ion

SO_{4} + H_{2}O = H_{2}SO_{4} + O

[Illustration: Fig. 33]

That new substances are formed at the cathode and anode may be shown in
the following way. A U-tube, such as is represented in Fig. 33, is
partially filled with a solution of sodium sulphate, and the liquid in
one arm is colored with red litmus, that in the other with blue litmus.
An electrode placed in the red solution is made to serve as cathode,
while one in the blue solution is made the anode. On allowing the
current to pass, the blue solution turns red, while the red solution
turns blue. These are exactly the changes which would take place if
sodium hydroxide and sulphuric acid were to be set free at the
electrodes, as required by the theory.

~The properties of electrolytes depend upon the ions present.~ When a
substance capable of dissociating into ions is dissolved in water, the
properties of the solution will depend upon two factors: (1) the ions
formed from the substance; (2) the undissociated molecules. Since the
ions are usually more active chemically than the molecules, most of the
chemical properties of an electrolyte are due to the ions rather than to
the molecules.

The solutions of any two substances which give the same ion will have
certain properties in common. Thus all solutions containing the copper
ion (Cu^{++}) are blue, unless the color is modified by the presence of
ions or molecules having some other color.

EXERCISES

1. Distinguish clearly between the following terms: electrolysis,
electrolyte, electrolytic dissociation, ions, solute, solvent, solution,
saturated solution, and supersaturated solution.

2. Why does the water from some natural springs effervesce?

3. (a) Why does not the water of the ocean freeze? (b) Why will ice
and salt produce a lower temperature than ice alone?

4. Why does shaking or stirring make a solid dissolve more rapidly in a
liquid?

5. By experiment it was found that a certain volume of water was
saturated at 100 deg. with 114 g. of potassium nitrate. On cooling to 0 deg. a
portion of the substance crystallized. (a) How many grams of the
substance remained in solution? (b) What was the strength of the
solution at 18 deg.? (c) How much water had been used in the experiment?

6. (a) 10 g. of common salt were dissolved in water and the solution
evaporated to dryness; what weight of solid was left? (b) 10 g. of
zinc were dissolved in hydrochloric acid and the solution evaporated to