Mercury nitrate monohydrate Chemical Properties

Melting point:

79 °C(lit.)

Density 

1.025 g/mL at 25 °C

vapor density 

11 (vs air)

storage temp. 

Store at RT.

solubility 

soluble in H2O, dilute acid solutions

form 

Liquid

Specific Gravity

4.39

color 

White to off-white

Odor

Slight nitric acid odor

Water Solubility 

Soluble in water.

Sensitive 

Hygroscopic

Merck 

14,5880

Exposure limits

ACGIH: TWA 0.025 mg/m3 (Skin)
NIOSH: IDLH 10 mg/m3; TWA 0.05 mg/m3; Ceiling 0.1 mg/m3

CAS DataBase Reference

7783-34-8(CAS DataBase Reference)

Safety Information

Hazard Codes 

T+,N,T,O,Xn

Risk Statements 

26/27/28-33-50/53-34-23/24/25-8-20/21/22-51/53-52/53

Safety Statements 

13-28-45-60-61-36/37/39-26-17-36/37

RIDADR 

UN 1625 6.1/PG 2

WGK Germany 

3

RTECS 

OW8225000

F 

3-8

TSCA 

Yes

HazardClass 

6.1

PackingGroup 

II

HS Code 

28521000

Toxicity

LD50 orally in Rabbit: 26 mg/kg LD50 dermal Rat 75 mg/kg

MSDS

• Language:English Provider:SigmaAldrich
• Language:English Provider:ACROS
• Language:English Provider:ALFA

Mercury nitrate monohydrate Usage And Synthesis

Chemical Properties

The monohydrate is a white crystalline or powdery substance; density 4.3g/cm3; decomposes on heating; soluble in water and nitric acid; insoluble in alcohol.
It is stable and hygroscopic. Mercuric nitrate is incompatible with mercuric nitrate in contact with organic materials, powdered metals, petroleum hydrocarbons, hypophosphoric acid, unsaturates, and aromatics, which react violently.

Uses

Mercury(II) nitrate is used in the preparation of other mercury compounds; in organic synthesis; and as an analytical standard for mercury.

Preparation

Mercury(II) nitrate is prepared by dissolving mercury in excess hot concentrated nitric acid. Upon evaporation of the solution, large colorless deliquescent crystals of monohydrate, Hg(NO3)2•H2O, form.
It also is obtained by boiling a solution of mercury(I) nitrate or by the action of light on mercury(I) nitrate:
Hg2(NO3)2 → Hg + 2HgNO3

Reactions

Gentle heating of mercury(II) nitrate gives mercury(II) oxide evolving nitrogen and oxygen:
Hg(NO3)2 → HgO + 2NO2 + ½ O2
However, on strong heating, mercury nitrate decomposes to mercury metal:
Hg(NO3)2 → Hg + 2NO2 + O2
When excess alkali hydroxide is added to a solution of mercury(II) nitrate, a yellow precipitate of HgO is obtained.
Addition of potassium thiocyanate solution forms a white precipitate of mercury(II) thiocyanate:
Hg2+ + 2SCN¯ → Hg(SCN)2
Addition of a small amount of alkali iodide to mercury(II) nitrate solution precipitates mercury(II) iodide:
Hg2+ + 2I¯ → HgI2
Similarly, mercury(II) cyanide precipitates upon the addition of potassium cyanide to mercury(II) nitrate solution:
Hg2+ + 2CN¯ → Hg(CN)2

Toxicity

Mercury(II) nitrate is highly toxic by ingestion and possibly other routes of exposure. The LD50 oral for the dihydrate in mouse is 25 mg/kg.

Chemical Properties

Mercuric nitrate is a white to yellowish crystalline solid with an odor like nitric acid. Normally exists as the hemihydrate or the dihydrate

Uses

Mercury(II) nitrate is used as an oxidizing agent involved in organic synthesis. Its reaction with acetone yielded an organometallic compound containing mercury. In addition, it serves as a nitrification agent and analytical reagents used in the laboratory. It is involved in the preparation of mercury fulminate.

Potential Exposure

Mercuric nitrate is used in making other chemicals; in felt manufacture and in making mercury fulminate

Shipping

UN1625 Mercuric nitrate, Hazard Class: 6.1; Labels: 6.1-Poisonous materials.

Purification Methods

Its solubility in H2O containing 1% HNO3 is 7.7%. Recrystallise it from a warm saturated solution of dilute HNO3 and cool to room temperature slowly to give elongated prisms. Rapid cooling gives plates. The colourless crystals should be stored in the dark. POISONOUS. [Grdenic J Chem Soc 1312 1956.]

Incompatibilities

A strong oxidizer. Reacts violently with combustibles, petroleum hydrocarbons; reducing agents; aldehydes, ammonia, ketones, phosphorus. Reacts with acetylene, alcohol, phosphine, and sulfur to form shocksensitive compounds. Aqueous solution attacks most metals. Vigorous and dangerous reaction with petroleum hydrocarbons. Incompatible with organic materials; acetylene, ethanol, phosphine, sulfur, hypophosphoric acid. Inorganic mercury compounds are incompatible with acetylene, ammonia, chlorine dioxide; azides, calcium (amalgam formation), sodium carbide; lithium, rubidium, copper. Decomposes in heat or on exposure to light, producing toxic fumes (mercury, nitrogen oxides)

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