Identify the products formed when chlorine reacts with cold and dilute sodium hydroxide solution.
- A$NaCl, NaClO_3, H_2O$
- B$NaCl, NaClO_4, H_2O$
- C$NaCl, NaOCl, H_2O$
- D$NaCl, HCl, H_2O$
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$(a)$ Number of $S-S$ bonds in $H_2S_nO_6$ is $(n-1)$.
$(b)$ When $F_2$ reacts with $H_2O$,it forms $HF$,$O_2$,and $O_3$.
$(c)$ $XeF_6$ on hydrolysis shows a disproportionation reaction.
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$(b)$ When $F_2$ reacts with $H_2O$,it forms $HF$,$O_2$,and $O_3$.
$(c)$ $XeF_6$ on hydrolysis shows a disproportionation reaction.
$(d)$ $Al$ metal on reacting with dilute $NaOH$ gives a white precipitate of $Al(OH)_3$ as a final product.
Why does fluorine not show disproportionation reaction?
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