Equivalent weight of ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ as oxidant in acidic medium is

Equivalent Weight of K₂Cr₂O₇ as an Oxidant in Acidic Medium

Steps:

1. Reaction in acidic medium:

   Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O

   In this reaction, Cr₂O₇²⁻ is reduced to Cr³⁺, involving 6 electrons per mole of Cr₂O₇²⁻.

2. Molar mass of K₂Cr₂O₇:

   • 2K = 2 × 39.1
   • 2Cr = 2 × 51.996
   • 7O = 7 × 16

   Total molar mass = 294.2 g/mol.

3. Equivalent weight formula:

   Equivalent weight = Molar mass / Number of electrons (n)

   Substituting the values:

   Equivalent weight = 294.2 / 6 = 49.03 g/equiv.

Final Answer:

The equivalent weight of K₂Cr₂O₇ as an oxidant in acidic medium is 49.03 g/equiv.