5/6/2016Week ThreeWeek ThreeDue: 12:00am on Tuesday, May 10, 2016You will receive no credit for items you complete after the assignment is due. Grading PolicyExercise 15.7Part AWhy is there more than one definition of acid­base behavior? Which definition is the right one?ANSWER:3393 Character(s) remainingIn 1777, a french chemist by the name of Lavoisier first statedthat oxygen was found within acid which was incorrect. Anacid dissociates in water and produces H ions. In 1923, Lewisstated that an acid is a substance that accepts one pair ofSubmitted, grade pendingExercise 15.34Part AIdentify each of the following as an acid or a base.Drag the appropriate items to their respective bins.ANSWER:Correcthttps://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=42887761/255/6/2016Week ThreePart BWrite a chemical equation for NaOH(aq) showing how it is an acid or a base according to the Arrhenius definition.Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:NaOH(aq)→Na+(aq) + OH−(aq)CorrectPart CWrite a chemical equation for H2 SO 4 (aq) showing how it is an acid or a base according to the Arrhenius definition.Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:H 2 SO 4 (aq)→2H+(aq) + SO 42−(aq)CorrectPart DWrite a chemical equation for HI(aq) showing how it is an acid or a base according to the Arrhenius definition.Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:HI(aq)→H+(aq) + I−(aq)CorrectPart EWrite a chemical equation for Ca(OH) 2 (aq) showing how it is an acid or a base according to the Arrhenius definition.Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:Ca(OH) (aq)→Ca22+(aq) + 2OH−(aq)CorrectExercise 15.36For each of the following, identify the Bronsted­Lowry acid, the Bronsted­Lowry base, the conjugate acid, and the conjugate base.Part ADrag the appropriate labels to their respective targets.ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=42887762/255/6/2016Week ThreeCorrectPart BDrag the appropriate labels to their respective targets.ANSWER:CorrectPart CDrag the appropriate labels to their respective targets.https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=42887763/255/6/2016Week ThreeANSWER:CorrectPart DDrag the appropriate labels to their respective targets.ANSWER:Correcthttps://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=42887764/255/6/2016Week ThreeExercise 15.42Classify each of the following acids as strong or weak.Part AHFANSWER:strongweakCorrectPart BHCHO 2ANSWER:strongweakCorrectPart CH 2 SO4ANSWER:strongweakCorrectPart DH 2 CO 3ANSWER:strongweakCorrectPart EWrite an expression for the acid ionization constant (Ka ) for HCHO2 .ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=42887765/255/6/2016Week ThreeKa =Ka =Ka =Ka =[H3 O+[CHO2−[HCHO 2 ][CHO2−[HCHO 2 ][H3 O+[HCHO 2 ][CHO2[H3 O+−[CHO2−[H2 O][HCHO 2 ]Part FWrite an expression for the acid ionization constant (Ka ) for HF.ANSWER:Ka =Ka =Ka =Ka =[H3 O+−[F[HF][H3 O+[HF]−−[F[F[H3 O+[HF][HF][H3 O+[F− ]Part GWrite an expression for the acid ionization constant (Ka ) for H2 CO 3 .ANSWER:Ka =Ka =[H2 CO 3 ][H3 O[H3 O++−[HCO 3 ]−[HCO 3 ][H2 CO 3 ]−Ka =Ka =[HCO 3 ][H3 O[H3 O++[H2 CO 3 ][H2 CO 3 ]−[HCO 3 ]Exercise 15.44Part ARank the following solutions in order of decreasing [H3 ORank solutions from largest to smallest [H3 O++.. To rank items as equivalent, overlap them.ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=42887766/255/6/2016Week ThreeIncorrect; Try Again; 5 attempts remainingExercise 15.124Identify the Lewis acid and Lewis base from among the reactants in each of the following equations.Part AAg+(aq) + 2NH 3 (aq) ⇌ Ag(NH 3 )+2(aq)ANSWER:AgAg+is the Lewis base and NH3 is the Lewis acid.+is the Lewis acid and NH3 is the Lewis base.CorrectPart BAlBr 3 + NH 3 ⇌ H 3 NAlBr 3ANSWER:AlBr 3is the Lewis base and NH 3 is the Lewis acid.AlBr 3is the Lewis acid and NH 3 is the Lewis base.CorrectPart CCl−(aq) + AlCl 3 (aq) ⇌ AlCl 4−(aq)ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=42887767/255/6/2016Week Three−AlCl 3is the Lewis acid and Cl is the Lewis base.AlCl 3is the Lewis base and Cl is the Lewis acid.−CorrectExercise 15.56Determine the pH of each of the following solutions.Part A5.0×10−2 M HIExpress your answer to two decimal places.ANSWER:pH= 1.30CorrectPart B9.54×10−2 M HClO 4Express your answer to three decimal places.ANSWER:pH= 1.020CorrectPart Ca solution that is 4.8×10−2 M in HClO 4 and 5.4×10−2 M in HClExpress your answer to two decimal places.ANSWER:pH= 0.99CorrectPart Da solution that is 1.11% HCl by mass (Assume a density of 1.01 g/mL for the solution.)Express your answer to three decimal places.ANSWER:pH= 0.512Correcthttps://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=42887768/255/6/2016Week ThreeExercise 15.66Part ACalculate the pH of a formic acid solution that contains 1.36% formic acid by mass. (Assume a density of 1.01 g/mL for the solution.)Express your answer to two decimal places.ANSWER:pH=0.53Incorrect; Try Again; 4 attempts remainingExercise 15.76Part AFind the pH of a 0.130 M solution of a weak monoprotic acid having Ka=2.0×10−5.=1.3×10−3.Express your answer to two decimal places.ANSWER:pH= 2.79CorrectPart BFind the percent dissociation of this solution.Express your answer using two significant figures.ANSWER:1.2 %CorrectPart CFind the pH of a 0.130 M solution of a weak monoprotic acid having KaExpress your answer to two decimal places.ANSWER:pH=1.38Incorrect; Try Again; 5 attempts remainingPart DFind the percent dissociation of this solution.Express your answer using two significant figures.ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=42887769/255/6/2016Week Three31.5%Incorrect; Try Again; 5 attempts remainingPart EFind the pH of a 0.130 M solution of a weak monoprotic acid having Ka=0.18.Express your answer to two decimal places.ANSWER:pH=0.818Incorrect; Try Again; 5 attempts remainingPart FFind the percent dissociation of this solution.Express your answer using two significant figures.ANSWER:1.17%Incorrect; Try Again; 5 attempts remainingExercise 15.90Amphetamine (C 9 H13 N) is a weak base with a pKb of 4.2.Part ACalculate the pH of a solution containing an amphetamine concentration of 250 mg/L .Express your answer to one decimal place.ANSWER:pH=11.26Incorrect; Try Again; 5 attempts remainingExercise 15.100Part ADetermine whether each of the following salts will form a solution that is acidic, basic, or pH ­neutral.Drag the appropriate items to their respective bins.ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877610/255/6/2016Week ThreeIncorrect; Try Again; 5 attempts remainingExercise 15.108Write chemical equations and corresponding equilibrium expressions for each of the two ionization steps of carbonic acid.Part AWrite chemical equations for first ionization step of carbonic acid.Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:Part BThis question will be shown after you complete previous question(s).Part CWrite chemical equations for second ionization step of carbonic acid.Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:Part DThis question will be shown after you complete previous question(s).https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877611/255/6/2016Week ThreeExercise 15.13Part AChoose an equation for the autoionization of water and an expression for the ion product constant for water (Kw ).ANSWER:Kw =[H3 O[OHKw = [H 3 OKw = [H 3 OKw =[OH+−++−[H3 O+ [OH[OH−−+Part BWhat is the value of Kw at 25 ∘ C ?ANSWER:Kw = 1.0 ⋅ 10Kw = 1.8 ⋅ 10Kw = 1.0 ⋅ 10Kw = 1.8 ⋅ 10−14−16−7−10Exercise 15.17In most solutions containing a strong or weak acid, the autoionization of water can be neglected when calculating [H3 O+.Part AExplain why this is so.ANSWER:Essay answers are limited to about 500 words (3800 characters maximum, including spaces).3785 Character(s) remaining(none provided)Exercise 15.48Part ACalculate [H3 O + ] in the following aqueous solution at 25 ∘ C : [OH− ]=1.8×10−9 M .Express your answer using two significant figures.ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877612/255/6/2016Week Three[H 3 O+M=Part BClassify the solution as acidic or basic.ANSWER:acidicbasicPart CCalculate [H3 O+in the following aqueous solution at 25 ∘ C : [OH−=2.6×10−2 M .=6.1×10−12 M .Express your answer using two significant figures.ANSWER:[H 3 O+M=Part DClassify the solution as acidic or basic.ANSWER:acidicbasicPart ECalculate [H3 O+in the following aqueous solution at 25 ∘ C : [OH−Express your answer using two significant figures.ANSWER:[H 3 O+M=Part FClassify the solution as acidic or basic.ANSWER:acidicbasicExercise 15.50Calculate [H3 O+and [OH−for each of the following solutions.Part ApH =8.58https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877613/255/6/2016Week ThreeExpress your answer using two significant figures. Enter your answers numerically separated by a comma.ANSWER:[H 3 O+, [OH−=MPart BpH =11.20Express your answer using two significant figures. Enter your answers numerically separated by a comma.ANSWER:[H 3 O+, [OH−=MPart CpH =2.82Express your answer using two significant figures. Enter your answers numerically separated by a comma.ANSWER:[H 3 O+, [OH−=MExercise 15.54The value of Kw increases with increasing temperature.Part AIs the autoionization of water endothermic or exothermic?ANSWER:endothermicexothermicExercise 16.8Part AWhat factors influence the effectiveness of a buffer? What are the characteristics of an effective buffer?ANSWER:Essay answers are limited to about 500 words (3800 characters maximum, including spaces).3785 Character(s) remaining(none provided)Exercise 16.11https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877614/255/6/2016Week ThreePart AThe pH at the equivalence point of the titration of a strong acid with a strong base is 7.0. However, the pH at the equivalence point of the titration of aweak acid with a strong base is above 7.0. Why?ANSWER:Essay answers are limited to about 500 words (3800 characters maximum, including spaces).3785 Character(s) remaining(none provided)Exercise 16.28A formic acid solution has a pH of 3.25.Part AWhich of the following substances will raise the pH of the solution upon addition?Check all that apply.ANSWER:KClNaBrHClNaCHO 2Part BThis question will be shown after you complete previous question(s).Exercise 16.32Part ACalculate the percent ionization of a 0.14 M formic acid solution in pure water.Express your answer using two significant figures.ANSWER:%Part BCalculate the percent ionization of a 0.14 M formic acid solution in a solution containing 0.11 M potassium formate.Express your answer using two significant figures.ANSWER:%https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877615/255/6/2016Week ThreePart CExplain the difference in percent ionization in the two solutions.ANSWER:Essay answers are limited to about 500 words (3800 characters maximum, including spaces).3785 Character(s) remaining(none provided)Exercise 16.42Calculate the pH of the solution that results from each of the following mixtures.Part A160.0 mL of 0.27 M HF with 230.0 mL of 0.31 M NaFExpress your answer using two decimal places.ANSWER:pH=Part B170.0 mL of 0.11 M C 2 H5 NH 2 with 270.0 mL of 0.22 M C 2 H5 NH 3 ClExpress your answer using two decimal places.ANSWER:pH=Exercise 16.50For each of the following solutions, calculate the initial pH and the final pH after adding 0.010 mol of NaOH .Part AFor 200.0 mL of pure water, calculate the initial pH and the final pH after adding 0.010 mol of NaOH .Express your answers using two decimal places separated by a comma.ANSWER:pH initial, pHf inal =Part BFor 200.0 mL of a buffer solution that is 0.240 M in HCHO2 and 0.310 M in KCHO 2 , calculate the initial pH and the final pH after adding 0.010mol of NaOH .Express your answers using two decimal places separated by a comma.ANSWER:pH initial, pHf inal =https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877616/255/6/2016Week ThreePart CFor 200.0 mL of a buffer solution that is 0.315 M in CH3 CH2 NH 2 and 0.285 M in CH3 CH2 NH 3 Cl , calculate the initial pH and the final pH afteradding 0.010 mol of NaOH .Express your answers using two decimal places separated by a comma.ANSWER:pH initial, pHf inal =Exercise 16.62Two 28.0 mL samples, one 0.100 Mthese two titrations.HCland the other 0.100 MHF, were titrated with 0.200 MKOH. Answer each of the following questions regardingPart AWhat is the volume of added base at the equivalence point for HCl ?ANSWER:mLPart BWhat is the volume of added base at the equivalence point for HF?ANSWER:mLPart CPredict whether the pH at the equivalence point for each titration will be acidic, basic, or neutral.ANSWER:neutral for HF, and basic for HClneutral for HCl , and acidic for HFneutral for HCl , and basicfor HFneutral for HF, and acidic for HClneutral for bothPart DPredict which titration curve will have the lowest initial pH .ANSWER:HFcurveHClcurveExercise 16.64The graphs below labeled (a) and (b) show, the titration curves for two equal­volume samples of bases, one weak and one strong. Both titrations werehttps://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877617/255/6/2016Week Threecarried out with the same concentration of strong acid.Part AWhat is the approximate pH at the equivalence point of (a) curve?Express your answer as a whole number.ANSWER:pH=Part BWhat is the approximate pH at the equivalence point of (b) curve?Express your answer as a whole number.ANSWER:pH=Part CWhich curve corresponds to the titration of the strong base and which one to the weak base?ANSWER:Graph (a) represents a strong base and graph (b) represents a weak base.Graph (b) represents a strong base and graph (a) represents a weak base.Exercise 16.68A 20.0­mL sample of 0.125 M HNO 3 is titrated with 0.150 MNaOH.Part ACalculate the pH for at least five different points throughout the titration curve and make a sketch of the curve.https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877618/255/6/2016Week ThreeANSWER:Exercise 16.78and the resulting titration curve is shown in the figure.A 0.446­g sample of an unknown monoprotic acid was titrated with 0.105 MKOHPart ADetermine the molar mass of the acid.Express your answer using two significant figures.ANSWER:g/molPart BDetermine pKa of the acid.ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877619/255/6/2016Week Three12.02.04.08.0Exercise 16.82Phenolphthalein has a pKa of 9.7 and is colorless in its acid form and pink in its basic form.Part AFor pH=2.1 calculate [In−/[HIn].Express your answer using two significant figures.ANSWER:[In−/[HIn]=Part BPredict the color of a phenolphthalein solution.ANSWER:colorlesspinkPart CFor pH=5.0 calculate [In−/[HIn].Express your answer using two significant figures.ANSWER:[In−/[HIn]=Part DPredict the color of a phenolphthalein solution.ANSWER:colorlesspinkPart EFor pH=7.9 calculate [In−/[HIn].Express your answer using two significant figures.ANSWER:[In−/[HIn]=https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877620/255/6/2016Week ThreePart FPredict the color of a phenolphthalein solution.ANSWER:colorlesspinkPart GFor pH=11.5 calculate [In − ]/[HIn] .Express your answer using two significant figures.ANSWER:[In−/[HIn]=Part HPredict the color of a phenolphthalein solution.ANSWER:colorlesspinkExercise 16.86Part AWrite a balanced equation for the dissolution of CaCO 3 .Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:Part BWrite an expression for Ksp for the dissolution of CaCO 3 .ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877621/255/6/2016Week Three2+Ksp = [Ca2+Ksp = [CaK sp =2[CO32−[Ca[CaCO 3 ][CO 3[CaCO 3 ]2+K sp =32−[CaCO 3 ]2−K sp =2−[Ca2+ ][CO 32+K sp =[CO[Ca2−[CO 3[CaCO 3 ]2+Ksp = [Ca[CO2−32Part CWrite a balanced equation for the dissolution of PbCl2 .Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:Part DWrite an expression for Ksp for the dissolution of PbCl2 .ANSWER:K sp =K sp =[Pb[PbCl 2 ][Cl−2[PbCl 2 ]Ksp = [PbK sp =2+2+[Pb2+2[Cl[Cl−−2[PbCl 2 ][PbCl 2 ]K sp =[PbKsp = [PbKsp = [Pb2+2+2+[Cl[Cl[Cl−−−22Part EWrite a balanced equation for the dissolution of AgI .Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:Part FWrite an expression for Ksp for the dissolution of AgI .ANSWER:https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877622/255/6/2016Week ThreeKsp = [AgK sp =K sp =[AgK sp =[I+−2[AgI][AgI][AgKsp = [AgK sp =+++[Ag+[I2−[I[I−−[AgI][I−[AgI]Ksp = [Ag+[I−Exercise 16.90Part AUse the molar solubility 1.08 × 10 −5Min pure water to calculate Ksp for BaCrO 4 .Min pure water to calculate Ksp for Ag 2 SO3 .Min pure water to calculate Ksp for Pd(SCN) 2 .ANSWER:Ksp=Part BUse the molar solubility 1.55 × 10 −5ANSWER:Ksp=Part CUse the molar solubility 2.22 × 10 −8ANSWER:Ksp=Exercise 16.96Calculate the molar solubility of CuX(Ksp = 1.27 × 10−36)in each of the following.Part Apure waterExpress your answer using three significant figures.ANSWER:S=MPart BM CuClhttps://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877623/255/6/2016Week Three0.28 M CuCl 2Express your answer using two significant figures.ANSWER:S=MPart C0.19 M Na 2 XExpress your answer using two significant figures.ANSWER:S=MExercise 16.100Part ADetermine whether or not Hg 2 Br 2 will be more soluble in acidic solution than in pure water.ANSWER:will be more solublewill not be more solublePart BThis question will be shown after you complete previous question(s).Part CDetermine whether or not Mg(OH)2 will be more soluble in acidic solution than in pure water.ANSWER:will be more solublewill not be more solublePart DThis question will be shown after you complete previous question(s).Part EDetermine whether or not CaCO 3 will be more soluble in acidic solution than in pure water.ANSWER:will be more solublewill not be more solublehttps://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877624/255/6/2016Week ThreePart FThis question will be shown after you complete previous question(s).Part GDetermine whether or not AgI will be more soluble in acidic solution than in pure water.ANSWER:will be more solublewill not be more solublePart HThis question will be shown after you complete previous question(s).Score Summary:Your score on this assignment is 14.8%.You received 0.62 out of a possible total of 4.16 points.https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=428877625/25