Exam II c

Exam II c - :EI'HHVIE 1 Chemistry 1392.2 Exam 2 LE fl er...

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Unformatted text preview: ' '- :EI'HHVIE 1- Chemistry 1392.2 Exam 2 March 19, 2003 LE___ fl er on Hie SCILI'fljm-‘L Be careful to erase mmp1c1e1y If you change an Eur ensue: 5; don ’I be careless! EDH'I'HD- m A'aaas'idnoo asvus - J swuvw‘num 2|an . I I] fiEil—Lfijéfifl :n- Calculate the pH of a saturated solution of magnesium hydroxide in water. _ rep for Mann); =15 x 10'“ j' . t 4r '4 m ‘+ r; so 105: O H); 4" H50 e" .‘ a B' 12'3 NEH—)3 m" . . : a “3 Mayhem; taor- Q |\ .x 31‘ C. [3.7 113?: I- 1:; w 9'”: CFrB>ragjg E" : [so [as H * - v -|'-._ 1' , “ ,1 . .. . l'gfi/E) J {Eu I a II lag-"J 2. How many moles of solid sodium hypobrornite { [0} should be added to 1.00 L of ease M HBrO to form a buffer of pH 9.15? 3 mm} = 2.5 x 19'? 144 : c213 - ... C“? :29? FE; a. 0.014 Nebraefl -a- Iteiro as. W 4+ libre- B. 1.0 . o5 onrt C. 5.7 1 L + FF, ET - 0 0.13: Va :- a- s it ID“? = Ciglsii—mj . E none of the above Eflnfirag = ,w i 4,; 1 ‘ n m] 3. The acid-base indicator bromthymol blue is a weak acid. The yellow acid and blue base forms of the indicator are present in equal concentrations vvhen the pH is 6.80. What is the K f b ? "' a or romthymolblue HY + 1m: we + ?H:L-9O A. 4.153 I ht“ 3‘ 2'17‘105 "An = “13% 0*“) f t. s3 v'l o“? ~' ' girders M ma“? ~. I'd"j = ' 5: <1 I : ill-“=1 + Iml“ Misfire-I a" I :' r-Ji. ~ E none ofthe above t - J; at , E j 3 The solubility of CantZs] in water at 35ft: is 1.24 x 10‘3 molfl... What is the value of Ksp for Canis) at this-temperature? A. 1.5:»: 10"5 (ED 7fixflfi Cilia; 6i Ca + 3 l: C 24x10'3 3 9'53 D 1.9x10'9 I 3, B none of the above {5 11%: #53 =7.owo‘*‘-‘I ./ Afar the hypoioflite ion {10'} = 4.3 x 10“. What is the equilibrium constant / K; for the following reaction? FEW HIOiiaq} + OH-[aq] 101an + 20m kb:a.gwpaq A. 4.3 x In”3 x i 1 _ a. B. 5.2x10'6 1;: -— #- KQ “la-H ‘0 at: at: Git C- "- qt '3‘: "'tn 5" a} I .4 4-" "‘H—_ ' e: ._ ’ u sylluflll. : E. 2.3 x 10'11 wt A 50.00 mL solution of 0.200 M HCl is titrated with_0.100 M NH3 (ammonia). What is the pH of the solution after the addition of 50.00 mi. of the ammonia? fig : Kg» 1, .531 x man “I- Kh for ammonia - _ 10'5 id: A. 12.7 Ham}. 4— §“a fl Nita? + QR." 1.3 t awk— Mi' — “*3 .“am . .aoom .1091“ fla _ :HLHLJE: C- 4-7 F lineman firm-a1 "f Sfifil: 3504 Us (10:) I D 9.3 “uh sfim ’Lflg'm {-1. So KID-’9; :3pr ( togm) E. Not enough infomat|$1his Wm solve the problem. W '3 ‘5’ 1+ -- a a =. l' '. ., ft" " S Hfii 'r 030 iiib' itt Ii ‘3' i «7 In the titration of 50.00 mL of 0.05000 M KOH with 0.1500 M HC], after 10.00 mi. of ' the HCI has been added, the pH is A. 12.0 its-a + flag." “JR Lia-.0 “40“ + UN 4- 9'@ 13‘3" 5: iii-am .isoo“ our + H #9 H10 C. 2.0 a sauna] I. an t .. Ii h‘fl Llufii-hni ... D. 1.3 ,-~-s . “'5 "3.1.7: “EM E. fth b i m" V?— "i noneo ea ove hi2“ _ .a M ht , i use? |". ‘5 . Tittate 50.00 mL of 0.1000 M aniline, cantata2 (an aromatic amine that behaves in a similar manner to ammonia}, with 0.1000 M HBI- What is the pH of the resulting solution after the addition of 10.00 mL of the acid? K1, {Cut-1,1011; = 4.3 x l 0‘” 33 Ca gamma + stir F? C W590" 4* 5’7. __ C itilo SGML “mi "5 "if: “‘1 m, I Wan “MUM l \fi'w K! .9 amp-5 Jla ;.-.__1.. -.__ _,......-_-..._.._ .1.._ "w 4- . “1 firm I. . I 1 E. none of the above _ j?“ (I; "0 W] e 1- 1‘- Ir_ i__.._o—._.-- - “in I “is: I‘ll- A yes '. 1... : ‘nb?m. K- :F ia"5 5 :3}.- i‘th l" 15 ‘3 H q “a... .. . . to" *DWIKa a w. - at“ ......—1 _ . . -a raaa JILL- a , Titrate 50.00 mL of 0.1000 M aniline, (3.5%th2 (an aromatic amine that heha‘tfiS in a / similar manner to ammonia), with 0.1000 M HNOH. What is the [DI-1‘] of the resulting solution after the addition of 25.00 mL of the acid? Kb {C‘HFNHZJ = 4.3 I 10" “ . - -10 in 4'3“; lo "M ‘ Col-lam ii; 4- ill-iing (1. ohm} + + NILE. a. 2.3 x 10519! " 3’ *' SDmL 6.115%].- C. 3.0 X 10—8 M . iousm - ibwf‘fv D. 1.7 X M 4W 3"} Md Q-JJfi fl. 1H! E. none of the above _ 3': a, “Li‘” 7'7 x j . . Cwfic ew- Hme mam. to M to “i: W l 0. Titrate 50.00 mL of 0.1000 M aniline, CfiHfiNH: (an aromatic amine that behaves in a similar manner to ammonia), with 0.1000 M HCIO... What is the pH of the resulting solution after the addition of 50.00 ml. of the acid? Kb {gmflg = 4.3 x 10'1" A. 11.0 aqhfiua -i- tacit-3a out. hum-“£5 “ Mo“ {a 3‘3 ’WDH - r. I. i “an: m m J— ‘3 W51 “I'- C. 5.3 _ .. G :3. 1 WE ks L—Hfl—J}; Liswo z [it o. 3.? ' ‘1: 1°an “F “W” '1 'Esii. 1.? me it..- 13. Not enough information is given to solve the problem. I 1'0 e 94.?“ l 1. For a sqution that is 0.250 M CH3NH; (methylamine. H... = 4.4 x 10“) and + ‘ + 0.300 M KOH,_;CH3Nl-13 ]1s wE’NEH + KG“ -_'~_a) my”; NH 3 + A. 3.7 x 10 M ' E - 1's or in. t 1W” KO B. 5.3 K 104“ mm” '31.? ':-10'4M*‘ Kc, T— Q. a 7 Pi ED“ 'i .1:- l'itit‘lial ; § I'll-*1“ D. 0.030 M ' m“- . '3 'l“ . '3 E. none of the above: _ _ __ _ c .. l ,_.u C m 3C3“ long . "an; e "..r- q» _ _ . Kb: ifliyfg“? KEN-j {J J J _ totiu'a- .ots'w'.r ' 12. Calculate the pH at the equivalence point in a titration of 25.0 mL of 0.120 M formic acid, HCOQH, with 0.105 M NaOH. Kmmfic acid) = 1.8 it 104 *- a?“ A. 5.75 '35“ “v ' - t- ”: '- 25 (LL; - F;— NA. H; 03* 13‘ "1' N00“ ‘5“ " 4.50 at = “‘L "D gm 3?” “fr-"LT... 4' H «i.- .33 11 950 a 09401-5 I _ it. 1...: fl.- .esos M E. none ofthe above ‘ (g), it} -- it -- i.“ x E .1: 565119 .i _ What is the equilibrium constant for tho roastion Agl‘zmh‘ifaq) + l‘lisq} AgHs} + 2 CN-{aq} ifofor AngNb'tsq}: 1.0 x 102' and K's]; for AgHs} = 8.3 x 10'”? E. 3-21m)” I 4% .5 X " s so; 5D) 1.2-1Itlfl'5 E. 3.1):10'1'5 ® Consider the following reactions: E W) + 6 NH3{sq) Nimgk2+taq) -Kf= 5.63: log NitOHLo) ' 352%) + 2 OH'tan K5,, = 2.0): 10-13 What is the molar solubility of§i£QHhflJ in a solution in Which the equilibrium [NI-I3} is 1.00 M? 5 wingéflom IL; 39; is}; (magi, + $0 ii" 323:1.er s, X o . fl " B. 0.38M m 11D“? r: [a H53 {passion} © 1.1:: 104 M sow-"H" D. 1.1x1tr4M Ema—3“, R“... I II 1. [law’leLl ‘-. {r («lg-‘3; :ruomf '5 For 33(1th Ksp = 6.0 it 10*":I at 25°C. What is the concentration in moLr'L at 3"3l‘1ili13'rllnmP EMQDJJ ‘fi- 3‘“ 1" 53m; H ' E none of tho above @A' $333: missus-Moose??? t! ' *1 ,s: g. Lluxioflib 3 [+13 . .s x = “I! E- nonoofthssbovo S SJ'X Io ® onus is molar solubilin of 0(0ng in s solution buffered at pH: 4.02:: 64; r q Ks? for Cr{OH)3(s) = 6.7 x 10‘“. A. 1.9 x 10'12M R's-F IEF3+ EN}? is? ND 1" FD” T )0 . : B. 6.7 it mum (of; Qws 3': U was: CW3: 1km“ I c 1.9 3: 109m _ _ - 6.? x 10-19:»: soc"; ‘1 4:7 o. . _ .olfi _ What is the pH ofa 0.0200 M solution of H2804? For Ka :1; x 11]:2 d ' A- 1-49 as 01.19 .9 a- ssay-«1. also .I ' - m- 1' d”! + 1.70 ' Raf-Mag 5 a + r C. 1.61 _., J .3 Hi I _ . 3gb“- @ 1 84 K“ i a?! b 3 in“ F+SUL1T H15 rims . PH i i _ 4 five _~ none of theabover Lid} :1. a: :5 Beam“ 0 4 .{iejtrtra at“? I hit. W 1'1th ‘3 .x" 13. K... for M gFfls) = 3.? x 10;? Mix 500 mi. of 0.00400 M Mg{N03}2{aq) with see 1111.. of 0.0080M KFand Matisse); 't H: ma 1;; + tarts... . _ . WM? semi. A. QSP e» Ksp, a preclprtate forms. 5” . ofl‘ifil’fi. ' . . . + - i fl“ —-—-.._. I i4.3-:-".'£""=-- :-"-.'.-'5.‘-"-=-'r".-'- -'.:i-..:':i-'...F=.-i.5';—" .353 n fifiiiiw-p’i. Li W .J. :1 mm i __ E) 05'] «c Kgp. a precipitate forms. * .1 "_ L_ W e .053 mk D. - Qsp = Ksp. the. system is at eQuilibrium. 3' "MI .-. .oe am. E. none of the above : Cm '3 [tit-jg” imm‘ ms? {mot-Jar“, We)0 = €50!qu its? “’2' G 1 9'. To increase the concentration of acetic acid in the following equilibrium, Haas!) . + H2010) H30+ifl¢0 + Ac'taq} A. add H20. yin B. add OH‘- 7‘." II" . ._ HitL _. add the conjugate acid of OH'. :7? {33.3. ’x. fir. \ d T"i'..:~ u=.=-.:.';":i'i" 1.3.” .-. ' ifithfim— a}: '-r 3. fl "t II ' ' - '- r 4' in 15. none of the above a } .. t‘ N . fifthfifl 2 ll. A buffer solution with a pH of 9.00 may be obtaingib;mixing 36.00 mL of 0.200 M j- 'Q_Q1%_Wilh 64.00 ml. of 0.200 M NH4CI {Kn for Nflfi = 5.6 a: 10'”). By adding 1.00 rnL of 1.00 M NaOH- to the solution, the pH is changed to ___ f)“ _ Cf 9.03 . ' ll * 11; (Li. + h N Cil'i“ “Wee “NW-:2 . t 3.9? 3.11 .353“ J CH3” M9 1 9.09 3* .Jaom 'fiD‘DM Q‘lxlb‘ " M I. him" _ .. 1'...- q“ E . CED 8-90 5‘ 'fiem " 5“”“””‘“‘L' a ' ' vffia'ne'fm .u i 1'” ’ L43) 2 1. The acid-base indicator bromthymol blue is a weak acid. The yellow acid and blue base forms of the indicator are present in equal concentrations when the pH is'6.80. The indicator color is considered to be “pure” blue when the ratio of base to acid is 10:1. What is the pH when the indicator is “pure” blue in solution? A. 6.80 _ s. 6.90' ell-ta. can 7* ’ C“ 6'70 , ""11 -',}:l.'i'r]k to "3 _ a: .' ' “ill 7.30 H L f @ 1 ".4 F The pH of human blood is controlled by several buffer systems including the HECQsHJCfig' system. If the concentration of HQ); in blood plasma is 0.024 M, what must the / .concentiation of HECOE, he to achieve a blood pH of 7.4. pKa 1 [mega] = 6.1 at 1' physiological temperatures A. 0.024M ‘>< : gagyiosg B. 2.0 x 10'3 M w: o C. 0.48M :gggw—o so sis-0'3 M . is. ours so: 0. + osmi— i - s 3 mg- “$33 23. $711332“? the following swim act as wieicflh his: to ether to forman “#7. ML" A. 50.0 mL oi 0.500 M am:2 and 50.0 mL of 0.500 M 1304-3 “if ' sis-o a. 50.0 mL of 0.500 some3 and 25.0 mLéof 0.500 M Miller " C. 50.0 mL oi0.500 1v? NH3 and 25.0w": of 1.000 M HCI - o. 50.0 mL of 0.500 M Nfisand 50.0,mL of 0.500 M NHsCl mL of 0.500.M Pdf- CE 250 mi. of 0.500 M HCl and 50.0 _ ‘ ' —-——o Hie? s U" —3 24. How man};r mmol of KOH must be added to 100 mL of a 0.100 M solution of acetic acid {Ka : 1.3 x 105} to give a buffer having a pH of 5.0? " 5* 3-] Koli 4 90c; 0.10 Jr Klflfé all—:5 B. 4.0 1o‘ffl‘bw x. .I-. C 9 10.0 is Autos-AA s s ‘ m ,- .. s H c . fl- -.._: 3 D_ 5;? tar.“ :ll E/‘Z ; Ihr r"... I “3' I - I. - I .; ' ' t " ' ' 1" _'.I . E: ' iii-11!;- ’ -. flit... .I [In 3;. .w’l f" fog};in ELL? {- A solution consists of 0.0501541 3.0g” and 0023-31 ___C_o_2+. Hydroxide ion is slowly added to the solution as KOH. What is the concentration of Ca2+ when l'itlg2+ begins to precipitate? Esp for Culflfl)2 = 2.2 x 10'”; K31, for Mg{0fl] 2 = 1.8 I 10'1 I 25. A. 1.2-s1049 é 3.5;:10"? X- D. :09 x 113: @MDC‘JEHRDE QQAED'QQ a 3.353 as H‘A’ " - . .x ‘ _ i. I H w '1'“! @930 I 6.131041 J (by?) (3314} so: is d? . @1417: ("Gk/t5“: ,_ r—w .. Calculate K; of Ctl(CN}42', if it is found that in a solution tliat is 0.0500 M in Cu(CN)42‘ _.// and {180 M in free CN', the concentration of (3113+ is 1.2 x 10‘2‘5 M. x Cu“ {an} + 4CN'(aq} A. 1-024 ‘ffli Cums B. 1.0x10'25 _ 1; Cut} '1 : - X G“ c. 3.0::102" Kt- 9"“ - ’0 y r ‘ E ‘7 kD-u- 1.01'1025' 5: :1- Slc: X1 i E. none of the abet-'e ii 2?. What is the molar concentration of l'ttlg‘_F2 above solid Mg{OH)2 in a hufi‘er solution made from 250 m1. of 0.10 M (CH3)3N, trimethylamine, and 500 mL of 0.10 M (CHgkNHCI, the conjugate acid? Kb for {CH3)3N =-6.4 x 10'5 lisp for MgtOl—I]; = 1.6 x 10'” A. 3.9 x 10" B. 9.8 x 10'5 C. 4.3 x 10"; =13. --1-.'.6 I 1&3! E. none of the above ...
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This test prep was uploaded on 04/16/2008 for the course CHE 1302 taught by Professor Young during the Spring '08 term at Baylor.

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Exam II c - :EI'HHVIE 1 Chemistry 1392.2 Exam 2 LE fl er...

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