Copper(II) sulfate
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Copper(II) sulfate is an inorganic compound with formula CuSO4.
Table of contents
- 1Names
- 2Formulae and structures
- 3Properties
- 4Constituents
- 5Thermodynamic properties
- 6Solubility
- 7Hazards
- 8Preparations
- 9Chemical reactions
- 10References
- 11Related substances
- 12Related categories
Names
List of substance names
Nomenclature
Name
- Typical name
- Copper(II) sulfate
- Compositional nomenclature
- Copper(II) sulfate
- Additive nomenclature
- Copper(2+) tetraoxidosulfate(2−)
- Other names
- Blue vitriol
- Cupric sulfate
Formulae and structures
List of formulae
Formula name
Formula
- Typical formula
- CuSO4
- Compositional formula
- CuSO4
- Structural formula
- Other structural formulas
- Lewis structure
- Colored Lewis structure
Properties
List of substance properties
Item
Value
- Name
- Copper(II) sulfate
- Formula
- CuSO4
- Appearance
- Colorless solidAnhydrate
- Blue solidPentahydrate, 5 hydrate
- Odor
- Odorless
- Molar mass
- 159.60 g/mol
- Density
- 3.603 g/cm3[1]Solid
- 3.60 g/cm3[2]Solid
- 2.284 g/cm3[1]Solid, 16°C, Pentahydrate
- 2.286 g/cm3[2]Solid, Pentahydrate
- Melting point
- >560 °C[1]Decompose
- 560 °C[2]Decompose
- 200 °C[1]Pentahydrate to anhydrate
- 110 °C[2]Pentahydrate, decompose
- Boiling point
- –
Constituents
Constituent ions
| Ion | Name | Charge number | Number |
|---|---|---|---|
| Cu2+ | Copper(II) ion | 2 | 1 |
| SO42− | Sulfate ion | -2 | 1 |
Constituent atoms
| Atom | Name | Oxidation state | Number |
|---|---|---|---|
| Cu | Copper | +2 | 1 |
| S | Sulfur | +6 | 1 |
| O | Oxygen | −2 | 4 |
Ratio of atoms
| Atom | Atomic weight | Number | Atomic ratio | Weight ratio |
|---|---|---|---|---|
| Cu | 63.546 | 1 | 16.67% | 39.82% |
| S | 32.06 | 1 | 16.67% | 20.09% |
| O | 15.999 | 4 | 66.67% | 40.10% |
Thermodynamic properties
Phase transition properties
Item
Value
- Enthalpy of fusion
- –
- Enthalpy of vaporization
- –
- Enthalpy of vaporization at 25°C
- –
- Enthalpy of other transition
- –
Standard thermodynamic properties
State | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| Crystalline solid | −771.36[3] | −661.8[3] | 109.[3] | 100.0[3] |
| Ionized aqueous solution | −844.50[3] | −679.04[3] | −79.5[3] | – |
| Un−ionized aqueous solution | – | −692.18[3] | – | – |
| Crystalline solid 1 hydrate | −1085.83[3] | −918.11[3] | 146.0[3] | 134.[3] |
| Crystalline solid 3 hydrate | −1684.31[3] | −1399.96[3] | 221.3[3] | 205.[3] |
| Crystalline solid 5 hydrate | −2279.65[3] | −1879.745[3] | 300.4[3] | 280.[3] |
Solubility
Qualitative solubility
Solubility in water (g/100 g, Pentahydrate)[1]
| 0°C | 10°C | 20°C | 30°C | 40°C | 60°C | 80°C | 100°C |
|---|---|---|---|---|---|---|---|
| 23.1 | 27.5 | 32 | 37.8 | 44.6 | 61.8 | 83.8 | 114 |
Solubility in water (g/100 g)[4]
| 0°C | 10°C | 20°C | 25°C | 30°C | 40°C | 50°C | 60°C | 80°C | 100°C | 120°C | 140°C | 160°C | 180°C |
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| 14.3 | 17.4 | 20.7 | 22.7 | 25 | 28.5 | 33.3 | 40 | 55 | 75.4 | 78.6 | 80.2 | 78.6 | 75.4 |
Solubility in glycerol (g/100 g, Pentahydrate)[4]
| 16°C |
|---|
| 36.3 |
Solubility in glycerol (g/100 g, Pentahydrate)[4]
| 15.5°C |
|---|
| 30 |
Solubility in methanol (g/100 g, Pentahydrate)[4]
| 18°C |
|---|
| 15.6 |
Solubility in hydrazine (g/100 g)[4]
| 20°C |
|---|
| 2 |
Solubility in ethanol (g/100 g, Pentahydrate)[4]
| 0°C |
|---|
| 1.1 |
Solubility in methanol (g/100 g)[4]
| 18°C |
|---|
| 1.05 |
Solubility in formic acid (g/100 g, 95%, Pentahydrate)[4]
| 18.5°C |
|---|
| 0.05 |
Solubility in ethylene glycol (g/100 g solution, Pentahydrate)[4]
| 14.6°C |
|---|
| 7.6 |
Solubility curve (g/100 g)
Solubility curve (g/100 g solution)
Hazards
GHS label[5]
Item
Value
- Hazard pictograms
- Signal word
- Danger
- Hazard statements
- H301: Toxic if swallowed
- H314: Causes severe skin burns and eye damage
- H318: Causes serious eye damage
- H317: May cause an allergic skin reaction
- H361: Suspected of damaging fertility or the unborn child
- H370: Causes damage to organs
- H370: Causes damage to nervous system
- H370: Causes damage to blood system
- H370: Causes damage to liver
- H370: Causes damage to kidney
- H335: May cause respiratory irritation
- H372: Causes damage to organs through prolonged or repeated exposure
- H372: Causes damage to respiratory system through prolonged or repeated exposure
- H373: May cause damage to organs through prolonged or repeated exposure
- H373: May cause damage to liver through prolonged or repeated exposure
- H400: Very toxic to aquatic life
- H410: Very toxic to aquatic life with long lasting effects
Physical hazards[5]
Health hazards[5]
Environmental hazards[5]
Preparations
Reaction of acid and base
The reaction of sulfuric acid and copper(II) hydroxide yields copper(II) sulfate and water.
Reaction of base and acidic oxide
The reaction of copper(II) hydroxide and sulfur trioxide yields copper(II) sulfate and water.
Reaction of basic oxide and acid
The reaction of copper(II) oxide and sulfuric acid yields copper(II) sulfate and water.
Reaction of basic oxide and acidic oxide
The reaction of copper(II) oxide and sulfur trioxide yields copper(II) sulfate.
Reaction of salt of weak acid and strong acid
The reaction of salt of weak acid and strong acid can yield copper(II) sulfate.
Reaction of inactive metal and oxidizing acid
The reaction of and sulfuric acid yields copper(II) sulfate, sulfur dioxide, and water.
Reaction of nonmetal and hydroxide base
The reaction of and copper(II) hydroxide yields copper(II) sulfate, copper(II) sulfide, and water.
Decomposition
Decomposition of thermally decomposable substance can yield copper(II) sulfate.
Chemical reactions
Electrolytic dissociation
Electrolytic dissociation of copper(II) sulfate yields copper(II) ion and sulfate ion.
Reaction with strong base
The reaction of copper(II) sulfate and strong base yields salt of strong base and copper(II) hydroxide.
Reaction with dehydrating acid
The reaction of copper(II) sulfate and phosphoric acid yields copper(II) phosphate, sulfur trioxide, and water.
Reaction with reducing species
The reaction of reducing species and copper(II) sulfate yields a variety of products.
Reaction with oxidizable species
The reaction of oxidizable species and copper(II) sulfate yields a variety of products.
Precipitation reaction
When a certain chemical species is present in aqueous solution, it reacts with copper(II) sulfate to form a precipitate.
Decomposition
Decomposition of copper(II) sulfate yields copper(II) oxide and sulfur trioxide.
Electrolysis of aqueous solution
Electrolysis of aqueous copper(II) sulfate yields a variety of products.
References
List of references
- 1James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ Density, 3.603 g/cm3 - p.42
- ^ Density, 2.284 g/cm3 - p.42
- ^ Melting point, >560 °C - p.42
- ^ Melting point, 200 °C - p.42
- ^ Qualitative solubility, Soluble in glycerol - p.42
- ^ Qualitative solubility, Soluble in methanol - p.42
- ^ Qualitative solubility, Insoluble in ethanol - p.42
- ^ Solubility in Water (g/100 g), See the table - p.336
- 2John R. Rumble Jr, David R. Lide, Thomas J. Bruno (2019)CRC Handbook of Chemistry and Physics 100th EditionCRC Press
- ^ Density, 3.60 g/cm3 - p.4-44
- ^ Density, 2.286 g/cm3 - p.4-44
- ^ Melting point, 560 °C - p.4-44
- ^ Melting point, 110 °C - p.4-44
- 3Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -771.36 kJ · mol−1
- ^ ΔfG°, -661.8 kJ · mol−1
- ^ S°, 109. J · K−1 · mol−1
- ^ Cp°, 100.0 J · K−1 · mol−1
- ^ ΔfH°, -844.50 kJ · mol−1
- ^ ΔfG°, -679.04 kJ · mol−1
- ^ S°, -79.5 J · K−1 · mol−1
- ^ ΔfG°, -692.18 kJ · mol−1
- ^ ΔfH°, -1085.83 kJ · mol−1
- ^ ΔfG°, -918.11 kJ · mol−1
- ^ S°, 146.0 J · K−1 · mol−1
- ^ Cp°, 134. J · K−1 · mol−1
- ^ ΔfH°, -1684.31 kJ · mol−1
- ^ ΔfG°, -1399.96 kJ · mol−1
- ^ S°, 221.3 J · K−1 · mol−1
- ^ Cp°, 205. J · K−1 · mol−1
- ^ ΔfH°, -2279.65 kJ · mol−1
- ^ ΔfG°, -1879.745 kJ · mol−1
- ^ S°, 300.4 J · K−1 · mol−1
- ^ Cp°, 280. J · K−1 · mol−1
- 4Atherton Seidell (1919)Solubilities of Inorganic and Organic Compounds: A Compilation of Quantitative Solubility Data From the Periodical LiteratureD. Van Nostrand Company
- ^ Solubility in Water (g/100 g), See the table - p.272
- ^ Solubility in Glycerol (g/100 g), See the table - p.277
- ^ Solubility in Glycerol (g/100 g), See the table - p.277
- ^ Solubility in Methanol (g/100 g), See the table - p.277
- ^ Solubility in Hydrazine (g/100 g), See the table - p.277
- ^ Solubility in Ethanol (g/100 g), See the table - p.277
- ^ Solubility in Methanol (g/100 g), See the table - p.277
- ^ Solubility in Formic acid (g/100 g), See the table - p.277
- ^ Solubility in Ethylene glycol (g/100 g solution), See the table - p.277
- 5Chemical Management CenterGHS Classification ResultsNational Institute of Technology and Evaluation
