Question

Determine the concentration in terms of molarity of KMnO4 by titrating it against standard FAS solution

Write down this experiment by following points

1) Aim
2) Appratus
3)observation table
4) chemicals
5)calculation
6)observations
7)Result​

Answer 1

Answer:

The titration of potassium permanganate (KMnO4) against Mohr salt is an example of redox titration. In close proximity to the endpoint, the action of the indicator is analogous to the other types of visual colour titrations in oxidation-reduction (redox) titrations.

Explanation:

2KMnO4 + 3H2SO4 → K2SO4 + 2MnSO4 + 3H2O + 5[O]

Oxidation half reaction –

[2FeSO4(NH4)2SO4.6H2O + H2SO4 + [O] → Fe2(SO4)3 + 2(NH4)2SO4 + 13H2O] x 5

Overall reaction –

2KMnO4 + 10FeSO4(NH4)2SO4.6H2O+ 8H2SO4 → K2SO4+ 2MnSO4+ 5Fe2(SO4)3+ 10(NH4)2SO4+ 68H2O

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Answer 2

The experiment to perform titration to calculate the concentration of potassium permanganate against FAS solution.

Explanation

EXPERIMENT TO DETERMINE THE CONCENTRATION OF POTASSIUM PERMANGANATE -

AIM

To determine the concentration of potassium permanganate by titrating it against standard ferrous ammonium sulphate solution.  

MATERIAL REQUIRED  

Measuring flask, burette, burette stand, pipette, conical flask, funnel, weighing funnel, potassium permanganate solution, dilute sulphuric acid, ferrous ammonium sulphate.

OBSERVATION TABLE

The observation table is given below -

CHEMICAL REACTIONS

Reduction half-reaction

$2KMnO-4 + 3H_2SO_4$ → $K_2SO_4 + 2MnSO_4 + 3H_2O + 5[O]$

Oxidation half-reaction  

$[2FeSO_4(NH_4)_2SO_4.6H_2O] + H_2SO_4 + [O]$ →$Fe_2(SO_4)_3 + 2(NH_4)_2SO_4 + [13H_2O]5$

The overall reaction -  

$2KMnO_4 + 10FeSO_4(NH_4)_2SO_4.6H_2O + 8H_2SO_4$ → $K_2SO_4 + 2MnSO_4 + 5Fe_2(SO_4)_3 + 10(NH_4)_2SO_4 + 68H_2O$

Ionic reactions -

Oxidation         $[Fe^2^+$ →   $Fe^3^+ + e^-] 5$

Reduction        $MnO_4^- + 8H^+ + 5e^-$→ $Mn^2^+ + 4H_2O$

CALCULATION

The strength of unknown solution can be determined by -

              $a_1M_1V_1$  = $a_2M_2V_2$      ---------(1)

$M_1$ and $M_2$ are the molarity of $KMnO_4$ and AFS solution respectively and $V_1$ and $V_2$ are the volumes of the two solutions. a is the number of electrons gained or lost during a half-cell reaction.

               STRENGTH = MOLARITY × MOLAR MASS

The molar mass of potassium permanganate = 158

$a_1$= 5, $M_1$ = M, $V_1$= 7.2

$a_2$ = 1, $M_2$ = 1/20, $V_2$ = 10

In equation 1,         5M(7.2) = 1 × $\frac{1}{20}$ × 10

                               M = $\frac{1}{10}$ × $\frac{1}{7.2}$

Strength =  × 158 = 2.2

RESULT

The strength of potassium permanganate solution is 2.2 g/L.  

The molarity of the potassium permanganate solution is M/72.