Solubility chart

Source: Wikipedia, the free encyclopedia.

A solubility chart is a chart describing whether the

ionic compounds formed from different combinations of cations and anions dissolve in or precipitate
from solution.

The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C (298.15 K)). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate. For detailed information on exact solubility of compounds, see solubility table.

For compounds with multiple hydrates, the solubility of the most soluble hydrate is shown.

Some compounds like nickel oxalate will not precipitate immediately even though they are insoluble, requiring a few minutes to precipitate out.[1]

Ions names and symbols Halogens Chalcogens Pnictogens Crystallogens
Fluoride
F− 		Chloride
Cl− 		Bromide
Br− 		Iodide
I− 		Perchlorate
ClO−
4 		Oxide
O2− 		Hydroxide
OH− 		Sulfide
S2− 		Sulfate
SO2−
4 		Nitrate
NO−
3[a] 		Phosphate
PO3−
4 		Carbonate
CO2−
3[a] 		Cyanide
CN− 		Thiocyanate
SCN− 		Acetate
C
2H
3O−
2 		Oxalate
C
2O2−
4
Hydrogen H+ S S S S S
S
 S sS S
S
 S S S S S S
Ammonium NH+
4[a] 		S S S S S
S[b]
S
R
 S S S S S S S S
Lithium Li+ sS S S S S R S R S S sS sS S S S S
Sodium Na+ S S S S S R S R S S S S S S S S
Potassium K+ S S S S sS R S R S S S S S S S
S
Rubidium Rb+ S S S S sS R S R S S S S S S[3] S S
Caesium Cs+ S S S S sS R S R S S S S S S S S
Beryllium Be2+ S S S R S[4] I I R S S I sS R S[5]
S
 S
Magnesium Mg2+ sS S S S S R I R S S I sS R S[6] S sS
Calcium Ca2+ I S S S S R sS R sS S I I R S[7] S sS
Strontium Sr2+ sS S S S S R sS R sS S sS I S S[8] S I
Barium Ba2+ sS S S S S R S R I S I[9] sS S S S I
Aluminium Al3+ sS S S S[c] S[10] I I R S S I R R S[11] S I
Gallium Ga3+
I
 S
S
R
 S[10] I I R sS S I R R S[12] S ?
Manganese(II) Mn2+ sS S S S S[13] I I I S S I I S S[14] S
I
Iron(II) Fe2+ sS S S S S I I I S S I I S S S sS
Cobalt(II) Co2+ sS S S S S[15] I I I S S I I I S S I
Nickel(II) Ni2+ S S S S S I I I S S I I
I
 S S I[1]
Copper(II) Cu2+ sS S S ? S I I
I
 S S I I[d] I I S
I
Zinc Zn2+ sS S S S S[16] I I I S S I I I S[17] S I
Cadmium Cd2+ S S S S S[18] I I I S S I
I
 sS sS[17] S
I
Mercury(II) Hg2+ R S sS I S[19] I I I R S I I S sS S sS[20]
Vanadium(III) V3+ I S S S S[21] I I I sS S
I
 ? ? S ? ?
Chromium(III) Cr3+ sS S S S S I I I S S I I S S S ?
Iron(III) Fe3+ S[e] S S R S[22] I
I
 I S S sS
R[23]
 S S[24] S[25][f]
sS
Gold(III) Au3+ R S sS ? ? I I I ? ? I I S ? sS ?
Tin(II) Sn2+ S S S S S[26] I I I S ? I I ? I[27] R sS
Lead(II) Pb2+ sS sS sS sS S I sS I I S I
I
 sS sS S I
Silver Ag+ S I I I S I
I
 I sS S I I I I sS I
Mercury(I) Hg2+
2 		R I I I S[28] I ? ? sS S[g] ? I I ? S[29][g] ?
  Fluoride
F− 		Chloride
Cl− 		Bromide
Br− 		Iodide
I− 		Perchlorate
ClO−
4 		Oxide
O2− 		Hydroxide
OH− 		Sulfide
S2− 		Sulfate
SO2−
4 		Nitrate
NO−
3[a] 		Phosphate
PO3−
4 		Carbonate
CO2−
3[a] 		Cyanide
CN− 		Thiocyanate
SCN− 		Acetate
C
2H
3O−
2 		Oxalate
C
2O2−
4
Key
S highly soluble or miscible ≥20 g/L
sS slightly soluble 0.1~20 g/L
I relatively insoluble <0.1 g/L
R reacts with or in water —
? unavailable —

See also

  • Solubility rules

Notes

  1. ^ a b c d e Compounds that include ammonium (NH+
    4    ), chlorate (ClO−
    3    ), or nitrate (NO−
    3    ) are soluble without exceptions. Compounds that include carbonate (CO2−
    3    ) are insoluble, unless the compound includes group 1 elements or ammonium.[2]
  2. ^ "Ammonium oxide" does not exist. However, its theoretical molecular formula (NH+
    4    )2O2− represents that of aqueous ammonia.
  3. ^ Partial electrolysis.
  4. ^ The commonly encountered basic copper carbonate (CuCO3(OH)2) is insoluble in water. True copper(II) carbonate (CuCO3) is rare and reacts with water to form basic copper carbonate.
  5. ^ Anhydrous FeF3 is slightly soluble in water; FeF3·3H2O is much more soluble in water.
  6. ^ The commonly encountered basic iron(III) acetate ([Fe3O(OAc)6(H2O)3]OAc) is insoluble in water. True iron(III) acetate (Fe(OAc)3) is rare and is soluble in water.
  7. ^ a b Slowly decomposes in water.

References

  1. ^
    doi:10.1021/j150508a027
    .
  2. ^ "Solubility Table". intro.chem.okstate.edu.
  3. doi:10.1071/PH890389
    .
  4. doi:10.3891/acta.chem.scand.15-1875
    .
  5. doi:10.1139/v67-459
    .
  6. doi:10.1107/S0567740882005433
    .
  7. doi:10.1515/znb-2002-1213
    .
  8. doi:10.1002/1521-3749(200107)627:7<1693::AID-ZAAC1693>3.0.CO;2-U
    .
  9. doi:10.1021/ed400741k
    .
  10. ^
    doi:10.1021/ja01266a041
    .
  11. doi:10.1016/0022-1902(71)80004-0
    .
  12. doi:10.1139/v69-032
    .
  13. ^ "44318 Manganese(II) perchlorate hexahydrate, 99.995% (metals basis)". Alfa Aesar. Alfa Aesar. Retrieved 16 September 2022.
  14. doi:10.1016/S0020-1693(00)82345-2
    .
  15. S2CID 102316324
    .
  16. ISBN 9780470842898
    .
  17. ^
    doi:10.1246/bcsj.6.163
    .
  18. doi:10.1071/CH9711361
    .
  19. doi:10.1080/00958979009409182
    .
  20. ^ "Properties of substance: mercury(II) oxalate Group of substances". Chemister. Chemister. Retrieved 13 September 2022.
  21. doi:10.1021/j100726a018
    .
  22. doi:10.1016/0022-1902(78)80304-2
    .
  23. ^ "Iron (III) Carbonate Formula". softschools.com. p. 1. Retrieved 19 August 2022.
  24. doi:10.1246/cl.1973.43
    .
  25. S2CID 94447648
    .
  26. doi:10.1016/0022-1902(68)80389-6
    .
  27. doi:10.1139/v78-333
    .
  28. doi:10.1039/JR9630001181
    .
  29. ^ National Center for Biotechnology Information. "PubChem Compound Summary for CID 61181, Mercurous acetate". PubChem.
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