The reaction, $P_4+3NaOH+3H_{2}O⟶3Na{H}_{2}P{O}_2+P{H}_{3}P\_4+3NaOH+3H\_2O\backslash longrightarrow3NaH\_2PO\_2+PH\_3$ is an example of :

What volume of 0.40 M $N{a}_2{S}_2{O}_{3}Na\_2S\_2O\_3$ would be required to react with the $I_{2}I\_2$ liberated by adding excess of KI to 50mL of 0.20 M $CuS{O}_{4}CuSO\_4$ solution?

What is the normality of $KMn{O}_{4}KMnO\_4$ solution to be used as an oxidant in acidic medium, which 4 contains 15.8 g of the compound in 100 mL of solution?

What volume of 1N $K_{2}C{r}_2{O}_{7}K\_2Cr\_2O\_7$ solution is required to oxidise (in acidic solution) a solution containing 10 g of $FeS{O}_{4}FeSO\_4$? (mol. wt. of $FeS{O}_4=152FeSO\_4=152$)

A solution of $KMn{O}_{4}KMnO\_4$ is reduced to $Mn{O}_{2}MnO\_2$. The normality of solution is 0.6. The molarity is

Number of $K^{+}K^+$ ions and moles of $K^{+}K^+$ ions present in 1 litre of $\frac{N}{5}\backslash frac\; N5$ $KMn{O}_{4}KMnO\_4$ acidified solution respectively are

A solution containing $2.68\times 10^{-3}2.68\; \backslash times\; 10^\{-3\}$ mol of $A^{n+}A^\{n+\}$ ions requires $1.61\times 10^{-3}1.61\; \backslash times\; 10^\{-3\}$ mol of $Mn{O}_4^{-}MnO\_4^-$ for the oxidation of $A^{n+}A^\{n+\}$ to $A{O}_3^{-}AO\_3^-$ in acidic medium. The value of n is

Number of moles of $K_{2}C{r}_2{O}_{7}K\_2Cr\_2O\_7$ reduced by one mole of $S{n}^{2+}Sn^\{2+\}$ions in acidic medium is

The equivalent weight of used as an oxidizing agent in acidic medium is (atomic weight of Ba = 137.34 and Cr = 52)

The equivalent mass of $KI{O}_{3}KIO\_3$ in the reaction given is $Cr(OH{)}_3+4O{H}^{-}+KI{O}_3⟶2Cr{O}_4^{2-}+KI+5H_{2}OCr(OH)\_3+4OH^-+\; KIO\_3\; \backslash longrightarrow\; 2CrO^\{2-\}\_4+\; KI\; +\; 5H\_2O$, (M = molecular mass of $KI{O}_{3}KIO\_3$)