Jump to content

Solubility chart: Difference between revisions

From Wikipedia, the free encyclopedia
Browse history interactively
← Previous editNext edit →
Content deleted Content added
VisualWikitext
mercury(I) carbonate is insoluble (from solubility table)
add note on basic copper carbonate
Line 381: Line 381:
| bgcolor="#99CCFF" | [[Copper(II) nitrate|S]]
| bgcolor="#99CCFF" | [[Copper(II) nitrate|S]]
| bgcolor="#99CCFF" | [[Copper(II) acetate|S]]
| bgcolor="#99CCFF" | [[Copper(II) acetate|S]]
| bgcolor="#FFCCCC" | [[Basic copper carbonate|I]]{{efn|group=lower-alpha|The commonly encountered basic copper carbonate (CuCO<sub>3</sub>(OH)<sub>2</sub>) is insoluble in water. True [[copper(II) carbonate]] (CuCO<sub>3</sub>) is rare and reacts with water to form basic copper carbonate.}}
| bgcolor="#FFCCCC" | [[Basic copper carbonate|I]]
| bgcolor="#99CCFF" | [[Copper(II) sulfate|S]]
| bgcolor="#99CCFF" | [[Copper(II) sulfate|S]]
| bgcolor="#FFCCCC" | [[Copper(II) oxalate|I]]
| bgcolor="#FFCCCC" | [[Copper(II) oxalate|I]]
Line 495: Line 495:
|- align="center"
|- align="center"
! [[Iron]](III) Fe<sup>3+</sup>
! [[Iron]](III) Fe<sup>3+</sup>
| bgcolor="#99CCFF" | [[Iron(III) fluoride|S]]{{efn|group=lower-alpha|Anhydrous FeF<sub>3</sub> is slightly soluble in water, FeF<sub>3</sub>·3H<sub>2</sub>O is much more soluble in water.}}
| bgcolor="#99CCFF" | [[Iron(III) fluoride|S]]{{efn|group=lower-alpha|Anhydrous FeF<sub>3</sub> is slightly soluble in water; FeF<sub>3</sub>·3H<sub>2</sub>O is much more soluble in water.}}
| bgcolor="#99CCFF" | [[Iron(III) chloride|S]]
| bgcolor="#99CCFF" | [[Iron(III) chloride|S]]
| bgcolor="#99CCFF" | [[Iron(III) bromide|S]]
| bgcolor="#99CCFF" | [[Iron(III) bromide|S]]

Revision as of 20:06, 18 February 2023

A solubility chart is a chart with a list of ions and how, when mixed with other ions, they can become precipitates or remain aqueous.

The following chart shows the solubility of multiple independent and various compounds, in water, at a pressure of 1 atm and at room temperature (approx. 25 °C (298.15 K)). Any box that reads "soluble" results in an aqueous product in which no precipitate has formed, while "slightly soluble" and "insoluble" markings mean that there is a precipitate that will form (usually, this is a solid); however, "slightly soluble" compounds such as calcium sulfate may require heat to form its precipitate. Boxes marked "other" can mean that many different states of products can result. For more detailed information of the exact solubility of the compounds, see the solubility table.

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

Some compounds, such as nickel oxalate, will not precipitate immediately even though it is insoluble and requires a few minutes to precipitate out.[1]

Ions names and symbols Fluoride
F− 		Chloride
Cl− 		Bromide
Br− 		Iodide
I− 		Oxide
O2− 		Sulfide
S2− 		Hydroxide
OH− 		Cyanide
CN− 		Thiocyanate
SCN− 		Perchlorate
ClO−
4 		Nitrate
NO−
3[a] 		Acetate
C
2H
3O−
2 		Carbonate
CO2−
3[a] 		Sulfate
SO2−
4 		Oxalate
C
2O2−
4 		Phosphate
PO3−
4
Ammonium NH+
4[a] 		S S S S S* R S S S S S S S S S S
Hydrogen H+ S S S S S sS S S S S S S S S S S
Lithium Li+ sS S S S R R S S S S S S sS S S sS
Sodium Na+ S S S S R R S S S S S S S S S S
Potassium K+ S S S S R R S S S sS S S S S S S
Rubidium Rb+ S S S S R R S S S sS S S S S I I
Caesium Cs+ S S S S R R S S S sS S S S S I S
Beryllium Be2+ S S S R I R I R S S[3] S S sS S I S
Magnesium Mg2+ sS S S S I R I R S S S S sS S sS I
Calcium Ca2+ I S S S R R sS R S S S S I sS sS I
Strontium Sr2+ sS S S S R R sS S S S S S I sS I sS
Barium Ba2+ sS S S S R R S S S S S S sS I I I[4]
Aluminium Al3+ sS S S S[b] I R I R S S[5] S S R S I I
Gallium Ga3+ I S S R I R I ? S S[5] S S R sS ? I
Mercury(I) Hg2+
2 		R I I I I ? ? sS[6] sS[7] S[8] S[c] S[9][c] I I ? ?
Manganese(II) Mn2+ sS S S S I I I S I S[10] S S I S I I
Iron(II) Fe2+ sS S S S I I I S S S S S I S sS I
Cobalt(II) Co2+ sS S S S I I I I S S[11] S S I S I I
Nickel(II) Ni2+ S S S S I I I I S S S S I S I[1] I
Copper(II) Cu2+ sS S S ? I I I I I S S S I[d] S I I
Zinc Zn2+ sS S S S I I I I S S[12] S S I S I I
Tin(II) Sn2+ S S S S I I I ? I[13] S[14] S R I S sS I
Mercury(II) Hg2+ R S S I I I I S sS S[15] S S I R sS[16] I
Lead(II) Pb2+ sS sS sS sS I I sS sS sS S S S I I I I
Vanadium(III) V3+ I S S S I I ? ? S S[17] S ? ? sS ? I
Chromium(III) Cr3+ sS S sS S I I I S S S S S I S ? I
Iron(III) Fe3+ S[e] S S R I I I S S S S I R[18] S sS sS
Silver Ag+ S I I I I I I I I S S sS I sS I I
Gold Au3+ I S sS I I I I S ? ? S S I S ? ?
  Fluoride
F− 		Chloride
Cl− 		Bromide
Br− 		Iodide
I− 		Oxide
O2− 		Sulfide
S2− 		Hydroxide
OH− 		Cyanide
CN− 		Thiocyanate
SCN− 		Perchlorate
ClO−
4 		Nitrate
NO−
3[a] 		Acetate
C
2H
3O−
2 		Carbonate
CO2−
3[a] 		Sulfate
SO2−
4 		Oxalate
C
2O2−
4 		Phosphate
PO3−
4
  • Note: "Ammonium oxide" does not exist. However, its theoretical molecular formula (NH+
    4    )2O2− accurately represents that of aqueous ammonia.
Key (water needed to dissolve 1 gram of solute):
S soluble 0.01 ~ 50 mL
sS slightly soluble 50 mL ~ 10 L
I insoluble 10 L and up
X other —
R reacts with water —
? unavailable —

See also

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. ^ Partial electrolysis
  3. ^ a b Slowly decomposes in water.
  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.

References

  1. ^ a b J. A. Allen (1953). "The Precipitation of Nickel Oxalate". J. Phys. Chem. 57 (7): 715–716. doi:10.1021/j150508a027.
  2. ^ "Solubility Table". intro.chem.okstate.edu.
  3. ^ Birgitta Carell; Åke Olin (1961). "Studies on the Hydrolysis of Metal Ions. 37. Application of the Self-Medium Method to the Hydrolysis of Beryllium Perchlorate". Acta Chemica Scandinavica. 15: 1875–1884. doi:10.3891/acta.chem.scand.15-1875.
  4. ^ Hazen, Jeffery L.; Cleary, David A. (July 2, 2014). "Yielding Unexpected Results: Precipitation of Ba3(PO4)2 and Implications for Teaching Solubility Principles in the General Chemistry Curriculum". Journal of Chemical Education. 91 (8): 1261–1263. doi:10.1021/ed400741k.
  5. ^ a b Laurence S. Foster (1939). "(I) The Reaction of Gallium with Perchloric Acid and (II) the Preparation and Properties of Gallium Perchlorate Hydrates". Journal of the American Chemical Society. 61 (11): 3122–3124. doi:10.1021/ja01266a041.
  6. ^ "Mercury(I) cyanide". Chemical Book.
  7. ^ "Mercurous thiocyanate". Chemical Book.
  8. ^ "Mercury(I) perchlorate tetrahydrate". Chemical Book.
  9. ^ National Center for Biotechnology Information. "PubChem Compound Summary for CID 61181, Mercurous acetate". PubChem.
  10. ^ "44318 Manganese(II) perchlorate hexahydrate, 99.995% (metals basis)". Alfa Aesar. Alfa Aesar. Retrieved 16 September 2022.
  11. ^ E. Kamieńska-Piotrowicz (1999). "Conductometric Studies of Cobalt(II) Perchlorate in Acetonitrile-Water Solutions". Zeitschrift für Physikalische Chemie. 210 (1). doi:10.1524/zpch.1999.210.Part_1.001.
  12. ^ Lili Lin; Xiaohua Liu; Xiaoming Feng (2014). "Zinc(II) Perchlorate Hexahydrate". Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons, Ltd. doi:10.1002/047084289X.rn01657.
  13. ^ Tewfik B. Absi; Ramesh C. Makhija; Mario Onyszchuk (1978). "Synthesis and vibrational spectra of tin(II) isothiocyanate adducts with some O- and N-donor ligands". Canadian Journal of Chemistry. 56 (15): 2039–2041. doi:10.1139/v78-333.
  14. ^ C.G.Davies; J.D.Donaldson (1968). "Tin(II) perchlorate trihydrate". Journal of Inorganic and Nuclear Chemistry. 30 (10). Chelsea College of Science and Technology: 2635–2639. doi:10.1016/0022-1902(68)80389-6.
  15. ^ Franco Cristiani; Francesco Demartin; Francesco A. Devillanova; Angelo Diaz; Francesco Isaia; Gaetano Verani (1990). "Reactivity of Mercury(II) Perchlorate Towards 5,5 -Dimethylimidazolidine-2- Thione-4-One. Structure of Bis(5,5-Dimethylimidazolidine-2-Thione-4-One)Mercury(II) Perchlorate Triaquo". Journal of Coordination Chemistry. 21 (2): 137–146. doi:10.1080/00958979009409182.
  16. ^ "Properties of substance: mercury(II) oxalate Group of substances:". Chemister. Chemister. Retrieved 13 September 2022.
  17. ^ Burkhart, M J; Newton, T W (1969). "THE KINETICS OF THE REACTION BETWEEN VANADIUM(II) AND NEPTUNIUM(IV) IN AQUEOUS PERCHLORATE SOLUTIONS". J. Phys. Chem. 73 (6): 1741–1746. doi:10.1021/j100726a018.
  18. ^ "Iron (III) Carbonate Formula". softschools.com. p. 1. Retrieved 19 August 2022.
Retrieved from "https://en.wikipedia.org/w/index.php?title=Solubility_chart&oldid=1140168771"