Define electrolyte and nonelectrolyte and identify each of

Name: Justin RothCollege ID: 0360782Thomas Edison State CollegeGeneral Chemistry I (CHE-111)Section no.: 5Semester and year: Jan 2016Written Assignment 5: Chemical Reactions in SolutionAnswer all assigned questions and problems and show all work.1. Define electrolyte and nonelectrolyte and identify each of the following substancesas a strong electrolyte weak electrolyte or nonelectrolyte: (5 points)Electrolyte: a substance which dissociates in a solutionNon-electrolyte: a substance which do not dissociates in a solutiona. H2O-Weak Electrolyteb. KCl-Strong Electrolytec. HNO3- Strong Electrolyted. CH3COOH- Weak Electrolytee. C12H22O11 – Non-Electrolyte(Reference: Chang 4.9)2. Write ionic and net ionic equations for the following reactions: (8 points)a.b.c.d.AgNO3 Na2SO4 ?BaCl2 ZnSO4 ?(NH4)2CO3 CaCl2 ?NaNO3 KCl ?(Reference: Chang 4.21)3. With reference to Table 4.2 suggest one method by which you might separate (a) K from Ag (b) Ba2 from Pb2 (c) NH4 from Ca2 and (d) Ba2 from Cu2 . All cationsare assumed to be in aqueous solution and the common anion is the nitrate ion. (8points) (a) add NaCI (b) add NaF (c) add Na2CO3 (d) Na2SO4(Reference: Chang 4.24)4. Give the oxidation number of the underlined atoms in the following molecules andions: (7 points)a. ClF= 1 b. IF7 = 7 1 c.d.e.f.g.h.i.j.k.l.m.n.CH4 = 4C2H2 =1C2H4 =2K2CrO4 = 6 K2Cr2O7 =6 KMnO4 =7 NaHCO3 = 4 O2 = 0NaIO3 =5 K2O =-2PF6 = 6AuCl4 = 4(Reference: Chang 4.47)5. For the following reactions identify the type (combination combustion decomposition displacement methathesis [double-displacement)] neutralization) balance the reaction and for the redox reactions identify the oxidizing agent andreducing agent. (12 points)(a)(b)(c)(d)(e)(f)CH4 O2 ? CO2 H2O= CH4=reducing agent O2=oxidizing agentHCl NaOH ? H2O NaCl= NeutralizationH2 O2 ? H2O= H2= reducing agent O2= oxidizing agentCaCO3 HCl ? CaCl2 CO2 H2O= MethathesisZn HCl ? ZnCl2 H2 = Zn= reducing agent HCL= oxidizing agentNaCl ? Na Cl2 = decomposition reaction6. Calculate the molarity of each of the following solutions: (4 points)a. 29.0 g of ethanol (C2H5OH) in 545 mL of solutionb. 9.00 g of sodium chloride (NaCl) in 86.4 mL of solution(Reference: Chang 4.65)(a)29/12×2 1×6 16=.63.63/(1545/1000)=1.156M(b) 9x(1/58.44)=.154mol NaCI.154/86.4×10^-3 = 1.78m7. Calculate the mass of KI in grams required to prepare 5.00 × 102 mL of a 2.80 Msolution. (3 points)(Reference: Chang 4.59)5×10^2mL=500mL=.5L2.8=moles/.5L 1.4×166=232.4KI8. How many grams of NaCl are required to precipitate most of the Ag ions from 2.50× 102 mL of 0.0113 M AgNO3 solution? Write the net ionic equation for thereaction. (5 points)Ag ?Ag(Reference: Chang 4.53)2 2.83×10^-3 mol NaCIx (58.443gNaCl/1 mol NaCl)= .165 g NaCl(9. What volume of 0.416M Mg(NO3)2 should be added to 255 mL of 0.102 M KNO3 toproduce a solution with a concentration of 0.278 M NO3– ions? Assume volumes areadditive. (4 points)(Reference: Chang 4.69)(.832 mol/L)(x) (.102mol/L)(255 mL)=b(.278mol/L) (255 x).832x 26.01=70.89 .278x.554x=44.88x=81.01083mL10. Describe how to prepare 1.00 L of 0.646 M HCl solution starting with 2.00 M HClsolution. (4 points)(Reference: Chang 4.73).646MxL= .646 mole HCl.646=2Mx(L) HCI=32.3L 1L-.323=.677L=.323.2 M HCl .677L water11. Calculate the volume in mL of a 1.420 M NaOH solution required to titrate thefollowing solutions: (9 points)a. 25.00 mL of a 2.430 M HCl solutionMoles HCl = 0.02500 x 2.430 = 0.06075HCl NaOH = NaCl H2Omoles HCl = moles NaOHNaOH= 0.06075 mol / 1.420 M =0.04278 L =42.78 mlb. 25.00 mL of a 4.500 M H2SO4 solutionMoles H2SO4 = 0.02500 x 4.500 = 0.1125H2SO4 2 NaOH = Na2SO4 2 H2OMoles NaOH = 2 x 0.1125 =0.2250NaOH = 0.2250 / 1.420 = 0.1585 L = 158.5 mLc. 25.00 mL of a 1.500 M H3PO4 solutionMoles H3PO4 = 0.02500 x 1.500 = 0.03750H3PO4 3 NaOH = Na3PO4 3 H2Omoles NaOH needed = 3 x 0.03750 = 0.1125NaOH = 0.1125 / 1.420 = 0.07923 L = 79.23 mL(Reference: Chang 4.91)12. A 325 mL sample of solution contains 25.3 g of CaCl2. (4 points)a. Calculate the molar concentration of Cl– in the solution.25.3g x (1 mol CaCl2/110.9g CaCl2) x (2 mol Cl-/1 mol CaCl2)=.456 mol Cl.456 mol Cl-/ .325L=1.40M Clb. How many grams of Cl– are in 0.100 L of this solution?1.40m*35.45g=49.63g Cl- in 1 L49.63*.100L=4.96g3 (Reference: Chang 4.148)13. A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2. (8points)a.b.c.d.Write the balanced molecular equation for the reaction.Write the net ionic equation for the reaction.How many grams of precipitate will form?What is the concentration of Ag NO3? Ca2 and Cl? in the final solution (assumevolumes are additive).14. Based on oxidation number consideration explain why carbon monoxide is flammablebut carbon dioxide is not. (4 points)(Reference: Chang 4.141)CO has a lower oxidation state thatn C in CO2 hence CO is more flammable as itcan easily oxide.15. The alcohol content in a 10.0 g sample of blood from a driver required 4.23 mL of0.07654 M K2Cr2O7 for titration. If the current legal limit of blood alcohol content is0.08 percent by mass should the driver be prosecuted for drunken driving? What is thepercent alchohol in the driver’s blood? (7 points)3 C2H5OH (ethanol) 2 K2Cr2O7 8 H2SO4 ? 3 HC2H3O2 2Cr2(SO4)3 2 K2SO4 11 H2O(Reference: Chang 4.154)(3/2)x(4.23ml)x(0.7654 M) = 4.86 mMole alcohol = 0.224g alcohol .224% mass16. Write balanced chemical equations for the following: (8 points)a. A solution of sulfuric acid (battery acid) is neutralized with a solution of sodiumhydroxide.H2SO4 2NaOH = Na2SO4 2H2Ob. The combustion of iron metal produces iron(III) oxide (rust).4Fe 3O2 ?2Fe2O3c. When sodium metal is dropped into water it fizzes.2Na(s) 2HOH(l) =2NaOH(aq) H2(g)d. The science fair “volcano reaction” is produced by mixing sodium bicarbonate(baking soda) with vinegar (a solution of acetic acid HC2H3O2).NaHCO3 (CH3COOH)HC2H3O2(aq)=CH3COON9 (Nac2H3O2)H2O CO2(g)4