Solutions--Chemistry-Geek解決的方案化學(xué)怪才

1、SolutionsWhy does a raw egg swell or shrink when placed in different solutions?Chemistry I Chapters 15 & 16Chemistry I HD Chapter 15ICP Chapter 22SAVE PAPER AND INK! When you print out the notes on PowerPoint, print Handouts instead of Slides in the print setup. Also, turn off the backgrounds (Tools

2、OptionsPrintUNcheck Background Printing)!Some DefinitionsA solution is a _ mixture of 2 or more substances in a single phase. One constituent is usually regarded as the SOLVENT and the others as SOLUTES.Parts of a SolutionSOLUTE the part of a solution that is being dissolved (usually the lesser amou

3、nt)SOLVENT the part of a solution that dissolves the solute (usually the greater amount)Solute + Solvent = SolutionSoluteSolventExamplesolidsolidsolidliquidgassolidliquidliquidgasliquidgasgasDefinitionsSolutions can be classified as saturated or unsaturated.A saturated solution contains the maximum

4、quantity of solute that dissolves at that temperature.An unsaturated solution contains less than the maximum amount of solute that can dissolve at a particular temperatureExample: Saturated and Unsaturated FatsUnsaturated fats have at least one double bond between carbon atoms; monounsaturated means

5、 there is one double bond, polysaturated means there are more than one double bond. Thus, there are some bonds that can be broken, chemically changed, and used for a variety of purposes. These are REQUIRED to carry out many functions in the body. Fish oils (fats) are usually unsaturated. Game animal

6、s (chicken, deer) are usually less saturated, but not as much as fish. Olive and canola oil are monounsaturated.Saturated fats are called saturated because all of the bonds between the carbon atoms in a fat are single bonds. Thus, all the bonds on the carbon are occupied or “saturated” with hydrogen

7、. These are stable and hard to decompose. The body can only use these for energy, and so the excess is stored. Thus, these should be avoided in diets. These are usually obtained from sheep and cattle fats. Butter and coconut oil are mostly saturated fats.DefinitionsSUPERSATURATED SOLUTIONS contain m

8、ore solute than is possible to be dissolvedSupersaturated solutions are unstable. The supersaturation is only temporary, and usually accomplished in one of two ways:Warm the solvent so that it will dissolve more, then cool the solution Evaporate some of the solvent carefully so that the solute does

9、not solidify and come out of solution. SupersaturatedSodium AcetateOne application of a supersaturated solution is the sodium acetate “heat pack.”IONIC COMPOUNDSCompounds in Aqueous SolutionMany reactions involve ionic compounds, especially reactions in water aqueous solutions.KMnO4 in waterK+(aq) +

10、 MnO4-(aq)How do we know ions are present in aqueous solutions?The solutions _They are called ELECTROLYTESHCl, MgCl2, and NaCl are strong electrolytes. They dissociate completely (or nearly so) into ions.Aqueous SolutionsAqueous SolutionsSome compounds dissolve in water but do not conduct electricit

11、y. They are called nonelectrolytes.Examples include:sugarethanolethylene glycolIts Time to Play Everyones Favorite Game Show Electrolyte or Nonelectrolyte!Electrolytes in the BodyCarry messages to and from the brain as electrical signalsMaintain cellular function with the correct concentrations elec

12、trolytesMake your own50-70 g sugarOne liter of warm waterPinch of salt200ml of sugar free fruit squashMix, cool and drinkConcentration of SoluteThe amount of solute in a solution is given by its concentration.Molarity(M)=moles soluteliters of solution1.0 L of water was used to make 1.0 L of solution

13、. Notice the water left over.PROBLEM: Dissolve 5.00 g of NiCl26 H2O in enough water to make 250 mL of solution. Calculate the Molarity.Step 1: Calculate moles of NiCl26H2OStep 2: Calculate MolarityNiCl26 H2O = 0.0841 MStep 1: Change mL to L.250 mL * 1L/1000mL = 0.250 LStep 2: Calculate.Moles = (0.05

14、00 mol/L) (0.250 L) = 0.0125 molesStep 3: Convert moles to grams.(0.0125 mol)(90.00 g/mol) = 1.13 gUSING MOLARITYmoles = MVWhat mass of oxalic acid, H2C2O4, isrequired to make 250. mL of a 0.0500 Msolution?Learning CheckHow many grams of NaOH are required to prepare 400. mL of 3.0 M NaOH solution?1)

15、12 g2)48 g3) 300 gAn IDEAL SOLUTION is one where the properties depend only on the concentration of solute.Need conc. units to tell us the number of solute particles per solvent particle.The unit “molarity” does not do this!Concentration UnitsTwo Other Concentration Unitsgrams solutegrams solutionMO

16、LALITY, m% by mass =% by mass m of solution= mol solutekilograms solventCalculating ConcentrationsDissolve 62.1 g (1.00 mol) of ethylene glycol in 250. g of H2O. Calculate molality and % by mass of ethylene glycol. Calculating ConcentrationsCalculate molality Dissolve 62.1 g (1.00 mol) of ethylene g

17、lycol in 250. g of H2O. Calculate m & % of ethylene glycol (by mass).Calculate weight %Learning CheckA solution contains 15 g Na2CO3 and 235 g of H2O? What is the mass % of the solution? 1) 15% Na2CO32) 6.4% Na2CO33) 6.0% Na2CO3Using mass %How many grams of NaCl are needed to prepare 250 g of a 10.0

18、% (by mass) NaCl solution? Try this molality problem25.0 g of NaCl is dissolved in 5000. mL of water. Find the molality (m) of the resulting solution.m = mol solute / kg solvent25 g NaCl 1 mol NaCl 58.5 g NaCl= 0.427 mol NaClSince the density of water is 1 g/mL, 5000 mL = 5000 g, which is 5 kg0.427

19、mol NaCl 5 kg water= 0.0854 m salt waterColligative PropertiesOn adding a solute to a solvent, the properties of the solvent are modified.Vapor pressure decreasesMelting point decreasesBoiling point increasesOsmosis is possible (osmotic pressure)These changes are called COLLIGATIVE PROPERTIES. They

20、depend only on the NUMBER of solute particles relative to solvent particles, not on the KIND of solute particles.Change in Freezing Point The freezing point of a solution is LOWER than that of the pure solventPure waterEthylene glycol/water solutionChange in Freezing Point Common Applications of Fre

21、ezing Point DepressionPropylene glycolEthylene glycol deadly to small animalsCommon Applications of Freezing Point DepressionWhich would you use for the streets of Bloomington to lower the freezing point of ice and why? Would the temperature make any difference in your decision?sand, SiO2Rock salt,

22、NaClIce Melt, CaCl2Change in Freezing Point Change in Boiling Point Common Applications of Boiling Point ElevationBoiling Point Elevation and Freezing Point Depression T = Kmii = vant Hoff factor = number of particles produced per molecule/formula unit. For covalent compounds, i = 1. For ionic compo

23、unds, i = the number of ions present (both + and -)CompoundTheoretical Value of iglycol1NaCl2CaCl23Ca3(PO4)25Boiling Point Elevation and Freezing Point Depression T = KmiSubstance Kb benzene 2.53 camphor 5.95 carbon tetrachloride 5.03 ethyl ether 2.02 water 0.52 m = molalityK = molal freezing point/

24、boiling point constantSubstance Kf benzene 5.12 camphor 40. carbon tetrachloride 30. ethyl ether 1.79 water 1.86 Change in Boiling Point Dissolve 62.1 g of glycol (1.00 mol) in 250. g of water. What is the boiling point of the solution?Kb = 0.52 oC/molal for water (see Kb table).SolutionTBP = Kb m i

25、1.Calculate solution molality = 4.00 m2.TBP = Kb m i TBP = 0.52 oC/molal (4.00 molal) (1) TBP = 2.08 oC BP = 100 + 2.08 = 102.08 oC (water normally boils at 100)Calculate the Freezing Point of a 4.00 molal glycol/water solution.Kf = 1.86 oC/molal (See Kf table)SolutionTFP = Kf m i = (1.86 oC/molal)(4.00 m)(1