Redox Reactions

Thiosulphate reacts differently with iodine and bromine in the reactions given below: $$\begin{aligned} & 2 \mathrm{~S}_2 \mathrm{O}_3^{2-}+\mathrm{I}_2 \rightarrow \mathrm{S}_4 \mathrm{O}_6^{2-}+2 \mathrm{I}^{-} \\ & \mathrm{S}_2 \mathrm{O}_3^{2-}+5 \mathrm{Br}_2+5 \mathrm{H}_2 \mathrm{O} \rightarrow 2 \mathrm{SO}_4^{2-}+4 \mathrm{Br}^{-}+10 \mathrm{H}^{+} \end{aligned}$$ Which of the following statement justifies the above dual behaviour of thiosulphate?

The number of ions from the following that are expected to behave as oxidising agent is : $$\mathrm{Sn}^{4+}, \mathrm{Sn}^{2+}, \mathrm{Pb}^{2+}, \mathrm{Tl}^{3+}, \mathrm{Pb}^{4+}, \mathrm{Tl}^{+}$$

The correct order of the oxidation states of nitrogen in NO, N₂O, NO₂ and N₂O₃ is :

Oxidation number of potassium in K₂O. K₂O₂ and KO₂ respectively is :

The compound that cannot act both as oxidising and reducing agent is :

The oxidation states of nitrogen in NO, NO₂, N₂O and NO$$_3^ -$$ are in the order of :

Identify the process in which change in the oxidation state is five :

The oxidation states of 'P' in H₄P₂O₇, H₄P₂O₅ and H₄P₂O₆, respectively, are :

50 mL of 0.5 M oxalic acid is needed to neutralize 25 mL of sodium hydroxide solution. The amount of NaOH in 50 mL of the given sodium hydroxide solution is -

While titrating dilute HCl solution with aqueous NaOH, which of the following will not be required?