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Name: __________________________________Date: ___________________Period: _____Review Chemistry I Honors Unit 12: Solutions and EquilibriumA solution consists of a _solute___ dissolved in a ___solvent__.A solution is a ___homogeneous____ mixture. (which means _same_ throughout)Is this type of mixture a pure substance, a compound, both, or neither? (circle one)Classify the following materials as: solution (S) or heterogeneous mixture (M)__S__a. smoky air__S__g. salt water (NaCl + H2O)___S_b. sugar water (C12H22O11 + H2O)__S__h. milk___S_c. vinegar (HC2H3O2 + H2O)__M__i. soda with bubbles__S__d. Gatorade__S__j. oil-based paint__X__e. pure iodine (I2)__S__k. fog___X_f. pure distilled water (H2O)__S__l. ethanol in water (C2H5OH + H2O)There is a relatively large amount of solute dissolved in a concentrated / dilute solution. (circle one)There is much more ___solute___ than solvent_____ in a dilute solution.Molarity is the ratio of _moles_ of __solute__ per _liter_ of _solvent_.A 3.0 molar solution (3.0 M) has _____ mole(s) of solute in every _____ liter(s) of solution.To dilute a solution, you can add more ___solvent__ which will change the molarity of the solution, but will not change the number of __moles__ of solute.A(n) __electrolyte__ is an ionic (or very polar) compound that forms __ions insolution and will conduct electricity.Nonpolar covalent compounds (like H2O , C8H18 , CCl4 , C2H5OH) are typically _nonconductive__.Complete the phrase that describes the types of substances that will generally dissolve in each other:like dissolves _like. Therefore, polar solvents (like water) can dissolve _polar or ionic solutes (like alcohols, sugars, ionic compounds, etc.). But nonpolar solutes (like fats, oils, hydrocarbons, etc.) will dissolve in nonpolar solvents.A solution is formed by adding methanol, CH3OH, to water. Identify each of the following intermolecular attractions as breaking or forming in the solution process: (circle answers)breaking / formingmethanol – methanolbreaking / formingwater – waterbreaking / formingmethanol – waterIn general, the stronger the intermolecular attractions between solute and solvent molecules, the ___greater__ the solubility.In general, the __weaker__ the intermolecular attractions between solute and solute molecules, the lower the solubility.A tincture of iodine can be used as a disinfectant. This solution is can be made by mixing:2 g of solid iodine (I2)3 g of sodium iodide (NaI)55 g of liquid ethanol (C2H5OH)40 g of water (H2O)The solvent in this mixture is best identified as ___ because C has more volume or mass__.A. I2 B. NaIC. C2H5OH D. H2O Three factors that typically cause a solid to dissolve faster in a liquid are:increase / decrease __temperatures_________________________increase / decrease _solvent____increase / decrease ____concentration_______________________Gases dissolve faster in liquids at _lower__ temperatures and at higher _pressures__.Label each solution as saturated, unsaturated, or supersaturated based on the addition of solute:2014855298450200003382645165100200005251453937002000020243801035050200002084705-635000unsaturated_____supersaturated___saturatedA solution that contains less solute than can be dissolved at that temperature is __unsaturated_.If solute crystals are added to a saturated solution, the crystals will… ________fall to the bottom undisolved______________________________________.If the addition of a seed crystal causes dissolved solute to crystallize, the original solution was _supersaturated___.For # 19-23, consider the graph of solubility curves below.-488950146050020000322897511049019. Which substance has the lowest solubility at 20oC? __KClO3________02000019. Which substance has the lowest solubility at 20oC? __KClO3________38100-5080003238500127020. If 40 g of KCl is dissolved in 100 g of water at 80oC, then the solution is __unsaturated___.02000020. If 40 g of KCl is dissolved in 100 g of water at 80oC, then the solution is __unsaturated___.322897510160021. If 80 g of KNO3 is dissolved in 100 g of water at 40oC, then the solution is _supersaturated__.02000021. If 80 g of KNO3 is dissolved in 100 g of water at 40oC, then the solution is _supersaturated__.32099253175022. If 80 g of KNO3 is dissolved in 100 g of water at 50oC, then the solution is _saturated_.02000022. If 80 g of KNO3 is dissolved in 100 g of water at 50oC, then the solution is _saturated_.321500511874523. How many grams of NH4Cl can dissolve in 100 g of water at 70oC? 60 g02000023. How many grams of NH4Cl can dissolve in 100 g of water at 70oC? 60 g24.When a reaction has reached equilibrium, which one of the following could NEVER be true?A.there are more products than reactantsB. there are more reactants than productsC.there are no reactants leftD.the reactants are still changing into productsE.the products are changing back into reactants 25.When a reaction has reached equilibrium, which of the following is TRUE?A.the reaction stopsB. the forward reaction continuesC.the reverse reaction continuesD.BOTH the forward and reverse reactions continue26.A chemical reaction in is dynamic equilibrium when the relative forward and reverse rates of thereaction are _constant_, and the total amounts of reactant and product are __constant__.-762006223000R(g) ? P(g)27. Two gases were placed in a container and allowed to reach equilibrium shown in the equation above. The diagram below shows how the concentrations of gases R and P in this system changed over time.5614670139700[R]020000[R]4076700403225005105400130873500358076595250concentration (M)00concentration (M)4076700234950004076700136715500407670011684000At time A, the concentrations of R and P are:constant / equal / zero .At time B, the forward rate of reaction is:56388003175[P]020000[P]greater than / equal to / less than567690015430500427672514287500the reverse rate of the reaction.413321573025A020000A553339074295C020000C497205071755B020000B470471575565time (s)020000time (s)At time C, concentrations of R and P are:constant / equal / zero .4038600495300028.Circle the letter of each sentence that is TRUE about the saturated solution pictured here:A.The total amount of dissolved solute remains constant.B.The total mass of undissolved crystals remains constant.C.When the rate of solvation equals the rate of crystallization,a state of dynamic equilibrium exists. D.If more solute were added to the container,the total amount of dissolved solute would increase.3605530-278765molL020000molL3208655-172085M =020000M =4598035-166370M1V1 = M2V2020000M1V1 = M2V23199130-30353000For #29-34, you may use the following formulas:What is the molarity of a solution that contains 9.50 moles of solute in 3.00 L of solution?(Ans:3.17 M)What is the molarity of a solution containing 116 g NaCl of solute in 775 mL of solution?(Ans:2.55 M)How many moles of solute are in 3.20 L of a 1.50 M solution of sodium chloride?(Ans.4.80 mol)How many moles of solute are in 40.0 mL of a 0.615 M solution?(0.0246 mol)How many liters of a 0.510 M solution are contain 0.242 moles of solute?(Ans: 0.475 L)What mass of glucose (C6H12O6, 180.18 g/mol) is needed to make 5.00 mL of a 0.200 M solution?(Ans: 0.180 g)3605530-278765molL020000molL3208655-172085M =020000M =4598035-166370M1V1 = M2V2020000M1V1 = M2V23199130-30353000For #35-38, you may use the following formulas:How many mL of a 0.150 M NaBr solution are needed to make 100 mL of 0.0500 M NaBr?(Ans: 33.3 mL)If 20.0 mL of 12.1 M HCl is used to make a 5.00 L aqueous solution, what is the molarity of the dilute solution? (hint: choose mL or L, not both)(Ans: 0.0484 M )Cu(s) + 2 AgNO3(aq) Cu(NO3)2(aq) + 2 Ag(s)37. Solid copper is added to an aqueous solution of silver nitrate shown in the reaction above. What volume of 1.65 M AgNO3(aq) solution is needed to react completely with 0.250 moles of Cu(s) ? (Ans:0.303 L or 30.3 mL)2 Al(s) + 3 ZnCl2(aq) 2 AlCl3(aq) + 3 Zn(s)38. Solid aluminum is added to an aqueous solution of zinc chloride shown in the reaction above. What volume of 1.20 M ZnCl2(aq) solution is needed to react completely with 9.44 grams of Al(s) ? (Ans:0.437 L or 43.7 mL)2 KI(aq) + Pb(NO3)2(aq) 2 KNO3(aq) + PbI2(s)39. Aqueous solutions of potassium iodide and lead(II) nitrate are mixed to produce solid lead(II) iodide precipitate shown in the reaction above. If 12.7 mL of 0.425 M KI(aq) solution is added to an excess of Pb(NO3)2(aq) , what is the maximum mass of PbI2(s) precipitate that could be recovered? 37484055080( molar mass of PbI2 = 461.00 g/mol )020000( molar mass of PbI2 = 461.00 g/mol )(Ans: 1.24 g) ................
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