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| 1. |
An unknown oxidising agent contains the element Y in + 5 state. If it takes 26.98 ml of 0.1326 N Na_2SO_3 to reduce 7.16x10^(-1) mole of YO(OH)_2, to a lower state, the final oxidation state of Y is- |
| Answer» Solution :(C) 26.98 mL. of 0.1326 N solution of `Na_2SO_3`, contains (26.98) (0.1326) miliequivalents of `Na_2SO_3`, By DEFINITION eq. wt. of `Na_2SO_3`, is that weight which would cause a one electron reduction of a oxidising agent USED is 7.16 `xx 10^(-1)` millimoles then the no. of electrons involved in the redox reaction is `(26.98 x 0.1326/7.16 x0.1)= 5` electrons`Y^(5+) +5e^(-) rarr Y^(0)` and the final oxidation state of Y is zero. | |