2Types of mixtures Heterogeneous mixture: Suspension: Colloids: Heterogeneous mixtures do not blend smoothly. Individual substances can still be seenSuspension:A suspension is a heterogeneous mixture where particles will settle to the bottom if left undisturbed.Example: sand in water.Colloids:Colloids are heterogeneous mixtures where particles will not settle to the bottom.Example: Milk
3Homogeneous MixturesHomogeneous mixtures are mixtures where a substance is dissolved in another substance. These are also called solutions.Parts of a solution:Solute: The substance that is dissolvedSolvent: The substance that does the dissolvingWhen a solute readily dissolves in a solvent it is said to be soluble.Two liquids that can be combined to make a solution are said to be miscible.
4A solute that does not readily dissolve in a solvent is said to be insoluble. Two liquids that do no mix to form a new solution are said to be immiscible.
5Solution Concentration Concentration is the measure of how much solute is dissolved in the solution.There are many ways to measure concentrationPercent by mass:(Mass of solute/Mass of solution) x 100Percent by volume:(Volume of solute/Volume of solution) x 100Molarity:Moles of solute/Liter of solutionMolality:Moles of solute/Kilograms of solventMole Fraction:Moles of solute/Moles of solute + Moles of solvent
6Percent by massIn order to maintain a sodium chloride concentration similar to ocean water, an aquarium must contain 3.6g NaCl per g of water. What is the percent by mass of NaCl in the solution?3.5%What is the percent by mass of NaHCO3 in a solution containing 20.0 g of NaHCO3 dissolved in mL of H2O?3%
7Percent by VolumeWhat is the percent by volume of ethanol in a solution that contains 35mL of ethanol dissolved in 155mL of water?18%
8MolarityA mL intravenous solution contains 5.10 g of glucose. What is the molarity of the solution? The molar mass of glucoes is g/mol0.282M
9If you have 1500 g of a bleach solution with a percent by mass of NaOCl of 3.62 % how many grams of NaCOl are in the solution?54.3 gWhat is the percent by volume of isopropyl alcohol in a solution that contains 24 mL of isopropyl alcohol in 1.1 L of water?2.1 %Calculate the molarity of 1.6 L of a solution containing 1.55 g of KBr.8.13 x 10-3
10MolalityIn the lab a student adds 4.5 g of NaCl to g of water. Calculate the molaity of the solution.0.77 mol/kg
11Preparing SolutionsHow would you prepare 1 L of a 1.5 molar CuSO4 Solution?Diluting Solutions:Dilution equation M1V1 = M2V2Calculate the new volume if you wanted to dilute the above solution to 0.5 molar.
12Diluting Solutions Remember Molarity = (Moles of solute/Liters of solvent)The Dilution Equation:M1V1 = M2V2Example:What volume of a 2.00M CaCl2 solution would you use to make 0.50 L of a 0.300M solution?M1 = 2.00MV1 = ?M2 = 0.300MV2 = 0.5L(2.00M)(V1) = (0.300M)(0.5L)V1 = L
13What volume of a 3. 00M KI solution would you use to make 0 What volume of a 3.00M KI solution would you use to make L of a 1.25M KI solution?125mLHow many milliliters of a 5.0M H2SO4 stock solution would you need to prepare 100.0mL of 0.25M H2SO4?5.0mL
14Mole FractionTo express concentration as a mole fraction we need to know the number of moles of solute and the number of moles of solvent.The mole fraction is calculated by dividing the number of moles of either the solute or solvent by the total number of moles in the solution.
15ExampleIf we have a solution that contains 36 g of HCl and 64 g of H2O. What are the mole fractions of HCl and H2O?HCl:H2O:
16PracticeWhat is the mole fraction of NaOH in an aqueous solution that contains 22.8% NaOH by mass?If the mole fraction of H2SO4 is an aqueous solution is 0.325, what is the percent by mass of H2SO4
17Factors Affecting Solvation Many physical factors affect the solubility of a solute.Such as:TemperaturePressurePolaritySolvation is the process of surrounding solute particles with solvent particles.
18Aqueous ionic solutions Many ionic compounds are soluble in water. Why?Water is a polar molecule.Why might an ionic compound not be water soluble?
19Heat of solutionThe overall energy change that occurs during the formation of a solution is called the heat of solution.certain solvation processes are exothermic while others are endothermic.
20Factors that affect solvation Agitation:Stirring or shaking moves solvated particles away from the surface of the solid and allows more solute particles to move into solution.Surface Area:Breaking the solute into small pieces increases the available surface area and increase the rate of solvation.Temperature:As temperature increase so does the rate of solvation.
21Types of solutions Unsaturated: Saturated: Supersaturated solution: A solution that more solute could be dissolved in.Saturated:In a saturated solution the rate of solvation and the rate of crystallization are in equilibrium.Supersaturated solution:A super saturated solution is a solution that has more solute dissolved in it that it would normally allow.
22Solubility of GasesUnlike solid solutes the solubility of gases (CO2, or O2 for example) increases as the temperature of the solvent goes down.The solubility of gases is also affected by pressure. How?Think about soda.
23Henry’s LawHenry’s Law states that at a constant temperature, the solubility (S) of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.Henry’s LawS1/P1 = S2/P2Example:If 0.85g of a gas at 4.0 atm of pressure dissolves in 1.0 L of water at 25o C, how much will dissolve in 1.0 L at 1.0 atm at the same temperature?0.21 g
24Decompression Sickness Decompression sickness is a term used to describe the effects of a drop in external pressure on a persons body.One common symptom of decompression sickness is AGE, Arterial Gas Embolism.The bubbles that form in the blood stream from gas leaving solution can restrict blood flow.
26Boiling Point Elevation Dissolving a solute in a solution raises the boiling point of the solution.This is called boiling point elevation.We can calculate the difference in boiling point (Δ Tb) by multiplying a solutions molality by a constant we look up for our particular solvent (Kb).Δ Tb = Kbm
27What is the boiling point of a 0 What is the boiling point of a 0.625m aqueous solution of a nonelectrolyte?
28What is the boiling point of a 0 What is the boiling point of a 0.4m aqueous solution of Ca(OH)2 (A strong electrolyte) Kb = oC/m
29Molal Boiling Point Elevation Constants. SolventBoiling Point (oC)Kb (oC/m)Water100.00.512Benzene80.12.53Chloroform61.73.63Ethanol78.51.22
30Freezing Point Depression Adding a solute to a solvent also lowers the solvents freezing point.The equation is very similar to boiling point elevation.ΔTf = Kf mSolventFreezing Point (oC)Kf (oC/m)Water0.001.86Benzene5.55.12Ethanol-114.11.99
31ExampleSodium chloride is often used to prevent icy roads and to freeze ice cream. What are the boiling point and freezing point of a 0.029m AQUEOUS solution of sodium chloride?BP: CFP: oC
33Calculate the freezing and boiling point of a solution containing 6 Calculate the freezing and boiling point of a solution containing 6.42 g of sucrose (a nonelectrolyte) in g of water.Tf = oCTb = oCCalculate the freezing and boiling point of a solution containing 23.7 g of Copper (II) sulfate (A strong electrolyte) in 250 g of waterTf = oCTb = oCCalculate the freezing and boiling point of a solution containing 0.15 moles of the compound naphthalene, a nonelectrolyte in 175 g of benzene (Normal F.P. = 5.5, Normal B.P. = 80.1, Kf = 5.12, Kb = 2.53)Tf = 1.1 oCTb = 82.3 oC