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I. The Nature of Solutionsp 118 REVIEW BOOKHW P 120 Q 1 TO 7

Solutions

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MARCH 29

• DEFINITIONS – SOLUTION – SOLUTE – SOLVENT – HOMOGENEOUS MIXTURE

• CONCENTRATION – DILUTE VS CONCENTRATED

• THE NATURE OF SOLUTIONS

• SOLVATION

• SOLUBILITY

• FACTORS THAT AFFECT SOLUBILITY

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Some DefinitionsSome DefinitionsA solution is a A solution is a

HOMOGENEOUS HOMOGENEOUS mixture of 2 or more mixture of 2 or more substances in a substances in a single phase. single phase.

One constituent is One constituent is usually regarded as usually regarded as the the SOLVENTSOLVENT and and the others as the others as SOLUTESSOLUTES..

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A. Definitions

• Solution - Solution - homogeneous mixture

Solvent Solvent - present in greater amount

Solute Solute - substance being dissolved

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Parts of a Solution• SOLUTE – the part of a solution that is

being dissolved (usually the lesser amount). Uniformly spread in the solvent

• SOLVENT – the part of a solution that dissolves the solute (usually the greater amount)

• Solute + Solvent = Solution

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What happens when a solute dissolves in a solvent?

• SolvationSolvation – – the process of dissolving

solute particles are separated and pulled into solution

solute particles are surrounded by solvent particles

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How Does a Solution Form?

As a solution forms, the solvent pulls solute particles apart and surrounds, or solvates, them.

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APRIL 2

• Characteristics of a liquid solution

• Types of solution

• Solubility and factors that affect it

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CHARACTERISTICS OF A LIQUID SOLUTION

• 1.- Homogeneous mixtures, particles are evenly spread.

• 2.- Dissolved particles are too small to be seen, therefore solutions are clear and do not disperse light.

• 3.- Can not be separated by filtration. Dissolved particles are too small and will pass trough any filter.

• 4.- Stable. Dissolved particles will not come out of the solution and will not settle.

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Solutions are not always liquids• Solutions are homogeneous mixtures of

two or more pure substances.

• In a solution, the solute (present in smaller amount) is dispersed uniformly throughout the solvent (present in largest amount).

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Solutions

Homogeneous mixtures.

Solvation is the process by which the solution forms.

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CONCENTRATIONThe amount of solute in the solution.

Relative terms

• Diluted: Small amount of solute in relation to the amount of solvent

• Concentrated: Large amount of solute in relation with the solvent.

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Solubility

A measure of how much solute can be dissolved in an amount of solvent at a given temperature.

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A substance can be…

• Soluble in a solvent.

• Example: sugar is soluble in water.

• Miscible is the term used when the two components are liquids.

• Example: alcohol and water are miscible

• Insoluble in a solvent

• Example: sand is insoluble in water.

• Immiscible is the term used when the two components are liquids.

• Example: oil and water are immiscible

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What affects Solubility?

1. Nature of Solute

2. TemperatureTemperature

3. Pressure

* graph

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Nature of Solute

• A polar solute molecule (alcohol) dissolves in a polar solvent (water).

• A nonpolar solute (oil paint) dissolves in a nonpolar solvent (turpentine)

“Like Dissolves Like”

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Solubility for ionic compoundsTable F

• This table is used to predict if a double replacement reaction will occur. If it the reaction produces an insoluble compound

it occurs. If the products of the reaction are filtered the insoluble compound will remain in the filter paper

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Table F

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Questions• Is NaCl soluble?

Yes!

• Is AgBr soluble?

No!

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Determining Electrical Conductivity

• When a solution is soluble, it has ions that can conduct electricity (electrolytes)

Ex. NaClEx. NaCl

• When a solution is insoluble, it cannot When a solution is insoluble, it cannot conduct electricity (conduct electricity (non-electrolytesnon-electrolytes or or poor electrolytes)poor electrolytes)

Ex. AgBrEx. AgBr

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When temperature increases…

• Solubility of a gas decreases

• Solubility of a solid increases

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3 Pressure• Makes gas more

soluble

ex. Soda canex. Soda can

• Has almost no effect on liquids and solids

-High pressure forces carbon dioxide into water to make soda.

- When you open the cap, there is less pressure on the soda b/c the soda fizzes and gas escapes.

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• Gases are more soluble athigh pressures

EX: nitrogen narcosis, the “bends,” soda

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C. Solubility

• SolubilitySolubility– maximum grams of solute that will

dissolve in 100 g of solvent at a given temperature

– varies with temp

– based on a saturated solution

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C. Solubility

• Solubility Solubility CurveCurve– shows the

dependence of solubility on temperature

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C. Solubility

SATURATED SOLUTION

no more solute dissolves

UNSATURATED SOLUTIONmore solute dissolves

SUPERSATURATED SOLUTION

becomes unstable, crystals form

concentration

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C. Solubility

• Solids are more soluble at...Solids are more soluble at...– high temperatures.

• Gases are more soluble at...Gases are more soluble at...– low temperatures &

– high pressures (Henry’s Law).

– EX: nitrogen narcosis, the “bends,” soda

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DefinitionsDefinitions

Solutions can be classified as Solutions can be classified as saturatedsaturated or or ununsaturatedsaturated..

A A saturatedsaturated solution contains solution contains the maximum quantity of the maximum quantity of solute that dissolves at that solute that dissolves at that temperature.temperature.

An An unsaturatedunsaturated solution solution contains less than the contains less than the maximum amount of solute maximum amount of solute that can dissolve at a that can dissolve at a particular temperatureparticular temperature

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SupersaturatedSupersaturatedSodium AcetateSodium Acetate

• One application One application of a of a supersaturated supersaturated solution is the solution is the sodium acetate sodium acetate “heat pack.”“heat pack.”

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Concentration of SoluteConcentration of SoluteConcentration of SoluteConcentration of Solute

The amount of solute in a solution The amount of solute in a solution is given by its is given by its concentrationconcentration.

Molarity (M) = moles soluteliters of solution

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1.0 L of 1.0 L of water was water was

used to used to make 1.0 L make 1.0 L of solution. of solution. Notice the Notice the water left water left

over.over.

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PROBLEM: Dissolve 5.00 g of PROBLEM: Dissolve 5.00 g of NiClNiCl22•6 H•6 H22O in enough water to O in enough water to make 250 mL of solution. make 250 mL of solution. Calculate the Molarity.Calculate the Molarity.

PROBLEM: Dissolve 5.00 g of PROBLEM: Dissolve 5.00 g of NiClNiCl22•6 H•6 H22O in enough water to O in enough water to make 250 mL of solution. make 250 mL of solution. Calculate the Molarity.Calculate the Molarity.

Step 1: Step 1: Calculate moles Calculate moles of NiClof NiCl22•6H•6H22OO

5.00 g • 1 mol

237.7 g = 0.0210 mol

0.0210 mol0.250 L

= 0.0841 M

Step 2: Step 2: Calculate MolarityCalculate Molarity

[NiClNiCl22•6 H•6 H22OO ] = 0.0841 M

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Step 1: Step 1: Change mL to L.Change mL to L.

250 mL * 1L/1000mL = 0.250 L250 mL * 1L/1000mL = 0.250 L

Step 2: Step 2: Calculate.Calculate.

Moles = (0.0500 mol/L) (0.250 L) = 0.0125 molesMoles = (0.0500 mol/L) (0.250 L) = 0.0125 moles

Step 3: Step 3: Convert moles to grams.Convert moles to grams.

(0.0125 mol)(90.00 g/mol) = (0.0125 mol)(90.00 g/mol) = 1.13 g1.13 g

USING MOLARITYUSING MOLARITYUSING MOLARITYUSING MOLARITY

moles = M•Vmoles = M•V

What mass of oxalic acid, What mass of oxalic acid, HH22CC22OO44, is, is

required to make 250. mL of a 0.0500 Mrequired to make 250. mL of a 0.0500 Msolution?solution?

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Learning Check

How many grams of NaOH are required to prepare 400. mL of 3.0 M NaOH solution?

1) 12 g

2) 48 g

3) 300 g

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Two Other Concentration Two Other Concentration UnitsUnits

grams solutegrams solutegrams solutiongrams solution

% by mass% by mass = =

% by mass% by mass

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Two Other Concentration Two Other Concentration UnitsUnits

grams solutegrams solutegrams solutiongrams solution

Ppm =Ppm =

Ppm = parts per millionPpm = parts per million

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Try this molality problem

• 25.0 g of NaCl is dissolved in 5000. mL of water. Find the molality (m) of the resulting solution.

m = mol solute / kg solvent

25 g NaCl 1 mol NaCl

58.5 g NaCl= 0.427 mol NaCl

Since the density of water is 1 g/mL, 5000 mL = 5000 g, which is 5 kg

0.427 mol NaCl

5 kg water= 0.0854 m salt water

40Calculating Calculating ConcentrationsConcentrations

Dissolve 62.1 g (1.00 mol) of ethylene glycol in 250. g Dissolve 62.1 g (1.00 mol) of ethylene glycol in 250. g of Hof H22O. Calculate molality and % by mass of O. Calculate molality and % by mass of

ethylene glycol.ethylene glycol.

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• DO NOW – REVIEW CONCENTRATIONS

• COLLIGATIVE PROPERTIES

• Hw Review Book P 129-131 q38 to 50

42Calculating Calculating ConcentrationsConcentrations

Dissolve 62.1 g (1.00 mol) of ethylene glycol in 250. g Dissolve 62.1 g (1.00 mol) of ethylene glycol in 250. g

of Hof H22O. Calculate m & % of ethylene glycol (by mass).O. Calculate m & % of ethylene glycol (by mass).

Dissolve 62.1 g (1.00 mol) of ethylene glycol in 250. g Dissolve 62.1 g (1.00 mol) of ethylene glycol in 250. g

of Hof H22O. Calculate m & % of ethylene glycol (by mass).O. Calculate m & % of ethylene glycol (by mass).

%glycol = 62.1 g

62.1 g + 250. g x 100% = 19.9%%glycol =

62.1 g62.1 g + 250. g

x 100% = 19.9%

Calculate weight %Calculate weight %

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Learning Check

A solution contains 15 g Na2CO3 and 235 g of

H2O? What is the mass % of the solution?

1) 15% Na2CO3

2) 6.4% Na2CO3

3) 6.0% Na2CO3

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Using mass %

How many grams of NaCl are needed to prepare 250 g of a 10.0% (by mass) NaCl solution?

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Colligative PropertiesColligative PropertiesOn adding a solute to a solvent, the properties On adding a solute to a solvent, the properties

of the solvent are modified.of the solvent are modified.

• Vapor pressure Vapor pressure decreasesdecreases

• Melting point Melting point decreasesdecreases

• Boiling point Boiling point increasesincreases

These changes are called These changes are called COLLIGATIVE COLLIGATIVE PROPERTIESPROPERTIES. .

They depend only on the They depend only on the NUMBERNUMBER of solute of solute particles relative to solvent particles, not on particles relative to solvent particles, not on the the KINDKIND of solute particles. of solute particles.

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Change in Freezing Change in Freezing Point Point

The freezing point of a solution is The freezing point of a solution is LOWERLOWER than that of the pure solventthan that of the pure solvent

Pure waterPure waterEthylene glycol/water Ethylene glycol/water

solutionsolution

47Change in Freezing Change in Freezing Point Point

Common Applications Common Applications of Freezing Point of Freezing Point DepressionDepression

Propylene glycol

Ethylene glycol – deadly to small animals

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Common Applications Common Applications of Freezing Point of Freezing Point DepressionDepression

Which would you use for the streets of New York to lower the freezing point of ice and why? Would the temperature make any difference in your decision?

a) sand, SiO2

b) Rock salt, NaCl

c) Ice Melt, CaCl2

Change in Freezing Change in Freezing Point Point

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Change in Boiling Point Change in Boiling Point Common Applications Common Applications

of Boiling Point of Boiling Point ElevationElevation

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Calculate the Freezing Point of a 4.00 molal Calculate the Freezing Point of a 4.00 molal glycol/water solution.glycol/water solution.

KKff = 1.86 = 1.86 ooC/molal (See KC/molal (See Kff table) table)

SolutionSolution

∆∆TTFPFP= (1.86 = (1.86 ooC/molal)(4.00 m)(1)C/molal)(4.00 m)(1)

∆∆TTFP FP = 7.44 = 7.44

FP = 0 – 7.44 = -7.44 FP = 0 – 7.44 = -7.44 ooCC(because water normally freezes at 0)(because water normally freezes at 0)

Freezing Point Freezing Point DepressionDepression

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At what temperature will a 5.4 molal solution At what temperature will a 5.4 molal solution of NaCl freeze?of NaCl freeze?

SolutionSolution

∆∆TTFPFP = K = Kff • m • i • m • i

∆ ∆TTFPFP = (1.86 = (1.86 ooC/molal) • 5.4 m • 2C/molal) • 5.4 m • 2

∆ ∆TTFP FP = 20.1= 20.1 ooCC

FP = 0 – 20.1 = -20.1 FP = 0 – 20.1 = -20.1 ooCC

Freezing Point Freezing Point DepressionDepression

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Preparing SolutionsPreparing SolutionsPreparing SolutionsPreparing Solutions

• Weigh out a solid Weigh out a solid solute and dissolve in a solute and dissolve in a given quantity of given quantity of solvent.solvent.

• Dilute a concentrated Dilute a concentrated solution to give one solution to give one that is less that is less concentrated.concentrated.