E3: Solubility Constants for Compounds at 25°C
- Page ID
- 9065
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Although all compounds have a characteristic solubility in water at a given temperature, some families of compounds are more soluble than others and it is useful to know certain general rules of solubility. We call any substance insoluble its solubility is less than 0.01 mol/L. If its solubility is greater than 0.1 mol/L, we call it soluble. If its solubility is between 0.01 and 0.1 mol/L, we say that it is slightly soluble. The following solubility rules can be used to determine solubilities in water, with the disclaimer that they don't always hold, nor do they include every ion which is in common use, but they are good to have nearby when needed:
- All sodium, potassium, and ammonium salts are soluble.
- All nitrates, acetates and perchlorates are soluble.
- All silver, lead and mercury(I) salts are insoluble.
- All chlorides, bromides and iodides are soluble.
- All carbonates, sulfides, oxides and hydroxides are insoluble.
- All sulfates are soluble except strontium sulfate and barium sulfate.
| Compound Name | Compound Formula | Ksp |
|---|---|---|
| Aluminum phosphate | AlPO4 | 9.84 × 10−21 |
| Barium bromate | Ba(BrO3)2 | 2.43 × 10−4 |
| Barium carbonate | BaCO3 | 2.58 × 10−9 |
| Barium chromate | BaCrO4 | 1.17 × 10−10 |
| Barium fluoride | BaF2 | 1.84 × 10−7 |
| Barium iodate | Ba(IO3)2 | 4.01 × 10−9 |
| Barium nitrate | Ba(NO3)2 | 4.64 × 10−3 |
| Barium sulfate | BaSO4 | 1.08 × 10−10 |
| Barium sulfite | BaSO3 | 5.0 × 10−10 |
| Beryllium hydroxide | Be(OH)2 | 6.92 × 10−22 |
| Bismuth arsenate | BiAsO4 | 4.43 × 10−10 |
| Bismuth iodide | BiI3 | 7.71 × 10−19 |
| Cadmium carbonate | CdCO3 | 1.0 × 10−12 |
| Cadmium fluoride | CdF2 | 6.44 × 10−3 |
| Cadmium hydroxide | Cd(OH)2 | 7.2 × 10−15 |
| Cadmium iodate | Cd(IO3)2 | 2.5 × 10−8 |
| Cadmium phosphate | Cd3(PO4)2 | 2.53 × 10−33 |
| Cadmium sulfide | CdS | 8.0 × 10−27 |
| Calcium carbonate | CaCO3 | 3.36 × 10−9 |
| Calcium fluoride | CaF2 | 3.45 × 10−11 |
| Calcium hydroxide | Ca(OH)2 | 5.02 × 10−6 |
| Calcium iodate | Ca(IO3)2 | 6.47 × 10−6 |
| Calcium phosphate | Ca3(PO4)2 | 2.07 × 10−33 |
| Calcium sulfate | CaSO4 | 4.93 × 10−5 |
| Cesium perchlorate | CsClO4 | 3.95 × 10−3 |
| Cesium periodate | CsIO4 | 5.16 × 10−6 |
| Cobalt(II) arsenate | Co3(AsO4)2 | 6.80 × 10−29 |
| Cobalt(II) hydroxide | Co(OH)2 | 5.92 × 10−15 |
| Cobalt(II) phosphate | Co3(PO4)2 | 2.05 × 10−35 |
| Copper(I) bromide | CuBr | 6.27 × 10−9 |
| Copper(I) chloride | CuCl | 1.72 × 10−7 |
| Copper(I) cyanide | CuCN | 3.47 × 10−20 |
| Copper(I) iodide | CuI | 1.27 × 10−12 |
| Copper(I) thiocyanate | CuSCN | 1.77 × 10−13 |
| Copper(II) arsenate | Cu3(AsO4)2 | 7.95 × 10−36 |
| Copper(II) oxalate | CuC2O4 | 4.43 × 10−10 |
| Copper(II) phosphate | Cu3(PO4)2 | 1.40 × 10−37 |
| Copper(II) sulfide | CuS | 6.3 × 10−36 |
| Europium(III) hydroxide | Eu(OH)3 | 9.38 × 10−27 |
| Gallium(III) hydroxide | Ga(OH)3 | 7.28 × 10−36 |
| Iron(II) carbonate | FeCO3 | 3.13 × 10−11 |
| Iron(II) fluoride | FeF2 | 2.36 × 10−6 |
| Iron(II) hydroxide | Fe(OH)2 | 4.87 × 10−17 |
| Iron(III) hydroxide | Fe(OH)3 | 2.79 × 10−39 |
| Iron(III) sulfide | FeS | 6.3 × 10−18 |
| Lanthanum iodate | La(IO3)3 | 7.50 × 10−12 |
| Lead(II) bromide | PbBr2 | 6.60 × 10−6 |
| Lead(II) carbonate | PbCO3 | 7.40 × 10−14 |
| Lead(II) chloride | PbCl2 | 1.70 × 10−5 |
| Lead(II) fluoride | PbF2 | 3.3 × 10−8 |
| Lead(II) hydroxide | Pb(OH)2 | 1.43 × 10−20 |
| Lead(II) iodate | Pb(IO3)2 | 3.69 × 10−13 |
| Lead(II) iodide | PbI2 | 9.8 × 10−9 |
| Lead(II)selenite | PbSeO4 | 1.37 × 10−7 |
| Lead(II) sulfate | PbSO4 | 2.53 × 10−8 |
| Lead(II) sulfide | PbS | 8.0 × 10−28 |
| Lithium carbonate | Li2CO3 | 8.15 × 10−4 |
| Lithium fluoride | LiF | 1.84 × 10−3 |
| Lithium phosphate | Li3PO4 | 2.37 × 10−11 |
| Magnesium carbonate | MgCO3 | 6.82 × 10−6 |
| Magnesium fluoride | MgF2 | 5.16 × 10−11 |
| Magnesium hydroxide | Mg(OH)2 | 5.61 × 10−12 |
| Magnesium phosphate | Mg3(PO4)2 | 1.04 × 10−24 |
| Manganese(II) carbonate | MnCO3 | 2.24 × 10−11 |
| Manganese(II) iodate | Mn(IO3)2 | 4.37 × 10−7 |
| Mercury(I) bromide | Hg2Br2 | 6.40 × 10−23 |
| Mercury(I) carbonate | Hg2CO3 | 3.6 × 10−17 |
| Mercury(I) chloride | Hg2Cl2 | 1.43 × 10−18 |
| Mercury(I) fluoride | Hg2F2 | 3.10 × 10−6 |
| Mercury(I) iodide | Hg2I2 | 5.2 × 10−29 |
| Mercury(I) oxalate | Hg2C2O4 | 1.75 × 10−13 |
| Mercury(I) sulfate | Hg2SO4 | 6.5 × 10−7 |
| Mercury(I) thiocyanate | Hg2(SCN)2 | 3.2 × 10−20 |
| Mercury(II) bromide | HgBr2 | 6.2 × 10−20 |
| Mercury (II) iodide | HgI2 | 2.9 × 10−29 |
| Mercury(II) sulfide (red) | HgS | 4 × 10−53 |
| Mercury(II) sulfide (black) | HgS | 1.6 × 10−52 |
| Neodymium carbonate | Nd2(CO3)3 | 1.08 × 10−33 |
| Nickel(II) carbonate | NiCO3 | 1.42 × 10−7 |
| Nickel(II) hydroxide | Ni(OH)2 | 5.48 × 10−16 |
| Nickel(II) iodate | Ni(IO3)2 | 4.71 × 10−5 |
| Nickel(II) phosphate | Ni3(PO4)2 | 4.74 × 10−32 |
| Palladium(II) thiocyanate | Pd(SCN)2 | 4.39 × 10−23 |
| Potassium hexachloroplatinate | K2PtCl6 | 7.48 × 10−6 |
| Potassium perchlorate | KClO4 | 1.05 × 10−2 |
| Potassium periodate | KIO4 | 3.71 × 10−4 |
| Praseodymium hydroxide | Pr(OH)3 | 3.39 × 10−24 |
| Rubidium perchlorate | RbClO4 | 3.00 × 10−3 |
| Scandium fluoride | ScF3 | 5.81 × 10−24 |
| Scandium hydroxide | Sc(OH)3 | 2.22 × 10−31 |
| Silver(I) acetate | AgCH3CO2 | 1.94 × 10−3 |
| Silver(I) arsenate | Ag3AsO4 | 1.03 × 10−22 |
| Silver(I) bromate | AgBrO3 | 5.38 × 10−5 |
| Silver(I) bromide | AgBr | 5.35 × 10−13 |
| Silver(I) carbonate | Ag2CO3 | 8.46 × 10−12 |
| Silver(I) chloride | AgCl | 1.77 × 10−10 |
| Silver(I) chromate | Ag2CrO4 | 1.12 × 10−12 |
| Silver(I) cyanide | AgCN | 5.97 × 10−17 |
| Silver(I) iodate | AgIO3 | 3.17 × 10−8 |
| Silver(I) iodide | AgI | 8.52 × 10−17 |
| Silver(I) oxalate | Ag2C2O4 | 5.40 × 10−12 |
| Silver(I) phosphate | Ag3PO4 | 8.89 × 10−17 |
| Silver(I) sulfate | Ag2SO4 | 1.20 × 10−5 |
| Silver(I) sulfide | Ag2S | 6.3 × 10−50 |
| Silver(I) sulfite | Ag2SO3 | 1.50 × 10−14 |
| Silver(I) thiocyanate | AgSCN | 1.03 × 10−12 |
| Strontium arsenate | Sr3(AsO4)2 | 4.29 × 10−19 |
| Strontium carbonate | SrCO3 | 5.60 × 10−10 |
| Strontium fluoride | SrF2 | 4.33 × 10−9 |
| Strontium iodate | Sr(IO3)2 | 1.14 × 10−7 |
| Strontium sulfate | SrSO4 | 3.44 × 10−7 |
| Thallium(I) bromate | TlBrO3 | 1.10 × 10−4 |
| Thallium(I) bromide | TlBr | 3.71 × 10−6 |
| Thallium(I) chloride | TlCl | 1.86 × 10−4 |
| Thallium(I) chromate | Tl2CrO4 | 8.67 × 10−13 |
| Thallium(I) iodate | TlIO3 | 3.12 × 10−6 |
| Thallium(I) iodide | TlI | 5.54 × 10−8 |
| Thallium(I) thiocyanate | TlSCN | 1.57 × 10−4 |
| Thallium(III) hydroxide | Tl(OH)3 | 1.68 × 10−44 |
| Tin(II) hydroxide | Sn(OH)2 | 5.45 × 10−27 |
| Tin(II) sulfide | SnS | 1.0 × 10−25 |
| Yttrium carbonate | Y2(CO3)3 | 1.03 × 10−31 |
| Yttrium fluoride | YF3 | 8.62 × 10−21 |
| Yttrium hydroxide | Y(OH)3 | 1.00 × 10−22 |
| Yttrium iodate | Y(IO3)3 | 1.12 × 10−10 |
| Zinc arsenate | Zn3(AsO4)2 | 2.8 × 10−28 |
| Zinc carbonate | ZnCO3 | 1.46 × 10−10 |
| Zinc fluoride | ZnF2 | 3.04 × 10−2 |
| Zinc hydroxide | Zn(OH)2 | 3 × 10−17 |
| Zinc selenide | ZnSe | 3.6 × 10−26 |
| Zinc sulfide (wurtzite) | ZnS | 1.6 × 10−24 |
| Zinc sulfide (sphalerite) | ZnS | 2.5 × 10−22 |
Source of data: CRC Handbook of Chemistry and Physics, 84th Edition (2004); sulfide data from Lange’s Handbook of Chemistry, 15th Edition (1999).