View source for Sea salt

{| style='float:right;' class="wikitable sortable"
|+Dissolved ions in seawater over 50mg/L
!Cation
!Molarity
!Anion
|-
| ||0.535||[[Chlorine|Cl<sup>-</sup>]]
|-
|[[Sodium|Na<sup>+</sup>]]||0.459||
|-
| ||0.009||{{#Chem:SO4}}
|-
|[[Magnesium|Mg<sup>2+</sup>]]||0.051||
|-
|[[Calcium|Ca<sup>2+</sup>]]||0.009||
|-
|[[Potassium|K<sup>+</sup>]]||0.009||
|-
| ||0.002||{{#Chem: HCO3<sup>-</sup>}}
|-
| ||0.00082||[[Bromine|Br<sup>-</sup>]]
|}
__TOC__
[[Salt water|Seawater]] contains just about every element in ''some'' small quantity. The materials over 50mg/L is a shorter list.{{br}}
==Character==
For seawater and many brines, the order of deposition is:<ref name=EB>{{cite pub
|publication=Encyclopedia Britannica
|title=Salt: Salt Manufacture
|url=https://www.britannica.com/science/salt/Salt-manufacture
|courtesy=Encyclopedia Britannica
|first1=John M.
|last1=Hills
|first2=Frank Osborne
|last2= Wood
|first3=et al
|year=2019
|Issue=December
}}</ref>
# [[calcium carbonate]]
# [[calcium sulfate]]
# [[sodium chloride]]
# [[magnesium sulfate]]
# '''potassium magnesium chloride hexahydrate''' ({{#Chem:KCl*MgCl2*6H2O}})
# [[magnesium chloride]]

 Once it has been concentrated, the brine is run through a series of crystallizing pans, usually four in number, where the salt is deposited as evaporation proceeds. In the first crystallizing pan, the brine is concentrated to a specific gravity of 1.23 and remains partly contaminated with calcium sulfate. The specific gravity of the solution in the pan increases slowly during crystallization of the salt, reaching 1.24 in the second pan. In the third pan the specific gravity of the solution reaches 1.25, and the salt deposited there contains small amounts of magnesium sulfate as an impurity. The final solution, termed bitterns, has a specific gravity of 1.25–1.26 and is used in some countries (United States and Israel) in the manufacture of potash, bromine, epsom salts (magnesium sulfate), and magnesium chloride.<ref name=EB />

==Purification==
===Removal of sulfate and bicarbonate===
To remove the 0.011 mol of these, add a small amount soluble calcium. (0.5g/L [[calcium oxide]] or 0.75g/L of [[calcium hydroxide]]) This will cause calcium carbonate and calcium sulfate to precipitate.
:{{#Chem: CaO + NaHCO3 = CaCO3 + NaOH}}
:{{#Chem: Ca(OH)2 + NaHCO3 = CaCO3 + NaOH + H2O}}
:{{#Chem: CaO + Na2SO4 + H2O = CaSO4 + 2NaOH}}
:{{#Chem: Ca(OH)2 + Na2SO4 = CaSO4 + 2NaOH}}

===Removal of calcium and magnesium===
With [[Calcium]] and [[Magnesium]] combined for 0.06 mol/L, adding 0.06mol of soluble ash (7-8g/L) should precipitate most of the alkali earth metal content.
: {{#Chem: (Ca/Mg)Cl2(aq) + (Na/K)2CO3(aq) = (Ca/Mg)CO3(s) + 2(Na/K)Cl(aq) }}
This leaves sodium/potassium chloride/carbonate in solution, which can be more easily separated by crystallization

==See Also==
==References==
<references/>
[[Category:Crude Mixtures]][[Category:Minerals]]