SolutionSolution

Homogeneous mixture Homogeneous mixture in a single phase.in a single phase.

Classification of MatterClassification of Matter

MatterMatter

PureSubstances

Mixtures

HomogeneousMixtures

HeterogeneousMixtures

Elements Compounds

Also called Also called solutionssolutions

Also called Also called suspensionssuspensions

SolventSolvent

Substance you have the Substance you have the most of. Substance that most of. Substance that

retains its phase. retains its phase. Dispersing medium.Dispersing medium.

SoluteSolute

Substance you have the Substance you have the least of. Substance that least of. Substance that

dissolves. dissolves.

Dilute SolutionDilute Solution

Relatively small amount of Relatively small amount of solute.solute.

Concentrated SolutionConcentrated Solution

Relatively large amount of Relatively large amount of solute.solute.

Aqueous SolutionAqueous Solution

Water is the solvent.Water is the solvent.

NaClNaCl(aq)(aq)

Solution of NaCl dissolved in Solution of NaCl dissolved in water!water!

SolubleSoluble

Capable of being dissolved.Capable of being dissolved.

SolubilitySolubility

Maximum amount of 1 Maximum amount of 1 substance that will dissolve substance that will dissolve

in a given amount of in a given amount of another substance.another substance.

Factors that influence Factors that influence solubilitysolubility

Temperature for all systems Temperature for all systems & pressure for systems & pressure for systems

involving gases.involving gases.

Factors that influence the Factors that influence the rate of dissolving.rate of dissolving.

•TemperatureTemperature•Stirring or agitationStirring or agitation•Surface Area of soluteSurface Area of solute•Amount of solute already Amount of solute already presentpresent

What kind of change is What kind of change is dissolving?dissolving?

Physical changePhysical change

How does a chemist How does a chemist represent the dissolving of a represent the dissolving of a

covalentlycovalently bonded bonded substance?substance?

CC66HH1212OO66(s) (s) C C66HH1212OO66(aq)(aq)

How does a chemist How does a chemist represent the dissolving of represent the dissolving of

an an ionicallyionically bonded bonded substance?substance?

NaCl(s) NaCl(s) Na Na+1+1 (aq) + Cl(aq) + Cl--

11(aq)(aq)

What happens to an ionic What happens to an ionic substance when it substance when it

dissolves?dissolves?

It separates into ions.It separates into ions.

What is the equation for What is the equation for the dissolving of CaBrthe dissolving of CaBr22??

CaBrCaBr22(s) (s) Ca Ca+2+2(aq) + 2Br(aq) + 2Br--

11(aq)(aq)

Molecule-Ion AttractionMolecule-Ion Attraction

Interaction between water Interaction between water molecules and ions in solution.molecules and ions in solution.

What kind of molecule is What kind of molecule is HH22O?O?

Polar – the O end is a bit Polar – the O end is a bit negative & the H’s are a bit negative & the H’s are a bit

positive.positive.

Is the orange ion positive or negative & how do you know?

Is the orange ion positive or negative & how do you know?

Units of Solubility?Units of Solubility?

Grams of solute per 100 grams Grams of solute per 100 grams of solventof solvent

What happens to the What happens to the solubility of all gases as the solubility of all gases as the

temperature increases?temperature increases?

The solubility of gases The solubility of gases as the as the temperature temperature

What happens to the What happens to the solubility of most solids as solubility of most solids as

the temperature increases?the temperature increases?

The solubility of most solids The solubility of most solids as the temperature as the temperature ..

What do you need to What do you need to conduct electricity?conduct electricity?

Mobile charged particles!Mobile charged particles!

Electrolyte?Electrolyte?

A substance that dissolves in A substance that dissolves in water to produce a solution water to produce a solution

that conducts an electric that conducts an electric current!current!

Nonelectrolyte?Nonelectrolyte?

A substance that dissolves in A substance that dissolves in water to produce a solution water to produce a solution that does not conduct an that does not conduct an

electric current!electric current!

Saturated solutionSaturated solution

Contains the maximum amount Contains the maximum amount of dissolved solute at that of dissolved solute at that

temperature.temperature.

Supersaturated solutionSupersaturated solution

Contains more than the Contains more than the maximum amount of dissolved maximum amount of dissolved

solute at that temperature.solute at that temperature.

Unsaturated solutionUnsaturated solution

Contains less than the Contains less than the maximum amount of dissolved maximum amount of dissolved

solute at that temperature.solute at that temperature.

PrecipitationPrecipitation

The opposite of dissolving. A The opposite of dissolving. A solid comes out of solution.solid comes out of solution.

Dynamic EquilibriumDynamic Equilibrium

Term used to describe a Term used to describe a saturated solution. saturated solution.

Precipitation & dissolving are Precipitation & dissolving are ocurring at the same rates. No ocurring at the same rates. No

net change.net change.

How do you test a solution How do you test a solution for saturation?for saturation?

Throw a crystal of the solute Throw a crystal of the solute into the solution & observe into the solution & observe

what happens.what happens.

What are 3 possible What are 3 possible outcomes of the saturation outcomes of the saturation

test?test?

•Crystal dissolves – Soln was Crystal dissolves – Soln was unsaturated.unsaturated.•No change in crystal – Soln was No change in crystal – Soln was saturated.saturated.•Crystal gets larger – Soln was Crystal gets larger – Soln was supersaturated.supersaturated.

What are 3 regions of a What are 3 regions of a solubility curve?solubility curve?

•On the trace – saturated On the trace – saturated solution.solution.•Above the trace – Above the trace – supersaturated solution.supersaturated solution.•Below the trace – unsaturated Below the trace – unsaturated solution.solution.

ConcentrationConcentration

•A number that describes A number that describes how much solute compared how much solute compared to how much solution or how to how much solution or how much solvent.much solvent.

PercentPercent

Part over Whole X 100%Part over Whole X 100%

Molarity (M)Molarity (M)

Molarity = Molarity = # moles solute# moles soluteLiters of solutionLiters of solution

No. of Particles

No. of Moles

No. of Grams

No. ofLiters

X formula mass

X 22.4 L/molX 6.02 X 1023

by F.M.

by 6.02 X 1023

by 22.4

Mole Map

Parts per Million (PPM)Parts per Million (PPM)

PPM = PPM = grams solutegrams solute X X 10000001000000grams solutiongrams solution

How much KCl will dissolve in 300 grams of water at 50C?

Use the graph to set up a proportion.

Problem:

42 g KCl = X g KCl

100 g H2O 300 g H2O

X = 126 g KCl

88 g KNO3 in 100 g H2O at 50C.

20 g KNO3 in 100 g H2O at 10C.

88 g – 20 g = 68 g KNO3 precipitates.

50 to 10 - How much KNO3 precipitates?

source

Measuring Heat of Solution

If Temperature of H2O , dissolving was exothermic. If temperature of H2O , dissolving was endothermic.

Factors affecting SolubilityFactors affecting Solubility

•TemperatureTemperature•PressurePressure•Nature of the Solvent & SoluteNature of the Solvent & Solute

Nature?Nature?

•IonicIonic•Polar CovalentPolar Covalent•Nonpolar CovalentNonpolar Covalent

““Like Dissolves Like”Like Dissolves Like”

Nature of Nature of SoluteSolute

Nonpolar Nonpolar SolventSolvent

Polar Polar SolventSolvent

NonpolarNonpolar SolubleSoluble InsolubleInsoluble

PolarPolar InsolubleInsoluble SolubleSoluble

IonicIonic InsolubleInsoluble SolubleSoluble

MolarityC X VolumeC = MolarityD X VolumeD

MC X VC = MD X VD

Dilution Problems

Colligative PropertyColligative Property

Depends on the concentration of Depends on the concentration of the solute, NOT on the nature of the solute, NOT on the nature of

the solute. Does not matter if ions the solute. Does not matter if ions or neutral particles are in solution.or neutral particles are in solution.

What are 2 colligative What are 2 colligative properties?properties?

Freezing Point Depression & Freezing Point Depression & Boiling Point ElevationBoiling Point Elevation

Which solution has the most Which solution has the most dissolved particles?dissolved particles?

a)a)1 mole of C1 mole of C66HH1212OO66 in 1 Liter in 1 Liter HH22OO

b)b)1 mole of NaCl in 1 Liter H1 mole of NaCl in 1 Liter H22OO

c)c) 1 mole of CaBr1 mole of CaBr22 in 1 Liter H in 1 Liter H22OO