Aim: Using Table G to Predict SolubilityAim: Using Table G to Predict Solubility

Do Now: Take out HW

Complete #7-12 on page 9 of the packet

Do Now: Take out HW

Complete #7-12 on page 9 of the packet

Aim: Using Table F to Predict SolubilityAim: Using Table F to Predict Solubility

Table F gives us information on the solubility of various compounds in solution

You can predict the solubility of a compound or of the two products of a double replacement reaction

Table F gives us information on the solubility of various compounds in solution

You can predict the solubility of a compound or of the two products of a double replacement reaction

Recognizing & Understanding Double Replacement ReactionsRecognizing & Understanding

Double Replacement Reactions

Double reactions contain 2 ionic compounds Not every potential double replacement

reaction will occur

3 situations that ensure a DR reaction occurs: One of the products is a solid (a precipitate) One of the products is a gas A molecular substance such as water is formed

Double reactions contain 2 ionic compounds Not every potential double replacement

reaction will occur

3 situations that ensure a DR reaction occurs: One of the products is a solid (a precipitate) One of the products is a gas A molecular substance such as water is formed

3 Possible Outcomes of Double Replacement

3 Possible Outcomes of Double Replacement

One of the products must be: A solid

A gas

A molecular compound, like water

One of the products must be: A solid

A gas

A molecular compound, like water

Predicting Solubility with Table F

Predicting Solubility with Table F

Directions Circle the symbol of the first ion or element Underline the symbol of the second ion or

element Switch them around Use Table F to predict the solubility

Directions Circle the symbol of the first ion or element Underline the symbol of the second ion or

element Switch them around Use Table F to predict the solubility

Predicting Double Replacement

Products & Solubility

Predicting Double Replacement

Products & Solubility KI + Pb(NO3)2 +

1. Predict products: reactants swap places 2. Determine solubility of products

Example: For the reaction between LiBr and BaNO3, predict the products and determine their solubility

KI + Pb(NO3)2 +

1. Predict products: reactants swap places 2. Determine solubility of products

Example: For the reaction between LiBr and BaNO3, predict the products and determine their solubility

HomeworkHomework

Complete page 11 of the packet Complete page 11 of the packet

Aim: What are some factors that affect solubility?

Aim: What are some factors that affect solubility?

Do Now: packet page 12 Do Now: packet page 12

Dissolving DemoDissolving Demo

Styrofoam Salt Sugar

Styrofoam Salt Sugar

Unequal SolubilitiesUnequal Solubilities

Not all solutes dissolve to the same extent in the same solvent

Examples: NaNO3: 125g/100g

water at 60° C NaCl: ~39g/100g

water at 60° C

Not all solutes dissolve to the same extent in the same solvent

Examples: NaNO3: 125g/100g

water at 60° C NaCl: ~39g/100g

water at 60° C

But Why?But Why?

Factors Affecting SolubilityFactors Affecting Solubility

Temperature

Pressure

Particle size

Nature of the solute & solvent (polarity)

Temperature

Pressure

Particle size

Nature of the solute & solvent (polarity)

Solubility Factors: TemperatureSolubility Factors: Temperature

Solids: as temp , solubility

Liquids: as temp , solubility

Gas: as temp , solubility

Solids: as temp , solubility

Liquids: as temp , solubility

Gas: as temp , solubility

Solubility Factors: Pressure

Solubility Factors: Pressure

Solids: as pressure , no effect Liquids: as pressure , no effect Gas: as pressure , solubility

Solids: as pressure , no effect Liquids: as pressure , no effect Gas: as pressure , solubility

Applying principles of solubility and pressure, explain why soda goesflat when you open thecan.

Soda CarbonationSoda Carbonation

Solubility Factors: Particle Size

Solubility Factors: Particle Size

Particle size: smaller particles dissolve faster than larger particles

Stirring can increase the rate of dissolving and the solubility

Particle size: smaller particles dissolve faster than larger particles

Stirring can increase the rate of dissolving and the solubility

Solubility Factors: PolaritySolubility Factors: Polarity “Like Dissolves Like” Rule

Nonpolar solutes dissolve in nonpolar solvents Polar solutes dissolve in polar solvents

“Like Dissolves Like” Rule

Nonpolar solutes dissolve in nonpolar solvents Polar solutes dissolve in polar solvents

Solution VideoSolution Video

http://www.youtube.com/watch?v=VTmfQUNLlMY

http://www.youtube.com/watch?v=VTmfQUNLlMY

Complete pages 13 & 14 in the packet HW: page 15 in the packet

Complete pages 13 & 14 in the packet HW: page 15 in the packet

Colligative PropertiesColligative Properties

Colligative properties are physical properties of solutions that depend on the concentration of solute in a given amount of solvent

Dependent on how much solute is present, which is influenced by the nature of the solute

Greater concentration gives greater effects

Colligative properties are physical properties of solutions that depend on the concentration of solute in a given amount of solvent

Dependent on how much solute is present, which is influenced by the nature of the solute

Greater concentration gives greater effects

ElectrolytesElectrolytes

Electrolytes are substances that separate to produce ions when dissolved in a solution Conduct electricity, turn on light bulb tester Ex: ionic compounds (salts), acids, bases

Nonelectrolytes do not produce ions (stay in one piece) in solution Do not conduct electricity, do not turn on light bulb

tester Ex: sugars, alcohols

Electrolytes are substances that separate to produce ions when dissolved in a solution Conduct electricity, turn on light bulb tester Ex: ionic compounds (salts), acids, bases

Nonelectrolytes do not produce ions (stay in one piece) in solution Do not conduct electricity, do not turn on light bulb

tester Ex: sugars, alcohols

Electrolytes vs. NonelectrolytesElectrolytes vs. Nonelectrolytes

Electrolytes

Nonelectrolytes

Electrolytes

Nonelectrolytes

Electrolyte or Nonelectrolyte?Electrolyte or

Nonelectrolyte? Electrolytes

Ionic substances Acids: X-H

Bases M-OH

Electrolytes Ionic substances

Acids: X-H Bases M-OH

Nonelectrolytes Sugars Alcohols

Nonelectrolytes Sugars Alcohols

Colligative PropertiesColligative Properties

Boiling Point Elevation the temperature at which a liquid normally boils

goes up when solute particles are dissolved

Freezing Point Depression the temperature at which a liquid normally freezes

goes down when solute particles are dissolved

Boiling Point Elevation the temperature at which a liquid normally boils

goes up when solute particles are dissolved

Freezing Point Depression the temperature at which a liquid normally freezes

goes down when solute particles are dissolved

Boiling Point ElevationBoiling Point Elevation

The boiling point of a solution increases when solute particles are added

Example: Adding salt to water raises the water’s boiling point Water now gets hotter than 100° C (102-103°)

before it boils, and pasta will cook faster

The boiling point of a solution increases when solute particles are added

Example: Adding salt to water raises the water’s boiling point Water now gets hotter than 100° C (102-103°)

before it boils, and pasta will cook faster

Freezing Point DepressionFreezing Point Depression

The freezing point of a solution decreases when solute particles are added

Example: Putting salt on roads causes ice to melt Ice’s freezing point becomes lower than 0°, so

water stays liquid at temperatures where it would normally be solid ice

The freezing point of a solution decreases when solute particles are added

Example: Putting salt on roads causes ice to melt Ice’s freezing point becomes lower than 0°, so

water stays liquid at temperatures where it would normally be solid ice

Vapor PressureVapor Pressure

When a substance that is normally solid or liquids at room temperature enters the gas phase, it is called a vapor

Pressure exerted by this vapor is vapor pressure

When a substance that is normally solid or liquids at room temperature enters the gas phase, it is called a vapor

Pressure exerted by this vapor is vapor pressure

Do Now and HWDo Now and HW

Now: Complete pages 16 to 18 of the packet

HW: Complete pages 24 and 25 of the packets

Now: Complete pages 16 to 18 of the packet

HW: Complete pages 24 and 25 of the packets

ConcentrationConcentration

Concentration is the amount of solute dissolved in a solution

Several ways to express concentration: Grams solute/100mL solvent (Table G) % composition by mass % composition by volume Parts per Million Molarity

Concentration is the amount of solute dissolved in a solution

Several ways to express concentration: Grams solute/100mL solvent (Table G) % composition by mass % composition by volume Parts per Million Molarity

Percent CompositionPercent Composition

Labels often list ingredients as a percent by mass or percent by volume

Labels often list ingredients as a percent by mass or percent by volume

Percent Compositionby Mass and by Volume

Percent Compositionby Mass and by Volume

Ratio of the mass (or volume) of one part compared to the mass (or volume) of the whole

Usedw/ solids

Usedw/ liquids

Percent CompositionPercent Composition

What is the percent by mass of sodium hydroxide if 5g of NaOH are added to 50g of water?

What is the percent by volume of alcohol is 50mL of ethanol is diluted with water to form a total volume of 3000mL?

What is the percent by mass of sodium hydroxide if 5g of NaOH are added to 50g of water?

What is the percent by volume of alcohol is 50mL of ethanol is diluted with water to form a total volume of 3000mL?

Parts Per Million (ppm)Parts Per Million (ppm)

If you divide a pie into 10 equal pieces, each piece is a part-per-ten (1/10th)

Divide the pie into a million pieces, and each piece is a part per million, (1/1,000,000th)

If you divide a pie into 10 equal pieces, each piece is a part-per-ten (1/10th)

Divide the pie into a million pieces, and each piece is a part per million, (1/1,000,000th)

Parts Per Million (ppm)Parts Per Million (ppm)

Similar to percent composition, parts per million is a ratio between mass of the solute and the total mass of solution

Useful for very dilute solutions In swimming pools, only 2g of chlorine for every 2

million g of water

Similar to percent composition, parts per million is a ratio between mass of the solute and the total mass of solution

Useful for very dilute solutions In swimming pools, only 2g of chlorine for every 2

million g of water

At 40 C, carbon dioxide has a solubility of 0.0972g/100g H2O. What is the concentration of CO2, expressed in parts per million?

At 40 C, carbon dioxide has a solubility of 0.0972g/100g H2O. What is the concentration of CO2, expressed in parts per million?

A substance has a solubility of 350ppm. How many grams of the substance are present in 1.0L of a saturated solution?

A substance has a solubility of 350ppm. How many grams of the substance are present in 1.0L of a saturated solution?

Now: find review book q’s HW: complete page 27 of the packet

Now: find review book q’s HW: complete page 27 of the packet

Molarity (M)Molarity (M)

Measures concentration in moles

Higher molarity = more concentrated Important to note that molarity is moles of

solute per liter of solution, not solvent

Measures concentration in moles

Higher molarity = more concentrated Important to note that molarity is moles of

solute per liter of solution, not solvent

Molarity (M)

Molarity (M)

Example: What is the molarity of a solution that contains 4.0 moles of NaOH in 0.50 L of solution?

Example: What is the molarity of a solution that contains 4.0 moles of NaOH in 0.50 L of solution?

Now: complete pages 21 and 22 of the packet

HW: complete page 26 of the packet

Now: complete pages 21 and 22 of the packet

HW: complete page 26 of the packet