Skip to main content
Chemistry LibreTexts

Characteristic Reactions of Mercury Ions (Hg²⁺ and Hg₂²⁺)

  • Page ID
    97274
    • Most common oxidation states: +1, +2
    • M.P. -38.87º
    • B.P. 356.57º
    • Density 13.546 g/cm3
    • Characteristics: Mercury is one of the few liquid elements. It dissolves in oxidizing acids, producing either \(\ce{Hg^{2+}}\) or \(\ce{Hg_2^{2+}}\), depending on which reagent is in excess. The metal is also soluble in aqua regia ( a mixture of hydrochloric and nitric acids) to form \(\ce{HgCl4^{2-}}\).

    Mercury(I) Ion: Hg₂²⁺

    Mercury(I) compounds often undergo disproportionation, producing black metallic mercury and mercury(II) compounds.

    Chloride Ion

    Soluble chlorides, including hydrochloric acid, precipitate white mercury(I) chloride, also known as calomel:

    \[\ce{Hg_2^{2+}(aq) + 2Cl^{-}(aq) <=> Hg2Cl2(s)}\]

    Hg11a.gif

    Aqueous ammonia reacts with \(\ce{Hg2Cl2}\) to produce metallic mercury (black) and mercury(II) amidochloride (white), a disproportionation reaction:

    \[\ce{Hg2Cl2(s) + 2NH3(aq) -> Hg(l) + HgNH2Cl(s) + NH4^{+}(aq) + Cl^{-}(aq)}\]

    Hg11b.gif

    Aqueous Ammonia

    Aqueous ammonia produces a mixture of a white basic amido salt and metallic mercury:

    \[\ce{2Hg_2^{2+}(aq) + 4NH3(aq) + NO3^{-}(aq) + H2O(l) -> 2Hg(l) + Hg2ONH2NO3(s) + 3NH4^{+}(aq)}\]

    Hg13ppt.gif

    The precipitate is not soluble in excess aqueous ammonia.

    Sodium Hydroxide

    Black finely divided mercury metal and yellow mercury(II) oxide (\(\ce{HgO}\)) are precipitated by \(\ce{NaOH}\):

    \[\ce{Hg_2^{2+}(aq) + 2OH^{-}(aq) -> Hg(l) + HgO(aq) + H2O(l)}\]

    Hg14ppt.gif

    Reducing Agents

    Reducing agents, such as \(\ce{Sn^{2+}}\) and \(\ce{Fe^{2+}}\), reduce mercury(I) to the metal:

    \[\ce{Hg_2^{2+}(aq) + 2Fe^{2+}(aq) -> 2Hg(l) + 2Fe^{3+}(aq) }\]

    Hg15ppt.gif

    Consult an activity series or a table of reduction potentials for other possible reducing agents.

    No Reaction

    \(\ce{SO4^{2-}}\) (unless solutions are concentrated; solubility of mercury(I) sulfate is 0.06 g per 100 mL of water at 25oC)

    Mercury(II) Ion: Hg²⁺

    Characteristic reactions of \(\ce{Hg^{2+}}\)

    Chloride Ion

    No reaction is visible, but Hg(II) will be present as \(\ce{[HgCl4]^{2-}}\).

    Aqueous Ammonia

    Aqueous ammonia produces white amido salts whose composition depends on the mercury(II) salt present in the solution:

    \[\ce{HgCl2(aq) + 2NH3(aq) <=> HgNH2Cl(s) + 2NH4^{+}(aq) + Cl^{-}(aq)}\]

    Sr5b1.gif

    These salts are not soluble in excess aqueous ammonia, but do dissolve in acids:

    \[\ce{HgNH2Cl(s) + 2H^{+}(aq) + Cl^{-}(aq) <=> HgCl2(aq) + NH4^{+}(aq) }\]

    Hg23bppt.gif

    Sodium Hydroxide

    A yellow precipitate of \(\ce{HgO}\) is produced by \(\ce{NaOH}\):

    \[\ce{Hg^{2+}(aq) + 2OH^{-}(aq) -> HgO(s) + H2O(l)}\]

    \[\ce{HgCl2(s) + 2OH^{-}(aq) -> HgO(s) + H2O(l) + 2Cl^{-}(aq)}\]

    Hg24a.gif

    The mercury(II) oxide precipitate is insoluble in excess hydroxide but is soluble in acids:

    \[\ce{HgO(s) + 2H^{+}(aq) <=> Hg^{2+}(aq) + H2O(l)}\]

    Water.gif

    Hydrogen Sulfide

    Hydrogen sulfide precipitates black mercury(II) sulfide, the least soluble of all sulfide salts.

    \[\ce{Hg^{2+}(aq) + H2S(aq) <=> HgS(s) + 2H^{+}(aq)}\]

    \[\ce{[HgCl4]^{2-}(aq) + H2S(aq) <=> HgS(s) + 2H^{+}(aq) + 4Cl^{-}(aq)}\]

    Hg25a1.gif

    Mercury(II) sulfide is insoluble in 6 M \(\ce{HNO3}\) or 12 M \(\ce{HCl}\), even if heated. However, it is soluble in aqua regia (3:1 HCl:HNO3) and in hot dilute \(\ce{NaOH}\) containing excess sulfide.

    \[\ce{3HgS(s) + 12Cl^{-}(aq) + 2NO3^{-}(aq) + 8H^{+}(aq) -> 3[HgCl4]^{2-}(aq) + 2NO(g) + 3S(s) + 4H2O(l)}\]

    \[\ce{HgS(s) + S2^{-}(aq) <=> [HgS2]^{2-}(aq)}\]

    Tin(II) Chloride

    Tin(II) chloride reduces \(\ce{Hg(II)}\) to \(\ce{Hg(I)}\) or to metallic \(\ce{Hg}\), giving a white or gray precipitate:

    \[\ce{2[HgCl4]^{2-}(aq) + [SnCl4]^{2-}(aq) <=> Hg2Cl2(s) + [SnCl6]^{2-}(aq) + 4Cl^{-}(aq)}\]

    Hg25a2.gif

    No Reaction

    \(\ce{SO4^{2-}}\) (may precipitate as a mixed sulfate-oxide - a basic sulfate - \(\ce{HgSO4 \cdot 2HgO}\))