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 concentrated or hot H<sub>2</sub>SO<sub>4</sub>, [[hydrochloric acid]], NaCl solution<br>Insoluble in [[acetone]], [[ammonia]], [[ethanol]]
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| 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, it's extremely difficult to acquire by the amateur chemist.
+
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==
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*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

Mercury(II)sulfate
Mercury(II) 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
−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.

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.

References

Relevant Sciencemadness threads