Difference between revisions of "Sodium bisulfate"
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===Chemical=== | ===Chemical=== | ||
Sodium bisulfate will react with [[sodium chloride]] to release [[hydrogen chloride]]. | Sodium bisulfate will react with [[sodium chloride]] to release [[hydrogen chloride]]. | ||
| + | |||
:NaHSO<sub>4</sub> + NaCl → Na<sub>2</sub>SO<sub>4</sub> + HCl | :NaHSO<sub>4</sub> + NaCl → Na<sub>2</sub>SO<sub>4</sub> + HCl | ||
| + | |||
Sodium bisulfate is an acid salt. Heating (and even just sitting) can release [[sulfuric acid]] vapors, from small amounts to large quantities of fumes. | Sodium bisulfate is an acid salt. Heating (and even just sitting) can release [[sulfuric acid]] vapors, from small amounts to large quantities of fumes. | ||
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==Availability== | ==Availability== | ||
| − | Sodium bisulfate is available as a pH lowering chemical for swimming pools. | + | Sodium bisulfate is available as a pH lowering chemical for swimming pools in most hardware stores. |
==Preparation== | ==Preparation== | ||
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==Projects== | ==Projects== | ||
| − | *Make [[hydrochloric acid]] | + | *Make [[hydrogen chloride]] and [[hydrochloric acid]] |
*Make [[sodium pyrosulfate]] and [[sulfur trioxide]] | *Make [[sodium pyrosulfate]] and [[sulfur trioxide]] | ||
*Make nitric acid (it will give off mostly [[nitrogen dioxide]] fumes if you use an alkali nitrate)<ref>http://www.sciencemadness.org/talk/viewthread.php?tid=18767</ref><ref>https://www.youtube.com/watch?v=TtPiwbRA4N8</ref> | *Make nitric acid (it will give off mostly [[nitrogen dioxide]] fumes if you use an alkali nitrate)<ref>http://www.sciencemadness.org/talk/viewthread.php?tid=18767</ref><ref>https://www.youtube.com/watch?v=TtPiwbRA4N8</ref> | ||
Revision as of 20:17, 9 July 2017
 Sodium bisulfate.
| |
| Names | |
|---|---|
| IUPAC name
Sodium hydrogen sulfate
| |
| Other names
Bisulfate of soda
Sodium acid sulfate | |
| Properties | |
| NaHSO4 | |
| Molar mass | 120.06 g/mol (anhydrous) 138.07 g/mol (monohydrate) |
| Appearance | Colorless solid |
| Density | 2.742 g/cm3 (anhydrous) 1.8 g/cm3 (monohydrate) |
| Melting point | 58.5 °C (137.3 °F; 331.6 K) (monohydrate) 315 °C (anhydrous, decomposes) |
| Boiling point | Decomposes |
| 28.5 g/100 ml (25 °C) 100 g/100 ml (100 °C) | |
| Solubility | Insoluble in ammonia, ethanol, pyridine, toluene, xylene |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Sodium sulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium bisulfate, also known as sodium hydrogen sulfate is the sodium salt of the bisulfate anion, with the molecular formula NaHSO4. It is an acid salt, formed by the partial neutralization of sulfuric acid with an equivalent of sodium, usually sodium chloride or sodium hydroxide.
Contents
Properties
Chemical
Sodium bisulfate will react with sodium chloride to release hydrogen chloride.
- NaHSO4 + NaCl → Na2SO4 + HCl
Sodium bisulfate is an acid salt. Heating (and even just sitting) can release sulfuric acid vapors, from small amounts to large quantities of fumes.
Physical
Sodium bisulfate is a white dry granular product, soluble in water. The anhydrous form is hygroscopic. Solutions of sodium bisulfate are acidic, 1 M solution having a pH of < 1.
Availability
Sodium bisulfate is available as a pH lowering chemical for swimming pools in most hardware stores.
Preparation
Sodium bisulfate is made by mixing stoichiometric quantities of sodium hydroxide or sodium chloride and sulfuric acid.
- NaOH + H2SO4 → NaHSO4 + H2O
- NaCl + H2SO4 → NaHSO4 + HCl
Projects
- Make hydrogen chloride and hydrochloric acid
- Make sodium pyrosulfate and sulfur trioxide
- Make nitric acid (it will give off mostly nitrogen dioxide fumes if you use an alkali nitrate)[1][2]
Handling
Safety
Sodium bisulfate will irritate the skin, eyes and mucous tissues on contact. Despite being a salt rather than a fully saturated acid, sodium bisulfate solutions have a much lower pH than many acids themselves, and should be treated with care. Prolonged exposure will damage the tissues.[3] Do not attempt to smell sodium bisulfate. It is common for a sample to release sulfuric acid vapors, and these can build up in a container.[4]
Storage
Sodium bisulfate should be stored in closed bottles. You should open them periodically to release any acid vapors inside.
Disposal
Sodium bisulfate is not very dangerous to the environment, though it should be neutralized first before disposal.
References
- ↑ http://www.sciencemadness.org/talk/viewthread.php?tid=18767
- ↑ https://www.youtube.com/watch?v=TtPiwbRA4N8
- ↑ http://www.sciencelab.com/msds.php?msdsId=9927267
- ↑ "The Volatile Chemist's" personal experience
