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1. r.atmtatE- lie mkffll d ttmt needed ta readl lhB equvaierm 1D1t In the llndlDn
d a 25.0 r:nlsam,pm ol1'0,,BO mcil NIOH(lq) by 1.10 1molll 1-Diaq). .-■i tn: IL12 LJ
2. Fm the fflndil!Jn il1S11q:111 PmbJem ~
,(,a) wllllt Is 1he EDK1!I tlmllon 1d IIIIEllmBd M·(lq) RI the pH at 118 mutlCJJI lfflr
5.0 oid·U,e sodium h)ltrmtii8 IOidlon, NalJHlaq)~has bil!!B!I llddad?
(D} llhll"ls 1h11 ammnt {11 IIIOIII) Df lRBldEtl M1•(aql 1M 'lhe ptt 1of b-.dlon
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and 'Iha I'll DI 'l b!•Sfll'llltian during ttb-all•1
~ 'Wflln 1DJJJ ml Df D.2CIOi nriolW1. Nalll(aq} Is &dcled? ra g mmot pH - ~
(:1)1 when 1am ml or 0.200 ITIGM!.. rtacH,AqJ t, ~ cr.IJ [1m: 1 mmotj pH •iLeeJ
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Dm
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whlf119.3 mlDf thebase IIIISbeen ,llided.
(a) Mlat I& ·BIB cam:aubdoo of Ille aid~ _. 01ffi'2 1m'L]
1
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Questions
I. A 25.0 ml ..mpl.- of hydrochloric acid, HCl(aq).
is tilnll<d with 67.2 ml of0.125 mol/l potassium
hydroxide solution, KOH(aq). What is the
concentration of the acid? C£iil
2. In a titration, 15.00 ml ofhydrodtloric acid,
Hd(aq). is titni.ted with stond.irdiud sodium
hydnmde wlution, NaOH(aq). lhe amount
concentration of each solution is 0.250 mol/L a.,
(a) Whal is the amow,I of H • (nq) and the pH of
the sample beforc NaOH(aq) is added?
(b) What is the amount ofH-(aq) and 1hr pH of the
solution after I 0.0 ml ofNaOH(aq) is added!
(c) What is the pH at the equivalence point?
3. A student titrates 4-0.0 ml of household ammonia
solution, NH,(aq). wilh 25.0 ml of0.50 mol/l
hydrochloric acid, HCl(aq). C!I
(a) What is the cun<'mlrillion of the ammonlli solution!
(b) What is the pH at the equiv;,lencc point?
4. Acc1ysalicylic acid (ASA) is the pain reliev,r in
Aspirin. ASA Is a weak acid with K, 3.2 X io- •.
One Aspirin tablet was ground up and dissolved in
25.0 ml of water. It was titrated using 0.15 m ol/L
sodium hydroxide. To reach the endpoint, 98.J mL
=
of base wu required. m
(al Determine the-conuntration of the ASA
solution.
(bl What amount of ASA was present in the tablet!
(c) What was the pH at the equivalencc point!
5. A 50.00 ml sample of 0 ,30 mollt methanoic acid,
HC01H(aq), is titrated with 0.30 mol/t sodium
hydroxide solution, NaOH(aq). •
(a) What volume of base is required lo r,ach the
endpoint?
(b) What is the pH b<forr 1i11111ion ~gins?
(c) Whal is the pH of the solution at the
rquivale.o~ point?
6. If 10.0 ml of 0.500 mol/l sodium hydroxide
solution, NaOH(aq). is added lo 30.0 ml of
0.340 mol/l hrdrocyan;ic acid, HCN(aq), what is
the pH of thc solution! a.,
7. Would cresol red be a good indicator for a titration
of a strong add with a•trong base? Explain. c:J m
8. In a titration. 50.00 ml of 0,100 mol/L ethanoi< add,
HC2H,O,(aq), is titrated with stand•rdized 0.100
mol/L powsium hydroxide solution. KOH(oq). c:i 111
(a) \\'hat b the amount of unreacted HC,H,01(aq)
and thc pH of the sample bcfore titration?
(b) Whal is the arnow,I of unrcaet<d etbanolc add
and the pH of the solution after I 0.0 ml ofbasc
is added1
(c) What is the pH when 30.0 ml of base is •dded1
(d) What amount and ,•olumc of litranl must ht
added lo reach thc equivalence point?
(e) What is a good indicator for this litratiool Why?
9. R=h a •digital titrato<," Create an illustrated
report to compare ils advanrag<s and disadvantages 10
the traditional titration setup, vfl IDDP
. WEBLNC
8. 7 Acid-Base Titration
617
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