In the reaction of sodium thiosulphate with I | vedclass

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Question

(A) The balanced chemical equation is: $2 Na_2S_2O_3 + I_2 \longrightarrow Na_2S_4O_6 + 2 NaI$. In this reaction, the oxidation state of sulfur in $Na

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molar mass of sodium thiosulphate

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(A) The balanced chemical equation is: $2 Na_2S_2O_3 + I_2 \longrightarrow Na_2S_4O_6 + 2 NaI$. In this reaction, the oxidation state of sulfur in $Na_2S_2O_3$ changes from $+2$ to $+2.5$ in $Na_2S_4O_6$. The change in oxidation state per sulfur atom is $0.5$. Since there are $2$ sulfur atoms in $Na_2S_2O_3$, the total change in oxidation state (n-factor) is $2 	imes 0.5 = 1$. The equivalent weight $E$ is given by the formula $E = \frac{M}{n	ext{-factor}}$, where $M$ is the molar mass. Thus, $E = \frac{M}{1} = M$. Therefore, the equivalent weight is equal to the molar mass of sodium thiosulphate.

In the reaction of sodium thiosulphate with $I_2$ in aqueous medium, the equivalent weight of sodium thiosulphate is equal to:

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