DOC.
2
25
^i_^kcc
Cj
"k
in
relative
measure.
One
obtains in this
same
measure
the quantities
cm/e
separately
by
carrying
out
an
analogous
investigation
with
a
metal in such
a
way
that the
salts and electrodes
in I
and
II contain the
same
metal,
but that
e,
i.e.,
the
valency
(electrical
charge)
of
the
metal
ion, is different
on
the
two
sides.
The
value of the quantities
cm
in this
measure can
then
be
obtained
for the individual metals.
A
series
of such
experiments
thus leads
to
the
ratios of the
cm's,
i.e., the
constants
for the molecular attraction of
metal
ions. This series of
cm's
must
be
independent
of
the
nature
of
the salts
used,
and
the ratios
of
the
cm's
thus obtained
must
be independent of
the
nature
of the
two
solvents
on
which
we
based the
investigation.
A
further
requirement
must be
that
cm
must
prove
to be
independent
of the
electrical
charge
(valency) displayed
by
the ion. If this is the
case,
the
above
assumption
that
the
molecular forces
do not act
upon
the electrical
charges
is
correct.
If
one
wishes
to
determine the absolute value
of
the
quantities
cm
at
least
approximately,
one
can
do
so by
taking
the
approximate
value of
k
for
both solvents
from
the results
of
the
previously
cited
paper using
the formula
c
= Eca.
It
has to be noted here, of
course,
that
just
for the
two
liquids
most obviously
suggesting
themselves
as
solvents,
namely
water and
alcohol, it
has not been
possible
to
demonstrate the validity
of
the
law
of attraction
from
the
phenomena
of
capillarity,
evaporation, and compressibility.
[11]
Our
results could
equally
well
serve as a
basis for
studying
the solvent
constants
cl,
however,
by
basing
the investigation
on
two
metal ions
and
varying
the
solvent,
so
that then
the quantity
2
rC
n
-
rC
II
m m m
mi
E
n
j
2
n
is
to
be
considered
as
constant.
By
also
using
mixtures for
solvents,
the
investigation
might
be
extended
to
all electrically nonconductive
liquids.
From
such
experiments
it is
possible to calculate relative values of the