Ex. No.: 1 COMPARISON OF POTASSIUM PERMANGANATE solutions
Date:
AIM
To compare the normalities of the two given Potassium permanganate solutions A and B and to estimate the amount of crystalline Potassium permanganate present in 500 ml of the weaker solution. You are provided with a standard solution of Ferrous ammonium sulphate containing 39.2 grams in one litre.
PROCEDURE
TITRATION - I: STANDARDISATION OF KMnO4 (A)
The burette is filled with the given KMnO4 (A) solution and titrated against 20ml of Ferrous ammonium sulphate solution pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titre value, the normality of KMnO4 (A) is calculated.
TITRATION - I I: STANDARDISATION OF KMnO4 (B)
The burette is filled with the given KMnO4 (B) solution and titrated against 20ml of Ferrous ammonium sulphate solution pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted and the titration is repeated for concordant value. From the titer value, the normality of KMnO4 (B) is calculated. From the normalities of Potassium permanganate solutions A and B the weaker solution and the amount of KMnO4 present in 500ml is calculated, knowing that the equivalent mass of Potassium permanganate is 31.6.
SIMPLE PROCEDURE
Sl No.
|
CONTENTS
|
TITRATION - I
|
TITRATION - II
|
1
|
Burette Solution
|
Potassium permanganate (A)
|
Potassium permanganate (B)
|
2
|
Pipette Solution
|
20 ml of Ferrous ammonium sulphate
|
20 ml of Ferrous ammonium sulphate
|
3
|
Acid Added
|
20 ml of 2N Sulphuric acid
|
20 ml of 2N Sulphuric acid
|
4
|
Temperature
|
Lab temperature
|
Lab temperature
|
5
|
Indicator
|
Self-indicator (KMnO4)
|
Self-indicator (KMnO4)
|
6
|
Endpoint
|
Appearance of permanent pale pink colour
|
Appearance of permanent pale pink colour
|
7
|
Equivalent mass of KMnO4 = 31.6
| ||
NORMALITY OF STANDARD SOLUTION
Amount of Ferrous ammonium sulphate present in 1 litre = 39.2 g
Normality of Standard Ferrous ammonium sulphate = Mass per litre / Equivalent mass
= 39.2 / 392
\ Normality of Standard Ferrous ammonium sulphate = 0.1 N
TITRATION - I : KMnO4 (A) Vs STANDARD Ferrous ammonium sulphate
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Ferrous ammonium sulphate
ml
|
Initial
ml
|
Final
ml
|
KMnO4 (A)
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of Ferrous ammonium sulphate = V1 = 20 ml
Normality of Ferrous ammonium sulphate = N1 = 0.1 N
Volume of KMnO4 (A) = V2 =
Normality of KMnO4 (A) = N2 = ?
V1 X N1 = V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality of KMnO4 (A) = N
TITRATION - II : KMnO4 (B) Vs STANDARD Ferrous ammonium sulphate
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Ferrous ammonium sulphate
ml
|
Initial
ml
|
Final
ml
|
KMnO4 (B)
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of Ferrous ammonium sulphate = V1 = 20 ml
Normality of Ferrous ammonium sulphate = N1 = 0.1 N
Volume of KMnO4 (B) = V2 =
Normality of KMnO4 (B) = N2 = ?
V1 X N1 = V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality of KMnO4 (B) = N
COMPARISON
1. Normality of KMnO4 (A) =
2. Normality of KMnO4 (B) =
\ The Weaker KMnO4 solution is = KMnO4 (____)
AMOUNT CALCULATION
Amount of KMnO4 present in 500ml of the weaker solution
= Equivalent mass x Normality x 500 / 1000
= Equivalent mass x Normality x 500 / 1000
= 31.6 x x 500 / 1000
= gram
RESULT
1. Normality of KMnO4 (A) = N
2. Normality of KMnO4 (B) = N
3. The Weaker KMnO4 solution is = KMnO4 (____)
4. Amount of crystalline KMnO4 present in 500ml of the weaker solution = gram
Ex. No: 2 COMPARISON OF Ferrous ammonium sulphate solutions
Date:
AIM
To compare the normalities of the two given Ferrous ammonium sulphate solutions A and B, and to estimate the amount of crystalline Ferrous ammonium sulphate present in 750 ml of the stronger solution. You are provided with a standard solution of KMnO4 containing 3.16 grams in one litre.
PROCEDURE
TITRATION - I : STANDARDISATION OF Ferrous ammonium sulphate (A)
The burette is filled with the given KMnO4 solution and titrated against 20ml of Ferrous ammonium sulphate solution (A) pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titre value, the normality of Ferrous ammonium sulphate (A) is calculated.
TITRATION - I I: STANDARDISATION OF Ferrous ammonium sulphate (B)
The burette is filled with the given KMnO4 solution and titrated against 20ml of Ferrous ammonium sulphate solution (B) pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titer value, the normality of Ferrous ammonium sulphate (B) is calculated. From the normalities of Ferrous ammonium sulphate solutions A and B the stronger solution and the amount of Ferrous ammonium sulphate present in 750ml is calculated knowing that the equivalent mass of Ferrous ammonium sulphate is 392.
SIMPLE PROCEDURE
Sl No
|
CONTENTS
|
TITRATION - I
|
TITRATION - I I
|
1
|
Burette Solution
|
Potassium permanganate
|
Potassium permanganate
|
2
|
Pipette Solution
|
20 ml of Ferrous ammonium sulphate (A)
|
20 ml of Ferrous ammonium sulphate (B)
|
3
|
Acid Added
|
20 ml of 2N Sulphuric acid
|
20 ml of 2N Sulphuric acid
|
4
|
Temperature
|
Lab temperature
|
Lab temperature
|
5
|
Indicator
|
Self-indicator (KMnO4)
|
Self-indicator (KMnO4)
|
6
|
Endpoint
|
Appearance of permanent pale pink colour
|
Appearance of permanent pale pink colour
|
7
|
Equivalent mass of Ferrous ammonium sulphate = 392
| ||
NORMALITY OF STANDARD SOLUTION
Amount of KMnO4 present in 1 litre = 3.16 g
Normality of Standard KMnO4 = Mass per litre / Equivalent mass
= 3.16 / 31.6
\ Normality of Standard KMnO4 = 0.1 N
TITRATION - I : STANDARD KMnO4 Vs Ferrous ammonium sulphate (A)
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Ferrous ammonium sulphate (A)
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of Ferrous ammonium sulphate (A) = V1 = 20 ml
Normality of Ferrous ammonium sulphate (A) = N1 = ?
Volume of KMnO4 = V2 =
Normality of KMnO4 = N2 = 0.1 N
V1 X N1 = V2 X N2
Therefore, N1 = V2 X N2 / V1
=
Normality of Ferrous ammonium sulphate (A) = N
TITRATION - I I : STANDARD KMnO4 Vs Ferrous ammonium sulphate (B)
INDICATOR: KMnO4 (SELF-INDICATOR)
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Ferrous ammonium sulphate (B)
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of Ferrous ammonium sulphate (B) = V1 = 20 ml
Normality of Ferrous ammonium sulphate (B) = N1 = ?
Volume of KMnO4 = V2 =
Normality of KMnO4 = N2 = 0.1 N
V1 X N1 = V2 X N2
Therefore, N1 = V2 X N2 / V1
=
Normality of Ferrous ammonium sulphate (B) = N
COMPARISON
1.Normality of Ferrous ammonium sulphate (A) = N
2.Normality of Ferrous ammonium sulphate (B) = N
\ The Stronger Ferrous ammonium sulphate solution is = Ferrous ammonium sulphate (__)
AMOUNT CALCULATION
present in 750ml of the stronger solution = Equivalent mass x Normality x 750 /1000
= 392 x x 750 / 1000
= gram
RESULT
1. Normality of Ferrous ammonium sulphate (A) = N
2. Normality of Ferrous ammonium sulphate (B) = N
3. The Stronger Ferrous ammonium sulphate solution = Ferrous ammonium sulphate (__)
4. Amount of crystalline Ferrous ammonium sulphate present in 750ml of the Stronger solution
= gram
= gram
Ex No.: 3 COMPARISON OF Ferrous sulphate solutions
Date:
AIM
To compare the normalities of the two given Ferrous sulphate solutions A and B, and to estimate the amount of crystalline Ferrous sulphate present in 1250 ml of the weaker solution. You are provided with a standard solution of KMnO4 containing 1.6 grams in 500 ml.
PROCEDURE
TITRATION - I : STANDARDISATION OF Ferrous sulphate (A)
The burette is filled with the given KMnO4 solution and titrated against 20ml of Ferrous sulphate (A) solution pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titre value, the normality of Ferrous sulphate (A) is calculated.
TITRATION - I I: STANDARDISATION OF Ferrous sulphate (B)
The burette is filled with the given KMnO4 solution and titrated against 20ml of Ferrous sulphate (B) solution pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titer value, the normality of Ferrous sulphate (B) is calculated. From the normalities of Ferrous sulphate solutions A and B the weaker solution and the amount of Ferrous sulphate present in 1250ml is calculated knowing that the equivalent mass of Ferrous sulphate is 278.
SIMPLE PROCEDURE
S.
No
|
CONTENTS
|
TITRATION - I
|
TITRATION - I I
|
1
|
Burette Solution
|
Potassium permanganate
|
Potassium permanganate
|
2
|
Pipette Solution
|
20 ml of Ferrous sulphate (A)
|
20 ml of Ferrous sulphate (B)
|
3
|
Acid Added
|
20 ml of 2N Sulphuric acid
|
20 ml of 2N Sulphuric acid
|
4
|
Temperature
|
Lab temperature
|
Lab temperature
|
5
|
Indicator
|
Self-indicator (KMnO4)
|
Self-indicator (KMnO4)
|
6
|
Endpoint
|
Appearance of permanent pale pink colour
|
Appearance of permanent pale pink colour
|
7
|
Equivalent mass of Ferrous sulphate = 278
| ||
NORMALITY OF STANDARD SOLUTION
Amount of KMnO4 present in 500ml = 1.6 g
Amount of KMnO4 present in 1 litre = 1.6 x 2 = 3.2 g
Normality of Standard KMnO4 = Mass per litre / Equivalent mass
= 3.2 / 31.6
\ Normality of Standard KMnO4 = 0.1013 N
TITRATION - I : STANDARD KMnO4 Vs Ferrous sulphate (A)
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Ferrous sulphate (A)
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of Ferrous sulphate (A) = V1 = 20 ml
Normality of Ferrous sulphate (A) = N1 = ?
Volume of KMnO4 = V2 =
Normality of KMnO4 = N2 = 0.1013 N
V1 X N1 = V2 X N2
Therefore, N1 = V2 X N2 / V1
=
Normality of Ferrous sulphate (A) = N
TITRATION - I I : STANDARD KMnO4 Vs Ferrous sulphate (B)
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Ferrous sulphate (B)
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of Ferrous sulphate (B) = V1 = 20 ml
Normality of Ferrous sulphate (B) = N1 = ?
Volume of KMnO4 = V2 =
Normality of KMnO4 = N2 = 0.1013 N
V1 X N1 = V2 X N2
Therefore, N1 = V2 X N2 / V1
=
Normality of Ferrous sulphate (B) = N
COMPARISON
1. Normality of Ferrous sulphate (A) = N
2. Normality of Ferrous sulphate (B) = N
\ The Weaker Ferrous sulphate solution is = Ferrous sulphate (____)
AMOUNT CALCULATION
present in 1250ml of the weaker solution = gram
RESULT
1. Normality of Ferrous sulphate (A) = N
2. Normality of Ferrous sulphate (B) = N
3. The Weaker Ferrous sulphate solution is = Ferrous sulphate (____)
4. Amount of crystalline Ferrous sulphate present in 1250 ml of the weaker solution
= gram
Qn. No: 1, 2 & 3 COMPARISON OF __________________________Solutions
AIM
To compare the normalities of the two given KMnO4 / Ferrous ammonium sulphate / Ferrous sulphate solutions A and B, and to estimate the amount of crystalline ___________________________ present in ________ ml of the weaker / stronger solution. You are provided with a standard solution of ________________containing ________ grams in ____________.
SIMPLE PROCEDURE
Sl. No
|
CONTENTS
|
TITRATION - I
|
TITRATION - I I
|
1
|
Burette Solution
|
Potassium permanganate__
|
Potassium permanganate__
|
2
|
Pipette Solution
|
20 ml of ______________
|
20 ml of _____________
|
3
|
Acid Added
|
20 ml of 2N Sulphuric acid
|
20 ml of 2N Sulphuric acid
|
4
|
Temperature
|
Lab temperature
|
Lab temperature
|
5
|
Indicator
|
Self-indicator (KMnO4)
|
Self-indicator (KMnO4)
|
6
|
Endpoint
|
Appearance of permanent pale pink colour
|
Appearance of permanent pale pink colour
|
7
|
Equivalent mass of _______________________ = ______________
(solution to be estimated)
| ||
NORMALITY OF STANDARD SOLUTION
Amount of ______________ present in 1 litre = _________ g x 1000 ml / _________ ml
= _________ g
Normality of Standard _________________ = Mass per litre / Equivalent mass
= ______ / ______
\ Normality of Standard ______________ = _____________ N
TITRATION - I : STANDARD __________________ Vs ___________________ (A)
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
_____________
ml
|
Initial
ml
|
Final
ml
|
KMnO4 ___
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of _____________ = V1 =
Normality of_______________ = N1 =
Volume of KMnO4 ___ = V2 =
Normality of KMnO4 ___ = N2 =
V1 X N1 = V2 X N2
Therefore, _____ = ________ / ______
=
Normality of _______________ (A) = N
TITRATION - I I : STANDARD_________________ Vs ___________________(B)
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
_____________
ml
|
Initial
ml
|
Final
ml
|
KMnO4 ___
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of _____________ = V1 =
Normality of_______________ = N1 =
Volume of KMnO4 ___ = V2 =
Normality of KMnO4 ___ = N2 =
V1 X N1 = V2 X N2
Therefore, _____ = ________ / ______
=
Normality of ____________________ (B) = N
COMPARISON
1. Normality of ______________ (A) = N
2. Normality of ______________ (B) = N
\ The Weaker / Stronger _________________solution is = ______________ (____)
AMOUNT CALCULATION
= Equivalent mass x Normality x ___/1000
= ________x ________ x _____ / 1000
= gram
RESULT
1. Normality of ______________ (A) = N
2. Normality of ______________ (B) = N
3. The Weaker / Stronger ________________ solution is = __________ (___)
4. Amount of crystalline ___________________ present in _______ml of the weaker / stronger solution = gram
Ex. No.: 4 ESTIMATION OF OXALIC ACID
Date:
AIM
To estimate the amount of crystalline Oxalic acid present in 500 ml of the given solution. You are provided with 0.1 N Ferrous ammonium sulphate as standard solution and Potassium permanganate as the link solution.
PROCEDURE
TITRATION - I : STANDARDISATION OF KMnO4
The burette is filled with the given KMnO4 solution and titrated against 20ml of Ferrous ammonium sulphate solution pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titre value, the normality of KMnO4 is calculated.
TITRATION - I I : STANDARDISATION OF OXALIC ACID
The burette is filled with the given KMnO4 solution and titrated against 20ml of Oxalic acid solution pipetted out into a clean conical flask, mixed with equal volume of 2N dilute Sulphuric acid and heated to 700C. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the normality of Oxalic acid solution, the amount of Oxalic acid present in 500ml is calculated, knowing the equivalent mass of Oxalic acid is 63.
SIMPLE PROCEDURE
S.
No
|
CONTENTS
|
TITRATION - I
|
TITRATION - I I
|
1
|
Burette Solution
|
Potassium permanganate
|
Potassium permanganate
|
2
|
Pipette Solution
|
20 ml of Ferrous ammonium sulphate
|
20 ml of Oxalic acid
|
3
|
Acid Added
|
20 ml of 2N Sulphuric acid
|
20 ml of 2N Sulphuric acid
|
4
|
Temperature
|
Lab temperature
|
60 - 700 C
|
5
|
Indicator
|
Self-indicator (KMnO4)
|
Self-indicator (KMnO4)
|
6
|
Endpoint
|
Appearance of permanent pale pink colour
|
Appearance of permanent pale pink colour
|
7
|
Equivalent mass of Oxalic acid = 63
| ||
Normality of Standard Ferrous ammonium sulphate = 0.1 N
TITRATION - I : KMnO4 Vs STANDARD Ferrous ammonium sulphate
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Ferrous ammonium sulphate
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of Ferrous ammonium sulphate = V1 = 20 ml
Normality of Ferrous ammonium sulphate = N1 = 0.1 N
Volume of KMnO4 = V2 =
Normality of KMnO4 = N2 = ?
V1 X N1 = V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality of KMnO4 = N
TITRATION - I I : STANDARD KMnO4 Vs OXALIC ACID
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Oxalic acid
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of KMnO4 = V1 =
Normality of KMnO4 = N1 =
Volume of Oxalic acid = V2 = 20 ml
Normality of Oxalic acid = N2 = ?
V1 X N1 = V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality Of Oxalic Acid = N
AMOUNT CALCULATION
Amount of Oxalic acid present in 500ml of the solution =
Equivalent mass x Normality x 500/1000
= 63 x x 500 /1000
= gram.
RESULT
1. Normality of KMnO4 = N
2. Normality of Oxalic acid = N
3. Amount of crystalline Oxalic acid present in 500ml of the solution = gram
Ex. No.: 5 ESTIMATION OF FERROUS AMMONIUM SULPHATE
Date:
AIM
To estimate the amount of crystalline Ferrous ammonium sulphate present in 750 ml of the given solution. You are provided with 0.1025 N Oxalic acid as standard solution and Potassium permanganate as the link solution.
PROCEDURE
TITRATION - I : STANDARDISATION OF KMnO4
The burette is filled with the given KMnO4 solution and titrated against 20ml of Oxalic acid solution pipetted out into a clean conical flask, mixed with equal volume of 2N dilute Sulphuric acid and heated to 700C. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titre value, the normality of KMnO4 is calculated.
TITRATION - I I : STANDARDISATION OF Ferrous ammonium sulphate
The burette is filled with the given KMnO4 solution and titrated against 20ml of Ferrous ammonium sulphate solution pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titre value, the normality of Ferrous ammonium sulphate is calculated. From the normality of Oxalic acid solution, the amount of Oxalic acid present in 500ml is calculated, knowing the equivalent mass of Ferrous ammonium sulphate is 392.
SIMPLE PROCEDURE
S. No
|
CONTENTS
|
TITRATION - I
|
TITRATION - II
|
1
|
Burette Solution
|
Potassium permanganate
|
Potassium permanganate
|
2
|
Pipette Solution
|
20 ml of Oxalic acid
|
20 ml of Ferrous ammonium sulphate
|
3
|
Acid Added
|
20 ml of 2N Sulphuric Acid
|
20 ml of 2N Sulphuric acid
|
4
|
Temperature
|
60 - 700 C
|
Lab temperature
|
5
|
Indicator
|
Self-indicator (KMnO4)
|
Self-indicator (KMnO4)
|
6
|
Endpoint
|
Appearance of permanent pale pink colour
|
Appearance of permanent pale pink colour
|
7
|
Equivalent Mass of Ferrous ammonium sulphate = 392
| ||
Normality of Standard Oxalic acid = 0.1025 N
TITRATION - I : KMnO4 Vs Std. OXALIC ACID
INDICATOR: KMnO4(SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Oxalic acid
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of Oxalic acid = V1 = 20 ml
Normality of Oxalic acid = N1 = 0.1025 N
Volume of KMnO4 = N1 =
Normality of KMnO4 = N2 = ?
V1 X N1 = V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality of KMnO4 = N
TITRATION - I I: STANDARD KMnO4 Vs FERROUS ammonium sulphate
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Ferrous ammonium sulphate
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of KMnO4 = V1 =
Normality of KMnO4 = N1 =
Volume of Ferrous ammonium sulphate = V2 = 20 ml
Normality of Ferrous ammonium sulphate = N2 =?
V1 X N1 = V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality of Ferrous Ammonium Sulphate = N
Amount of crystalline Ferrous ammonium sulphate present in 750ml
= Equivalent mass x Normality x 750 / 1000
= Equivalent mass x Normality x 750 / 1000
= 392 x x 750 / 1000
= gram
= gram
RESULT
1. Normality of KMnO4 = N
2. Normality of Ferrous ammonium sulphate = N
3. Amount of crystalline Ferrous ammonium sulphate present in 750 ml of the solution
= gram
Ex. No.: 6 ESTIMATION OF FERROUS SULPHATE
Date:
AIM
To estimate the amount of crystalline Ferrous sulphate present in 250 ml of the given solution. You are provided with 0.0952 N Ferrous ammonium sulphate as standard solution and Potassium permanganate as the link solution.
PROCEDURE
TITRATION - I : STANDARDISATION OF KMnO4
The burette is filled with the given KMnO4 solution and titrated against 20ml of Ferrous ammonium sulphate solution pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titre value, the normality of KMnO4 is calculated.
TITRATION - II : STANDARDISATION OF FeSO4
The burette is filled with the given KMnO4 solution and titrated against 20ml of FeSO4solution pipetted out into a clean conical flask and mixed with equal volume of 2N dilute Sulphuric acid. The endpoint is the appearance of permanent pale pink colour. The final burette reading is noted, and the titration is repeated for concordant value. From the titre value, the normality of FeSO4 is calculated. From the normality of Ferrous Sulphate solution, the amount of FeSO4 present in 250ml it is calculated knowing the equivalent mass of Ferrous Sulphate is 278.
SIMPLE PROCEDURE
S. No
|
CONTENTS
|
TITRATION - I
|
TITRATION - II
|
1
|
Burette Solution
|
Potassium permanganate
|
Potassium permanganate
|
2
|
Pipette Solution
|
20 ml of Ferrous ammonium sulphate
|
20 ml of FeSO4
|
3
|
Acid Added
|
20 ml of 2N Sulphuric acid
|
20 ml of 2N Sulphuric acid
|
4
|
Temperature
|
Lab temperature
|
Lab temperature
|
5
|
Indicator
|
Self-indicator (KMnO4)
|
Self-indicator (KMnO4)
|
6
|
Endpoint
|
Appearance of permanent pale pink colour
|
Appearance of permanent pale pink colour
|
7
|
Equivalent mass of FeSO4 = 278
| ||
Normality of Standard Ferrous ammonium sulphate = 0.0952 N
TITRATION - I : KMnO4 Vs STANDARD Ferrous ammonium sulphate
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
Ferrous ammonium sulphate
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of Ferrous ammonium sulphate = V1 = 20 ml
Normality of Ferrous ammonium sulphate = N1 = 0.0952 N
Volume of KMnO4 = V2 =
Normality of KMnO4 = N2 =?
V1 X N1 = V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality of KMnO4 = N
TITRATION - II : STANDARD KMnO4 Vs FeSO4
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
FeSO4
ml
|
Initial
ml
|
Final
ml
|
KMnO4
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of KMnO4 = V1 =
Normality of KMnO4 = N1 =
Volume of FeSO4 = V2 = 20 ml
Normality of FeSO4 = N2 = ?
V1 X N1 = V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality of FeSO4 = N
Amount CALCULATION
Amount of crystallineFeSO4 present in 250ml = Equivalent mass x Normality x 250 / 1000
= 278 x x 250 / 1000
= gram.
RESULT
1. Normality of KMnO4 = N
2. Normality of FeSO4 = N
3. Amount of crystalline Ferrous sulphate present in 250ml of the solution = gram
Qn. No.: 4, 5 & 6.
ESTIMATION OF OXALIC ACID / FERROUS AMMONIUM SULPHATE / FERROUS SULPHATE
AIM
To estimate the amount of crystalline _____________________________________ present in ________ml of the given solution. You are provided with ____________N _________________ as standard solution and Potassium permanganate as the link solution.
SIMPLE PROCEDURE
S. No
|
CONTENTS
|
TITRATION - I
|
TITRATION - II
|
1
|
Burette Solution
|
Potassium permanganate
|
Potassium permanganate
|
2
|
Pipette Solution
|
20 ml of _______________
|
20 ml of ______________
|
3
|
Acid Added
|
20 ml of 2N Sulphuric acid
|
20 ml of 2N Sulphuric acid
|
4
|
Temperature
|
_______________________
|
_____________________
|
5
|
Indicator
|
Self-indicator (KMnO4)
|
Self-indicator (KMnO4)
|
6
|
Endpoint
|
Appearance of permanent pale pink colour
|
Appearance of permanent pale pink colour
|
7
|
Equivalent mass of _______________________________ = _________
(solution to be estimated)
| ||
NORMALITY OF STANDARD SOLUTION
Normality of Standard _________________ = ___________________N
TITRATION - I : KMnO4 Vs STANDARD _____________________________
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
_____________
ml
|
Initial
ml
|
Final
ml
|
KMnO4 ___
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of ____________________ = V1 = 20 ml
Normality of _______________________ = N1 = N
Volume of KMnO4 = V2 = ml
Normality of KMnO4 = N2 = ?
V1 X N1= V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality of KMnO4 = N
TITRATION - II : STANDARD KMnO4 Vs __________________________
INDICATOR: KMnO4 (SELF-INDICATOR)
Sl
|
Volume of
|
Burette Readings
|
Volume of
|
Concordant
| |
No
|
_____________
ml
|
Initial
ml
|
Final
ml
|
KMnO4 ___
ml
|
Titer Value
ml
|
1
|
20
|
0
| |||
2
|
20
|
0
| |||
CALCULATION
Volume of KMnO4 = V1 = ml
Normality of KMnO4 = N1 = N
Volume of _________________ = V2 = 20 ml
Normality of ________________ = N2 = ?
V1 X N1 = V2 X N2
Therefore, N2 = V1 X N1 / V2
=
Normality of ____________________ = N
Amount CALCULATION
_________ml of the given solution = Equivalent mass x Normality x ______ / 1000
= ________x_____x _______ / 1000
= gram.
RESULT
1. Normality of KMnO4 = N
2. Normality of ____________________ = N
3. Amount of crystalline __________ present in ____ml of the solution = gram
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