Difference between revisions of "Silver sulfate"
From Sciencemadness Wiki
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| ImageAlt = | | ImageAlt = | ||
| ImageName = | | ImageName = | ||
| − | | ImageCaption = Silver(I) sulfate sample. | + | | ImageCaption = Silver(I) sulfate sample and original bottle. |
| ImageFile1 = | | ImageFile1 = | ||
| ImageSize1 = | | ImageSize1 = | ||
| Line 53: | Line 53: | ||
| BoilingPt_ref = | | BoilingPt_ref = | ||
| BoilingPt_notes = | | BoilingPt_notes = | ||
| − | | Density = 5.45 g/cm<sup>3</sup> (at | + | | Density = 5.45 g/cm<sup>3</sup> (at 20 °C) |
| Formula = Ag<sub>2</sub>SO<sub>4</sub> | | Formula = Ag<sub>2</sub>SO<sub>4</sub> | ||
| HenryConstant = | | HenryConstant = | ||
| Line 59: | Line 59: | ||
| MolarMass = 311.799 g/mol | | MolarMass = 311.799 g/mol | ||
| MeltingPt = | | MeltingPt = | ||
| − | | MeltingPtC = 652.2–660 | + | | MeltingPtC = 652.2–660.0 |
| MeltingPt_ref = | | MeltingPt_ref = | ||
| MeltingPt_notes = | | MeltingPt_notes = | ||
| Line 68: | Line 68: | ||
| SolubleOther = Soluble in conc. sulfuric acid<br>Slightly soluble in acetates, [[acetone]], alcohols, amides, aq. acids, [[diethyl ether]]<br>Insoluble in [[ethanol]] | | SolubleOther = Soluble in conc. sulfuric acid<br>Slightly soluble in acetates, [[acetone]], alcohols, amides, aq. acids, [[diethyl ether]]<br>Insoluble in [[ethanol]] | ||
| Solvent = | | Solvent = | ||
| − | | VaporPressure = | + | | VaporPressure = ~0 mmHg |
}} | }} | ||
| Section3 = {{Chembox Structure | | Section3 = {{Chembox Structure | ||
| Line 89: | Line 89: | ||
}} | }} | ||
| Section6 = {{Chembox Hazards | | Section6 = {{Chembox Hazards | ||
| − | | AutoignitionPt = | + | | AutoignitionPt = Non-flammable |
| − | | ExploLimits = | + | | ExploLimits = Non-flammable |
| ExternalMSDS = [http://www.sciencelab.com/msds.php?msdsId=9927585 ScienceLab] | | ExternalMSDS = [http://www.sciencelab.com/msds.php?msdsId=9927585 ScienceLab] | ||
| − | | FlashPt = | + | | FlashPt = Non-flammable |
| LD50 = | | LD50 = | ||
| LC50 = | | LC50 = | ||
| Line 102: | Line 102: | ||
}} | }} | ||
| Section7 = {{Chembox Related | | Section7 = {{Chembox Related | ||
| − | | OtherAnions = | + | | OtherAnions = |
| OtherCations = [[Copper(II) sulfate]]<br>[[Mercury(II) sulfate]] | | OtherCations = [[Copper(II) sulfate]]<br>[[Mercury(II) sulfate]] | ||
| OtherFunction = | | OtherFunction = | ||
| OtherFunction_label = | | OtherFunction_label = | ||
| − | | OtherCompounds = | + | | OtherCompounds = [[Silver nitrate]]<br>[[Silver perchlorate]] |
}} | }} | ||
}} | }} | ||
| Line 113: | Line 113: | ||
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Silver sulfate darkens upon exposure to light, though this process requires many hours. | + | Silver sulfate darkens upon exposure to strong light, though this process requires many hours. |
| + | |||
| + | Silver sulfate will react with an aq. solution of NaOH to yield [[silver oxide]], under strong stirring, which can work even if the silver sulfate is not fully dissolved in water, as all the dissolved silver from the solution that precipitates is immediately replaced by more silver that further dissolves in the solution. However, for the reaction to be complete, the silver sulfate particles must be very fine, as any large pieces of silver sulfate will get coated by silver oxide, which blocks the displacement reaction. | ||
| + | |||
| + | : Ag<sub>2</sub>SO<sub>4</sub> + 2 NaOH → Ag<sub>2</sub>O + Na<sub>2</sub>SO<sub>4</sub> + H<sub>2</sub>O | ||
===Physical=== | ===Physical=== | ||
| − | Silver sulfate is a white solid, extremely poorly soluble in water (0.83 g/100 | + | Silver sulfate is a white solid, extremely poorly soluble in water (0.83 g/100 ml at 25 °C), but soluble in concentrated [[sulfuric acid]]. It is quite stable under ordinary conditions of use and storage, though it darkens upon exposure to air or light. |
==Availability== | ==Availability== | ||
| − | Silver sulfate is sold by various chemical suppliers. | + | Silver sulfate is sold by various chemical suppliers, though it's not cheap. |
==Preparation== | ==Preparation== | ||
| − | Silver sulfate can be prepared by reacting concentrated sulfuric acid with [[silver nitrate]]: | + | Silver sulfate can be prepared by reacting concentrated [[sulfuric acid]] with [[silver nitrate]]: |
| + | |||
: 2 AgNO<sub>3</sub> + H<sub>2</sub>SO<sub>4</sub> → Ag<sub>2</sub>SO<sub>4</sub> + 2 HNO<sub>3</sub> | : 2 AgNO<sub>3</sub> + H<sub>2</sub>SO<sub>4</sub> → Ag<sub>2</sub>SO<sub>4</sub> + 2 HNO<sub>3</sub> | ||
| + | |||
| + | Alternatively, a sulfate salt, like [[sodium sulfate]] can be used instead of sulfuric acid. | ||
| + | |||
| + | : 2 AgNO<sub>3</sub> + Na<sub>2</sub>SO<sub>4</sub> → Ag<sub>2</sub>SO<sub>4</sub> + 2 NaNO<sub>3</sub> | ||
| + | |||
| + | Hot sulfuric acid will dissolve silver metal, forming silver sulfate: | ||
| + | |||
| + | : 2 Ag + 2 H<sub>2</sub>SO<sub>4</sub> → Ag<sub>2</sub>SO<sub>4</sub> + SO<sub>2</sub> + 2 H<sub>2</sub>O | ||
==Projects== | ==Projects== | ||
*Silver plating | *Silver plating | ||
| + | *Compound collecting | ||
==Handling== | ==Handling== | ||
===Safety=== | ===Safety=== | ||
| − | Silver sulfate should not be handled without protection, as it will darken when exposed to light. | + | Silver sulfate should not be handled without protection, as it will darken when exposed to light, thus staining the skin. |
===Storage=== | ===Storage=== | ||
| − | + | Silver sulfate should be kept in closed bottles, away from light and air. | |
===Disposal=== | ===Disposal=== | ||
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=62071 Silver sulfate] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=62071 Silver sulfate] | ||
*[http://www.sciencemadness.org/whisper/viewthread.php?tid=13230 Sulphur trioxide from silver sulphate] | *[http://www.sciencemadness.org/whisper/viewthread.php?tid=13230 Sulphur trioxide from silver sulphate] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=71787 Silver sulfate] | ||
[[Category:Chemical compounds]] | [[Category:Chemical compounds]] | ||
Latest revision as of 22:02, 5 November 2023
 Silver(I) sulfate sample and original bottle.
| |
| Names | |
|---|---|
| IUPAC name
Silver sulfate
| |
| Other names
Disilver(1+) sulfate
Silver(I) sulfate | |
| Identifiers | |
| Jmol-3D images | Image |
| |
| Properties | |
| Ag2SO4 | |
| Molar mass | 311.799 g/mol |
| Appearance | White solid |
| Odor | Odorless |
| Density | 5.45 g/cm3 (at 20 °C) |
| Melting point | 652.2–660.0 °C (1,206.0–1,220.0 °F; 925.4–933.1 K) |
| Boiling point | 1,085 °C (1,985 °F; 1,358 K) |
| 0.57 g/100 mL (0 °C) 0.69 g/100 mL (10 °C) 0.83 g/100 mL (25 °C) 0.96 g/100 mL (40 °C) 1.33 g/100 mL (100 °C) | |
| Solubility | Soluble in conc. sulfuric acid Slightly soluble in acetates, acetone, alcohols, amides, aq. acids, diethyl ether Insoluble in ethanol |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
200.4 kJ/mol |
| Std enthalpy of
formation (ΔfH |
−715.9 kJ/mol |
| Hazards | |
| Safety data sheet | ScienceLab |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Silver nitrate Silver perchlorate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Silver sulfate is an ionic compound of silver with the formula Ag2SO4, mainly used in silver plating and as a non-staining substitute to silver nitrate. It is also used in analytical chemistry.
Contents
Properties
Chemical
Silver sulfate darkens upon exposure to strong light, though this process requires many hours.
Silver sulfate will react with an aq. solution of NaOH to yield silver oxide, under strong stirring, which can work even if the silver sulfate is not fully dissolved in water, as all the dissolved silver from the solution that precipitates is immediately replaced by more silver that further dissolves in the solution. However, for the reaction to be complete, the silver sulfate particles must be very fine, as any large pieces of silver sulfate will get coated by silver oxide, which blocks the displacement reaction.
- Ag2SO4 + 2 NaOH → Ag2O + Na2SO4 + H2O
Physical
Silver sulfate is a white solid, extremely poorly soluble in water (0.83 g/100 ml at 25 °C), but soluble in concentrated sulfuric acid. It is quite stable under ordinary conditions of use and storage, though it darkens upon exposure to air or light.
Availability
Silver sulfate is sold by various chemical suppliers, though it's not cheap.
Preparation
Silver sulfate can be prepared by reacting concentrated sulfuric acid with silver nitrate:
- 2 AgNO3 + H2SO4 → Ag2SO4 + 2 HNO3
Alternatively, a sulfate salt, like sodium sulfate can be used instead of sulfuric acid.
- 2 AgNO3 + Na2SO4 → Ag2SO4 + 2 NaNO3
Hot sulfuric acid will dissolve silver metal, forming silver sulfate:
- 2 Ag + 2 H2SO4 → Ag2SO4 + SO2 + 2 H2O
Projects
- Silver plating
- Compound collecting
Handling
Safety
Silver sulfate should not be handled without protection, as it will darken when exposed to light, thus staining the skin.
Storage
Silver sulfate should be kept in closed bottles, away from light and air.
Disposal
Best to recycle it.
References
Relevant Sciencemadness threads
Categories:
- Chemical pages without CAS Registry Number
- Articles without EBI source
- Chemical pages without ChemSpiderID
- Chemical pages without DrugBank identifier
- Articles without KEGG source
- Articles without InChI source
- Articles without UNII source
- Articles containing unverified chemical infoboxes
- Chemical compounds
- Inorganic compounds
- Silver compounds
- Sulfates
