exam2practicesolution

exam2practicesolution - Name: Exam [l (Page 2 of l I} Part...

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Unformatted text preview: Name: Exam [l (Page 2 of l I} Part I: Multiple Choice, Concepts {3 points each) Select them answer and enter your choice on the cow.r she t — No partial credit l. {3 pts) Which of the following is the conjugate bfiée of‘l-lS-OJ? .Ily- _- [a] insol ’_.._- ' (cursor if; (c) 3042- 91) “3304+ (e) 504- 2. (3 pts} List the following acids in order of increasing strenth‘? (a) HzTeCIo ‘1 H2330; "‘1 H2504 [b] HZSBU‘; ‘1' HETBflq "-17 H2304 [C] stBD4 "'5. H2304 *5 HzTfioe {(1} H3304 ‘1' HESBUll <5 H2T¢04 (E) H1304 ‘1' HzTEU4 ‘12 stfifld 3. [3 pts) A reaction will shift to the right if _._ :- {a) Q = K (b) C! 3* K {c} Q < K {d} All of these {e} None of these 4. [3 pts} All of the following may.r shift the position ofa reaction at equilibrium except (3] Temperature is increased (b) Concentration ofreactants is changed I‘ (chat. catalyst is added I (d) The volume of the container is decreased {c} all of these will afl'ect equilibrium Name: Exam II [Page 3 of I l] 5. (3 pts} How will the addition of sodium fluoride to hydrofluoric acid affect the pH? {a} the pH will decrease (ail the pH will increase .- - . J . ' _ j {c} the pH will not change I _ , \/ {a} the pH cannot be detennined {e} none of these a (3 pts} What is the relation bemoan KI, and Kc in the reaction below? Hs{s)+12{s) éé 2H1 {a} '-I@Kp=Kc I T as (b}Kp= am is a: " t/ ‘i' (bJKfiRTsz . _ __ : ;1_-s--~:“* to KP =(RT12KC *r- x- (a) KP = (RTJ‘Kc - T. (3 pts} Write the equiibrium constant expression for the reaction below r N: (a) + 3 H2 is) (‘9' 2 NH: {3} "(iii ms]: .2 3 [Nzlll‘lz] ,6” [bl lflfl '1’ - [Nzliflzl t t/ (c) magi [Nzlfl‘b]1 (d) mslmsfi [1"1‘13]2 (e) iflfllflgfi [Ham 8. (3 pts} Choose the Bronsted-Lowry acids and bases in the following equation [110' + NH}. NH] + OH- x / (a) acids: NHg', NH3 bases: H10, 0H “J (b) acids: NHL Hzo bases: NHg, oH' [c] acids: hle1 DH' bases: NHsj H20 {d} acids: H20, NH; bases: NH;', 0111' {e} acids: H20, DH' bases: HHz', NH; Name: Exam II {Page 4 of l l] 9. (3 pts) Phenol red indicator changes color from yellow to red in the pH range from 6.6 to 3.1:] What color would the indicator be in a solution oft}. 1 M~ Nam?) jgm are ._ :5 (b) yellow I'i ' ' If: (c) red—yellow 1‘/ (d) there isn't enough information here! {e} none of these It}. [3 pts) Which of the following would NflT be a good buffer? {a}} Sodium chloride and sodium hydroxide (b) Boric acid and sodium borate {c} Ammonium chloride and ammonium hydroxide [d] Potassium carbonate and potassium bicarbonate {e} All of these are great buffer combinations! re 1 l. (3 pts] 1|ul'u'hat is the buffer range for a benzoic acidfsodium benzoate buffer [K3 for . . . -5 benzoic acid is 6.3x“) } in; :1.“ :__ LT,- mt- Ilr-x {d} s.s-1c.s {e} 4.1—6.1 Name: Exam II (Page: 5 ufll} 1213 pts] The tintion curve for lilflmL offlJUflM HgPfla with ID. 190M NaflH is given below CI I ' D 2 4 E 31012141513202224 .D Estimate 11m pKaE of H3P04 {a} 2.2 {In} 4.3 {c} 1.2 {d} 9.3 (3} cannot be datermjnbd Name: Exam II [Page 6 of ] l} Part 11: Multiple Choice, Short Calculation;r Fill in the Blank (6 points each) Select the heat answer and enter your choice on the cover sheet — No partial credit 13. {5 pts) 14. (e piss} 15. {6 pts] (For # 13-18, enter your answer in the table or space provided} What is the value of Kc if {CO} = 0.1325, [H1] = 0.1313 and [CH30H} = HUBER for the following reaction CHsoH (g) (—4; co {3] + 2 H: {g} (a) 9.1x1o‘i (h) LSon'3 (e) note (:1) an (e) 6.6::102 1|What is the pH of a solution prepared by dissolving 1114433 of potassium hydroxide in sufficient pure water to prepare ZfiflflmL of solution?rl a 1i] A1 _ -. - '. 3:312 J"IL"';_j:"“} ' i" '9’ 3 ‘1'}. x a {cw c «a )- [c014 [e}2 ,3' “at J 5‘ l o r 5 Given the following 1) N20 [3) + V2 02 {g} 6—} 2 H0113} Kc = LTxifl'” R. 11) N2 (g) + 02 {g} {-9 2 no {g} K; = 4.1x1o‘“ Find the value for the equilibrium constant for the foIlowing reaction: N: {g} + 1,2; o; (g) (-+ Hail to) (a14,2x1o” . E . {h)t.ox1o"‘“ a _ {e} Lexie-9 ' - " " 3' (a) gene-13 in) gene-22 . Name: Exam 11 {Page T n1" 11] 16. {6 pta} A 0.632111 solution of a base has a p1[ = 11.53. What is the Ki. value far this base? [a]: "Salaam mafia \j - L _ (in) man 3%53 ; v.13: "' Q, (GE-Ema nae? _ (a) 1.11163 it ' L . {e} awn-3‘ n. [a [31.5) What valutne in mL at" t1.{15M-1\laGl-1 would have m headed to St}.an ofa. 1am H2304 to completer neutralize: the acid? {b} m 10am, ' ._/. '2 _-r __._ . (c) m £11111. J} ..I '. 1'. H'- 1‘ L _'.':M. genie. KIN _ [eT'FEEL lurth _ I I. u T J“; } PET} tau-emf?" - CM 1‘5. 1 13. (6 pta) Fill in the table below by predicting the effect (increase, decrease, ar no change} of the change given in the first calumn an the quantityr in the second culumn far this exothermic reaction at equilibrium. 5 CD [3) + 1205 (51 9912(3)"' 5 CO: (e) 4: Melt Ema - Lo ma 1 Eflect Change l[.11.]antit3,r _ (increase, decrease, nr nu change} Decrease the volume chuntainer CD (a) " Ra'ae the tern rature . . l W (r— L12 Add more 1205 {a} Name: Exam 11 (Page 3 of 11} 19. [45 pts} Fill in the table below by identifyMg whether a solution of each of the following is either acidic, basic, or neutral. Compound in aqueous solution Is the molecule acidic, basic, or neutral? ' -. s s tfi{?_): inns“ Part III: Long Answer (30 pts) Please show all work for galeulation — Partial credit ma}F be given / so. {5 pts} Calculate the [cost] in a solution ufflfl45M H3130; {Kal =-4.4x1o'?;1~:s2 = ammo“). “1035 t we? [mg Jr My ta “(3%; *‘H‘LQ “w Has ‘- mg L. Q i3 >< >1 , ‘3' Doug “K x “1 9W x2 ~ e - - i s x 0 1m=~usxfi x— [$39me :JHmfl-n “9‘23 21. (15 pts) You are given a mburfi'mfiflé mL of {HUM HF. Detemnne the pH of this solution. Please be sme to justify anyr assumption you make in solving this problem \éa : Lolosgfi‘l RP + Hm (—7 F was ' Us U I '- [T‘s % x a m 6. {Quilt—X X X 9% X ll“:th OWLXE :_ 4t _ "— film:- CM 0-1 03:50 X = Rwy-“saw e\ 'PH: *lvjlllgo) :1 35% 12 swat?“ —(p.tas:fi§ :23 343-" semi m— (=5 Name: Exam 11 (Page 9 of 1 I] *— / m *Lfifjlme‘t h} [f 2-5g of NaF are added to the beaker from above (assuming volume is constant], what is the new pH of the solution? H CL x 413. ' H? + Hie: ‘7 F‘— 4: t-‘Bfi I 0. tom G-Ii‘tm , _ pH: 33%) l _ . Min pm a WEB We; :31fi4y 01 ‘31:: e) If flit-rt moles of HE] is added to the solution from part b, wha‘tas the n p l? ‘ ma Ha=©mejm IU - may F‘ a age- "—1 HF t—l—he; EH D-L‘S’fiw‘t 108m wane E'- : ‘DH WE '— JJ 'nm't I)”: £2.00 . o ""*—-————.._. __.—, U. '2’]ngth ES {3501 Hill PH“: L5}: 5:51“ 3 He 1 .31 FB 1— .1::- _d.o f1 _ 3 annual * f" £332.71 “‘3‘ 22. (lflpts) A 25.flmL aampie of {HUM laetlo ae MCJHSOE Ka = 1.43:1!) ] ls floated wuth 0.115M KUH. What is the pH at the equivalence point?I 30111. (KLYL’H - 9‘" . P"? _.——-—._._._h H "H -o-- 014* H? W _ '_ ~ I: 1 w %\Ji UGEE‘BWSW j Tfifizmljotai‘fi) I i C$HSL33 “363 ens: - HEWJEmfl Weflewa‘t _. Illlflfi Lemhfl— I I. D" £5 G-L‘Dac)‘ 1' 9 Cate)»: Mao -/—, agate + one - i ‘wfiwke MEL ‘3 b _:_?.<_______._._.-__?E____><_... ._ _ h} what is the pH after 45_flmL of KDH have been added? ’_ fl 1 r: 1: ' "l ‘- H --_i:-; HCLH‘SLZ; a 6+!“ -. Hun + gnaw]— flflgw n “1'0 :3 . m x ' gt] *DUJSWX {.aEaLxLEQY-a y =. L‘ aw] : a omit—b {3: amp a, menu) '. ’T‘ — ibh’é' " I) F‘ . b l _ _ i \ WR—nifi: khan—3:33 + ‘uflfi— PDHJ— pH- 3 E ' ' __. ¢ F .___|_m_fl .__..__|_|_|_|_______,r . ' fiflmfit‘mt "P 5’“le - r. 1 1 I mama. . .. * _ JD. 2- 'r —: O l D -; {Ghev o .tflbL. Page —'lldc1‘LbH—"} :— TDQ'“: PH: ‘IQU’S ...
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This note was uploaded on 05/22/2011 for the course CHEM 2A taught by Professor Guo during the Fall '08 term at UC Davis.

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exam2practicesolution - Name: Exam [l (Page 2 of l I} Part...

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