Salts are defined as 'ionic compounds which contain cations other than
hydrogen and anions other than oxide or hydroxide'. However, salts may 
be more usefully considered as ionic compounds in which the ionizable 
hydrogen ions of an acid have been replaced by either metal or ammonium 
ions. A monoprotic acid, such as ethanoic acid, has one ionizable 
hydrogen, and so can only form a neutral salt: by contrast, a diprotic 
acid, such as carbonic acid, has two ionizable hydrogens, and so forms 
both neutral and acid salts. In general, neutral salts are less soluble 
in water but more thermally stable than their acid analogues; compare, 
for examples, sodium carbonate with sodium hydrogencarbonate or calcium 
carbonate with calcium hydrogencarbonate.
Complete the Table below, which summarizes the solubilities in water and the formulae of typical neutral salts (formally) derived from five acids [HCl(aq) ; H2SO4(aq) ; CH3COOH(aq) ; H2CO3(aq) ; and HNO3(aq)], by inserting the correct formula for each salt. * #
*  Each formula refers to the anhydrous salt, although many of these
compounds crystallize from aqueous solutions as hydrates; e.g., calcium
chloride-water (1/6). The anhydrous salt can sometimes be obtained from
from the hydrated salt either by the use of certain dehydrating agents 
(e.g., concentrated sulfuric acid), or by careful heating (though this
is often accompanied by thermal decomposition of the anhydrous salt).
#  Solubility in water at 20C: d = decomposes (i.e., hydrolyzes); i =
insoluble (< 1 g kg-); sl = slightly soluble (1 - 10 g kg-); and s =
soluble (> 10 g kg-).
  Ionic compounds, which tend to have high melting points, conduct 
electricity when their ions are free to move (i.e., in the molten state
or when dissolved in water: but not in the solid state).

Confirmatory tests for ions share two common features. First, each test 
is executed on a solution of the compound; this is usually prepared by 
dissolving the solid in either distilled water or dilute nitric acid. 
And second, reaction of an aqueous solution of the ion with the test 
reagent results in either the selective precipitation of the ion or the 
selective evolution of a characteristic gas.
Complete the Table below, which summarizes tests for ten common ions, by inserting the correct observation from this list: brown; dark-blue; milky-white; pale-blue; royal-blue; very pale-green; white.
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