An aqueous solution containing 0.10 g KIO3 (formula weight =214) was treated with excess of KI solution. The solution was acidified with HCl. The liberated I2 consumed 45.0 mL of thiosulphate solution to decolourise the blue strach-iodine complex. Calculate the molarity of the sodium thiosulphate solution. (Report your answer upto two decimal only)

An aqueous solution containing 0.10 g KIO3 (formula weight =214) was t

1.	An aqueous solution containing 0.10 g KIO3 (formula weight =214) was treated with excess of KI solution. The solution was acidified with HCl. The liberated I2 consumed 45.0 mL of thiosulphate solution to decolourise the blue strach-iodine complex. Calculate the molarity of the sodium thiosulphate solution. (Report your answer upto two decimal only)
Answer» An aqueous solution containing $0.10 g K I O_{3}$ (formula weight $= 214$ ) was treated with excess of $K I$ solution. The solution was acidified with $H C l$ . The liberated $I_{2}$ consumed $45.0 mL$ of thiosulphate solution to decolourise the blue strach-iodine complex. Calculate the molarity of the sodium thiosulphate solution. (Report your answer upto two decimal only)