The reaction
$C{l}_2+S_2{O_3}^{2-}+{OH}^{-}⟶{{SO}_4}^{2-}+{Cl}^{-}+H_{2}O$
Starting with $0.15$ mole $C{l}_2,0.010$ mole$S_2{O_3}^{2-}$and $0.30$ mole ${OH}^{-}$, mole of $C{l}_2$ left in solution will be

Q. The reaction : $C{l}_2\left(g\right)+S_2{O}_3^{2-}⟶S{O}_4^{2-}+C{l}^{-}$ is to be carried out in basic medium. Starting with $0.15$ moles of $C{l}_2$, $0.010$ moles of $S_2{O}_3^{2-}$ and $0.30$ moles of $O{H}^{-}$, how many moles of $O{H}^{-}$ will be left in solution after the reaction is complete? Assume no other reaction occurs.

Q. Which of the following species is reduced in the following (unbalanced) reaction?
$S_2{O}_3^{2-}+{Cl}_2⟶H{SO}_4^{-}+{Cl}^{-}$

Q. In a basic buffer, $0.0025$ mole of $N{H}_{4}Cl$ and $0.15mole$ of $N{H}_{4}OH$ are present. The $pH$ of the solution will be:

Q. The density of $3M$ solution of sodium thiosulphate (${Na}_2{S}_2{O}_3)$ is $1.56g/mL$. Calculate
(i) amount of ${Na}_2{S}_2{O}_3$ in % w/w
(ii) mole fraction of ${Na}_2{S}_2{O}_3$
(iii) Molality of ${Na}^{+}$ and $S_2{O}_3^{2-}$ ions

Q. In the reaction : $C{l}_2+O{H}^{-}\to C{l}^{-}+Cl{O}_4^{-}+H_{2}O$ ?