An aqueous solution containing 0.10 g KIO3 (formula weight=214.0) was treated with an excess of KI solution the solution was acidified with HCl. The liberated I2 consumed 45.0 " mL of " thiosulphate solution to decolourise the blue starch-iodine complex. Calculate the molarity of the sodium thosulphate solution.

Question

An aqueous solution containing 0.10 g KIO3​ (formula weight=214.0) was treated with an excess of KI solution the solution was acidified with HCl. The liberated I2​ consumed 45.0 " mL of " thiosulphate solution to decolourise the blue starch-iodine complex. Calculate the molarity of the sodium thosulphate solution.

Filo · Accepted Answer

Answer: (0.062M)Solution: The redox reaction involved are:  IO3−​+5I−+6H+→3I2​+3H2​O  I2​+2S2​O32−​→2I−+S4​O62−​  millimol of KiO3​ used =2140.1​×1000=0.467  ⇒ millimol of I2​ formed =3×0.467=1.4  ⇒ millimol of Na2​S2​O3​ consumed =2×1.4=2.8  ⇒ millimol of Na2​S2​O3​=452.8​=0.062M

Question Text	An aqueous solution containing 0.10 g $K I O_{3}$ (formula weight $= 214.0$ ) was treated with an excess of KI solution the solution was acidified with HCl. The liberated $I_{2}$ consumed 45.0 " mL of " thiosulphate solution to decolourise the blue starch-iodine complex. Calculate the molarity of the sodium thosulphate solution.
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