERTIES =
1. Increases boiling temperature
2. Lowers freezing temperature
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• COLLIGATIVE PROPERTIES
• COLLIGATIVE PROPERTIES – A PROPERTY OF A
SOLUTION THAT DEPENDS ON THE
CONCENTRATION OF THE SOLUTE PARTICLES.
• THE WORD COLLIGATIVE IS DERIVED FROM THE
LATIN COLLIGATUS MEANING BOUND
TOGETHER, SINCE THESE PROPERTIES ARE BOUND
TOGETHER BY THE FACT THAT THEY ALL DEPEND
ON THE NUMBER OF SOLUTE PARTICLES.
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• COLLIGATIVE PROPERTIES
• BOILING POINT ELEVATION – THE DIFFERENCE IN
TEMPERATURE BETWEEN THE BOILING POINTS OF
A SOLUTION AND OF THE PURE SOLVENT.
• FREEZING POINT DEPRESSION – IS THE
DIFFERENCE IN TEMPERATURE BETWEEN THE
FREEZING POINTS OF A SOLUTION AND OF THE
PURE SOLVENT.
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4. CONCENTRATION
Molarity MOLALITY
Symbol
Formula
Units
Example
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4. CONCENTRATIONMolarity MOLALITY
Symbol M m
Formula M = mol
L
m = mol
kg
Units mol = mol of SOLUTE
L = liters of solution
mol = mol of SOLUTE
kg = kilograms of
SOLVENT
Example 5 M, or 5 molar 5 m, or 5 molal
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5. COLLIGATIVE PROPERTIES
How many grams of KI must be
dissolved in 0.500 g of water to
produce a 0.060 molal KI
solution?
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5. COLLIGATIVE PROPERTIES1. Determine the molality of a solution of 560 g acetone, C3H6O in 0.620 kg of water.
2. What is the molality of a solution of 12.9 g of fructose, C6H12O6, in 31 g of water?
3. Determine the molal concentration of 71.5 g of linoleic acid, C18H32O2, dissolved in
525 g of C6H14.
4. How many moles of butanol, C4H10O must be dissolved in 0.125 kg of ethanol in
order to produce a 12.0 m solution?
5. Convert the answer above to grams!
6. What mass of urea, NH2CONH2, must be dissolved in 2250 g of water to make a
1.50 molal solution?
7. What mass of CaCl2 must be dissolved in 590.0 g of water to produce 0.82 molal
solution?
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5. COLLIGATIVE PROPERTIES1. Determine the molality of a solution of 560 g acetone, C3H6O in 0.620 kg of water.
2. What is the molality of a solution of 12.9 g of fructose, C6H12O6, in 31 g of water?
3. Determine the molal concentration of 71.5 g of linoleic acid, C18H32O2, dissolved in
525 g of C6H14.
4. How many moles of butanol, C4H10O must be dissolved in 0.125 kg of ethanol in
order to produce a 12.0 m solution?
5. Convert the answer above to grams!
6. What mass of urea, NH2CONH2, must be dissolved in 2250 g of water to make a
1.50 molal solution?
7. What mass of CaCl2 must be dissolved in 590.0 g of water to produce 0.82 molal
solution?
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• COLLIGATIVE PROPERTIES
• THE MAGNITUDE OF BP ELEVATION AND FP
DEPRESSIONS IS PROPORTIONAL TO THE
NUMBER OF SOLUTE PARTICLES DISSOLVED IN
THE SOLVENT.
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• COLLIGATIVE PROPERTIES
• WOULD A DILUTE OR CONCENTRATED SODIUM
FLUORIDE SOLUTION HAVE A HIGHER BOILING
POINT?
• IF EQUAL NUMBER OF MOLES OF KI AND MGF2
ARE DISSOLVED IN EQUAL AMOUNTS OF WATER,
WHICH SOLUTION WOULD HAVE THE HIGHEST:
• BOILING POINT
• FREEZING POINT
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MOLARITY MOLALITY
• VOLUME OF SOLUTE +
• VOLUME OF SOLVENT
• UNIT = M
BOTH MOLARITY AND MOLALITY MEASURE
CONCENTRATION
• MASS OF SOLVENT
IN KILOGRAMS
• UNIT = M
(ITALICIZED)
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• CALCULATING MOLALITY
• CALCULATE THE MOLALITY AND TOTAL MOLALITY
(IF APPLICABLE) OF A SOLUTION PREPARED BY
DISSOLIVING 10.0G OF NACL IN 600 G OF
WATER.
• CALCULATE THE MOLALITY AND TOTAL MOLALITY
(IF APPLICABLE) OF A SOLUTION PREPARED BY
DISSOLIVING 10.0G C12H22O11 OF IN 600 G OF
WATER.
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• CALCULATING MOLALITY
• HOW MANY GRAMS OF POTASSIUM IODIDE
MUST BE DISSOLVED IN 0.500 G OF WATER
TO PRODUCE A 0.060 MOLAL KI SOLUTION?
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• CALCULATING MOLALITY
• WHAT IS THE DIFFERENCE BETWEEN A 1M
AND A 1M SOLUTION?
• A 4 G SUGAR CUBE (C12H22O11) IS DISSOLVED IN A
350 ML TEACUP OF 80 °C WATER. WHAT IS THE
MOLALITY OF THE SUGAR SOLUTION IF THE DENSITY
OF WATER AT 80° = 0.975 G/ML
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• CALCULATING BP AND FP CHANGES
• BP
•ΔTB = KB * M
• FP
•ΔTF = KF * M
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• CALCULATING BP AND FP CHANGES
• KB, KF = THE MOLAL BP/FP CONSTANT, WHICH IS
EQUAL TO THE CHANGE IN BP/FP TEMPERATURE FOR
A 1 MOLAL SOLUTION.
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• CALCULATING BP AND FP CHANGES
• WHAT IS THE BOILING POINT OF A 1.5 MOL
SOLUTION THAT IN 800G OF WATER?
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• CALCULATING BP AND FP CHANGES
• WHAT IS THE BOILING POINT OF A 1.2 MOL
SOLUTION OF NACL IN 800G OF WATER?
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• CALCULATING BP AND FP CHANGES
• WHAT IS THE BP AND FP OF A 1.40 MOL SOLUTION
OF NA2SO4 IN 1750G OF WATER?
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• DETERMINING MOLAR MASS FROM ΔTB AND ΔTF
• MOLAR MASS =
• 7.5 G OF SOLUTE IS ADDED TO 22.60 G OF
WATER. THE WATER BOILS AT 100.78 DEGREES C.
WHAT IS THE MOLAR MASS OF THE SOLUTE?
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• DETERMINING MOLAR MASS FROM ΔTB AND ΔTF
• WHAT INFORMATION/MEASUREMENTS ARE
NEEDED TO FIND THE MOLAR MASS OF A
SOLUTE WHEN GIVEN THE BOILING POINT
ELEVATION, ΔTB, FOR AN AQUEOUS
SOLUTION?
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