Standardization of Can Alkality Titrimetric Analysis

INDEX

Standardization of NaOH by PHP.

Determination of strength of 0.1 HCl by 0.1N NaOH.

Experiment No. 01 Standardization of NaOH by PHP.

Object:

Standardization of can alkality titrimetric analysis.

Reaction:

PHP reacts with NaoH giving rise to the generation of

Colour change of the end point:

Colour change runs from the colourless solution of faint pink color at the end point.

Glass ware and apparatus:

Burette(50ml)

Conical flask (150 ml)

Pipette ( 20ml)

Volumetric flask ( 1000ml)

Reagents and chemicals:

PHP( )

NA

NaOH

Phenoptheline indicator.

Procedure:

Preparation of 0.1 N NaOH:

4 gram of NAOH was weight by balance and it was transferred to 1000ml volumetric flask containing about 1000ml of water. The flask was shaken gently to mixed. The solution was diluted to mark and mixed well.

Preparation of 0.1PHP (C_8 H_5 〖KO〗_4):

Exactly 2.04 gm PHP (phenoptheline indicator) weight by balance and transferred to 100ml volumetric flask containing about 100 ml of water. The flask was shaken gently to get substance dissolved. The solution was dilution to the mark and mixed.

Titration of 0.1N NaOH with PHP:

10ml of 0.1N NaOH was taken in a conical flask 2-3 drops of phenoptheline added. The solution was colourless and tritation was carried out with 0.1N PHP fill the end point is reached. The end point is indicated by the disappearance of the pink color get solution and three times to get the main values of the tritant

Calculation:

We know, Here,

(burette reading ×molecular weight of PHP)/(portence of PHP ×molecular weight of PHP) Burette point = 10.4

= (10.4×204.22/(1000×10))/(0.203 ×99.5/100) Portence of PHP = 99.5%

= (10.4×0.020422)/(0.203×0.995) Molecular weight of PHP = 204.22g

= 0.2123/0.201985

= 1.0 Factor

Normality of NaOH = 1.005 x 0.1 = 0.1005

Table: Showing titant values and normality of NaOH.

Initial burette rate (ml) Final burette rate (ml) Difference (ml) Average (ml) Normality of NaOH

NaOH S_1=(S_2 V_2)/V_1

0 10.3 10.3

0 10.3 10.5 10.4 0.1/005

0 10.3 10.4

Experiment No. 02 Determination of strength of 0.1 HCl by titrimetric analysis.

Object:

Standardization of 0.1N HCl by titrimetric analysis.

Reaction :

HCl reacts with NaOH giving rise to the generation of NaCl+H_2 O

HCl+NaOH →NaCl+ H_2 O

Colour change at the end point:

Colour change with phenotheline indicator runs from the colour of the solution to faint pink colour at the end point.

Glass wares and apparantes:

Burette (50ml)

Conicalflask ( 150ml)

Piptte (25ml)

Beaker (250ml)

Volumetric flask ( 1000ml)

Reagents and chemicals:

Hydrochloric acid (HCl)

NaOH

PHP indicator solution.

Procedure:

Preparation of 0.1N HCl: About 10ml HCl was dissolved in 1000ml of water in a 1000ml volumetric flask. The solution was shaken gently diluted to the mark with water and mixed well.

Preparation of 0.1N NaOH: 4.0 gm of NaOH was weight out. This was transferred to a 1000ml volumetric flask containing about 1000ml of water. The flask was shaken gently to get substance dissolved. This solution was diluted to get substance dissolved. This solution was diluted to the mark with H2O.

Tritation of 0.1N HCl with 0.1N NaOH: 10 ml of 0.1N HCl was taken in a conical flask. 2-3 drops of phenoptheline indicator were fill the end point was reached. The end point was indicator by the sudden appearance of faint pink colour just with the addition of single drop of titrant in the solution. Titration was carried out three times of get the main value of titrant.

Calculation:

We know, Here,

V_1 S_1= V_2 S_2 V_1= Volume of NaOH = 8.9

〖= V〗_2 S_2= V_1 S_1 S_1= Strength of NaOH = Factor x 0.1

= S_2 = (V_1 S_1 )/V_2 = 1.005 x 0.1 = 0.1005 x 0.1

= S_2