Quiz 1 - Quiz 1 — CHM 2046 — Spring 2009 — Prof C.R...

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Unformatted text preview: Quiz 1 — CHM 2046 — Spring 2009 — Prof. C.R. Martin IN ORDER TO RECEIVE FULL CREDIT YOU MUST SHOW ALL OF YOUR WORK 1 ALL WORK MUST BE CLEAR AND LEGIBLE Name: A ‘ ‘ ' UFID: ‘ - Why do Chemists prepare and use buffer solutions? 5_p_ts Chen/113%: y‘apom: b1§¥613 “i0 Cervical W ”WA 051: a solerCM They cw be. 1186:}: 310 611111/ 0111 $131 demodcni GXDGVMW‘ 2. What 15 the definition of a Lewis Acid and a Lewis Base? Provide an examples of a Lewis Acid/Base reaction that does not include a Brznsted acid. A (301313 CLCCCl \S 01H @12ch $503? mac—7610? A Lean: Eqse. 13 QA guano“ @011? (10/103- BE + NR3>H3N*E¥:3(1A C1015; awn/(Pk) !. 3. Why are all Lewis Bases also Bronsted bases? _1L . . ‘1\ Leo: 334563 (1 n be mRM‘teci Smge Cx Lewé @136 has 4 \owa&$a‘1v 0“)? elecirmnS 'EY degmiflcm ox BWnfieA base accepfi awaken MWQ :9.“ 1.311113 561335 ave Evasmlvecl E4563 4. For aqueous solutions of each of the following, predict whether the solution is acidic, basic, or neutral. (5‘) NaN03 Medtval (b)NH4F lagging-10 >Kb=l.Lli-l\ (c) CrC13 ACldlC (d) CH3COONH4 Kb: \g‘k : S. é, :- \O Hakim (e) KOCI FEaSi C 5. Calculate the pH of a 0.01 M fonnic acid (HCOOH) solution. 1 pt each - Ac‘dxc l , H6002? + H M3 [H600 Riv] :— -L Hgbgt’limg; o 9 i; K0: meow] \.‘4Z I -x 1-K l" (X)(_)( W cow? : V424! 0M x 040M &“ X1 ad 1 [RE-Ll so, x5" \q£_ q $51124, O Ol-X x = 1:393 XZ—l— \ 7i"! X-l7i‘é =1 C) I], : £23,.wa ~\ 72 Ll i 01qu- 40V '726 12‘32‘3uoo Z(|\ X: .15 '5 anérlEiS ‘ ’tnd3c ”Vesitklc, So [H*1:X=\3£3 ?\\; 403 UV] * “\03 [132 31 V 6. Calculate the pH of a 0.15 M NH3 solution. 5 pts ‘aé! . . NRSQ‘Q +l\zOm g2 “wily OWE“) , _ ' 0.5% O ‘ o i "f ~x +x +X (BAY-X . '. +X “NV N“ *1 O H’l _ _ _ (XXCXB ' . xvi—”ME z \Bt-S - am -°¢0-\‘5"‘xo"s . v; T XL KB: fi: \.82:S Lei—’5‘ 5—K. I6/O:E%9\“w LEE-3 POM = '\é$[°“~] ‘1 -\o. [Lei—~33 - fl 5' ' f 1—7 : r—r xlOO w m- m [M]: x = vet-3M Is; 7. A 35.00 mL solution of 0.25 M H1 is titrated with a 0.20 M NaOH. Calculate the pH for this solution after addition of the indicated amounts of the V NaOH solution. (a) 22.55 mL of NaOH 2.9.5 35ml. H1 (0.313le “13 _, 33.55ml— No.0“(clao mma\ 3&0 “>(lpm0‘ “I; mL E I ML No.0 \quo 8;?5Wnol HI " LLSlmmcl HI :- Ll’QQMMOl H1 (analq'\¢ \ - ( +13xtcm5c\ ; 4.9.4 mmol “l _ ~ ' : “it LHI] : Bfimt +3.55% ‘ 0.073223%: PE ‘2}- l 7 "‘ eofl‘ Gt \‘ ¥\\ 2 - lo? [W1 = —- logffllOZlSTfl 3* 3 ‘ ' _PH : \‘\S l (b) At the equivalence point OLA A ‘ 3 -\'l *wcécecl 5.1% (Joke cu Swan . \DY at: $3n‘on8 ESQSG, Jrlrxa ?\’\ 6:: ' 45m: equwcdevxce ficwfi XS . Hillier NetOmex 9"» N63; + “20 EQwvdence ‘JPO m4} .' . > §<—————\(———-—l( W\ Wt mL HI \mmd\ HI O.aOMMo\ m0 eqmvadence 139le VGWJMC + 5C) mL \L (c) 50.00 mL after the equivalence point 1% a MOINQO“ «r C), RS‘mmd “I: \ mmc‘ Nata“) QS7S mL Mao H (01“? (Rho “”B_ ngL H1< MML 91>(v—f—Hmmd “I ‘81Smmol m0“ “ $75: “named NQQ\‘\ :IO mmo\\\\v~0“ (Tt+?an~\-\ t (ana\¥*é\ 9‘ iOmanS‘ N40“ ; 0 \0q MNKQ“ :[OHTJ LNaO W] 1 ssmt.+43?smusnmL . Sm“ No.0“ ‘3 ‘? O H : ._ \68 [O “‘1 1' - \CJCACO' \Ocl\ ’ CL Sikmns base . p09: Moi iH:lLl—1>O¥\ 2 \L\-\.\Oc\ 8. Suppose you have 1.00 L of a 0.55 M HCOOH / 0.35 M NaHCOO buffer. What will be the pH of this buffer after 0.010 moles of pure HCl are added? 5 pts NWW page“ up a: Moor” + H30“ " 0.55—“M 0,35M 0,Q\M +é.0\ M ’ _o,o\ M ~o,o\ M EQuIL‘LBRluM O , 3-5 M +>< * ~>< m ,. ,0 I, 36¢:-X a3q+x ’ + x # {Hadoflifififl » (oat! mm \zwf W a \f—Piv‘l = use - x O? Wnfi Mm} MM: \3 60 aged Emma? [Marl (”3‘0 FR : $Mk ¥ \&3 {M0031 1 —\&$(Hi-L(\ + ‘63 W ...
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