Ionic compound having highest solubility in water












3














Which ionic compound has highest solubility in water? I can find CsBr having highest solubility with 1230 g/L at 25 ℃.



Note: compounds like ethanol are soluble to any extent in water, but they are covalent, not ionic.






inorganic-chemistry aqueous-solution solubility solutions liquids







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  • 2




    It would be interesting to split in the two cases of molar solubility and mass solubility, though the latter is easier to find data on directly.
    – Nicolau Saker Neto
    5 hours ago
















3














Which ionic compound has highest solubility in water? I can find CsBr having highest solubility with 1230 g/L at 25 ℃.



Note: compounds like ethanol are soluble to any extent in water, but they are covalent, not ionic.






inorganic-chemistry aqueous-solution solubility solutions liquids







share|improve this question




















  • 2




    It would be interesting to split in the two cases of molar solubility and mass solubility, though the latter is easier to find data on directly.
    – Nicolau Saker Neto
    5 hours ago














3












3








3







Which ionic compound has highest solubility in water? I can find CsBr having highest solubility with 1230 g/L at 25 ℃.



Note: compounds like ethanol are soluble to any extent in water, but they are covalent, not ionic.






inorganic-chemistry aqueous-solution solubility solutions liquids







share|improve this question















Which ionic compound has highest solubility in water? I can find CsBr having highest solubility with 1230 g/L at 25 ℃.



Note: compounds like ethanol are soluble to any extent in water, but they are covalent, not ionic.






inorganic-chemistry aqueous-solution solubility solutions liquids




inorganic-chemistry aqueous-solution solubility solutions liquids






share|improve this question















share|improve this question













share|improve this question




share|improve this question








edited 2 hours ago









andselisk

13.9k648103




13.9k648103










asked 6 hours ago









Harsh jainHarsh jain

5931514




5931514








  • 2




    It would be interesting to split in the two cases of molar solubility and mass solubility, though the latter is easier to find data on directly.
    – Nicolau Saker Neto
    5 hours ago














  • 2




    It would be interesting to split in the two cases of molar solubility and mass solubility, though the latter is easier to find data on directly.
    – Nicolau Saker Neto
    5 hours ago








2




2




It would be interesting to split in the two cases of molar solubility and mass solubility, though the latter is easier to find data on directly.
– Nicolau Saker Neto
5 hours ago




It would be interesting to split in the two cases of molar solubility and mass solubility, though the latter is easier to find data on directly.
– Nicolau Saker Neto
5 hours ago










3 Answers
3






active

oldest

votes


















3














There is not going to be a single definitive answer, primarily because of a wide gray zone surrounding the domain of ionic compounds. Besides, as Nikolau noted, the question is ambiguous.



If you want mass concentration, then look at $ce{InI3}$ which claims a whopping $13100~mathrm{g/L}$. Pity that it is probably ionic in name only, judging by the solubility in non-polar solvents. Well, then look at those mentioned by andselisk, though the ionic nature of some of them is also debatable, and then at the thallium formate (a component of Clerici solution) with $sim5000~mathrm{g/L}$.



If you want molar concentration, then the question is still ambiguous (are we looking at molarity or molality?), and the pretty strong contenders are $ce{NaOH}$, $ce{BeF2}$, $ce{LiClO3}$.



So it goes.






share|improve this answer





















  • True, $ce{InI3}$ is weird, but it's definitely not ionic and the reference for the solubility value dates back to 1940s or something:)
    – andselisk
    1 hour ago





















3














The following data is compiled from [1, pp. 4-44, 5-167]:



Table 1. Selected solubility values of the inorganic compounds with significant ionic character at $25~mathrm{^circ C}$.
$$
begin{array}{lc}
hline
text{Formula} & text{Solubility in water}/pu{g L-1}\
hline
ce{CsF} & 5730\
ce{SbF3} & 4920\
ce{LiClO3} & 4587\
ce{Pb(ClO4)2} & 4405\
ce{ZnCl2} & 4080\
hline
end{array}
$$



Solubility of antimony(III) trichloride $ce{SbCl3}$ is $9870~mathrm{g~L^{-1}}$ at $25~mathrm{^circ C}$, but technically it's not an ionic compound.



References




  1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97.






share|improve this answer























  • I've seen antimony trichloride before in tables, but it is apparently very easily hydrolysed, so perhaps it shouldn't be counted either way.
    – Nicolau Saker Neto
    31 mins ago










  • @NicolauSakerNeto Yep, you are right, and the same probably goes for $ce{ZnCl2}$. I also omitted $ce{ZnBr2}$ for similar reason (and it's covalency, too).
    – andselisk
    29 mins ago





















2














We can do better than that. Ammonium nitrate = 1500 g/L at 20°C.






share|improve this answer





















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    3 Answers
    3






    active

    oldest

    votes








    3 Answers
    3






    active

    oldest

    votes









    active

    oldest

    votes






    active

    oldest

    votes









    3














    There is not going to be a single definitive answer, primarily because of a wide gray zone surrounding the domain of ionic compounds. Besides, as Nikolau noted, the question is ambiguous.



    If you want mass concentration, then look at $ce{InI3}$ which claims a whopping $13100~mathrm{g/L}$. Pity that it is probably ionic in name only, judging by the solubility in non-polar solvents. Well, then look at those mentioned by andselisk, though the ionic nature of some of them is also debatable, and then at the thallium formate (a component of Clerici solution) with $sim5000~mathrm{g/L}$.



    If you want molar concentration, then the question is still ambiguous (are we looking at molarity or molality?), and the pretty strong contenders are $ce{NaOH}$, $ce{BeF2}$, $ce{LiClO3}$.



    So it goes.






    share|improve this answer





















    • True, $ce{InI3}$ is weird, but it's definitely not ionic and the reference for the solubility value dates back to 1940s or something:)
      – andselisk
      1 hour ago


















    3














    There is not going to be a single definitive answer, primarily because of a wide gray zone surrounding the domain of ionic compounds. Besides, as Nikolau noted, the question is ambiguous.



    If you want mass concentration, then look at $ce{InI3}$ which claims a whopping $13100~mathrm{g/L}$. Pity that it is probably ionic in name only, judging by the solubility in non-polar solvents. Well, then look at those mentioned by andselisk, though the ionic nature of some of them is also debatable, and then at the thallium formate (a component of Clerici solution) with $sim5000~mathrm{g/L}$.



    If you want molar concentration, then the question is still ambiguous (are we looking at molarity or molality?), and the pretty strong contenders are $ce{NaOH}$, $ce{BeF2}$, $ce{LiClO3}$.



    So it goes.






    share|improve this answer





















    • True, $ce{InI3}$ is weird, but it's definitely not ionic and the reference for the solubility value dates back to 1940s or something:)
      – andselisk
      1 hour ago
















    3












    3








    3






    There is not going to be a single definitive answer, primarily because of a wide gray zone surrounding the domain of ionic compounds. Besides, as Nikolau noted, the question is ambiguous.



    If you want mass concentration, then look at $ce{InI3}$ which claims a whopping $13100~mathrm{g/L}$. Pity that it is probably ionic in name only, judging by the solubility in non-polar solvents. Well, then look at those mentioned by andselisk, though the ionic nature of some of them is also debatable, and then at the thallium formate (a component of Clerici solution) with $sim5000~mathrm{g/L}$.



    If you want molar concentration, then the question is still ambiguous (are we looking at molarity or molality?), and the pretty strong contenders are $ce{NaOH}$, $ce{BeF2}$, $ce{LiClO3}$.



    So it goes.






    share|improve this answer












    There is not going to be a single definitive answer, primarily because of a wide gray zone surrounding the domain of ionic compounds. Besides, as Nikolau noted, the question is ambiguous.



    If you want mass concentration, then look at $ce{InI3}$ which claims a whopping $13100~mathrm{g/L}$. Pity that it is probably ionic in name only, judging by the solubility in non-polar solvents. Well, then look at those mentioned by andselisk, though the ionic nature of some of them is also debatable, and then at the thallium formate (a component of Clerici solution) with $sim5000~mathrm{g/L}$.



    If you want molar concentration, then the question is still ambiguous (are we looking at molarity or molality?), and the pretty strong contenders are $ce{NaOH}$, $ce{BeF2}$, $ce{LiClO3}$.



    So it goes.







    share|improve this answer












    share|improve this answer



    share|improve this answer










    answered 1 hour ago









    Ivan NeretinIvan Neretin

    22.9k34685




    22.9k34685












    • True, $ce{InI3}$ is weird, but it's definitely not ionic and the reference for the solubility value dates back to 1940s or something:)
      – andselisk
      1 hour ago




















    • True, $ce{InI3}$ is weird, but it's definitely not ionic and the reference for the solubility value dates back to 1940s or something:)
      – andselisk
      1 hour ago


















    True, $ce{InI3}$ is weird, but it's definitely not ionic and the reference for the solubility value dates back to 1940s or something:)
    – andselisk
    1 hour ago






    True, $ce{InI3}$ is weird, but it's definitely not ionic and the reference for the solubility value dates back to 1940s or something:)
    – andselisk
    1 hour ago













    3














    The following data is compiled from [1, pp. 4-44, 5-167]:



    Table 1. Selected solubility values of the inorganic compounds with significant ionic character at $25~mathrm{^circ C}$.
    $$
    begin{array}{lc}
    hline
    text{Formula} & text{Solubility in water}/pu{g L-1}\
    hline
    ce{CsF} & 5730\
    ce{SbF3} & 4920\
    ce{LiClO3} & 4587\
    ce{Pb(ClO4)2} & 4405\
    ce{ZnCl2} & 4080\
    hline
    end{array}
    $$



    Solubility of antimony(III) trichloride $ce{SbCl3}$ is $9870~mathrm{g~L^{-1}}$ at $25~mathrm{^circ C}$, but technically it's not an ionic compound.



    References




    1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97.






    share|improve this answer























    • I've seen antimony trichloride before in tables, but it is apparently very easily hydrolysed, so perhaps it shouldn't be counted either way.
      – Nicolau Saker Neto
      31 mins ago










    • @NicolauSakerNeto Yep, you are right, and the same probably goes for $ce{ZnCl2}$. I also omitted $ce{ZnBr2}$ for similar reason (and it's covalency, too).
      – andselisk
      29 mins ago


















    3














    The following data is compiled from [1, pp. 4-44, 5-167]:



    Table 1. Selected solubility values of the inorganic compounds with significant ionic character at $25~mathrm{^circ C}$.
    $$
    begin{array}{lc}
    hline
    text{Formula} & text{Solubility in water}/pu{g L-1}\
    hline
    ce{CsF} & 5730\
    ce{SbF3} & 4920\
    ce{LiClO3} & 4587\
    ce{Pb(ClO4)2} & 4405\
    ce{ZnCl2} & 4080\
    hline
    end{array}
    $$



    Solubility of antimony(III) trichloride $ce{SbCl3}$ is $9870~mathrm{g~L^{-1}}$ at $25~mathrm{^circ C}$, but technically it's not an ionic compound.



    References




    1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97.






    share|improve this answer























    • I've seen antimony trichloride before in tables, but it is apparently very easily hydrolysed, so perhaps it shouldn't be counted either way.
      – Nicolau Saker Neto
      31 mins ago










    • @NicolauSakerNeto Yep, you are right, and the same probably goes for $ce{ZnCl2}$. I also omitted $ce{ZnBr2}$ for similar reason (and it's covalency, too).
      – andselisk
      29 mins ago
















    3












    3








    3






    The following data is compiled from [1, pp. 4-44, 5-167]:



    Table 1. Selected solubility values of the inorganic compounds with significant ionic character at $25~mathrm{^circ C}$.
    $$
    begin{array}{lc}
    hline
    text{Formula} & text{Solubility in water}/pu{g L-1}\
    hline
    ce{CsF} & 5730\
    ce{SbF3} & 4920\
    ce{LiClO3} & 4587\
    ce{Pb(ClO4)2} & 4405\
    ce{ZnCl2} & 4080\
    hline
    end{array}
    $$



    Solubility of antimony(III) trichloride $ce{SbCl3}$ is $9870~mathrm{g~L^{-1}}$ at $25~mathrm{^circ C}$, but technically it's not an ionic compound.



    References




    1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97.






    share|improve this answer














    The following data is compiled from [1, pp. 4-44, 5-167]:



    Table 1. Selected solubility values of the inorganic compounds with significant ionic character at $25~mathrm{^circ C}$.
    $$
    begin{array}{lc}
    hline
    text{Formula} & text{Solubility in water}/pu{g L-1}\
    hline
    ce{CsF} & 5730\
    ce{SbF3} & 4920\
    ce{LiClO3} & 4587\
    ce{Pb(ClO4)2} & 4405\
    ce{ZnCl2} & 4080\
    hline
    end{array}
    $$



    Solubility of antimony(III) trichloride $ce{SbCl3}$ is $9870~mathrm{g~L^{-1}}$ at $25~mathrm{^circ C}$, but technically it's not an ionic compound.



    References




    1. Haynes, W. M.; Lide, D. R.; Bruno, T. J. CRC Handbook of Chemistry and Physics: A Ready-Reference Book of Chemical and Physical Data.; 2017; Vol. 97.







    share|improve this answer














    share|improve this answer



    share|improve this answer








    edited 1 hour ago

























    answered 2 hours ago









    andseliskandselisk

    13.9k648103




    13.9k648103












    • I've seen antimony trichloride before in tables, but it is apparently very easily hydrolysed, so perhaps it shouldn't be counted either way.
      – Nicolau Saker Neto
      31 mins ago










    • @NicolauSakerNeto Yep, you are right, and the same probably goes for $ce{ZnCl2}$. I also omitted $ce{ZnBr2}$ for similar reason (and it's covalency, too).
      – andselisk
      29 mins ago




















    • I've seen antimony trichloride before in tables, but it is apparently very easily hydrolysed, so perhaps it shouldn't be counted either way.
      – Nicolau Saker Neto
      31 mins ago










    • @NicolauSakerNeto Yep, you are right, and the same probably goes for $ce{ZnCl2}$. I also omitted $ce{ZnBr2}$ for similar reason (and it's covalency, too).
      – andselisk
      29 mins ago


















    I've seen antimony trichloride before in tables, but it is apparently very easily hydrolysed, so perhaps it shouldn't be counted either way.
    – Nicolau Saker Neto
    31 mins ago




    I've seen antimony trichloride before in tables, but it is apparently very easily hydrolysed, so perhaps it shouldn't be counted either way.
    – Nicolau Saker Neto
    31 mins ago












    @NicolauSakerNeto Yep, you are right, and the same probably goes for $ce{ZnCl2}$. I also omitted $ce{ZnBr2}$ for similar reason (and it's covalency, too).
    – andselisk
    29 mins ago






    @NicolauSakerNeto Yep, you are right, and the same probably goes for $ce{ZnCl2}$. I also omitted $ce{ZnBr2}$ for similar reason (and it's covalency, too).
    – andselisk
    29 mins ago













    2














    We can do better than that. Ammonium nitrate = 1500 g/L at 20°C.






    share|improve this answer


























      2














      We can do better than that. Ammonium nitrate = 1500 g/L at 20°C.






      share|improve this answer
























        2












        2








        2






        We can do better than that. Ammonium nitrate = 1500 g/L at 20°C.






        share|improve this answer












        We can do better than that. Ammonium nitrate = 1500 g/L at 20°C.







        share|improve this answer












        share|improve this answer



        share|improve this answer










        answered 5 hours ago









        Oscar LanziOscar Lanzi

        14.8k12646




        14.8k12646






























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