chemistry 02
TRANSCRIPT
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Experiment Number: 02Name of the Experiment: Standardization of CommercialHydrochloric Acid solution ith standardSodium Hydroxide solution
Course: CHE!"##$
Name: A%N%!%Ashrafuzzaman%&oll: 200'0(0$0)roup: A2
*artner+s &oll: 200'0(0$,-epartment: EEE
-ate of *erformance: 02"0#"200,
-ate of Submission: 0."0#"200,
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Chemical &ea5ents:1.
Standardi!ed $a"H solution2. HCl solution3. 5istilled %ater4. "xalic Acid
2. (henolphthalein 3. )ethyl "range
Experimental -ata:
Standardization of NaOH solution with standardOxalic Acid solution
Number of
Obser-
-vation
Volume of
NaOH
inml
Burettereading
in mlVolume
ofAcid
inml
Average
Readi
nginml
StrengthOf
NaOHN
nitialReadi
ng
!inalReadi
ng
6* *6 6./ *6.0 *6.*7.839 6.6783
96- *6 *6.0 -6.* 7.96/ *6 -6.* -7.7 7.8
Standardization of H"l solution with standard NaOHsolution
Number of
Burettereading
in mlVolume
ofAvera
geStreng
th
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Obser--
vation
Volume of
NaOHin
ml
Acidinml
Readinginml
OfH"lN
nitialReadi
ng
!inalReadi
ng
6* *6 *.7 -*./ *7.0*7.-// 6.62*/6- *6 -*./ 06.3 *7./
6/ *6 2.7 -0.7 *7.6
Calculation: "
:e ,no% that 6 acid 7 S acid 8 6 base7 S base
5etermination of the normality of $a"H ;##Here V acid = 9.867 ml
S acid = 0.1 N
V base = 10 ml
S base = ?
So, S base = ( 9.867 X 0.1) /10 N
= 0.09867 N
5etermination of normality of HCl ;Here
V acid = 19.233ml
S acid = ?
V base = 10 ml
S base < 6.67839 $So S HCl =dilute>< = 6.67839 ? *6 > @ *7.-// < 6.62*/ $
%e also ,no% V concen!aedX S concen!aed= V dil"eX S dil"e,
Here1 HCl=concentrated>< -.* mlS HCl=concentrated><
1 HCl=dilute> < *66 ml S HCl=dilute> < 6.62*/ $so S HCl=concentrated>< = *66 ? 6.62*/ > @ -.0
< -.*/93 $
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ut in the given HCl solution eBual amount of %ater andhydrochloric acid %ere present i.e. %ater ; hydrochloricacid %as *;*.
So the actual strength of HCl
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-> Another cause of error may rise from faulty burettereading.
'f these causes could be avoided %e could have got moreaccurate result of the strength of Commercial
Hydrochloric Acid.