ࡱ> y  bjbj /9{{MUm DDDXXX8tX$p&dd%%%ooooooo$JrtBoD%@%@%%%ox o)))%T8Do)%o))d,7jC/l&FgHoo0$pgd>v'>v7j>vD7jX%%)%%%%%oo,(%%%$p%%%%>v%%%%%%%%% : Pure Substances and Mixtures SubstanceElementCompoundHomogeneous Mixture (solution)Heterogeneous MixtureCan it be physically separated?Can it be chemically separated?WaterCalciumVinegar (water + acetic acid)Trail mixClassify each of the following substances and identify whether it can be physically/chemically seperated For a solution of iodine dissolved in ethanol, which is the solute? Which is the solvent? Iodine is the solute, ethanol is the HCl is a polar compound. Will it dissolve in water or oil? Benzene is a nonpolar compound. Will it dissolve in water or oil? Do you think sugar is a polar or nonpolar compound? Explain why. a polar compound because it dissolves in water. Solutions Describe three methods to increase the rate of dissolution for sugar in a cup of tea. the to increase its surface Explain the difference between rate of dissolution and solubility. Solubility describes how much of a solute can dissolve at a given temperature. How can you increase the solubility of a solid solute? Heating the solution usually increases the solubility of a solid solute. Name two things that increase the solubility of a gaseous solute and name two things that decrease: Increase: Decrease:g the temperature and \\ What effect do agitation and surface area have on solubility? and surface area have no effect on solubility. They only affect rate of dissolution. Of saturated, unsaturated and supersaturated, which word describes a solution with the maximum amount of dissolved solute for a given temperature? Which is less than the maximum? Which is more than the maximum? How is it possible to dissolve more than the maximum amount of solute for a given temperature? What happens to a supersaturated solution if it is disturbed? Solubility Curves Answer the following questions based on the solubility curve below.  Which salt is least soluble in water at 20C? KClO3 Which salt is least soluble at 50C? Ce2(SO4)3 How many grams of KCl can be dissolved in 100 g of water at 80C? 50 g At 40C, how much KNO3 can be dissolved in 100 g of water? 60 g Which salt shows the least change in solubility from 0 to 100C? NaCl At 30C, 90 g of NaNO3 are dissolved in 100 g of water. Is this solution saturated, unsaturated or supersaturated? unsaturated A saturated solution of KClO3 is prepared in 100 g of water at 80C. If the saturated solution is rapidly cooled from 80C to 50C, how many grams of precipitate are formed? 20 g Which two compounds show a decrease in solubility from 0C to 100C? NH3 and Ce2(SO4)3 Above what temperature does KClO3 become more soluble than NaCl? 80C A student wishes to prepare a supersaturated solution of 60 g NH4Cl in 100 g water at 50C. To what temperature must the student heat the solution to dissolve the NH4Cl before cooling it to 50C? 70C If the supersaturated solution from the previous question is disturbed, how many grams of NH4Cl will crystallize out? 10 g Molarity The answer for each problem is given in parentheses. YOU MUST SHOW YOUR WORK TO GET CREDIT. What is the molarity of a solution in which 2.51 mol NaCl are dissolved in 0.585 L of solution? (Ans. 4.29 M NaCl)  EMBED Equation.3  How many moles of KNO3 should be used to prepare 2.00 L of a 0.500 M solution? (Ans. 1.00 mol KNO3)  EMBED Equation.3  mol = (0.500 M)(2.00 L) = 1.00 mol = (0.10 M)(0.10 L) = 0.010 mol CuSO4 To what volume should 0.0667 mol of KCl be diluted in order to prepare a 0.250 M solution? (Ans. 0.267 L solution)  EMBED Equation.3   EMBED Equation.3   EMBED Equation.3  Solubility Rules Use the solubility chart in your notes or on the reference sheet to determine if the following compounds are soluble in water. Write the solubility rule that explains why the compound is soluble or insoluble. CompoundSoluble or insoluble?Why?strontium sulfateinsolubleSulfates are usually soluble, but strontium is an exception.magnesium nitratesolubleNitrates are soluble. There are no exceptions.lithium sulfidesolubleSulfides are usually not soluble, but akali metals (lithium) are exceptions.aluminum iodidesolubleIodides are usually soluble. Aluminum is not an exception.silver bromideinsolubleBromides are usually soluble, but silver is an exception.potassium chloridesolubleChlorides are usually soluble. Potassium is not an exception. Electrolytes Determine which of the following compounds are electrolytes. Write dissociation reactions for the electrolytes. CompoundIonic or Covalent?If ionic: soluble or insoluble?If ionic and soluble: electrolyteIf electrolyte: dissociation reactionNumber of ionsCaBr2ionicsolubleelectrolyteCaBr2 EMBED Equation.3 Ca2+ + 2 Br-3KOHionicsolubleelectrolyteKOH EMBED Equation.3 K+ + OH-2AgIionicinsolubleAl2(SO4)3ionicsolubleelectrolyteAl2(SO4)3 EMBED Equation.3 2Al3++3SO42-5H2OcovalentFill in the Blank:  _____________ will determine what substance will layer on top of another substance for _______________ liquids ___________ liquids are able to dissolve freely in one another ___________ are insoluble solids that collect at the bottom of a solution Water is different from other substances because it is ______ dense as a liquid and _____ dense as a solid Water is known as the _________ solvent because its polarity allows so many substances to dissolve in it The cohesion of water molecules creates a condition called _____________________ ___________ means that there are partial positive and partial negative charges in the molecule Water is found in groups of 5 because of _______________     Unit 11 Worksheets: Solution Chemistry  DOCVARIABLE TeacherVersion \* MERGEFORMAT  General Chemistry, 2010-2011 Page  PAGE 4 of  NUMPAGES 4 Unit 11 Worksheets: Solution Chemistry Name  DOCVARIABLE TeacherVersion \* MERGEFORMAT  General Chemistry, 2011-2012 Page  PAGE 1 of  NUMPAGES 1 Density Miscible More Universal Polarity Immiscible Precipitates Less Surface Tension Hydrogen Bonding  h i j % & ' ññññÉriea[RNJFhFThX_h*CJOJPJQJaJh h 5 h\95 h"05 hqB5'/8WmFfFf]Ff%$(&P#$/IfgdRBgdH  i j &  & Fgdwwh^hgd0 & Fgd gd0^gd0FfFf $(&P#$/IfgdRB& ' ( k l m B C ` * s   & Fgd`h^hgd_ & Fgdwwh^hgd & Fgdgdgdh & Fgdhh^hgdoqgdoq & Fgd gdoqh^hgdFT' ( k m B C G _ ` * ? 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