Solubility

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Author:
chemer
ID:
136926
Filename:
Solubility
Updated:
2012-02-22 03:40:24
Tags:
Midterm
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Description:
How to tell what compounds will dissociate into.
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  1. Na+, K+, and NH4+
    • form soluble ionic compounds
    • ex: NaCl, KNO3, and (NH4)2CO3
  2. nitrate ion (NO3-)
    • forms soluble ionic compounds
    • ex. Cu(NO3)2 and Fe(NO3)3
  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.
  4. 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.
  5. sulfides (S2-)
    • usually insoluble
    • exceptions: Na2S, K2S, (NH4)2S, MgS, CaS, SrS, and BaS
  6. oxides (O2-)
    • usually insoluble
    • exceptions: Na2O, K2O, SrO, and BaO, which are soluble and CaO which is slightly soluble
  7. 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
  8. chromates (CrO42-)
    usually insoluble
  9. phosphates (PO43-)
    usually insoluble
  10. carbonates (CO32-)
    usually insoluble

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