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
Sodium bisulfate.jpg
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.

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

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

  1. http://www.sciencemadness.org/talk/viewthread.php?tid=18767
  2. https://www.youtube.com/watch?v=TtPiwbRA4N8
  3. http://www.sciencelab.com/msds.php?msdsId=9927267
  4. "The Volatile Chemist's" personal experience

Relevant Sciencemadness threads