Assign $A, B, C, D$ from the given type of reaction.
$Pb(NO_3)_2 + 2NaOH \longrightarrow Pb(OH)_2 \downarrow + 2NaNO_3$

Thiosulphate reacts differently with iodine and bromine in the reactions given below:
$2 S_2 O_3^{2-} + I_2 \rightarrow S_4 O_6^{2-} + 2 I^{-}$
$S_2 O_3^{2-} + 4 Br_2 + 5 H_2 O \rightarrow 2 SO_4^{2-} + 8 Br^{-} + 10 H^{+}$
Which of the following statements justifies the above dual behaviour of thiosulphate?

Assign $A, B, C, D$ from the given type of reaction.
$CrCl_3$ $(aq)$ + $ZnSO_4$ $(aq)$ $\longrightarrow$ No reaction

What is the equivalent weight of the oxidizing agent in the following reaction?
$SO_2 + 2H_2S \to 3S + 2H_2O$

In which of the following reactions is there no change in the valency (oxidation state) of the elements?

Assign $A, B, C, D$ from the given type of reaction.
$PbCrO_4 \downarrow + 4NaOH \,(Excess) \longrightarrow Na_2[Pb(OH)_4] + Na_2CrO_4$