Find the depression in freezing point of solution when 3.2 gram non volatile solute with molar mass $$128 \mathrm{~gram} \mathrm{~mol}^{-1}$$ is dissolved in $$80 \mathrm{~gram}$$ solvent if cryoscopic constant of solvent is $$4.8 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$$.

What is the value of $$x$$ in order to balance following redox reaction?

$$\mathrm{Mn}_{(\mathrm{aq})}^{2+}+x \mathrm{ClO}_{3(\mathrm{aq})}^{-} \rightarrow \mathrm{MnO}_{2(\mathrm{~s})}+x \mathrm{ClO}_{2(\mathrm{aq})}$$

The reaction, $$3 \mathrm{ClO}^{-} \rightarrow \mathrm{ClO}_3^{-}+2 \mathrm{Cl}^{-}$$ occurs in two steps:

i. $$\quad 2 \mathrm{ClO}^{-} \rightarrow \mathrm{ClO}_2^{-}+\mathrm{Cl}^{-}$$

ii. $$\quad \mathrm{ClO}_2^{-}+\mathrm{ClO}^{-} \rightarrow \mathrm{ClO}_3^{-}+\mathrm{Cl}^{-}$$,

the reaction intermediate is:

Acetic acid dissociated to $$1.20 \%$$ in its $$0.01 \mathrm{~M}$$ solution. What is the value of its dissociation constant?