2000PracticeFinalKey

2000PracticeFinalKey - w Practice Final Exam 1 0 00 Name if...

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Unformatted text preview: w Practice Final Exam 1 0 00 Name if 0:; Introductory Chemistry 030.101 (Print) Last name First name ‘ ' Soc. Sec. # SHOW ALL WORK FOR FULL/PARTIAL CREDIT GIVE FINAL ANSWER ON THE LINE WHEN INDICATED Avagadro’s Number = 6.022 x 1023 R= 0.0821 L atrn moi“ K‘1 = 8.315 I motI K" For Ag+(aq) + NH3 2K1: 2.1 x 103 and K; = 8.2 x 103 K. for NH; is 5.6 x 10"" K3 for HF is 3.53 x10“1 Kw = 1.00 x10"M For H28: 1c,1 = 1.0 x107 and [(32 = 1.0 x10” Ka for HClis 1x107 K4, (H20) = 0.512 K kg moi" K3 for HN03 is 2 x 10‘ 5= 2° ~ (0.0592/n)10g Q . AG“ = -RTan = 411:2" F = Faraday’s constant = 96,485 C/mol I. (:1) Write a balanced chemical equation to represent the acid-base reaction between hydrobromic acid and calcium hydroxide. V . 02 H 6“. «f Cg<0i+)l_’; (2461“; "r 3,4219 hir+0fl' ,0 PAC)» (1)) Can chloride, Cl', act as a Bronsted~Low€fy acid? If so, give the formula of the conjugate Bronsted—Lowery base. N A 9 (c) Can hydroxide, OH‘, act as a Bronsted—Lowijy base? If so, give the formula of the conjugate Bronsted—Lowery acid. ya 3) ML 0 (d) Aqueous copperfll) ions react with ammonia to give a coordination complex according to the equation given below. Which species acts as a Lewis acid and which acts as a Lewis base? Gui; + 4NH3 -~—>[Cu(NH3)4]2+ a; if Lewis Acid Lewis Base LI #3 2. Calculate the pH of a buffer solution made by adding 0.100 mol of NH4C1 and 0.200 mol of NH3 to water and diluting to 1.000 L. Kw ‘ HID-(’4 thr My 00“? W + 0H“ tr i I At 0-100 w , 1 3'8 i ' 0H: 0.4 'N 4’4 4‘0! fde/iq’qf ' I Introductory Chemistry 030.101 Name‘fifl'a‘ .3. Suppose 0.100 mol of AgNO3 is dissolved in 1.00 L of a 1.00 M solution of NH3. Calculate the concentrations of the Ag+ and 13ig(NH3)+ ions present at equilibrium. \(x Wt KL M 190%» W», l‘l’éL 7.7 455g“ on? Agnew is pmmf Mil/3 OCAficoWQfld: olioofi Gigi: LOOM’Q‘LO-tto A} (MD: :3 Away mg W: O‘ioo O 939 )2 6.36M o m fl 0W4- [AgmHMLL/L [Ag] 7/0 4. (a) Calculate the pH at the equivalence point when a solution of 0. 10 M hydrofluoric acid, HF, is titrated with a solution of 0.10 M sodium hydroxide, NaOH. HF is a weak acid. - A ’4 — ‘ p 4 . ’0 _ 40 HF «r OH E: 147/0 ~t F «. 9633.51, :EBWJ/ Kit/2w! I 003“, ' EAL) ‘- O €9,8( l 9,2; MN m (it A: —/‘F as Coir]: (Ax/r31” T poll‘— 5'0” W 3 .45 AC fling/Y: WHTpéhL:IL/_ .Or/ ’— rt iW‘ Kine” = <0 ’1) *1: 940%, 27A: [Iv/é 5 pH .03 n61 4: (’0) Calculate the pH at the equivalence point when a solution of 0.10 M sodium fluofide, NaF, is titrated with a 0.10 M solution of hydrochloric acid, HCl. / . L, 1- l: {Hf '3 HF k: h’ Jim/03 asap/A HWY“? 8 '0( I“ ( ~ ~ 46 r4 ’3; (34/0:- 41c (£le”) M JM 4 0C 009’” («gut twin a 9430 r ‘ Introductory Chemistry 030.101 Name 5. (a) The solubility product of lead iodide, PM; is 7.1 x 10‘9 at 298 K. Calculate the solubility of this salt in moles per liter and find the molarity of the ions in a saturated solution of PbIz. 9811(5); Phi) ‘” grin) K: 7t! Mfg: flLIfJCI'Jlr— /)< (9453943 ,3 1. 0%]: A 9»; 421-3700 , pp -3 . _ , 3 » 3 Phi2 Solubility 1.2 W may/L [1313*] I. 9on [1'] Q. 1/ m (b) What would the solubility of PbIz be in 0.10 M sodium iodide? PL Ins) :3 flip <~ o1 Tun 26¢: 1.1m”: (Hill?) 2 (L ( MAW 0‘ MM ‘1 AC (040 4 34) J ram/w WI Smfié _ . 3M F? . ' CW “‘ 4!: an on ma . . /? WW “I 0”" + a” Pbizsmubintyiégflg wé’o/L (gammy "M €— Cg) 6. Hydrogen sulfide, H28, is initially present at 0.10 M concentration in water. Calculate the pH, an the ‘ molar concentrations of H28, 3%", and SH" present at equilibrium. '6‘) . J l . ‘ a. 1.’ His Wear: 630* No He + we: HBO +5 r4 010 5 2‘ L0 "New 1.07"“ 0 . w M «xx ’Y "’4 FILL—17".” ’fl WM « 46 ’ "I 4 I W 0"” "" A 0.0 “Vi/*3 (“m “3 [HzS]_O-_IC‘_ ( ’1‘ m1 4'1 k4 fllwfiii'w) r76 DMD/5‘ _ v" - f C: / 1: ’ _ - , km 1 0m ’ onto/xx o .10 1 (I. am “'43 [3H1—L———3 _ It A, i W ac (a an"??? [32‘] [Ox/D » I ‘- ’ 2. , ~I c/X v» [0“: q“ 0”] ([950 a1/Q1:1_0¥10 . 1‘ j - 7. In the space provFided draw a simple phase diagram, label the axis, and indicate the following with capita letters: A. critical point B. triple point C. normal boiling point D. normal freezing point B. solid phase V \ V ‘ .Introductory Chemistry 030.101 Name I . l A solution of hydrochloric acid (HCl) in water is 38.00% hydrochloric acid by Its density is 1.1886 g/crn3 at 20° C. Calculate the molarity, molality, and mole fraction of HCl in the solution. 1 ML— “ ‘Amn g fuel-{92% . SOL/Mb“ 1x (nggba—B — 31/ng ml» 501 m: fig) 1‘ -: 7 Marine a, [OHQZL mote Hi ‘ 33? 3 kit/Q 7‘ (gkqwéav , (M g H 0 Molarity [2 30¢ (DEL 3* Hto A WALT _ [Meg fit? Molality Y] f1: L : kind/I33 L 2 [‘23 [M a. 1 @9337 Mole fraction 0.07337 ' M‘flli 3. WI? 9. Calculate the boiling point elevation of a solution prepared from 0.571 g of LiF, a strong electrolyte, and 111 grams of water. («A Hf ., L1 Fang Let.) i” i7‘2) L2; (manic 7H- L‘F* M: ‘ . - 05 a 301-1?er 5T1 L kbm g? QC)qu *— 0-09‘3~0M{L :CQ)LO.UZ. M oxilllly) : anew? Boiling point elevation O , Q 03 10. Balance the equation given below and identify the oxidation and reduction half—reactions. Isthe overall cell reaction spontaneous in the direction indicated? Calculate 5°, AG°, and the equilibrium constant K, for the balanced reaction at 298.15 K. {12(5) + 2 e' -> 2T(aq), 5° = 0.54 V; Al3+(aq) + 3 e" 9 Al(s), 5° = —l.66V} Ilaq) + Al3+(aq) 912(5)+A1(S) We“- (21.74213 e MHZ-.7) We 3111;) -+ name) flair—"n (iii/£0 a v v vet—4M?) (VJ-303]" M : ear in K k . MW" fl Ag, _ "(.113L “0 3 251;: . Enid mun 2M 2 U ‘ (rainwater-’5') i b3“ : 3393"i§'§i§ “mm” t) (#0 .1 .n - ” “F 21 Spontaneous? Yes 01'@ 5° ’Q-QOV AG" 1.2:}‘X/01’ .T KL J 1411. Consider the galvanic cell shown. Calculate the electromotive force, 5, under the specified conditions: a) standard conditions; b) [2112*] = 10.0 M, [Cult] = 1.0 M, and c) [218*] = 1.0 M, [Cu2+] = 10.0 M. {Zn2+(aq) + 2 e“ -> Zn, 2" = —0.76 V; Cu2+(aq) + 2 e' —> Cu(s), 5° = 0.34 V} - a 533‘? ;_ Zn(s)lZnSO4(aq)llC'—!SO4(aq)lCu gj : 4 199:1 tr Q 2 fi " 6’? 43“ gdeeeEVieififZeofié a: ,zm~”%?bi$>c l0? .4 @163) gt”? .L' /”' (r1 L‘f % tuna 30.11.. (as) 260'“ W w 1' ...
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2000PracticeFinalKey - w Practice Final Exam 1 0 00 Name if...

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