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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.