Are most halide salts soluble in water

1. Salts containing Group I elements are soluble (Li+, Na+, K+, Cs+, Rb+). Exceptions to this rule are rare. Salts containing the ammonium ion (NH4+) are also soluble.
2. Salts containing nitrate ion (NO3-) are generally soluble.
3. Salts containing Cl -, Br -, I - are generally soluble. Important exceptions to this rule are halide salts of Ag+, Pb2+, and (Hg2)2+. Thus, AgCl, PbBr2, and Hg2Cl2 are all insoluble.
4. Most silver salts are insoluble. AgNO3 and Ag(C2H3O2) are common soluble salts of silver; virtually anything else is insoluble.
5. Most sulfate salts are soluble. Important exceptions to this rule include BaSO4, PbSO4, Ag2SO4 and SrSO4 .
6. Most hydroxide salts are only slightly soluble. Hydroxide salts of Group I elements are soluble. Hydroxide salts of Group II elements (Ca, Sr, and Ba) are slightly soluble. Hydroxide salts of transition metals and Al3+ are insoluble. Thus, Fe(OH)3, Al(OH)3, Co(OH)2 are not soluble.
7. Most sulfides of transition metals are highly insoluble. Thus, CdS, FeS, ZnS, Ag2S are all insoluble. Arsenic, antimony, bismuth, and lead sulfides are also insoluble.
8. Carbonates are frequently insoluble. Group II carbonates (Ca, Sr, and Ba) are insoluble. Some other insoluble carbonates include FeCO3 and PbCO3.
9. Chromates are frequently insoluble. Examples: PbCrO4, BaCrO4
10. Phosphates are frequently insoluble. Examples: Ca3(PO4)2, Ag3PO4
11. Fluorides are frequently insoluble. Examples: BaF2, MgF2 PbF2.

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    Are most halide salts soluble in water

  • Start by writing the chemical formulas of the reactants and of the products.

    • #"lead(II) nitrate " -> " Pb"("NO"_3)_2#
    • #"potassium iodide " -> " KI"#
    • #"lead(II) iodide " -> " PbI"_2#
    • #"potassium nitrate " -> " KNO"_3#

    Now, your reaction takes place in aqueous solutions. Three of the four chemical species involved in the reaction will be in the aqueous state, #"(aq)"#, and one, potassium iodide, will be in the solid state, #"(s)"#.

    The unbalanced chemical equation looks like this

    #"Pb"("NO"_ 3)_ (2(aq)) + "KI"_ ((aq)) -> "PbI"_ (2(s)) darr + "KNO"_ (3(aq))#

    To balance this chemical equation, multiply the potassium iodide by #2# and the potassium nitrate by #2#.

    You will end up with

    #"Pb"("NO"_ 3)_ (2(aq)) + 2"KI"_ ((aq)) -> "PbI"_ (2(s)) darr + 2"KNO"_ (3(aq))#

    If you want, you can write the complete ionic equation by breaking up the soluble compounds, i.e. the ones that are in the aqueous state, into their respective cations and anions

    #"Pb"_ ((aq))^(2+) + 2"NO"_ (3(aq))^(-) + 2"K"_ ((aq))^(+) + 2"I"_ ((aq))^(-) -> "PbI"_ (2(s)) darr + 2"K"_ ((aq))^(+) + 2"NO"_ (3(aq))^(-)#

    If you eliminate the spectator ions, i.e. the ions that are present on both sides of the equation

    #"Pb"_ ((aq))^(2+) + color(red)(cancel(color(black)(2"NO"_ (3(aq))^(-)))) + color(red)(cancel(color(black)(2"K"_ ((aq))^(+)))) + 2"I"_ ((aq))^(-) -> "PbI"_ (2(s)) darr + color(red)(cancel(color(black)(2"K"_ ((aq))^(+)))) + color(red)(cancel(color(black)(2"NO"_ (3(aq))^(-))))#

    you will get the net ionic equation

    #"Pb"_ ((aq))^(2+) + 2"I"_ ((aq))^(-) -> "PbI"_ (2(s)) darr#

    Lead(II) iodide is a yellow insoluble solid that precipitates out of the solution.

    Are most halide salts soluble in water

    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 symbolsFluoride
    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
    2
    H
    3
    O
    2
    Carbonate
    CO2−
    3
    [a]
    Sulfate
    SO2−
    4
    Oxalate
    C
    2
    O2−
    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
    Manganese(II) Mn2+sS S S S I I I S I S[6] 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[7] 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 R S I I
    Zinc Zn2+sS S S S I I I I S S[8] S S I S I I
    Tin(II) Sn2+S S S S I I I ? I[9] S[10] S R I S sS I
    Mercury(II) Hg2+R S S I I I I S sS S[11] S S I R sS[12] 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[13] 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[c] S S R I I I S S S S I R[14] 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
    2
    H
    3
    O
    2
    Carbonate
    CO2−
    3
    [a]
    Sulfate
    SO2−
    4
    Oxalate
    C
    2
    O2−
    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[edit]

    • Solubility rules

    Notes[edit]

    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. ^ Anhydrous FeF3 is slightly soluble in water, FeF3·3H2O is much more soluble in water.

    References[edit]

    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. ^ "44318 Manganese(II) perchlorate hexahydrate, 99.995% (metals basis)". Alfa Aesar. Alfa Aesar. Retrieved 16 September 2022.
    7. ^ 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.
    8. ^ 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.
    9. ^ 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.
    10. ^ C.G.Davies; J.D.Donaldson (1968). "Tin(II) perchlorate trihydrate". Journal of Inorganic and Nuclear Chemistry. Chelsea College of Science and Technology. 30 (10): 2635–2639. doi:10.1016/0022-1902(68)80389-6.
    11. ^ 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.
    12. ^ "Properties of substance: mercury(II) oxalate Group of substances:". Chemister. Chemister. Retrieved 13 September 2022.
    13. ^ 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.
    14. ^ "Iron (III) Carbonate Formula". softschools.com. p. 1. Retrieved 19 August 2022.

    Are halide salts soluble in water?

    Halides exist in natural water sources, such as rivers, lakes, and streams, due to their high solubility in water.

    Are halides generally soluble or insoluble?

    All NITRATES are soluble; and ALL halides are soluble EXCEPT for those of Pb2+ , Hg2+2 , mercurous ion , and Ag+ in aqueous solution.

    Which halide is most soluble?

    Therefore, the most soluble halide in water is Silver fluoride .

    Are most nitrate salts soluble in water?

    The nitrates, chlorates, and acetates of all metals are soluble in water.