Kool Aid Jello Chapter

Kool Aid Jello Chapter

How to make super kool aid or extreme jello

How to make super kool aid or extreme jello

Kool Aid drinks are solutionsKool Aid drinks are solutions• Solutions are homogenous mixtures of two

or more pure substances in a single phase• Contains a solvent and solute

– Solvent: dissolving medium (water)– Solute: dissolved substance(salt)

• Particle sizes are the smallest• Will not separate while standing• Do not filter• Do not scatter light• Colligative properties are affected

• Solutions are homogenous mixtures of two or more pure substances in a single phase

• Contains a solvent and solute– Solvent: dissolving medium (water)– Solute: dissolved substance(salt)

• Particle sizes are the smallest• Will not separate while standing• Do not filter• Do not scatter light• Colligative properties are affected

SolutionsSolutions

Muddy water is a SuspensionMuddy water is a Suspension• Suspensions are heterogeneous

mixtures that have the largest particles of all mixtures– Will separate upon standing– Can be filtered– Do scatter light– Colligative properties are unaffected– Examples: Muddy water, Cu Lab.

• Suspensions are heterogeneous mixtures that have the largest particles of all mixtures– Will separate upon standing– Can be filtered– Do scatter light– Colligative properties are unaffected– Examples: Muddy water, Cu Lab.

SuspensionsSuspensions

Milk/Gelatins are ColloidsMilk/Gelatins are Colloids

• Colloids are homogeneous mixtures that are medium in size.

• Particles remain dispersed in liquid due to random particle motion of surrounding molecules.– Will separate very slowly or not at all– Will not filter– Will scatter light– Colligative properties are unaffected.

• Colloids are homogeneous mixtures that are medium in size.

• Particles remain dispersed in liquid due to random particle motion of surrounding molecules.– Will separate very slowly or not at all– Will not filter– Will scatter light– Colligative properties are unaffected.

What is this scattering light?What is this scattering light?

Tyndall EffectTyndall Effect

• Light bounces off objects it cannot pass through, is scattered by objects, or passes right through objects.

• The scattering of light as it passes through a transparent medium is called the Tyndall Effect.

• Light bounces off objects it cannot pass through, is scattered by objects, or passes right through objects.

• The scattering of light as it passes through a transparent medium is called the Tyndall Effect.

• When focused light is shined on a homogeneous solution the light will not be scattered; it will pass right through.

• When focuses light is shined on a colloid the light will be scattered and no longer as focused.

• When focused light is shined on a homogeneous solution the light will not be scattered; it will pass right through.

• When focuses light is shined on a colloid the light will be scattered and no longer as focused.

What are they?What are they?• Oil and vinegar salad dressing?• Gelatin?• Starch in water?• Smoke in air?• Salt in water?• Clay in water?• Food coloring in water?

• Oil and vinegar salad dressing?• Gelatin?• Starch in water?• Smoke in air?• Salt in water?• Clay in water?• Food coloring in water?

• Carbon dioxide in water?• Steam in air?• Table sugar in water?• Milk?• Bleach?• Ammonia?• Tea?

• Carbon dioxide in water?• Steam in air?• Table sugar in water?• Milk?• Bleach?• Ammonia?• Tea?

More on SolutionsMore on Solutions

The M’s of it allThe M’s of it all

ConcentrationConcentration

• Different solutions can have different concentrations by dissolving more or less solute in a given amount of solvent

Concentrations is scaled on molality and molarity

• Different solutions can have different concentrations by dissolving more or less solute in a given amount of solvent

Concentrations is scaled on molality and molarity

MolarityMolarity

• Molarity(M) is defined as the number of moles of solute per liter of solution

• M=moles of solute/liters of solution

• Molarity(M) is defined as the number of moles of solute per liter of solution

• M=moles of solute/liters of solution

MolalityMolality

• Molality(m) is defined at the number of moles of solute divided by the number of kilograms of solvent

• M = moles of solute/kg of solvent

• Molality(m) is defined at the number of moles of solute divided by the number of kilograms of solvent

• M = moles of solute/kg of solvent

SolubilitySolubility

• Solubility is the chemical process in which chemicals are able to dissolve each other (able to mix well)

• The ability to mixed is determined by the types of bonds holding the chemical together.

• “like dissolve like”

• Solubility is the chemical process in which chemicals are able to dissolve each other (able to mix well)

• The ability to mixed is determined by the types of bonds holding the chemical together.

• “like dissolve like”

MiscibleMiscible

• Alcohol and water mix quite readily due to the stronger forces of attraction between the solvent and solute.

• Both water and alcohol are polar bonds and therefore can dissolve each other.

• Miscible is the ability to dissolve each other due to similar bonds

• Alcohol and water mix quite readily due to the stronger forces of attraction between the solvent and solute.

• Both water and alcohol are polar bonds and therefore can dissolve each other.

• Miscible is the ability to dissolve each other due to similar bonds

ImmiscibleImmiscible

• Immiscible chemicals have opposite forces of attraction and therefore DO NOT MIX

• Oil and water• Mystic sand and water

• Immiscible chemicals have opposite forces of attraction and therefore DO NOT MIX

• Oil and water• Mystic sand and water

Colligative Properties of

Solutions

Colligative Properties of

Solutions

Not freezing when cold or boiling when hot!

Not freezing when cold or boiling when hot!

Colligative PropertiesColligative Properties

• Some of the properties of solutions Some of the properties of solutions do not depend on the amount and do not depend on the amount and type of solute present in solution.type of solute present in solution.– Ie food coloring doesn’t affect the Ie food coloring doesn’t affect the

boiling point of water (much)boiling point of water (much)• Properties that depend on the Properties that depend on the

concentration of solute particles concentration of solute particles but not on their identity are called but not on their identity are called Colligative properties.Colligative properties.

• Some of the properties of solutions Some of the properties of solutions do not depend on the amount and do not depend on the amount and type of solute present in solution.type of solute present in solution.– Ie food coloring doesn’t affect the Ie food coloring doesn’t affect the

boiling point of water (much)boiling point of water (much)• Properties that depend on the Properties that depend on the

concentration of solute particles concentration of solute particles but not on their identity are called but not on their identity are called Colligative properties.Colligative properties.

Electrolyte and non ElectrolyteElectrolyte and non Electrolyte• Electrolytes are substances that

dissolve in water to give a solution that conducts an electric current– Sports drinks and salt water– Ionic compounds are usually strong

electrolytes because they separate completely in water

– Covalent compounds can be strong, weak or non electroyltes

• Electrolytes are substances that dissolve in water to give a solution that conducts an electric current– Sports drinks and salt water– Ionic compounds are usually strong

electrolytes because they separate completely in water

– Covalent compounds can be strong, weak or non electroyltes

• Non-electrolytesNon-electrolytes: a liquid or solid : a liquid or solid substance that does not allow the substance that does not allow the flow of an electric current, either in flow of an electric current, either in solution or in its pure state, such solution or in its pure state, such as water or sucrose.as water or sucrose.

• Nonvolatile substance is one that Nonvolatile substance is one that has little tendency to become a has little tendency to become a gas under existing conditionsgas under existing conditions

• Non-electrolytesNon-electrolytes: a liquid or solid : a liquid or solid substance that does not allow the substance that does not allow the flow of an electric current, either in flow of an electric current, either in solution or in its pure state, such solution or in its pure state, such as water or sucrose.as water or sucrose.

• Nonvolatile substance is one that Nonvolatile substance is one that has little tendency to become a has little tendency to become a gas under existing conditionsgas under existing conditions

Freezing point depressionFreezing point depression

The freezing point of a 1 molal solution of any nonelectrolyte solute in water is found to be 1.86 degrees lower than the freezing point of water.

Thus 1 mole of solute in 1 kg of water will equal -1.86 degree C

The freezing point of a 1 molal solution of any nonelectrolyte solute in water is found to be 1.86 degrees lower than the freezing point of water.

Thus 1 mole of solute in 1 kg of water will equal -1.86 degree C

• If you had 2 moles of solute in 1 kg of water the freezing point would be

-3.72 degree C. • This is 1.86 X 2• This 1.86 degree C/m is known as

molal freezing point constant (Kf)

• Molal Freezing point constant is the freezing point depression of the solvent in a 1 molal solution of a nonvolatile, non electrolyte solute.

• If you had 2 moles of solute in 1 kg of water the freezing point would be

-3.72 degree C. • This is 1.86 X 2• This 1.86 degree C/m is known as

molal freezing point constant (Kf)

• Molal Freezing point constant is the freezing point depression of the solvent in a 1 molal solution of a nonvolatile, non electrolyte solute.

Kf for substancesKf for substances

• Each solvent has its own characteristic molal freezing point constant.

• Kf is most accurate at 1 atm.

• Kf for water is -1.86, for Ether is -1.79 and Acetic Acid -3.90

• Each solvent has its own characteristic molal freezing point constant.

• Kf is most accurate at 1 atm.

• Kf for water is -1.86, for Ether is -1.79 and Acetic Acid -3.90

• The freezing point depression, ∆tf, is the difference between the freezing points of the pure solvent and a solution of a non electrolyte in that solvent, and it is directly proportional to the molal concentration of the solution.

• ∆∆ttff=Kf*m

• The freezing point depression, ∆tf, is the difference between the freezing points of the pure solvent and a solution of a non electrolyte in that solvent, and it is directly proportional to the molal concentration of the solution.

• ∆∆ttff=Kf*m

Did you know?Did you know?

• Some animals are able to survive freezing temperatures by producing natural antifreezes, substances that lower the freezing point of a liquid. In many freeze-tolerant insects, the antifreezes are alcohols and sugars.

• Examples are box turtles, painted turtles and garter snakes, sugar maples and white spruce.

• Some animals are able to survive freezing temperatures by producing natural antifreezes, substances that lower the freezing point of a liquid. In many freeze-tolerant insects, the antifreezes are alcohols and sugars.

• Examples are box turtles, painted turtles and garter snakes, sugar maples and white spruce.

Sugar MapleSugar Maple

• Taking a sugar substance from a tree can be used to create maple syrup

• The maple syrup aqueous solution boils at 219 degree F

• That is 7 degree higher than water.

• Why?

• Taking a sugar substance from a tree can be used to create maple syrup

• The maple syrup aqueous solution boils at 219 degree F

• That is 7 degree higher than water.

• Why?

Boiling point elevationBoiling point elevation

• The boiling point of a liquid is the temperature at which the vapor pressure of the liquid is equal to the prevailing atmospheric pressure.

• Vapor pressures of solutions containing nonvolatile solute is lower than the vapor pressure of the pure solvent.

• The boiling point of a liquid is the temperature at which the vapor pressure of the liquid is equal to the prevailing atmospheric pressure.

• Vapor pressures of solutions containing nonvolatile solute is lower than the vapor pressure of the pure solvent.

• This means that more heat will be required to raise the vapor pressure of the solution. Thus, the boiling point of a solution is higher than the boiling point of the pure substance.

• The molal boiling point constant, Kb, is the boiling point elevation of the solvent in a 1 molal solution of a nonvolatile, non electrolyte solute.

• This means that more heat will be required to raise the vapor pressure of the solution. Thus, the boiling point of a solution is higher than the boiling point of the pure substance.

• The molal boiling point constant, Kb, is the boiling point elevation of the solvent in a 1 molal solution of a nonvolatile, non electrolyte solute.

Boiling point elevationBoiling point elevation

• Boiling point elevation, ∆tb, is the difference between the boiling points of the pure solvent and a nonelectrolyte solution of that solvent, and it is directly proportional to the molal concentration of the solution.

• ∆tb=Kb*m

• Boiling point elevation, ∆tb, is the difference between the boiling points of the pure solvent and a nonelectrolyte solution of that solvent, and it is directly proportional to the molal concentration of the solution.

• ∆tb=Kb*m

What about Electrolytes?What about Electrolytes?

• Electrolytes break apart into ions. Each ion has an effect on boiling point and freezing points. If a solution has more or less ions it will change the boiling points and melting points even more.

• Electrolytes break apart into ions. Each ion has an effect on boiling point and freezing points. If a solution has more or less ions it will change the boiling points and melting points even more.

IonsIons

• ∆tb or f=Kb or f*m*n

• m=molality• n = number of ions

– Example • NaCl = Na+ and Cl- = 2 ions=2 n

• MgCl2= Mg+ and 2 Cl- =3 ions =3 n

• Fe2(SO4)3=2 Fe+3 and 3 SO4-2 = 5 ions or

5 n

• ∆tb or f=Kb or f*m*n

• m=molality• n = number of ions

– Example • NaCl = Na+ and Cl- = 2 ions=2 n

• MgCl2= Mg+ and 2 Cl- =3 ions =3 n

• Fe2(SO4)3=2 Fe+3 and 3 SO4-2 = 5 ions or

5 n

ExampleExample

• What is the new freezing point of 200 mL of water (Kf = -1.86 oC) if195 g of sucrose (C12H22O11) are added to it?

• What is the new freezing point of 200 mL of water (Kf = -1.86 oC) if195 g of sucrose (C12H22O11) are added to it?

195 g sucrose

342 g= .570 moles

.570 moles

.200 Kg= 2.85 molal

Now we can plug into ∆t∆tff=Kf*m

∆∆ttff=(-1.86oC) * (2.85 molal)

∆∆ttff= -5.3010C

This means the water will freeze This means the water will freeze 5.3015.301ooC below its freezing point.C below its freezing point.

∆tb or f=Kb or f*m*n∆tb or f=Kb or f*m*n

• Same as other formula, just adding n.

• NaCl, K2SO4, AlCl3, Al2O3.

• Same as other formula, just adding n.

• NaCl, K2SO4, AlCl3, Al2O3.