1* i (-

-:*-\\"{-*^,.-SChapter 1-6 questions

1. Which of the following statements does not accurately describe a characteristic property

of an Arrhenius acid?

a) An Arrhenius acid is a substance that increases the concentration of hydronium ion inwater.

produce a salt and water.

fu.t*Btb) An Arrhenius acid reacts with a base to

1tr1 An Arrhenius acid turns red litmus blue.- d) An Arrhenius acid tastes sour.e) An Arrhenius acid neutralizes a base.

a) An Arrhenius acid is an electrolyte.t6--l An Arrhenius acid turns red litmus blue.

'f An Arrhenius acid tastes sour.

f\*a' v

bt.n-e- !.t-nill2. Which of the following statements is incorrect?

ffi An Arrhenius base is an electron-pair acceptor.b) An Arrhenius acid increases the concentration of hydronium ion.

c) A Brpnsted-Lowry base is a proton acceptor.d) A Br@nsted-Lowry acid is a proton donor.e) Acids tend to be sour, and bases tend to be bitter.

3. Which of the following statements does not describe a characteristic of an Arrhenius acid?

f

!1v,,L- G:5 ! s'

d) An Arrhenius acid reacts with an Arrhenius base to produce a salt.

e) An Arrhenius acid reacts with CaCOg to produce COz.

4. Which of the following species is not capable of acting as an Arrhenius acid?

+j-

a) HzSOg

b) HSOg-'fSJ so'-

d) Hzo

e) HsO*

Aoa*s?* t* .5

t :r^{- n\-)

'^*"+.='le,

5.

6.

.l*"q1,AIt

- gea

--)'

u+ +\*fr ? ffc-.-*

Which of the following statements is correct concerning the neutralization of sulfurousacid by a strong base?

2OH- (oq) + H2SO3(aq) ) SOs2-(o q) + 2H2O(t)

a) HzSOg is an Arrhenius acid, but not a Bronsted-Lowry acid.

b) H2SO3 is a Br@nsted-Lowry acid, but not an Arrhenius acid."E HzSO3 is both an Arrhenius acid and a Br@nsted-Lowry acid.

d) HzSO: is neither an Arrhenius acid nor a Br6nsted-Lowry acid.e) HzSOg is a Lewis base.

Which are the Bronsted-Lowry bases in the following equilibrium?HcOO-(oq)+ Hzo(/) ==- HCOOH(oq)+ OH-(oq)

E.ldoD- +H2P € Hco"tl+bH-BAAg

a) HCOO- and HCOOH

U Hcoo-and oH-c) HzO and OH-d) HzO and HCOOH

e) H2O, HCOOH, and OH-

k- .x.".t&- b."K-

7. Which of the following pairs of species is not a conjugate acid-base pair?

a) o2-, oH-b) H2CO3, HCOg-

Icil Hruoz, Noz*VFd) Hocl, ocl-e) HSO+-, SO+2-

8. What is a conjugate acid-base pair for the following equilibrium?HrO(/) + HPO4z-(aq) '-=- HzPO+-(aq) + OH-(oq)

tfl HzO is an acid and OH- is its conjugate base.

b) HzO is an acid and HPO+2- is its conjugate base.

c) HPO+2- is an acid and OH- is its conjugate base.

d) HPO+2- is an acid and HzPOa- is its conjugate base.

e) HPOq2- is an acid and HzO is its conjugate base.

9. What is the conjugate acid of HzPO', (oq)?

a) HgO*

16r-1 HgPOa-Zi- uPoo'-d) HsP

e) PO+3-

10. What is a conjugate acid-base pair for the following equilibrium?H2O(/)+ NH4.(og) : NH:(oq)+ H3O*(oq)

a) HzO is an acid and H3O* is its conjugate base.

b |fl NHa* is an acid and NH3 is its coniugate base.c) c) HzO is an acid and NH3 is its conjugate base.

d) d) HzO is a base and NHg is its conjugate acid.e) e) HzO is a base and NHa* is its conjugate acid.

[\,FofiA

+ H,f

t'

+ n e&,''rB

+* \+p\9

11-. What is the conjugate base of HzPO+ (oq)?

a) HaO*

b) H:PO+

gl HPoo'-d) HsP

e) PO+3-

L2. Which of the following species is not amphiprotic?

r=.Il NrHu2*lE- b) NzHs-

c) H2POid) HPO42-

e) HSO:-

13. Which of the following species cannot act as a Lewis base?

a) s2-

b) sH-T-tT1 At3*

d) Hzo

e) HzS

L.u.^r.fi taaS'e is ci u' *\*"r$"^^ ?; &ge

14. Which of the following species cannot act as a Lewis base?

F Be2*

b) 02-c) OH-d) Hzo

e) HzOz

15. Which of the following species cannot act as a Lewis base?

a) N3-

b) NH2-

c) NHz-

d) NHs

T-611 NHq*

L6. Which of the following species cannot act as a Lewis acid?

a) K*

b) Mg'*c) Al3*

d) H*

fGilH-17. ln the reaction

CuO(s) + SOz(q) ) CuSO3(s),

a) Cu2* acts as a Lewis acid and SO32- acts as a Lewis base.

ry 3l :ff :: : iil: i::: ::: ::,1*1i""ff xx*

:l :;: :.*"1"#:;:f .#.,1'""j :' iT;T',,--.T:J:'":18. Consider the following reaction:

AeBr(s) + 2CN-(oq) ) Ae(cN)i@q) + Br-(aq)

The species that are acting as a Lewis acid and Lewis base, respectively, are

a) AgBr and Ag(CN)2-.

b) Ae(cN)i and Ag*.

c) Ag* and Br-.

d) Br- and CN-.

W Ag* and cN-'

19. Which of the following is not an example of an acid-base reaction?

a) Al(OH)g(s)+ 3H*(oq) ) Al3*(oq) + 3H2O

b) Al(oH)g(s)+ oH-(oq) ) Al(oH)a (oq)

c) cN-(oq)+ HzO(/) =- HcN(oq) + OH-(oq)

d ui,ffi ;?:ilfiLi.T:;?''''-"^ \t -l+

20. Which of the following species cannot act as a Lewis acid? \ r IPilit c,vr**F\.-q.,,* ..+ Ior--d"il i

:i i:1, -'l#F

N Lf L l., ,r,* i, ?*,$^-ole) Ag* '\ ,*.Lols (:\^€s\ffit^ Lt- \ -\ t o w;

2r. $r,.l;ll

hasthestronsestconjugatebase? -fY{l i:-t::#-\,€sa.* ,Y"

r b) Hoct t\J ,L

--\."*A g lo' {-*^" \43 vr'z"Jc-al" *---:-s

t.{iq, :i Xl,o- \ ';{a\ . * / ,,)s zz. Which of the following acids has the weakest conjugate base?\ro {-A ..,-r^ a) HF

..{' Igl fllX,r c) cH3cooH\ :i X|l; f*'* *ke---h*'^$rs'l-

----:d)a::4<-Aq tbwlr-n*{

a) HCIO4

b) Hclo3c) HCIO2

\Iil Hctoe) Hcl

23. Which of the following acids has the strongest conjugate base?

{-*"^ \t.o- r.rr"orKrar-- c-a,'bi* '5 ltnli- c_\rt,-f

'{€EilL\

24. The acid strength decreases in the series HBr > HSO+ > CH3COOH > HCN > HCOg-. Which

of the following is the strongest base?

TilJ co,'-*ui cru-

c) CH3COO-

d) soo2-

e) Br-

25. What is the leveling effect?a) All acids are 1,00% ionized in solvents other than water.

W All strong acids are 100% ionized in water.' c) An acid with a higher concentration in water has a lower pH than an acid with a lowerconcentration in water.

d) A base with a higher concentration in water has a lower pH than a base with a lowerconcentration in water.

e) All bases are 1,OO% ionized in water.

26. Which of the following reactions is not product-favored?a) HCI(oq)+ HzO(/) ) HrO*(oq)+ Cl-(aq)

b) HCIO+{oq)+ H2O(/) ) H:O*(aq)+ ClOa-(oq)

Tgl NHg(oq)+ Hzo(/) ) NHq.(as)+ oH-(aq)' d) NaOH(oq) ) Na*(oq)+ OH*(ag)

e) HzSOa(oq)+ H2O(/) ) HgO*(oq)+ HSOf(oq)

27. The reaction of which acid with water is product-favored?]-ill nitric acidw

b) chloric acid

c) nitrous acid

d) chlorous acid

e) phosphorous acid

28. Which of the following statements is true concerning an aqueous solution of the weakbase NHr?

a) NHa* is a stronger acid than H2O.

b) HzO is a stronger acid than H3O*.

c) OH- is a stronger acid than NH+*.

]U OH- is a stronger base than NH3.

e) NHg is a weaker base than HzO.

29. Which of the following statements is true concerning an aqueous solution of the strongacid HBr?

a) H2O is a stronger acid than HBr.

b) H3O* is a stronger acid than HBr.

C ED H20 is a stronger base than Br-.

I Ol Br- is a stronger acid than HzO.

e) Br- is a stronger base than OH-.

30. Which is the strongest acid?a) BHg

b) cH+

c) NHa

d) Hzo

EHrtb:g tf-*q'('

\*

31. Which of the following statements is incorrect?a) One reason why HCI is a stronger acid than HF is that Cl has a larger atomic radius

than F.

b) One reason why HCI is a stronger acid than HF is that the H-Cl bond is weaker thanthe H-F bond.

\gl One reason why HCI is a stronger acid than HF is that Cl is more electronegative than*/ F.

d) The acids HBr and Hl both appear equally strong in water.e) F- is a stronger base than Cl-.

32. Which solution has the highest pH?

fA:l o.1.o M HF{oq)

"tr o.1.o M Hct(oq)c) 0.tO M HBr(oq)d) o.to M Ht(aq)e) O.tO M HCIO+(aq)

33. Which of the following is the strongest acid in aqueous solution?ftn HrPoaL--b) HsAsO+

c) HEPOE

d) H3AsO3

e) HrSbO+

34. Which of the following is the strongest acid?

F-U Hclo4b) Hclo3c) HCIO2

d) Hcroe) Hcl

35. Which of the following solutes, dissolved in 1.0 kg of water, would be expected to providethe fewest particles and to freeze at the highest temperature?a) 0.10 mol HCIO4

b) 0.L0 mol HCIO3

c) 0.10 mol HCIO2

ffi o.ro mol HCloe) 0.10 mol HCI

\dsl

. \.--Q-&5' i-

Gd:-taz-..-\

T.e *"i5'f '*.,k;\gl^.5 R*

S$fr,.,\yl..s( **36. Rank H3POa , HzPOq , and HPO+2- in order of increasing acid strength.

a) H3PO+ < H2PO| < HPOa2-

b) HzPOa- < HPOa2- < H3POa

p HPo+z-< HzPo+-< HgPoa-dl HzPo+- < HrPo+ < HPo+2-

e) HPo+2- < HaPo+ < HzPo+-

37. The ionization constant of water at a temperature above 25'C is 3.3 * l-0 14. What is the pH

of pure water at this temperature?zHz}(l) H3O*(oq)+ OH-(oq)

i(w = ;q,lllo u-J '= 3'3x''J'$

- / l- l+ro3 -;.J

'ri-r- 4 2*..,'o : l. gl e k( c, I

38. The autoionization of water, as represented by the equation below, is known to be

endothermic. Which of the following correctly states what occurs as the temperature ofwater is raised?H2O(/)+ H2O(/) H3O*(og)+ OH (aq)

a) The pH of the water does not change, and the water remains neutral.b) The pH of the water decreases, and the water becomes more acidic.

fl The pH of the water decreases, and the water remains neutral.d) The pH of the water increases, and the water becomes more acidic.e) The pH of the water increases, and the water remains neutral.

39. What is the equilibrium concentration of amide ion (NHz ) in liquid ammonia at 25'C?("om" = dissolved in ammonia)2NH3(/)

3.6 x ro-24 M7.8 x l}-2a Mg.O x 1,0-2s M2.6 x Io-rz M1.3 x !o-r2 M \s n-'z I

kr € tQ.*n^**ht{

Niia(i) t '' ?) rq,..Q,

\':.: lJi::, ,,r,*a(-,

-l>

J lcr-

T-12

I , jft':'-*""-**

l(, ( -,2-Y

- rrl f,sX'c>

a) 1.3.52

flfl ol+c) 7.00d) 7.74e) 5.54

a)

b)

c)

d)

p\t -. --l.3fi*311 :- -{ nj(i,R\6x..1 ) = 6"*t4

-r$rf:l f r'r'r\r)

X

-\ il]'tu.s ,+gr<t'

40. What is the hydronium-ion concentration in a solution formed by combining 450 mL of0.1,0 M NaOH with 150 mL of 0.30 M HCI?

sh\a [..,__e W^\

;l orroo'Jro, Naor\o'+ *\%";2 NnSttLtu,

c) c) o3a M 4 '- '*\a> 0 'l Xo 4€ ' u'}x o '16 '

-:ffi L.0 x 'l.o-7 M 0, 0 1t5...^*\: c-1t! "'''\se) e) !]x10't3M t - ,..---..."-."'_

ryV*5 -n-*-f*j{ c-o--)$L* fft'--l .--4t. At 0"C, the ion-product constant of water,.K*] is L2O x 10-1s. What is the pH of pure l\,

water at 0"C?

a) ,.ooott r-'i, ^t--l "fi,i^-r..l- (L'3-1: \o

b) 7's6o fh,,o!: t[t'G-*t;'s u-r'3-*]

c) 6.880 '= 3'\6X..rB

F f:"trthese ) Pt= G*t'"%Ca'*o*..-8): l. 4ce, nOne isv-

42. The concentration of H:O* in a solution is 8 x 10-a M at25sC. What is its hydroxide-ionconcentration?

a)

b)

c)

d)

TGJ-\

SxIO-4 MLx !O'10 M2x !O-10 M2x !o-10 M!x !o'11 M

lon I" [H.(aq)]

14.0 - pOH

-log IH.(oq)]

-lon K"

"[oH]-log K*

l<w€ :GrJfl

?* - -l"*r r-n*-l

RH = \t{- * foH

fHfl =}i-^'3 "' LoH -!,

. . -i\LI rC) !us, I

€.x;+ - ! esx,:i",.{

46. Which of the following expressions is not equivalent to pH?

a)

b)

c)

d)

ril7,A

wc)

d)

e)

solution in which the pOH is 12.5 would be described as

very acidic.slightly acidic.neutral.very basic.

slightly basic. T+\:\(+- \?"

F \"5

caw-J -=

*T(,.;t 'is e\ vj * .^.[ i<- -sot..il*

48. A solution has a hydroxide-ion concentration of 0.0050 M. What is the pOH of thesolution?

'gP z'tb) 7.0c) 77.7

d) s.3e) 8.7

prc* :a- 3,saft t+ -llJ : -t:3C"s,ot>Sro)

49. What is the pH of a 0.075 M HCIO4 solution?a) Ls.Lz

@t.tzc) 12.88d) 1.L.4r

e) 2.s9

50. What is the pOH of a 0.047 M Hl solution?a) 15.33b) L.33

*...'--*::52. What is the pH of a 0.0088 M hydrochloric acid solut

Ft'eroO l-t e sV':^S '^.i"Q , tf,*^*t*'e- f*tt[",-*rzeJ qI- ^]Lo** _('\*K; 't i J

F\ c-\\ **;- - HzJ - CLb;

?U, *talt+=dJ

\, , -Y\olbo."s)=!l=$ IYrT: ?oR

- r'{ t )t- 2 ,,_\ _-[rq - r".v\-"i- 3.06 ( - \q - (-'g( ,:.,x:l) - \' ') lQ. 6J

51. What is the pH of the final solution when 25 mL of 0.021 M Hcl has been .OO6lffitrof 0.037 M HCI at 25sC? _- \ .* .^ -. ,-rJa) 1.9

'iE ,.s " -

C hnolai "d '+'l t(o "tl-t *)::;:;;.r-

T 3.s rr, \ trgk{ {r)"a1sxu'o');1)=t"^:':2.oi 3.3 (? ftorat0 FF4 n "-.-l*n i"gzx'{'ftta'Le) 2.7

ne-|*-$Lq- ffi=D'o3r'(a) e'27

. r- ^^c1r]9.-:5 ^'{&' I ,

r, r\ :rf Hr* }. -l'3f" 'a9}tP iil^ -\()f".pors) ') [_ , - t.Sd) 4.73 L

53.;l";::""ium-ion.fr""#"lutionis4.6xLo-uM.WhatisthepHofthesolution?a) 9.99

T-oil s.g+t4-c) 6.55d) 3.s1e) 2.00

po= -\.tLq"t'v'{t]= S"zq

54. At 25eC, what is the pH of a 10.0 M HNO3 solution?

fl-'o?S= -\'1 lD'

\5t"-]:: -L

ftmtg s,4*'13 *-.rdJ. .

b) o.oc) 1.0

d) 10.0e) 74.0

55. What is the approximate pH of a 0.1M NHs(oq) solution?

56. What pH should a solution have if its pH is about the same as that of vinegar?

Vi^*3^"' (( a- v.r-esr,i(- x-JZQ. )a 6

57. A solution has a pH value of 11.9,What is the pOH for this solution?T-al-l 1.0.64

T" q.fi p c,t\c) 7.oo \d) 3.36 ' ; 10' 6L{e) 4.37

58. Which solution has the highest pH?

p.u,t:-r+ V.s;z f'S\'=*ff n- t"az-

a) 7

b) 3

c) 7

El rte) 13

a) about 1b) about 3

t.fT about 5

d) about 8

e) about 11

Nt? *H3o € r-t *f, t

-L lLt - rotf= rc* -, 5 2-1

=, g'1 b"

,?il

-= \\,3 \-#

10

**r- \ .

G{--T\ \@l-bhv'

a) O.t M HCI

b) o.1. M Ba(oH)zc) 0.1M NH3

d) o.t M cH3cooH+dn o.1. M NaoHlL:/

59. The pOH of a solution is 5.24. What is the pH of the solution?a) 7.00

Vfl ata ic) 2.67 D F

d) s.24 \

e) 5.75

60. What is the pH of a 0.0041 M Ba(OH)2 solution?a) 2.O9

b) 11.61.

c) 2.39d) 9.20

-. 'D' t e) \rr.sr26L. What is the pOH of a 0.0029 M Ba(OH)z solution?

fielY V*?S. [+-Q"ort

4rp*U

I ,ob) L7.46c) 2.s4d) 8.8se) 1.L.76

a) 15.62

@r.ozc) 12.38 ,\ , r .\d) 1'0'27 P'\+ -z-l s"t | ':'bzc1'\e) 3-73f-J

65. What is the pH of a 0.0074 r u* ,"f #*a) 4.sL l* .E\*-:3 $^-:W-b) 16.13

. c) .2.r3 # t,'fp= t* * ?.r)+ \W !r^2, Y' - \,-+ * ( -t5(1-,-o

u1.t)e) s.oe U ,

66. What is the pOH of a 0.0042 M LIOH solution? : \! g-

67.

C"*l = &r o'Do)q - $,ocEB

Pcvh-=-tTCo'oofr):: Z-)4

.:--

62. A solution has a hydronium-ion concentration of 0.0080 M. What is its pOH?

a) 4.83 ,

-b) 2.to eS= - t'3 fo ''r-u€)c) 16.10 I * 2.0.161.

I$11.eo ;-T g.tt ) ?otf = \* - ]"t:1{1 = \\.ol o63. A solution has a hydroxide-ion concentration of 0.026lVl. What is its pH?

ffitz.+t ^rr F

'b) 17.65 ",,Do\{ - -\3(o.rab)c) 1s.59 \

d) 1.se : \"58se) 7.oo =) 1

rt64. What is the pOH of a O.O24 M HNOr solution?

V rn== a-Q&.

a) 5.47b) 16.38 ..tj\ - ^- {s-rr[-sFt-l@2.:a y J*' )d) tt.6z ' j--tsq b.eDY2-e) 8.s3 "#ZSWhat is the pH of a solution prffied 6y dissolving 0.832 g of NaOH(s) in 6.50 L of water?a) 2.495 '-----b) 12.31.8c) 1682 lwf,d-k. %'N\44 =:tt:-'*)'Y";i ;:;' r 1r

vo{ q\ /"-IJrrsos -Q B\Lb*nt{*/t,'1,Tr..e

; pD\} z- *t5B'>*C 11

-,/ \ _ 'i-uT'{

\\, b0p$ '(K-fdt c lq - 3'('r =

--7\. 7 tlx.-il

68. What is the pOH of a solution prepared by dissolving 0.578 g of KOH(s) in 6.00 L of water?

H,tt li.Z:r, huu\,'i\'y\t aH'- i t'' s'r s s . S$ .'\ /,,, cc L

c) 1..987 ' 5L''9',/

d) 7.000 -.{r {l ;- - i-.-.rft, i+ - \ ,-7

69.il,.J:.T:pHofa,I;"",,;;,;j*/,.1,ffi),,ffiedatSTP,in

r34flj.=}-,

enough water such that the total volume of the solution is 2.50 _L? (R = 0.0821 L . atm/(K '

= l::'f{ =Li!""R-e-.e"o.r-( Si-fr ler:$*

pir; n R i*mol))a) 1.2.1.27

tru 2.271.

c) 1.1..729

d) 7.oooe) 1..873

mol)) n._ Iy._ := r- ,,r, .! '\ t -3a) 12.472 l'\ = aq \ = / [''['{.'ux\ \/. 4.cl j;is',i

b) .2.306 ^ .'._' - /- - ,\ \ 5 *t";'X-r-l \, ro'coL'

ffi ,i.uno ;1 ,*.i,;.".t, :- ( i,l \ \d) 7.ooo t \ v / -f,tt -, \tr- o\-{e) 1.528 l- ;; iq .- [l ,..r-., r(.(t1r r*.-,t \

71,. Which of the following solutions has the highest hydroxide-ion coicentrEtionf -...-l '/

a) 0.1M HCI .. l,b) o.t M Hzso+ sc) a buffer sotution with pH = 5 -l>-* tU -.r..;Jt \ ==::d) a buffer solution with pOH = 12 \

f-"i j pure water r'72. A solution has a pH of IO.7 at 25sC. What is the hydroxide-ion concentration at 25eC?

a) 1,.O x 1,07 M , r \ ,. ..-1 -t ), 2,

g 5.o,1.0a.i pqtt=" r,.r- pH \_1 \_'rrr'J: {c,' 2

c) 2.0xLO-" M -- (r.( - i,:- I \ U.Ll vr*

q f".(d) 3.7 x'J.02 M ., \ ':

e) 3.3 M :r '3'.} \

--

73. A solution has a pOH of 5.44. What is its hydroxide-ion concentration?

;l iZ:131Y, { -- --.1 , ,-,'ro'*.i 2.8 x'J.os M l. o f+ j L: l \-

f- qfi 3.6 x 'r.06 M - a- '{{ -6-") ' 5.4M

w

:: 5,e5{Y;;4 M il-c{,Rr 6.r;4;"-ral,,, l '?rt -*

-(i\" t ttr sX'i' 'p1

F*o xr*l r*t

t4 -:-; o'. P i?:19'"".oleS70. What is the pOH of a solution prepared by dissolvingO.664 L of HCI(g), measured at STP, in

enough water such that the total volume of the solution is 6.00 L? (R = 0.0821 L . atm/(K '

74. The poH of a solution is 5.30. what is its hydronium-ion concentration?

12i-'F{r'l If$'\*+ q3)

\-. t'7 \

*.1

a) s.30 Mb) 5.0 x L0-6 M

D z.o x ro-e Md) 5.0 x L0-' Me) 2.0 x I}s M

75. The pH of a solution of a strong base is 10.38 at 25eC. What is its hydronium-ionconcentration?a) t.3 x t0'2 Mb) 3.4 x to'3 Mc) 2.4 x tO-4 Md) L.g x !O-4 M

JE 4.2x rorlM76. What is the hydroxide-ion concentration in a solution formed by combining 200. mL of

O.LG M HCI with 300. mL of 0.091 M NaOH at 25sC?

HCI(oq)+ NaOH(og) ) NaCl(aq)+ HzO(/)

T:;iI !.! x !o'12.M h^dkJq Nat)+ = u,Bx oaet6'..6xt'-r,M -0'

.i 1.ox1o7M -a:- D'oH3'*dd) o.oss Me) o.osr M lY's14 '{ t+t4 a o ' 2}:4L- : cr"o?2.

77. Which solution would cause blue litmus to turn red?

\+^dU = '{:":r"'r = [u

_t(: {* \68Xto fttt

r>O XQzL l^rf{/ '-/- -e_O,oaf3)

{o'o'4 -?. )

= +"1 (t-o -'ndls

*ry$ry

a) a solution of pH 10

b) 'a solution of pOH 4c) a solution of 0.10 M NaOH

d) a solution of 0.01 M NHs NAc"-q \Try. _z? ' W"Iot.""$5

b,5 u,-71" ryxuo

J_"T\ a solution of 0.005 M CH3COOH

^-*o p[t\+I =te*r-fI

1, ox,tu'(

9 "tK.:3 '

*\L-: [. o6rtru*94

M- \,.\ *^'-q13