88 THE THEORY OF IONIZATION- High Ionization of All Salt Solutions. The object of Ex-
periments 7 and 8 was to show the relative number of ions in
equivalent acid and base solutions and in the neutral solution re-
sulting from adding the two together. In Experiment 7 the
same electrodes held the same distance apart with the same vol-
ume of liquid between them were used on all three solutions tested.
Hence the brightness of the lamp was proportional to the number
of ions in the solution. But in Experiment 8 a different kind
of electrode was used, and, although a valid comparison of
the concentration of ions in the three solutions of that experiment
was obtained, the brightness of the lamp shown for the neutral
solutions of the two experiments gives no comparison of the num-
ber of ions. Remember that the neutral solution in each experi-
ment is 0.5N with respect to the salt.
Prepare again a neutral solution of sodium chloride by neutral-
izing normal sodium hydroxide with normal hydrochloric acid,
and a neutral solution of ammonium acetate by neutralizing
normal ammonium hydroxide with normal acetic acid. Test the
conductivity of both solutions with electrodes A and again test
both with electrodes B.
What general statement can be made about the ionization of
salts? Explain again (although the write-up of Experiment 8
should already contain the explanation) why the salt of a weak
acid and a weak base can be as highly ionized as the salt of a strong
acid and a strong base.
DISPLACEMENT OF WEAK ACIDS AND BASES- Displacement of a Weak Acid from its Neutral Salt by
Means of a Stronger Acid, (a) To 2 cc. of liV sodium benzoate
solution, NaC7H 6 O 2 , add a few drops of 6iV H 2 SO 4. At 30 drops
to the cubic centimeter how many drops of the 6iV acid would be
equivalent to the 2 cc. of liV salt? How does this experiment
illustrate the displacement* of a weak acid from its salt?
(b) Observe cautiously the odor of 6N acetic acid. Dilute
1 cc. with 5 cc. of water to make the solution 1N and see whether
the odor is still detectable in the cold. Warm the solution and see
if the odor is noticeable.
Warm 2 cc. of liV sodium acetate solution, NaC2H 3 O 2 , barely
to the boiling point. Remove it from the flame and observe