Question

C.B.R.
Observation Table:
Burette reading in mL
1
Il
Burette level
Pilot reading
3
OB
Final
9.6
0.0
0.0
Initial
Difference
ml
Calculation: From above chemical equation
2KMnO, + SH.CO. +3H SO, K SO, + 2MnSO, +8H,0 + 10CO,
2 moles S moles
2 * 158 g (316 g) = 1000 mL 5 M (molar mass of KMnO, = 158 g/mol)
2. 1000 ml 5 M oxalic acid = 316 g of KMnO,
316 x 10 x 0.1
.. 10 mL 0.1 M oxalic acid
1000 X 5
= 0.0632 g of KMnO,
Hence 2:3(x) C.B.R.ml of KMnO solution contains = 0.0632 g of KMnO,
1000 mL of KMnO contains
0.0632 x 1000
.(x) CBR
0.0632 x 1000
Hence molarity of KMnO, in the solution is
ya...(x) CBR * 158
Space for log calculation
Number
log
0.4
(x) CBR
...M​

Answer 1

Answer:

Normality of sodium thiosulfate = 0.026N

Explanation:

Step 1: The iodometric titration method is used to get the precise result for the normalcy of sodium thiosulphate solution. In this procedure, an excess potassium iodide solution is reacted with a standard potassium dichromate solution, and the freed iodine is then titrated against a sodium thiosulfate solution.

Step 2: The manufacturing of potassium chrome alum and the tanning of leather are the two principal uses of potassium dichromate. In order to make chromic acid, which is used to clean glassware and as an etchant for glass products, potassium dichromate can be utilised as a raw material.

Step 3: Normality of potassium dichromate solution $\left(\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7\right)=0.025 \mathrm{~N}$

Volume of potassium dichromate taken $=10 \mathrm{ml}$

Volume of sodium thiosulfate $\left(\mathrm{Na}_2 \mathrm{~S}_2 \mathrm{O}_3\right)$ used $=9.5 \mathrm{ml}$

Using normality equation:

N1V1 = N2V2

N2  = N1V1/ V2  

where N1  = normality of potassium dichromate

N2 = normality of thiosulfate solution

V2 = volume of thiosulfate solution

N2 = ( 0.025 N × 10ml) /9.5 ml = 0.026N

Normality of sodium thiosulfate = 0.026N

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