SALTS ========================================================================= | TYPE OF SALT | PERCENTAGE DISSOCIATION IN | 0.1 EQUIVALENT SOLUTION _____________________________________________|___________________________ | R^{+}R^{-} | 86 | R^{++}(R^{-})_{2} | 72 | (R^{+})_{2}R^{--} | 72 | R^{++}R^{--} | 45 | ========================================================================= The percentage dissociation is determined by studying the electrical conductivity of the solutions and by other physico-chemical methods, and the following general statements summarize the results: !Salts!, as a class, are largely dissociated in aqueous solution. !Acids! yield H^{+} ions in water solution, and the comparative !strength!, that is, the activity, of acids is proportional to the concentration of the H^{+} ions and is measured by the percentage dissociation in solutions of equivalent concentration. The common mineral acids are largely dissociated and therefore give a relatively high concentration of H^{+} ions, and are commonly known as "strong acids." The organic acids, on the other hand, belong generally to the group of "weak acids." !Bases! yield OH^{-} ions in water solution, and the comparative strength of the bases is measured by their relative dissociation in solutions of equivalent concentration. Ammonium hydroxide is a weak base, as shown in the table above, while the hydroxides of sodium and potassium exhibit strongly basic properties.