Input Range: Range: 0-200 and 0-20,000 microsiemens
Output Range: 0V to 4V
Calibration: Required every use
Default scaling Value:
There are 2 ranges; 20 mS and 200uS.
0.4V is approximately 1 mS
4V is approximately 20 mS
0.4V is approximately 10 uS
4V is approximately 200 uS
- Install the IX-ELVIS board into the National Instrument ELVIS platform
or the IX-myDAQ board onto the NI myDAQ. If using ELVIS, connect the ELVIS
power supply to the ELVIS unit and connect it to the computer via a USB
cable. Ensure both of the power switches are in the â€œonâ€ position. For
the myDAQ, connect it to the computer using the USB cable.
- Connect the MINI DIN7 connector of the CMN-100 to either CH1 or CH2 of
either the IX-ELVIS or IX-myDAQ board.
- Open the recording software, select the channel that the CMN-100 is
connected to and ensure the range is set to +/-5V.
- The CMN-100 should be calibrated within the expected range. For example:
If the expected range is 500uS to 1000uS perform a 2 point calibration with
the first point (SP1) at 400uS and the second point (SP2) at 1000uS.
*Note: If using the IX-MYDAQ the signal may be inverted.
The Effect of Concentration on the Conductivity of Solutions
Aim: To determine the effect of concentration on the conductivity of various
Note: Always begin testing samples with the conductivity selector switch in
the 0-200 uS range. While recording the conductivity of each test sample,
toggle the switch to the 0-20,000 uS position. This is especially important
for measuring solutions with higher conductivities.
- Follow the calibration procedure above.
- Add 50 ml deionized water to a 100 ml beaker.
- Place the CMN-100 conductivity meter in the beaker and click Record.
- When the recording on the Conductivity channel reaches a stable
baseline, record that it is DI Water.
- Add 1 drop of 1.0 M NaCl solution to the deionized water. Carefully
swirl the CMN-100 to ensure thorough mixing. Record the event.
- Add a second drop of 1.0 M NaCl solution to the beaker. Record the event
as it reaches a stable value.
- Add a third drop of 1.0 M NaCl solution to the beaker. Record the event
as it reaches a stable value.
- Continue following these steps until 10 drops of 1.0 M NaCl have been
added to the beaker.
- Click Stop to halt the recording.
- Save the File.
- Remove the conductivity meter from the beaker. Hold the meter over the
beaker used for collecting waste deionized water, and rinse it with a wash
bottle. Blot any drops of DI water from the meter and place the meter in the
beaker containing fresh DI water.
- Repeat steps 1 through 11 for both 1.0 M CaCl2 and 1.0 M AlCl3
- Discard the contents of each beaker as directed by your instructor
Conductivity is the ability of a substance to conduct an electric current.
The principle by which conductivity is measured is fairly simple - two
electrodes are placed in the solution, a potential is applied across the
electrodes, and the current is measured. Conductivity (G) is the inverse of
resistivity (R). This can be determined from the voltage and current values
according to Ohm's law: G = I/R = I (amps) / E (volts).
Since the ions in a solution facilitate the conductance of an electrical
current, the conductivity of a solution is proportional to its ion
concentration. Conductivity is generally measured in microsiemens (uS).
Microsiemens are the modern units of the inverse of resistivity or mho.
In some situations, however, conductivity may not correlate directly to
concentration. The graphs below illustrate the relationship between conductivity
and ion concentration for two common solutions. Notice that the graph is linear
for the sodium chloride solution, but not for a highly concentrated sulfuric
acid solution. Ionic interactions can alter the linear relationship between
conductivity and concentration in some highly concentrated solutions.
Ions that move through solution easily are better conductors. Small, fast moving
ions like hydrogen (H+) have a greater conductivity than do larger ions like
bromide ion (Br-), or heavily hydrated ions like the sulfate ion (SO42-).
Conductivity is a useful method for measuring how good a conductor a substance
will be. Conductive substances are usually referred to as electrolytes. Thus,
electrolytes are compounds that dissolve in water and dissociate into ions. In
solutions of electrolytes, several different substances may be present,
including complete, whole molecules and dissociated ions.
Strong electrolytes dissociate completely into ions. A 1.0 M solution of the
strong ionic electrolyte AB contains 1.0 M A+ ions, 1.0 M B- ions, and 0.0 M AB
molecules. In other words, the ions are the only substances present in a
solution of a strong electrolyte. Diluting a 1.0 M solution of AB with water to
0.50 M reduces the concentration of ions by one half, which also reduces the
conductivity of the solution by one half.
Weak electrolytes dissociate incompletely, or do not fully separate into their
respective ions. A 1.0 M solution of a weak electrolyte CD may contain less than
0.20 M C+ ions, the same molarity of D- ions, and greater than 0.80 M CD
molecules. In a solution of a weak electrolyte the main substance present is the
entire molecule, not necessarily the dissociated ions.
The dissociation of a weak electrolyte is an equilibrium process, in which
molecules are constantly dissociating, a forward reaction, and reforming, the
reverse reaction, at identical rates. At equilibrium, the forward and reverse
processes occur at the same rate, so molecules dissociate and reform at the same
rate, and the concentrations of the molecule, its positive ions and its negative
ions all remain constant.
The probability of spontaneous dissociation of a molecule is constant, but the
probability of reformation of the molecule from its ions depends on the
concentration of ions present; low concentration makes reformation infrequent
which makes the reverse reaction slower. This means that diluting a weak
electrolytic solution slows down the reverse reaction more than it slows down
the forward reaction. After dilution, dissociation outpaces reformation until
the concentrations of the ions rise, their reformation rate increases, and the
rate of the reverse reaction rises to match that of the forward reaction. As a
result, dilution leads to dissociation of additional molecules before
equilibrium is reached again. So diluting a 1.0 M solution of a weak electrolyte
to 0.50 M with water reduces the conductivity, but by less than the 50% expected
with strong electrolytes.