A solution contains 0.0100 mol of H3PO2 and 0.0100 mol of H3PO3. Both are completely oxidised to H3PO4 by excess AgNO3 solution, which is reduced to silver metal. The mass of silver formed (Ag = 108) is

JEE Advanced levelSingle correct optionDifficulty 3 of 3pn051

A solution contains $0.0100$ mol of $H X_{3} PO X_{2}$ and $0.0100$ mol of $H X_{3} PO X_{3}$ . Both are completely oxidised to $H X_{3} PO X_{4}$ by excess $AgNO X_{3}$ solution, which is reduced to silver metal. The mass of silver formed (Ag = 108) is

P changes from +1 to +5 in

H X_{3} PO X_{2}

(4 e

^{-}

) and from +3 to +5 in

H X_{3} PO X_{3}

(2 e

^{-}

). Each

Ag X^{+}

takes one electron.

Ag X^{+}

reduced =

0.0100 \times 4 + 0.0100 \times 2 = 0.0600

mol. Mass =

0.0600 \times 108 = 6.48 g