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It can be seen from the elemental potential diagram of mercury that Hg 2+ and Hg 2 2+ are medium-strength oxidants, and Hg 2 2+ will not undergo disproportionation reaction under standard conditions
.
A strong reducing agent can be used to reduce the two, controlling the amount of reducing agent can reduce Hg 2+ to Hg 2 2+ ; adding an oxidizing agent can oxidize Hg 2 2+ to Hg 2+ ; use reverse disproportionation in acidic medium The reaction converts Hg 2+ to Hg 2 2+
.
1.
Convert Hg(I) to Hg(Ⅱ)
Under the standard state, Hg 2+ does not undergo disproportionation reaction, but the standard electrode potential difference between Hg 2 2+ as an oxidant and as a reducing agent is very small
.
Therefore, reducing the concentration of Hg 2+ can shift the balance in favor of the disproportionation reaction.
A strong oxidant is added to the Hg 2 2+ solution to convert it into Hg 2+
.
2.
Conversion of Hg(Ⅱ) to Hg(I)
Using the reverse disproportionation reaction, Hg 2+ can be converted to Hg 2 2+
.
Use a strong reducing agent to reduce Hg 2+ to Hg 2 2+
