period - loudoun county public schools homework 15.4 (37 points) a. read pp 748 - 762 b. review your...
TRANSCRIPT
PERIOD:
HOMEWORK 15.1{40 points)
a. Read pp 719 -733b. Review your notes.c. Answer the following:
I. Calculate the pH of each of the following solutions:
(4 points)(a) 0.100 M HONH2 (K, = l.l x 10-8)-I-
Ho t.J 1-101 -I 1-t1. 0 t::-"':? /-/0 AI /-1" '"Ir .100 0
0/-1
c --y
.\-y
o+'¥
)t
_ .g-1,1 ~'O ~
_$
: 3. 32.'!-/0 M
P01-\ = Jf. ~2
iffl: 9.SJ}(4 points) (b) 0.100 M HONH3CI
140 N ~\ 3 ~ -"7 H0N I~3 i -I C1-I-)O/,,})-\ 3+ + /10/-/ --=7 1-13 0 t -I /10/1./1-/.;
.r _/00 0 0
C- -'Y- +'X-I-)l
t:. ,I-"X X)l
- IY1.0 'f 10
1,1 'l-IO-t' : -• I
)(~[H-tj ~ 3.0~'f..ID-~M
P 1-1 ~ 3. s~(1 point) (c) Pure water
OVER
(4 points) (d) A mixture containing 0.100 M HONH2 and 0.100 M HONH3CI
IiO;.J H:J. + t-I?. 0 ;;;:::? 1-10;.11/3" -I 0 f/ -. 100 .100
cf
[A-]pq: e 1<0-. -t JOj ~J =
= (~. 0 '-I I(
/,0 y./O-I'{) (, I 06 )
-~ /.1'110.8 t -4J ~
(4 points) 2. Calculate the percent dissociation of the solutions in lea) and led). Explain any difference._s3.39. '/-/6-; 100
({OO) 0, 03310
(5 points) 3. Calculate the pH after 0.10 mol ofNaOH is added to a 1.00L buffer solution consisting of 0.60 M HF(K, = 7.2 x 10-4)and 1.00 M KF.
OHB .10
-=7 F t /-/~0
o
1,00
+ . 10
/.) 0
(l, -.10 -.10
A[1\- )
f ~z: f' k~"1~j [\4A J
so
(5 points) 4. Calculate the pH after 0.20 mol ofHCI is added to a 1.00 L buffer solution consisting of 1.00 M HN02
(K, = 4.0 x 10-4)and 1.00 M NaN02.
H-t t tJOs ~ /-lA/Of}.,
8 , ao 1.00 1,00C -.JO -.~O +.~oA c) ,gO J,QO
[I\-jr 1-\ z P l<fA -r loj [,4A J =: -)oj "10 '1,/0 -I{ ~ .-i~( 'I. :~ )
=B
(5 points) 5. A buffered solution is made by adding 50.0g ofNH4CI to 1.00 L ofa 0.75 M solution ofNH3
(K, = 1.8 x 10'5). Calculate the pH of the final solution.
(J() SO. ~ IJI-I'ICJ '1'11....( tJl-lC{ Cf"M~ ,IJ W~ \..{ .::
I $3,SO
/,QY/O'IJ(
c ·s/, 6" X 10
_ '0
.:- S. S {g '/. 10
OVER
(8 points) 6. Calculate the pH after 0.10 M NaOH is added to a buffer solution consisting of 0.50 M CH3NH2(K, = 4.38 X 10-4)and 0.70 M CH3NH3CI.
A~ 'Ir~-'( = 1.00 l
C ~13fJ 1-13 CJ. -'7 CHJ IJH3 ~ ~ CJ -
(.1-\ 3 IJ~\:3+ -':> c.J-I3.v H a. + J-/-+~
OH of C).13 AI 113 of -'7 C1-/3 AI!/d- + ~o6 • /0 ,70 , SO
C -, 10 - , 10 +.10
A 0 .00 ,(pO
CI-b"-l 1-1 ~ H~O -'7 c..H3UH/ -t QH+- ~
T . &0 .(,0C.
E[A-J
a kC\. .• loj -fH~ [~AJ1
- '4 ) loj ( +)1.0110 _z: -loj (-y, 3&1-10-"
+
-= LJO, ~ L( )
PERIOD:
HOMEWORK 15.2(25 points)
a. Read pp 733 - 745b. Review your notes.c. Answer the following:
1. Calculate the pH after 0.15 mol solid NaOH is added to 1.00 L of each of the buffered solutions:
(5 points) (a) 0.050 M propanoic acid (HC3Hs02• K, = 1.3 X lO's) and 0.080 m sodium propanoate.
H C...,Hs O~ <.Cl.£''' OH - ((.o..~) -~ ell H.s 001 - ea.gl of ~ 0 (1)e . os . IS. 02C -.0 S - . o~ T I 0 sA 0 . )0 ,13
~ fl~ = r~ ~ ~ ~~}Jc.1.j (1.3110·')" kj (-':~!) s: 5.09
~, rJ0 o.iLd ~ •..a,i,v.:>. l~tLIK LA{ CI4A 0 H -, [0Ir J = .) 0
(5 points) (b) 0.50 M propanoic acid and 0.80 M sodium propanoate.It1O(i)
I-\C31-bO,:J <ao) -t OH- (~) -? C?l I~~O~ (Ct.~ ) ~
(j , So . IS . ~OC,- , IS - .IS- T ,13
A ,3S 0 ,QS
pl~ p~-t-~
[~Jloj (1.3 '1-10-!OJ + loj ( -\\- )s: ---- :.
[o.WA J
=lS.J;l If 2..p.eints,).{G.)..ls.th~.SQlutiQI:J,rn..patt.(a.)..stiJl.a.buffeJ:ed.solution.after. the NaOH has been added? Explain.
No _ V!v. ~ L, Jia.O/-{, ~4wA~~ -:tt ~f ~ ¥wdo ~ ~.3~ (b) 1.4.7 ~ r+ kf~ aar1f ytl,(M ~ (&<.).
OVER
(3 points) 2. Using the bases in Table 14.3, which base would be the best choice for preparing a pH = 5.00 buffer?Explain how to make 1.0L of this buffer. . _I. . il J/ _A 1
01H pH s: ~ .00 ~ ...w-t ~ OWl acux _WWL f f\a. tUQ.t .A1, S. 0 .
IY ,00 ~ f~ of f K~; tJ~ /twd tL 1'U4U --' If/:«H. tt fk'£ = It;.OO - s. 00 t: 9'(Jo.
So /(b ~ 1.0 '/10 - 9. 1.J!u.htJ dt(t~ ~ r~) C!; 1-& Ai I .wdAJ o I( - 1«(I)b = 1.7'1 (0-1• I<tt .: ~ : !~ 'f.{O -=4 i: s. fr8y 10-r.
pU < fl4.. LJ [I-1J k'. rc;w,tP'O . - ;._- ----~----
(
e- [~) k [cs/~.sIvlJ loj [Csl'lsAJIPJ: -, <i Add .SCHYl ./JJ.J",',.j'AA"s OJ ~ - 0."" ~,f8-Y..lO +-;j .•"\ I-(f~·-·-
- -""":J [Cs /·/sIJH .J [C5f~sIJJ = o. sq ..k /.00 l ~[Cs!-lSt.JHiJ
(10 points) 3. Sketch the titration curve for the titration of a generic weak acid HA with a strong base. The titrationreaction is:
On the curve indicate the points that correspond to the following:
(a) the stoichiometric (equivalence) point(b) the region with maximum buffering(c) pH = pKa(d) pH depends only on [HA](e) pH depends only on {A-](t) pH depends only on the amount of excess strong base added
Cd) ~ (6)
pH
;' J
NAME:
PERIOD:
HOMEWORK 15.3(25 points)
a. Read pp 722 - 736b. Review your notes.c. Answer the following:
(5 points) 1. Calculate the pH of a solution that is 0.50 M CH3NH2 and 0.70 M CH3NH3Cl.
CI-I3..JW,;} (~) ~ 11,;.0(.1) ~ (!JIJ I./~ + -r: OH-I .so • ?O 0
t -y +~ ~~f . S 0 - X • 70 t ')(
1)\ ~ [CH3tJH3-1J [owJ -f{ (x.)(.70tJ:)I'\I:J - _---- : l..3!ylO -
- [CI-I.?IJ1-1 l ] (, so -1c)::
x (.70)
t . s»1( ~ [olrJ s
pO /-1 = 3. $ 0
(5 points) 2. Calculate the pH after 0.10 mol ofNaOH is added to 1.00 L of the solution in Problem #1.
CI-I,a ~/-IJ ~(~) f 0(-/ (O-~) -'7 CHJAff.l;z (OJ) + 1-/20(1)(3 • 70 . /0 . $.0 0t -.10 _ ,0 -+./0
A . vO 0 . ~O
C.~J,\JI~2~) .J /-/lOrP) ~ (!.I/J AlI6 -I rap -I O/{(1;)I ,(,0 .c o 0c -xb .~-y:
[CI~3I\)H1+ ] [olrJk'b ~[CI-{ 3 JJ/-IJ ]
X z 4.38 'I.IO-tf pOI-! .;
,(,t'Y Y()'.)(.(,+~J
(.(.-"1)
- ---------][pl-l = 10. to '-I
::
3.3("
(15 points) 3. Consider the titration of 100.0 mL of 0.200 M acetic acid (K. = 1.8 x 10-5) by 0.100 M KOH.
Calculate the pH of the resulting solution after the following volumes ofKOH have been added:
(a). 0.0 mL KOHH+ (0.0) ~ C!1-/30l
-1-1 CL H 3 0'2- ("-t) -'>
(t:\~ )~
I , ;:)()O 0 0
C -"/. t~ t--y
f , ~--X '1 Y
[WI] [CI-hOl-J~ ().)('1-) X2--I<~: -5 - -;.
': ,. ~ 'f.. 10 :: ,~ -X .J[1-1Cl I-Is 01, J
2 - VX ~ 3. ~O '110 OVER
-y-< [HiJ z I 00 I q0 lfl-/ .: ~. 7;;-;
o H- (~) -"7 C2. (-I3 0" - C~t )"' I-ll 0 (J)
10l'>\nv ..f 0-10
oSvV\U [1.ICl-I-!30:J t; [C~H30z-] -t,ue ao a;I ~~ ,~~ f~
,af-J" p~:
(b). 50.0 mL KOH
H C ~ 1-13 0 "2- (Ct..f -t
!3 ;10,., ""~C. - s .»A IS""",.,.@
OH - (~ )
S,O 1'\'\ ,,,,...e-5.0
oH -I (tL~) of
ot-)C
ICE
'1--1Cl.. 1-) 302-
. 100
-y
. / - /( --,("X) (, 0333 ., ~J
(,/ -X)) - s
1\It = /. 8")( 1 0 =
(c). 100.0 mL KOHHC24302 (CA.t) 4
e ;(0 l>\."AC, .. 10
A. / 0 IVI t\\ ~
Cz. f./ 301. (d-b) -I I-h, 0(1)
o"I S. 0
s· a 'VI_v--!('1. 1./ J O~.. (t1.,,)
!J
.0333
,0333+-y
(~) (,033'3)s:
• I
x z: [H1]= S. if' y: /0 -s 1'1
[ to 14: .y, nJ
I- I ()
10 Mi\ol,.f
/~/tiJao: ~ ~
- 10j (1.3'110"') = @
(d). 150 mL KOH
oH - c; 1-13 02- - ("-0) of «» (1)H ('~ I-I 30 z ((0.1;' + ('V) -78 .;)0 ""'I~lr-f I S 'fI\ /\\,./ 0e "I~ - IS + I .sA S 0 1.s1'1'\~)
He, 1-13 0 l (Cl.o) ~ '? H of (t<.~) •• c. ~I30l- ("v')
I .o.;l0 ,0(,
L -Y- tll t-lCE IO~-")C X . 0(, t -x.
'<It ;; - s (x)(.o(, -\-'X\ (X)(.QCI)I,~)( 10 t: ::
('Od---x) (. OJ)
NAME: AtJ.s-wl:'il I(.r;i
PERIOD:
HOMEWORK 15.4(37 points)
a. Read pp 748 - 762b. Review your notes.c. Answer the following:
(& 1) (5 points) 1. A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.125 m NaOH,requiring 16.00 mL to reach the equivalence point. During the titration, the pH after adding 2.00 mL ofNaOH was6.912. Calculate the K. for the weak acid.AA jju Mw'~ ~J- : (ltg.COm L ) (0.12.$ Mmr-l/fhL)" .:I. 00 It1ru,J N~OJ.l ~dtl..td,v~
M~ -:tl~ t~..k ;),()O Mnt~ q-6 HA ~ ~ .J. OJ "" L rJt\.0 1-\ ~J. = ;>. 00 mL ( 0 . I 2.~ 1M f\'\...t 1M L) = (J, ~ SO", ""',..( 0 H - d.f1tJ.JJ
\--\,6j -t 0 ~\ - -"7 IY1.0 ,..A [1-1 +J:: I 0 - ft-l = 10 - (,.~11.. z: I. J. ~ X/ 0 -7e J.OO . ;;>.S 0 C)c. -r , 2 SO - . t..)"() + ."2r()
P\ 1.15 0
I-lA z:.:: '7 Ii of +
I f,l~/vT />.2.2'1-10-1
=
(6 points) 2. Two drops of indicator HIn (K. = 1.0 x 10-9), where HIn is yellow and In- is blue, are placed in
100.0mLofO.IOMHCI. HIt) e.2 11\- .,../-/7 l<tt: [.IIl-JO+:](a). What color is the solution initially? . .- [H1'11 ]
!-IL, ilXhH
(b). The solution is titrated with 0.10 M NaOH. At what pH will the color change (yellow to greenish yellow)occur? [\ rr J [ 8~ cl\Oll cJ ~ : 10 Hi] ~ 1'(..10- 1'1r l:lll-]
I(t\ = /. 0 'I ,0 -9 ; ,~ [Wt)
(c). What color will the solution be after 200.0 mL of NaOH has been added?
LJJJ ~;tt IU're-ir-.'''l pv-~ ,<UJ /ft ~/Q)( .& ~ k~ ~1:tJu ~n .wdJ d.n~~ JIu ~~~..wJJ.,Jv J4, .
In - fvwt
OVER
(4 points) 3. A solution has a pH of 4.5. What would be the color of the solution if each of the following indicatorswere added? (Use Fig. 15.8 on page 756)
(a). methyl orange ~
(b). alizarin ~
(c). bromcresol green
(d). phenolphthalein
(6 points) 4. Write balanced equations and the corresponding solubility product expressions for the dissolution ofeach of the following solids:
(b). Ce(103)3
Ce. (103)3 (S)
(c). BaF2
6CA. r-~(s) ~
l~~) (8 points) 5. Use the following data to calculate the K,p value for each solid.
(a). The solubility ofPb3(P04)2 is 6.2 X 10-12 mol/L
P6~(PO .•)llS) -=-:> 3 Pb"2.-+ (&"0 ) -t .J POI.( 1°('1)
I 0 0Cf
+3)(3-y.
( 3.":)() 3 ( s., /
+ ;;) y
IO?s (c." J. ¥ IO-,z. )~
Iq, q X I ; - .r]
cE
-')c
l'6l\) (4 points) 6. The concentration of Ag' in a solution saturated with Ag2C204 (s) is 2.2 X 10-4 M.Calculate Ksp for Ag2C204 •
1.-
Aj 2- (\.Ol( eS) ..c ? dA,j ~ t,) -+ e2-0"l eeo)T 0 oc +2~ tYf J1C v
J-x"" .;l. ~ "110-1{ fVl
,,/.- ,., ')( 10 -I( f'1
k'sf z: [As -I J 2 [Cz o; l- ] :0 ( d)- ') L (~) ::: q ~3
- Y ( /, I )(IO-tij3
- ~,"3)(( 0-"']
('(s{,) (4 points) 7. The Ksp for cadmium carbonate (CdC03) is 5.2 x 10-12. Calculate its solubility in moles/L.
Li 1-Cot. C03 (S) <:: ":> Cd CD) -t" CO 3 ("-b)
I 0 0C +x t-'Y
E X ~1<~f : LCJ Z~ J [Co/J ~ ('X) ()( ) X 2.
') - Il -v z,S. 0( "f..1 0 = _~A __ -:----;-l
X .s: \1.-;)-' _3_'1-_'O_-_(,_~_E-_l
OVER
PERIOD:
IIOMEWORK 15.5(30 points)
a. Read pp 762 - 780b, Review your notes.c. Answer the following:
(5 points) 1. For each of the following pairs of solids, determine which solid has the smallest molar solubility.
(a). CaF2 (Ksp= 4.0 x 10-11) or BaF2 (Ksp = 2.4 x 10-5)
t30Jl .ac-U fW>~ 3 ~ i-... ~" ~-MJf- ettn ~jJfU< 1<5;0 ~.1;-~(~~~~~.
\~F;(.n ~ ~4~ 1
:tC.
f
I(sp = lk jOi} [Al/,J = 1,0110-21
:- X 1-
1/ z: f 0 'X10 -l/ 11II.v-f+~ ,... L
X "I FePO ~ ~(9 points) 2. The Ksp for silver sulfate (Ag2S04) is 1.2 x 1O-s. Calculate the solubility of silver sulfate in each 0 t efollowing.
(b). Ca3~O~(KsP = l.3 x 10-32)or FeP04 (Ksp = l.0 x 10-22). Hint: You must calculate the solubility of each in orderto make the determination. 3
z+ -Gx 3 PO,-{(S) L ~ .J Co.- (~) + ~ fOy .o 0
+ 3 y + Jy.
3 v: ell3 1 3)'2. .s~I(1!-!] [pot/-] ::),3 'i-IO-n:. (3/<) (.;l')( = log -X
J(:: (I. : : ~ 0- 32- ) v- z: J I ~ 1, I0-1M~
F. .IJr~ -7?-+ ]-e. , VI( (S) c- J='"e (o.l) + fb, ('1»
o 0+"1
(a). Pure water
f-\.j :;. $0 <{ enI
tE
Cl As \,~ ') -l- SO<.f 2~<i )
o 0+d..-y +y
d..-X X
\~ Sf ~ LAS tJ 2 [ SO<f t-J ~1(= 1?,OIY ;:!j
-S"I. .;J. '1-10 =
OVER
b). 0.10 M AgN03
032 SOq cn ~ J-Aj ~ (~) +
I ~ICE
+ ~-y
k'Sf-r
I, .;l '1-) 0
1,2.%
d A~-t- (~')..\ SO'-{ ~-C~)
o e;)
d~ .J-t-'Y-
['\]4J 2. [SO'1'-] -: 11~110S"": (c;1)() 2. (.JtX)I, ~'f.. 10-5 z (Lj')CZ) (.) = ,g'X"L
X :!O. 003Q ~ 1(4 points) 3. For which salt in each of the following groups will the solubility depend on pH?
(a). ~AgCl, AgBr ~ «s. I .J./i. 4, I -/1~ f-'11{ .::u\.L.o.4 4a.xk '\llAJ{a,,~ ~ Q.,u ~. <.rr«
~ .mJj-., "",o::f clw...vv. _ l~ (h~l.o :tArJ QAt ce-~o~~ A •
(b). ~ PbCl2 -r - J I - J U H •~ 1, ""'0 a.wL. . ~ >M< ~o ~ ~
(c). Sr(N03)2~ ~ ~ (lA,J J jJ-~, do '11,~ !\AAI'€ ~.--i ~.w-litl ~4 ~~ f~ .
8C.A
(4 points) 4. Calculate the final concentrations ofK+ (aq), C20/- (aq), Ba2+ (aq), and Br (aq) in a solution preparedby adding 0.100 L of 0.200 M K2C204 to 0.150 L of 0.250 M BaBr2. (For BaC204, the Ksp= 2.3 x 10-8
).
M""Lu-( /< 2.. Cl-0'1 z (/00"", L ) (, J,OO '"":':' ) = ~O. 0
VV\ rY\ r-t & iSr-"L = (\SO "" L') ( . ~S 0 ':'~ ) " 37. SLot ~- f2
'{30. (~)-t Ct.0Ci ~) -~ IJe.. C,O'i n)37.S- ~o.o 0-2.0.0 -2.0.0 +'20·01/. S 0 2..D.O
'2..rO z: .0700 f'1
0,1&01'1
s: 0.30014
6a. c.O~l.'t (;1..0<1 2-(ril )(~)
-';> 60. ('1") +-c;:--
;:;: 3,:1 YJO-7r1J=~C.O. '-.]T .01 0 'X
C +"'i +'1E (L&hJ .: 0, 0700 r-, ].ol't')C yI~sp = L&1.~J[CO/J :; J. 3 '1-10
-g (.Ol+X)().).:
(4 points) 5. A solution contains 1.0 x 10-5 M Na3P04. What is the minimum concentration of AgN03 that wouldcause precipitation of solid Ag3P04 (Ksp = 1.8 x 10-18)?
Aj?> POq (S) ~ 5 Jj -r ("]) + fb'1 3~'b)
k'sf = I. z « 10 -Ik s: [AJ t) 3 [Po,/J
I. g '(.. f 0 -I ~ ::: t A5 -i ] 3 (/.(J "I- I 0 - s:)
[PO,! J];: [tJtt3 POlf 1'1t: I, o ¥ I O-r
c -131,0'1.10
z:
OVER
(4 points) 6. Write the equations for the stepwise formation of each of the following complex ions.
3+ 1+ \
CO (~H3)" r t.J~~) ~ Co (1J~3}; '1)3+
Co (fJt-l:,)s c,h tJI-l3L,) ~'7 CoC"Hh):+(rV
(b). ,Ni(CN)/
u: l+cab'> of eN -c~) ~ ~ Nt eN (;)
Nt CN t (' l .•CtJ - (~) ~ N(' (CJJ),) (i)
NC (ctJ);J (~) t C,tJ- ('b) ~ Ali (CN)a- (~,)
Nt: (CN)3 ('i) ~ CtJ- (~) ~ r Ai,; (ll\l)~ (CtfJ)