Solubility Guidelines and Strong Acids

Vocabulary practice flashcards covering aqueous solubility guidelines for soluble and insoluble compounds, insoluble/soluble exceptions, and strong acids with their complete ionization equations.

Hydrochloric acid ($HCl$)

A strong acid that completely ionizes in aqueous solution according to the equation $HCl(aq) \rightarrow H^+(aq) + Cl^-(aq)$.

Hydrobromic acid ($HBr$)

A strong acid that completely ionizes in aqueous solution according to the equation $HBr(aq) \rightarrow H^+(aq) + Br^-(aq)$.

Hydroiodic acid ($HI$)

A strong acid that completely ionizes in aqueous solution according to the equation $HI(aq) \rightarrow H^+(aq) + I^-(aq)$.

Nitric acid ($HNO_3$)

A strong acid that completely ionizes in aqueous solution according to the equation $HNO_3(aq) \rightarrow H^+(aq) + NO_3^-(aq)$.

Chloric acid ($HClO_3$)

A strong acid that completely ionizes in aqueous solution according to the equation $HClO_3(aq) \rightarrow H^+(aq) + ClO_3^-(aq)$.

Perchloric acid ($HClO_4$)

A strong acid that completely ionizes in aqueous solution according to the equation $HClO_4(aq) \rightarrow H^+(aq) + ClO_4^-(aq)$.

Sulfuric acid ($H_2SO_4$)

A strong diprotic acid whose first ionization is complete ($H_2SO_4(aq) \rightarrow H^+(aq) + HSO_4^-(aq)$), while its second ionization occurs only to a very small extent ($HSO_4^-(aq) \rightleftharpoons H^+(aq) + SO_4^{2-}(aq)$).

Additional Strong Acids ($+3\text{ more}$)

The three strong acids noted alongside the standard seven: selenic acid ($H_2SeO_4$), perbromic acid ($HBrO_4$), and bromic acid ($HBrO_3$).

Weak Acids

All acids other than the identified 7 (+3 more) strong acids, which do not ionize completely in aqueous solution.

Alkali Metal and Ammonium Compounds

Water-soluble compounds containing an alkali metal cation ($Li^+$, $Na^+$, $K^+$, $Rb^+$, $Cs^+$) or the ammonium ion ($NH_4^+$), with no insoluble exceptions.

Nitrate, Acetate, Chlorate, and Perchlorate Compounds

Water-soluble compounds containing $NO_3^-$, $C_2H_3O_2^-$, $ClO_3^-$, or $ClO_4^-$, with no insoluble exceptions.

Chloride, Bromide, and Iodide Compounds

Water-soluble halide compounds ($Cl^-$, $Br^-$, $I^-$), except when paired with $Ag^+$, $Hg_2^{2+}$, or $Pb^{2+}$.

Sulfate Compounds ($SO_4^{2-}$)

Water-soluble compounds containing sulfate, except when combined with $Ag^+$, $Hg_2^{2+}$, $Pb^{2+}$, $Ca^{2+}$, $Sr^{2+}$, or $Ba^{2+}$.

Carbonate, Phosphate, Chromate, Sulfide, and Sulfite Compounds

Water-insoluble compounds containing $CO_3^{2-}$, $PO_4^{3-}$, $CrO_4^{2-}$, $S^{2-}$, or $SO_3^{2-}$, except when combined with alkali metal cations ($Li^+$, $Na^+$, $K^+$, $Rb^+$, $Cs^+$) or $NH_4^+$.

Hydroxide and Oxide Compounds

Water-insoluble compounds containing $OH^-$ or $O^{2-}$, except when combined with alkali metal cations ($Li^+$, $Na^+$, $K^+$, $Rb^+$, $Cs^+$), $Ba^{2+}$, $Ca^{2+}$, or $Sr^{2+}$.

Insoluble Halide Exceptions

The specific metal cations that make chloride ($Cl^-$), bromide ($Br^-$), and iodide ($I^-$) compounds insoluble: $Ag^+$, $Hg_2^{2+}$, and $Pb^{2+}$.

Insoluble Sulfate Exceptions

The specific metal cations that precipitate with sulfate ($SO_4^{2-}$): $Ag^+$, $Hg_2^{2+}$, $Pb^{2+}$, $Ca^{2+}$, $Sr^{2+}$, and $Ba^{2+}$.

Soluble Hydroxide Exceptions

The specific cations that form water-soluble hydroxide ($OH^-$) compounds: $Li^+$, $Na^+$, $K^+$, $Rb^+$, $Cs^+$, $Ba^{2+}$, $Ca^{2+}$, and $Sr^{2+}$.