2
3
HI 4010 Fluoride Half-cell
HI 4010 Fluoride Half-cell
HI 4010 Fluoride Half-cell
HI 4010 Fluoride Half-cell
HI 4010 Fluoride Half-cell
HI 4110 Fluoride Combination Electrode
HI 4110 Fluoride Combination Electrode
HI 4110 Fluoride Combination Electrode
HI 4110 Fluoride Combination Electrode
HI 4110 Fluoride Combination Electrode
I.
I.
I.
I.
I. Introduction:
Introduction:
Introduction:
Introduction:
Introduction:
The Hanna HI 4010 and HI 4110 are ion selective elec-
trodes designed for the measurement of fluoride ions in
aqueous solutions. The HI 4010 is a solid state half-cell
sensor that requires a separate reference. The HI 4110 is a
combination ion selective electrode.
II
IIII
IIII.
Specifications
Specifications
Specifications
Specifications
Specifications
Type:
Solid State electrode with
a Lanthanum Fluoride
crystal membrane.
Ion(s) measured:
Fluoride (F
-
)
Measurement range: Saturated to 1X 10
-6
M
Saturated to 0.02 ppm
Interfering ions:
OH
-
Note:
Several other ions (Al
3+
, Fe
3+
) that complex with the
measured species will reduce the ion concentrations
measured directly. TISAB reagent should be used in most of
these cases. H
+
ion also forms HF species below pH 5.
Increase pH in these cases above 5 for a total fluoride
measurement.
Operating Temperature:
0-80
°
C
Operating pH:
5 to 8 pH
Dimensions:
12 mm (OD) X 120 mm
nominal insertion
(0.47
”
X 4.72
”
)
Connection:
BNC
III.
III.
III.
III.
III. Theory of Operation
Theory of Operation
Theory of Operation
Theory of Operation
Theory of Operation:::::
The HI 4010 or HI 4110 fluoride electrodes are potentio-
metric devices used for the rapid determination of free fluo-
ride ions in water, soft drinks, wine, emulsified foods, and
plating and pickling acids. The electrode functions as a
sensor or ionic conductor. The HI 4010 requires a separate
reference electrode to complete its electrolytic circuit. The
HI 4110 has a reference electrode incorporated in its de-
sign. The lanthanum fluoride crystalline pellet is practi-
cally insoluble in the test solutions being measured and
produces a potential change due to changes in the sample
’
s
ion activity. When the ionic strength of the sample is fixed,
the voltage is proportional to the concentration of fluoride
ions in solution and the electrode follows the Nernst equa-
tion.
E= E
a
+ 2.3 RT/nF log A
ion
E= observed potential
E
a
= Reference and fixed internal voltages
R= gas constant (8.314 J/K Mol)
n= Charge on ion (1-)
A
ion
=ion activity in sample
T= absolute temperature in K
F= Faraday constant (9.648 x 10
4
C/equivalent)
