аЯрЁБс;ўџ !ўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџ§џџџўџџџ ўџџџўџџџўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџRџџџџџџџџ РF€{`њћ1Л@CompObjџџџџџџџџџџџџ\WordDocumentџџџџџџџџx.ObjectPoolџџџџхЧљћ1ЛхЧљћ1Лўџџџўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџўџџџџџ РFMicrosoft Word 6.0 DocumentўџџџNB6WWord.Document.6;џў ўџ ђŸ…рOљhЋ‘+'Гй0Œ˜Чхњ  ! -9A IUr z„џџџџџџџџџџџџџџџџџџџџџџџџ'DWK Internal:Word 6.0:Templates:NormalCH142 Pretest III '95 Whitney King Whitney King'@X0[1Л@X0[1Л@Ь5зћ1Л@мЅhOР eYx.Y,p,pp,p,p,p,p,к,к,к,к,к,к,і,к,-^--------Y-[-[-[-[-[-[-&п-X7.A-p,-------p,p,------p,-p,-Y-„, Є,6p,p,p,p,-Y--G- Great Expectations Sheet III CH142, 1996 1. Predict the products of the following acid-base reaction. HCl(aq) + NaOH(aq) ? 2. The following reactants are mixed in equal molar portions. Predict if the resulting solution will be acidic, basic, neutral, or if there is not enough information given to tell for sure. H2SO4 (aq) + KOH(aq) ? 3. We mix 100. mL of 0.10 M HCl and 100. mL of 0.10 M NaCN. What is the pH of the resulting solution? Ka (HCN) = 4.0 x 10-10 4. We have 100. mL of 0.10 M HClO solution. What is the pH of the resulting solutions after 0, 10, 25, 50, and 60 mL of 0.20 M NaOH is added? pKa (HClO) = 7.46 5. We have 250. mL of a 0.20 M solution of NH4Cl. It has a pH = 4.97. If we add 10.0 mL of a 1.00 M NH3 solution, what will the pH be? Ka (NH4+) = 5.6 x 10-10 6. We have 100. mL of water. We add to this 0.50 g of NaCH3COO and 1.00 mL of 1.00 M CH3COOH. What is the pH of the resulting solution? Ka (CH3COOH) = 1.8 x 10-5 7. We have 100. mL of a 0.20 M solution of NaClO. How many milliliters of 0.10 M HClO should be added to make a buffer of pH = 7.2? Ka (HClO) = 3.5 x 10-8 8. We have 200. mL of a buffer solution containing 0.10 M CH3COOH and 0.10 M NaCH3COO. If we add 10.00 mL of 0.20 M NaOH to this solution, what will the resulting pH be? Ka (CH3COOH) = 1.8 x 10-5 9. Consider an electrochemical cell formed from a Cu(s) electrode submerged in an aqueous Cu(NO3)2 solution and a Cd(s) electrode submerged in a Cd(NO3)2 solution. The two electrodes are connected by a wire and the two solutions are connected by a salt bridge containing NaNO3 (aq). The following reaction takes place: Cu2+ (aq) + Cd(s) л Cu(s) + Cd2+ (aq) Draw the cell and label the parts (anode, cathode, etc.). Indicate which direction electrons will flow in the cell. 10. E for the following redox reaction is +1.05 V. 2Ag+ (aq) + Ni(s) л 2 Ag(s) + Ni2+ (aq) What is DG for this reaction? 11. Given the two following half reactions, Ni2+ (aq) + 2e- о Ni(s) Eo = -0.25 V Hg2+ (aq) + 2e- о Hg(l) Eo = +0.86 V calculate Eo for the following reaction: Hg2+ (aq) + Ni(s) л Ni2+ (aq) + Hg(l) 12. An electrochemical cell described by the equation Pd2+ + Cu л Cu 2+ + Pd has Eo =-0.65 V. If we know that the standard reduction potential of Cu2+/Cu is Eo = 0.34 V, what is the standard reduction potential for Pd2+/Pd? 13. Given the following two half reactions, Cd2+ (aq) + 2e- о Cd(s) Eo = -0.40 V Zr4+ (aq) + 4e- о Zr(s) Eo = -1.53 V determine Eo and the spontaneity of the following reaction 2 Cd2+ (aq) + Zr(s) л 2 Cd(s) + Zr4+ (aq) 14. Determine the cell potential for Ni(s) + Fe2+ (aq) л Ni2+ (aq) + Fe(s) where [Ni2+] = 0.60 M and [Fe2+] = 0.0030 M using the following standard reduction potentials. Ni2+ (aq) + 2e - Ni(s) Eo = -0.25 V Fe2+ (aq) + 2e - Fe(s) Eo = -0.44 V 15. Determine the equilibrium constant for the following reaction at 25oC. Cl2 (aq) + 2I- (aq) л 2 Cl- (aq) + I2 (aq) Eo = +0.825 V 16. How many coulombs of charge are required to deposit 1.00 g Ag from a solution of Ag+ (aq)? 17. If we electrolyze a solution of Ni2+ (aq) to form Ni(s) and use a current of 0.15 amps for 10 minutes, how many grams of Ni(s) are produced? 18. The space shuttle uses fuel cells for electricity, and one cell that has been proposed is based on hydrazine, N2H4 , and O2 . The reactions are a. N2H4 (aq) + 4 OH- (aq) о N2 (g) + 4 H2O(l) + 4e- b. O2 (g) + 2 H2O(l) + 4 e- о 4OH- (aq) (i) Which reaction occurs at the anode? ____________ (ii) If the cell is to produce 0.50 amps of current for 50.0 hours, how many grams of hydrazine (N2H4) must be present? (1 Faraday = 96,500 coulombs/mol e - ) (iii) What is the DGo and Eo for the reaction? 19. Consider the following half reactions: HALF REACTION Eo (V) F2 (g) + 2e- о 2 F- (aq) +2.87 I2 (g) + 2e- о 2I- (aq) +0.56 Cu2+ (aq) + 2e- о Cu(s) +0.34 Al3+ (aq) + 3e- о Al(s) -1.66 (i) Which is the strongest oxidizing agent? ____________ (ii) Which is the strongest reducing agent? ____________ (iii) Will Al(s) reduce Cu2+ (aq) to Cu(s)? ____________ (iv) Will F- (aq) reduce I2 (aq) to I- (g)? ____________ (v) Name the elements or ions that can be reduced by Cu(s). ____________ (vi) If you build a battery using the I2/I- and Al3+/Al half reactions, what is the voltage of the battery (assuming all reagents are at standard conditions)? 20. 50 mL of 1.0 M formic acid (CHO2H) is titrated with 2.0M NaOH. Ka = 1.8 x 10-4 a. What is the volume of NaOH added at the equivalence point? b. What is the value of Kb? c. What is the pH at the equivalence point? 21. a. Write half reactions for the following (unbalanced!) reaction that occurs in acidic solutions: Mn+2 + ClO3- ( MnO2 + Cl- b. Write the balanced equation when the reaction occurs in base. 22. Describe two ways an acetic acid/acetate ion buffer can be made. 23. Calculate the amount of CaSO4(s), in grams, that dissolves in 0.50 L of water. Ksp = 2.4 x 10-5 M2 Molar mass CaSO4 = 106.2 24. Calculate the amount of CaSO4(s) that forms in a solution of 1.0 x 10-2 M sulfate and 5.0 x 10-2 M calcium ion. ŽЁ|HHк(џсџсљEG(ќHHи(d'hаЯрЁБс;џў џџџўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџSummaryInformation(џџџџџџџџџџџџМџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџMicrosoft Word 6.0.14аЯрЁБс;џў џџџўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџ*oprsєѕ ЁЂфх HIMNO[^ЅІТУћќЄЅЗЙњћklpqƒєѕії2 3 4 5 Ц Ч     " њ ћ   6 7 Œ Ž ˜ ™ › œ Ј Љ Ф Ц а б г д р с   3 5 D E H J ќјјјєјјјјјєєјјјјєјєјјјјєјјјјјєђєєђєђєєђ№єєђ№№єђєh]ceceќџUc_J Ќ Ў Ж З Л Н Т У Ш Щ    Q S ž   Њ Ћ ­ Ў К Л ж и т у х ц ђ ѓ Y[ijxzСУЩЪЮаѕї  ac|}˜šГД%&0189>?HIRSКЛэястуфьэ#$%&23:;=>HIRSќњќќјќјќќќњјќќњјјќњќќњќќќќјќјќєќњќєјќќєєєєєќњєєќceќџh]ce`Sefpq{|~„…NOPQВГДЕЛМ45>?ABGHkluvxy}ЄІАБГДкмцчщъПС§ў  ЮЯбвкмŽЛНЗЙСТУФХЪЫвгƒСУХЦзй+ќќјіјќќієєєќјіјќјіјјјіјјі№№ь№ќјјщццщєущєщццщщJЎc hc hceќџceh]ceceќџZ+-DFYмќќњuc h*+ks’п+`h‡ˆ  ВДA`hєЛМ…б a Њ ѓ ћ ( 0  В Д щ ё ( M N §Р!§Р!ћР!,ћР!,ћР!,ћР!,ћР!,ћР!,ћР!,ћР!,ћР!,ћР!TћР!,ћџР!€ћР!,ћџР!ЌћР!,ћР!TћР!TћР!,ћР!TћР!TћР!,ћР!,ћР!TћР!,ћР!TћР!,ћР!,ћР!TћР!TћР!,ћР!TћР!,ћР!@ћР!,ћР!,ћР!,ћР!,ћР!,ћР!,ћР!@ћР!,ћР!@ћР!,-N | „ Д М ь є # + X ` ™ š е ж X ` Ž – Ц Ю ў GO€‚ЉБоц,QYˆПЧШ_aТУХўР!,ўР!,ўР!@ўР!,ўР!@ўР!,ўР!,ўР!,ўР!@ўР!,ўР!,ўР!,ўР!@ўР!,ўР!,ўР!,ўР!,ўР!,ўР!@ўР!,ўР!@ўР!,ўР!,ўР!,ўР!@ўР!,ўР!,ўР!,ўР!@ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!TўР!,ўР!,ўР!,ўР!,-Х TdfБї U‹“бй$d—˜а§%-\d”œЪвKS–žтъ08}—Ÿх.aiўР!,ўР!,ўР!,ўР!,ўР!,ўР!TўР!,ўР!,ўР!TўР!TўР!,ўР!,ўР!,ўР!,ўР!TўР!,ўР!,ўўР!,ўР!,ўР!,ўР!,ўР!TўР!,ўР!TўР!,ўР!@ўР!,ўР!@ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!TўР!,ўР!,ўР!,ўР!,ўР!TўР!,ўР!,ўР!,-iОПїLMГДде]^_стVWXYўР!@ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!@ўР!,ўР!,ўР!,ўР!,ўР!,ўР!,ўР!@ўР!,ўР!@ўР!,ўР!,ўР!,K @ёџ Normal ]a c"A@ђџЁ"Default Paragraph FontYY`џџџџџџџџџџѓо ЯYJ S+мN ХiYG Whitney King7DWK Internal:CHEM 142:CH142 Exams:CH142 Pretest III '96џ@ДЕДДН^MTimes New RomanTimes Symbol"MArialHelveticaMNew York MTimes" €аXНF"ФfXНFAƒ$€+ACH142 Pretest III '95 Whitney King Whitney KingаЯрЁБс;џў џџџўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџRџџџџџџџџ РFЁ;.ќ1Л#@CompObjџџџџџџџџџџџџ\WordDocumentџџџџџџџџ$Н.ObjectPoolџџџџхЧљћ1ЛхЧљћ1Лџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџ §џџџўџџџўџџџўџџџ"%&'()*+,-./0123456789:;ўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџSummaryInformation(џџџџџџџџџџџџМџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџўџџџўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџMicrosoft Word 6.0.15аЯраЯрЁБс;џў џџџўџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџџўџџџџџ РFMicrosoft Word 6.0 DocumentўџџџNB6WWord.Document.6;џў ўџ ђŸ…рOљhЋ‘+'Гй0Œ˜Чхњ  ! -9A IUr z„3СhШž § @@ˆФ0ahШc 'DWK Internal:Word 6.0:Templates:NormalCH142 Pretest III '95 Whitney King Whitney King'@X0[1Л@X0[1Л@XМќ1Л@мЅhOР eYН.Е,p,pp,p,p,p,p,к,к,к,к,к,к,і,к,Ц-^--------Y-[-[-[-[-[-[-&$.X|.A-Ep,-------p,p,------p,-p,-Y-„, Є,6p,p,p,p,-Y--G- Great Expectations Sheet III CH142, 1996 1. Predict the products of the following acid-base reaction. HCl(aq) + NaOH(aq) ? 2. The following reactants are mixed in equal molar portions. Predict if the resulting solution will be acidic, basic, neutral, or if there is not enough information given to tell for sure. H2SO4 (aq) + KOH(aq) ? 3. We mix 100. mL of 0.10 M HCl and 100. mL of 0.10 M NaCN. What is the pH of the resulting solution? Ka (HCN) = 4.0 x 10-10 4. We have 100. mL of 0.10 M HClO solution. What is the pH of the resulting solutions after 0, 10, 25, 50, and 60 mL of 0.20 M NaOH is added? pKa (HClO) = 7.46 5. We have 250. mL of a 0.20 M solution of NH4Cl. It has a pH = 4.97. If we add 10.0 mL of a 1.00 M NH3 solution, what will the pH be? Ka (NH4+) = 5.6 x 10-10 6. We have 100. mL of water. We add to this 0.50 g of NaCH3COO and 1.00 mL of 1.00 M CH3COOH. What is the pH of the resulting solution? Ka (CH3COOH) = 1.8 x 10-5 7. We have 100. mL of a 0.20 M solution of NaClO. How many milliliters of 0.10 M HClO should be added to make a buffer of pH = 7.2? Ka (HClO) = 3.5 x 10-8 8. We have 200. mL of a buffer solution containing 0.10 M CH3COOH and 0.10 M NaCH3COO. If we add 10.00 mL of 0.20 M NaOH to this solution, what will the resulting pH be? Ka (CH3COOH) = 1.8 x 10-5 9. Consider an electrochemical cell formed from a Cu(s) electrode submerged in an aqueous Cu(NO3)2 solution and a Cd(s) electrode submerged in a Cd(NO3)2 solution. The two electrodes are connected by a wire and the two solutions are connected by a salt bridge containing NaNO3 (aq). The following reaction takes place: Cu2+ (aq) + Cd(s) л Cu(s) + Cd2+ (aq) Draw the cell and label the parts (anode, cathode, etc.). Indicate which direction electrons will flow in the cell. 10. E for the following redox reaction is +1.05 V. 2Ag+ (aq) + Ni(s) л 2 Ag(s) + Ni2+ (aq) What is DG for this reaction? 11. Given the two following half reactions, Ni2+ (aq) + 2e- о Ni(s) Eo = -0.25 V Hg2+ (aq) + 2e- о Hg(l) Eo = +0.86 V calculate Eo for the following reaction: Hg2+ (aq) + Ni(s) л Ni2+ (aq) + Hg(l) 12. An electrochemical cell described by the equation Pd2+ + Cu л Cu 2+ + Pd has Eo =-0.65 V. If we know that the standard reduction potential of Cu2+/Cu is Eo = 0.34 V, what is the standard reduction potential for Pd2+/Pd? 13. Given the following two half reactions, Cd2+ (aq) + 2e- о Cd(s) Eo = -0.40 V Zr4+ (aq) + 4e- о Zr(s) Eo = -1.53 V determine Eo and the spontaneity of the following reaction 2 Cd2+ (aq) + Zr(s) л 2 Cd(s) + Zr4+ (aq) 14. Determine the cell potential for Ni(s) + Fe2+ (aq) л Ni2+ (aq) + Fe(s) where [Ni2+] = 0.60 M and [Fe2+] = 0.0030 M using the following standard reduction potentials. Ni2+ (aq) + 2e - Ni(s) Eo = -0.25 V Fe2+ (aq) + 2e - Fe(s) Eo = -0.44 V 15. Determine the equilibrium constant for the following reaction at 25oC. Cl2 (aq) + 2I- (aq) л 2 Cl- (aq) + I2 (aq) Eo = +0.825 V 16. How many coulombs of charge are required to deposit 1.00 g Ag from a solution of Ag+ (aq)? 17. If we electrolyze a solution of Ni2+ (aq) to form Ni(s) and use a current of 0.15 amps for 10 minutes, how many grams of Ni(s) are produced? 18. The space shuttle uses fuel cells for electricity, and one cell that has been proposed is based on hydrazine, N2H4 , and O2 . The reactions are a. N2H4 (aq) + 4 OH- (aq) о N2 (g) + 4 H2O(l) + 4e- b. O2 (g) + 2 H2O(l) + 4 e- о 4OH- (aq) (i) Which reaction occurs at the anode? ____________ (ii) If the cell is to produce 0.50 amps of current for 50.0 hours, how many grams of hydrazine (N2H4) must be present? (1 Faraday = 96,500 coulombs/mol e - ) (iii) What is the DGo and Eo for the reaction? 19. Consider the following half reactions: HALF REACTION Eo (V) F2 (g) + 2e- о 2 F- (aq) +2.87 I2 (g) + 2e- о 2I- (aq) +0.56 Cu2+ (aq) + 2e- о Cu(s) +0.34 Al3+ (aq) + 3e- о Al(s) -1.66 (i) Which is the strongest oxidizing agent? ____________ (ii) Which is the strongest reducing agent? ____________ (iii) Will Al(s) reduce Cu2+ (aq) to Cu(s)? ____________ (iv) Will F- (aq) reduce I2 (aq) to I- (g)? ____________ (v) Name the elements or ions that can be reduced by Cu(s). ____________ (vi) If you build a battery using the I2/I- and Al3+/Al half reactions, what is the voltage of the battery (assuming all reagents are at standard conditions)? 20. 50 mL of 1.0 M formic acid (CHO2H) is titrated with 2.0M NaOH. Ka = 1.8 x 10-4 a. What is the volume of NaOH added at the equivalence point? b. What is the value of Kb? c. What is the pH at the equivalence point? 21. a. Write half reactions for the following (unbalanced!) reaction that occurs in acidic solutions: Mn+2 + ClO3- ( MnO2 + Cl- b. 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