Water and Aqueous Solutions 1718 Notes.pdf · 2020. 7. 17. · Aqueous Solutions •Solute: what is...
Transcript of Water and Aqueous Solutions 1718 Notes.pdf · 2020. 7. 17. · Aqueous Solutions •Solute: what is...
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Water and Aqueous Solutions
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Homogeneous Mixtures
•A mixture that has only one phase.
•Called a “solution.”
Heterogeneous Mixtures
•A mixture that has 2 or more phases
•Examples include salad dressing, muddy
water
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Aqueous Solutions
•Solute: what is being dissolved
•Solvent: the medium that is doing the
dissolving
•Solution: the mixture of the solute and the
solvent
•Solvation: the process that occurs when a
solute dissolves
• Can be endo- or exo-thermic
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1. Solutions
•Homogeneous mixture of two or more pure
substances.
•Mixed to the level of molecules
•Particles smaller than 1 nm
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2. Suspensions
• Heterogeneous mixtures of pure substances
• Have larger particles than solutions >100nm
• Particles in a solvent are so large that they
settle out unless the mixture is constantly stirred
or agitated
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3. Colloids – particles dispersed between those in
solutions and suspensions that form mixtures
•Dispersed phase – colloidal particles
•Dispersing medium – phase holding the particles
•Emulsion – special liquid–liquid colloid
• Mayonnaise!
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Shows difference
between solution
and colloids
Suspended
particles catch
the light
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• Electrolytes: compounds that conduct and electric
current in aqueous solution or in the molten state
• Ionic compounds such as NaCl, CuSO4, NaOH
•Don’t use a hair dryer in the bathtub!
• Nonelectrolytes: compounds that do not conduct
an electric current in the aqueous or molten state
•Covalent compounds such as sugar, alcohol, and
pure water
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The ammeter measures the flow of electrons (current)
through the circuit. Phet Simulation
If the ammeter measures a current, and the bulb
glows, then the solution conducts.
If the ammeter fails to measure a current, and the bulb does
not glow, the solution is non-conducting.
Electrolytes vs. Non-electrolytes
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Factors affecting the rate of dissolution
1. Increasing surface area of the solute
• Which dissolves faster: sugar cube or
granulated sugar?
2. Agitation of a solution
• Does stirring help dissolve sugar?
3. Heating a Solvent
• Which dissolves sugar faster: hot tea or iced
tea?
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• Definition: physical state in
which the opposing
processes of dissolution and
crystallization of a solute
occur at equal rates
• http://phet.colorado.edu/en
/simulation/soluble-salts
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• Why does salt dissolve
in water but iodine does
not?
• Why does oil NOT mix
in water?
• Why does iodine
dissolve in alcohol but
salt does not?
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• “LIKE DISSOLVES LIKE”
•POLAR solutes dissolve in POLAR solutions
•NONPOLAR solutes dissolve in NONPOLAR
solutions
• WATER IS POLAR SO ONLY POLAR SUBSTANCES
WILL DISSOLVE IN IT!
• Salt is polar and dissolves in water
• Oil is nonpolar so it FLOATS on water and does
not combine with it! (salad dressing)
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Saturated solution: the maximum amount of solute
dissolved in a specific amount of solvent at that
temperature
•Anywhere along the line on the graph
Unsaturated solution: less than the maximum amount
of solute dissolved in a specific amount of solvent at a
temperature
•Anywhere below the line on the graph
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Supersaturated Solution:
more than the maximum
amount of solute dissolved in
a specific amount of solvent
•Usually have to increase
the temperature
•Above the line
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Solids increase in solubility as the temperature
increases
•The particles have more energy and can move
faster and create more collisions
Gases decrease in solubility as the temperature
increases
•The gas particles have more energy and tend to
move out of the solution!
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Why do fish die in warm weather?
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• Immiscible – liquids that are
not soluble in each other
• Miscible – liquids that
dissolve freely in one
another in any proportion
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Changes in pressure have very little effect on the
solubilities of liquids or solids in liquid solvents
Pressure increases the solubility of a gas in a liquid
• Henry’s Law: The solubility of a gas in a liquid is
directly proportional to the pressure of that gas on
the surface of the liquid.
𝑆1
𝑃1=
𝑆2
𝑃2
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Hsoln: the amount of heat energy absorbed or
released when 1 mole of a solute dissolves a
specific amount of a solvent
Endothermic: positive heat of solution
•Feels cold!
ex) Solute + solvent + heat solution
Exothermic: negative heat of solution
•Feels hot!
ex) solute + solvent solution + heat
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Endothermic
•Ammonium nitrate
•NH4NO3 (s) + H2O + Heat NH4+ (aq) + NO3
- (aq)
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Exothermic
• calcium chloride or magnesium sulfate
CaCl2 (s) + H2O Ca2+ (aq) + 2 Cl- (aq) + Heat
MgSO4 (s) + H2O Mg2+ (aq) + SO4- (aq) + Heat
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• The relative amount of solute in a given amount
of solvent
• Used to quantify what is in a solution
Dilute: More solvent less solute
Concentrated: More solute less solvent
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•Dilute
•More solvent less solute
•Concentrated
•More solute less solvent
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Concentration “[ ]” – measure of the amount of
solute in a given amount of solvent or solution
• Important for all medical & scientific fields!
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Dilute: little solute
dissolved in a
solvent
Concentrated:
plenty of solute
dissolved in a
solvent
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Molarity (M) – moles of solute in one liter of solution
Molarity (M) = amount of solute (mol)
liters of solution (L)
Interpret units:
• If there’s a 6 M HCl = 6 moles HCl/1 L soln
• If there’s a 0.5 M NaCl = 0.5 mol NaCl/1 L solution
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1. Weigh out 1 mole of salt = 58.44 g
2. Add salt to volumetric flask
3. Add enough dH2O to fill the flask.
4. Add a stirring rod & put on stir plate.
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Molarity is defined as moles of solute per liter of
solution where:
𝑀 =𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
𝐿𝑖𝑡𝑒𝑟 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛=
𝑛
𝑉
n = moles of solute
V = volume expressed in liters
So: 𝑀 = 𝑛
𝑉 and 𝑀 × 𝑉 = 𝑛
And YES, this means you will use algebra!!
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What is the molarity of a solution made by dissolving 85.0 g NaCl in
750. mL water?
Convert from grams to moles first:
85.0 𝑔 𝑁𝑎𝐶𝑙 ×1 𝑚𝑜𝑙𝑒 𝑁𝑎𝐶𝑙
58.44 𝑔 𝑁𝑎𝐶𝑙 = 1.4544 𝑚𝑜𝑙𝑒 = 1.45 𝑚𝑜𝑙 𝑁𝑎𝐶𝑙
Now solve for Molarity
𝑀 = 𝑛
𝑉 =
1.45 𝑚𝑜𝑙 𝑁𝑎𝐶𝑙
.750 𝐿 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛= 1.9333 = 1.93𝑀 𝑁𝑎𝐶𝑙
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Given a concentrated solution, how do you make
a dilute solution from it?
M1V1 = M2V2
Why do we learn about this??
• In lab when we order acids they are delivered
as concentrated solutions.
• We need to calculate how to dilute them to
concentrations that we can safely use.
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Example: How many liters of a 16.0 M HCl solution
are needed to make 0.500 L of a solution with a
concentration of 2.5 M HCl?
M1= 16.0 M V1= ? M2= 2.5 M V2 = 0.500 L
𝑉1 =
𝑀2𝑉2
𝑀1 =
2.5 𝑀∗0.500 𝐿
16.0 𝑀 =0.078125 L = 0.078 L
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Chapter 13
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Molality (m) – concentration of a soln expressed in
moles of solute per kilogram of solvent
Molality (m) = amount of solute (mol)
kilogram of solvent (kg)
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Molality (m) – concentration of a soln expressed in moles of
solute per kilogram of solvent
Molality (m) = amount of solute (mol)
kilogram of solvent (kg)
Interpret units:
• If there’s a 6 m HCl = 6 moles HCl/1 kg H2O
• If there’s a 0.5 m NaCl = 0.5 mol NaCl/1 kg H2O
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• 1 m HCl or 1 M HCl? Why?
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• 1 m HCl has 1 kg H2O = 1 L H2O
• 1 M HCl has enough H2O to make a 1 L
soln, therefore has less water
Answer:
• 1 M HCl is more concentrated!
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• A soln of iodine in carbon tetrachloride
is used when iodine is needed for
certain chemical tests. How much
iodine must be added to prepare a
0.480 m soln of iodine in CCl4 if 100.0
g of CCl4 is used?
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100.0 g CCl4 x 1 kg = 0.100 kg CCl4
1000 g
0.480 m = x mol I2 0.0480 mol I2
0.1000 kg CCl4
0.0480 mol I2 x 253.80 g I2 = 12.2 g I2
1 mol I2
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Ions in Aqueous Solutions and Colligative Properties
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Dissociation –
separation of
ions that occurs
when an ionic
compound
dissolves
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• Colligative Properties – properties that depend on the concentration of solute particles but not on their identity
• Examples
•Vapor pressure lowering which causes freezing point depression & boiling point elevation
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Definition: the difference in temperature between
the freezing points of a solution and the pure
solvent
•directly proportional to the molal
concentration of the solution
•Symbol: Tf
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• Molal Freezing Point Constant (Kf): the freezing-
point depression of the solvent in a 1 molal
solution of a nonvolatile, molecular solute
• Tf = Kf x m x D
• Kf of water = -1.86 oC * Kg/mol solute
• m = molal concentration (mol/kg)
• D = dissociation factor (number of particles)
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Definition: the difference in temperature between
the boiling points of a solution and the pure
solvent
•directly proportional to the molal
concentration of the solution
•Symbol: Tb
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Molal Boiling Point Constant (Kb): the boiling-point
elevation of the solvent in a 1 molal solution of a
nonvolatile, molecular solute
• Tb = Kb x m x D
• Kb of water = 0.51 oC * Kg/mol solute
• m = molal concentration
• D = dissociation factor (number of particles)
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• What is the freezing-point depression of water
in a solution of 17.1 g of sucrose, C12H22O11, in
200. g of water? What is the actual freezing
point of the soln?
• First calculate the molality of the solution.
• Plug this into the equation to determine Tf
• Tf = Kf x m x D
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• What is the freezing-point depression of water
in a solution of 17.1 g of sucrose, C12H22O11, in
200. g of water? What is the actual freezing
point of the soln?
• Tf = -1.86 0C/m x 0.25 m x 1 = -0.465 0C
MM = 342.30g/mol
0.0500 mol sucrose in .200 kg water
0.25 m sucrose
DF =1