Difference between revisions of "Mercury(II) sulfate"
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| pKb = | | pKb = | ||
| Solubility = Decomposes to [[sulfuric acid]] and HgSO<sub>4</sub>·2HgO | | Solubility = Decomposes to [[sulfuric acid]] and HgSO<sub>4</sub>·2HgO | ||
| − | | SolubleOther = Soluble in | + | | SolubleOther = Soluble in conc. [[hydrochloric acid]], [[nitric acid]], [[sulfuric acid]], [[Sodium chloride|NaCl]] solution<br>Insoluble in [[acetone]], [[ammonia]], [[ethanol]], halocarbons, hydrocarbons |
| Solvent = | | Solvent = | ||
| VaporPressure = | | VaporPressure = | ||
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}} | }} | ||
}} | }} | ||
| − | '''Mercury(II) sulfate''' or '''mercuric sulfate''', is the chemical compound '''HgSO<sub>4</sub>''', used in various chemical reactions. | + | '''Mercury(II) sulfate''' or '''mercuric sulfate''', is the chemical compound '''HgSO<sub>4</sub>''', a toxic and corrosive compound of mercury, used in various chemical reactions, though mostly used in analytical chemistry. |
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
Mercury(II) sulfate readily hydrolyzes in water, separating into the yellow mercuric subsulfate and [[sulfuric acid]]: | Mercury(II) sulfate readily hydrolyzes in water, separating into the yellow mercuric subsulfate and [[sulfuric acid]]: | ||
| + | |||
:3 HgSO<sub>4</sub> + 2 H<sub>2</sub>O → HgSO<sub>4</sub>·2HgO + 2 H<sub>2</sub>SO<sub>4</sub> | :3 HgSO<sub>4</sub> + 2 H<sub>2</sub>O → HgSO<sub>4</sub>·2HgO + 2 H<sub>2</sub>SO<sub>4</sub> | ||
| + | |||
| + | Heating mercury(II) sulfate above 450 °C will cause it to decompose, releasing hazardous mercury vapors: | ||
| + | |||
| + | : HgSO<sub>4</sub> → Hg + SO<sub>2</sub> + O<sub>2</sub> | ||
===Physical=== | ===Physical=== | ||
| − | Mercury(II) sulfate is a dense white solid, soluble in sulfuric acid, but insoluble in organic solvents. It decomposes when heated to 450 °C. Its density at standard conditions is 6.47 g/cm<sup>3</sup>. | + | Mercury(II) sulfate is a dense white solid, soluble in concentrated mineral acids, such as nitric acid, sulfuric acid, but insoluble in organic solvents. It hydrolyzes in contact with water, forming yellow mercuric subsulfate and sulfuric acid. Mercury sulfate decomposes when heated to 450 °C. Its density at standard conditions is 6.47 g/cm<sup>3</sup>. |
==Availability== | ==Availability== | ||
| − | Mercury(II) sulfate is sold by chemical suppliers. Due to its hazards, | + | Mercury(II) sulfate is sold by chemical suppliers. Due to its hazards, this compound is extremely difficult to acquire by the amateur chemist. In the EU, purchasing mercury compounds requires a hazard permit. |
==Preparation== | ==Preparation== | ||
Mercury(II) sulfate can be prepared by reacting hot concentrated [[sulfuric acid]] with elemental [[mercury]]: | Mercury(II) sulfate can be prepared by reacting hot concentrated [[sulfuric acid]] with elemental [[mercury]]: | ||
| + | |||
:Hg + 2 H<sub>2</sub>SO<sub>4</sub> → HgSO<sub>4</sub> + SO<sub>2</sub> + 2 H<sub>2</sub>O | :Hg + 2 H<sub>2</sub>SO<sub>4</sub> → HgSO<sub>4</sub> + SO<sub>2</sub> + 2 H<sub>2</sub>O | ||
It can also be made by reacting mercuric oxide with concentrated [[sulfuric acid]]. | It can also be made by reacting mercuric oxide with concentrated [[sulfuric acid]]. | ||
| + | |||
:HgO + H<sub>2</sub>SO<sub>4</sub> → HgSO<sub>4</sub> + H<sub>2</sub>O | :HgO + H<sub>2</sub>SO<sub>4</sub> → HgSO<sub>4</sub> + H<sub>2</sub>O | ||
| + | |||
| + | Concentrated acid needs to be used, to prevent hydrolysis. | ||
==Projects== | ==Projects== | ||
| Line 132: | Line 141: | ||
*Acetaldehyde synthesis from acetylene and water | *Acetaldehyde synthesis from acetylene and water | ||
*[[Phthalic anhydride]] synthesis | *[[Phthalic anhydride]] synthesis | ||
| + | *Removal of chloride ions in COD analysis | ||
==Handling== | ==Handling== | ||
===Safety=== | ===Safety=== | ||
| − | HgSO<sub>4</sub> is extremely toxic and its ingestion may be fatal. Reaction with water releases sulfuric acid, which is corrosive. The salt itself or as a solution is corrosive to many metals, such as [[aluminium]], [[copper]], [[iron]] (most steels), [[lead]], [[magnesium]], [[zinc]], etc. | + | HgSO<sub>4</sub> is extremely toxic and its ingestion may be fatal. Exposure to mercury compounds will cause severe neurological damage. Reaction with water releases sulfuric acid, which is corrosive. The salt itself or as a solution is corrosive to many metals, such as [[aluminium]], [[copper]], [[iron]] (most steels), [[lead]], [[magnesium]], [[zinc]], etc. |
===Storage=== | ===Storage=== | ||
Revision as of 16:07, 21 March 2018
_sulfate_bottle_sample.jpg) Mercury(II) sulfate sample and original bottle.
| |
| Names | |
|---|---|
| IUPAC name
Mercury(II) sulfate
| |
| Other names
Mercuric sulfate
Mercury persulfate Mercury bisulfate | |
| Properties | |
| HgSO4 | |
| Molar mass | 296.653 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 6.47 g/cm3 |
| Melting point | 450 °C (842 °F; 723 K) (decomposes) |
| Boiling point | Sublimes; decomposes |
| Decomposes to sulfuric acid and HgSO4·2HgO | |
| Solubility | Soluble in conc. hydrochloric acid, nitric acid, sulfuric acid, NaCl solution Insoluble in acetone, ammonia, ethanol, halocarbons, hydrocarbons |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
−707.5 kJ/mol |
| Hazards | |
| Safety data sheet | Fischer Scientific |
| Flash point | Non-flammable |
| Related compounds | |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Mercury(II) sulfate or mercuric sulfate, is the chemical compound HgSO4, a toxic and corrosive compound of mercury, used in various chemical reactions, though mostly used in analytical chemistry.
Contents
Properties
Chemical
Mercury(II) sulfate readily hydrolyzes in water, separating into the yellow mercuric subsulfate and sulfuric acid:
- 3 HgSO4 + 2 H2O → HgSO4·2HgO + 2 H2SO4
Heating mercury(II) sulfate above 450 °C will cause it to decompose, releasing hazardous mercury vapors:
- HgSO4 → Hg + SO2 + O2
Physical
Mercury(II) sulfate is a dense white solid, soluble in concentrated mineral acids, such as nitric acid, sulfuric acid, but insoluble in organic solvents. It hydrolyzes in contact with water, forming yellow mercuric subsulfate and sulfuric acid. Mercury sulfate decomposes when heated to 450 °C. Its density at standard conditions is 6.47 g/cm3.
Availability
Mercury(II) sulfate is sold by chemical suppliers. Due to its hazards, this compound is extremely difficult to acquire by the amateur chemist. In the EU, purchasing mercury compounds requires a hazard permit.
Preparation
Mercury(II) sulfate can be prepared by reacting hot concentrated sulfuric acid with elemental mercury:
- Hg + 2 H2SO4 → HgSO4 + SO2 + 2 H2O
It can also be made by reacting mercuric oxide with concentrated sulfuric acid.
- HgO + H2SO4 → HgSO4 + H2O
Concentrated acid needs to be used, to prevent hydrolysis.
Projects
- Detect tertiary alcohols
- Acetaldehyde synthesis from acetylene and water
- Phthalic anhydride synthesis
- Removal of chloride ions in COD analysis
Handling
Safety
HgSO4 is extremely toxic and its ingestion may be fatal. Exposure to mercury compounds will cause severe neurological damage. Reaction with water releases sulfuric acid, which is corrosive. The salt itself or as a solution is corrosive to many metals, such as aluminium, copper, iron (most steels), lead, magnesium, zinc, etc.
Storage
Mercury(II) sulfate should be stored in closed bottles, away from moisture, in a special cabinet.
Disposal
Best to take it to hazardous waste disposal centers.
