-
Na+, K+, and NH4+
- form soluble ionic compounds
- ex: NaCl, KNO3, and (NH4)2CO3
-
nitrate ion (NO3-)
- forms soluble ionic compounds
- ex. Cu(NO3)2 and Fe(NO3)3
-
chloride (Cl-), bromide (Br-), and iodide (I-) ions
- usually form soluble ionic compounds
- exceptions: Pb2+, Hg22+, Ag+, and Cu+ ions
- ex: CuBr2 is soluble but CuBr is not.
-
sulfate ion SO42+
- usually forms soluble ionic compounds
- exceptions: BaSO4, SrSO4, and PbSO4 which are insoluble and Ag2SO4, CaSO4, and Hg2SO4 which are slightly soluble.
-
sulfides (S2-)
- usually insoluble
- exceptions: Na2S, K2S, (NH4)2S, MgS, CaS, SrS, and BaS
-
oxides (O2-)
- usually insoluble
- exceptions: Na2O, K2O, SrO, and BaO, which are soluble and CaO which is slightly soluble
-
hydroxides (OH-)
- usually insoluble
- exceptions: NaOH, KOH, Sr(OH)2, and Ba(OH)2 which are soluble and Ca(OH)2 which is slightly soluble
-
chromates (CrO42-)
usually insoluble
-
phosphates (PO43-)
usually insoluble
-
carbonates (CO32-)
usually insoluble
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