- •8.1 Activity Coefficients
- •8.2 Equilibrium Constants
- •Table 8.5 Ionic Product Constant of Water
- •8.2.1 Proton-Transfer Reactions
- •8.2.2 Formation Constants of Metal Complexes
- •8.3 Buffer Solutions
- •8.3.1 Standard Reference pH Buffer Solutions
- •8.3.2 Standards for pH Measurement of Blood and Biological Media
- •8.3.3 Buffer Solutions Other Than Standards
- •Table 8.20 Potentials of Reference Electrodes in Volts as a Function of Temperature
- •8.4.1 Electrometric Measurement of pH
- •8.5 Indicators
- •Table 8.24 Mixed Indicators
- •8.6 Electrode Potentials
- •8.7 Conductance
8.104 |
|
|
|
SECTION 8 |
|
|
|
||
TABLE 8.13 |
Cumulative Formation Constants for Metal Complexes with Organic Ligands ( |
|
Continued |
) |
|||||
|
|
|
|
|
|
|
|
|
|
|
|
|
log K 1 |
|
log K 2 |
|
log K 3 |
log K 4 |
|
|
|
|
|
|
|
|
|
|
|
1,1,1-Trifluoro-3-2 |
-Thenoylacetone |
(TTA) |
|
|
|
|
|
|
|
Ba |
|
|
|
|
10.6 |
|
|
|
|
|
|
|
|
|
|
|
|
||
Cu(II) |
|
|
6.55 |
|
13.0 |
|
|
|
|
Fe(III) |
|
|
6.9 |
|
|
|
|
|
|
Ni |
|
|
10.0 |
|
|
|
|
|
|
Pr |
|
|
9.53 |
|
|
|
|
|
|
Pu(III) |
|
|
9.53 |
|
|
|
|
|
|
Pu(IV) |
|
|
8.0 |
|
|
|
|
|
|
Th |
|
|
8.1 |
|
|
|
|
|
|
U(IV) |
|
|
7.2 |
|
|
|
|
|
|
Zr |
|
|
3.03 [as ZrL |
3 ] |
|
|
|
|
|
Xylenol orange |
|
|
|
|
|
|
|
|
|
Bi |
|
|
5.52 |
|
|
|
|
|
|
Fe(III) |
|
|
5.70 |
|
|
|
|
|
|
Hf |
|
|
6.50 |
|
|
|
|
|
|
Tl(III) |
|
|
4.90 |
|
|
|
|
|
|
Zn |
|
|
6.15 |
|
|
|
|
|
|
Zr |
|
|
7.60 |
|
|
|
|
|
|
Zincon |
|
|
|
|
|
|
|
|
|
Zn |
|
|
13.1 |
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
8.3 BUFFER SOLUTIONS
8.3.1Standard Reference pH Buffer Solutions
The assigned values of pH |
|
s , according to the Bates-Guggenheim convention [ |
Pure Applied Chem. |
|
|||||||
1: 163 (1960)], for the primary standard solutions prepared from salts issued by the National Institute |
|
|
|
||||||||
for Science and Technology (NIST, US) (U.S.) are given in Table 8.14. These are smoothed values. |
|
|
|
||||||||
The ionic strength of these reference solutions is 0.1 or less. Strictly speaking the NIST scale uses |
|
|
|||||||||
a molality concentration system; however, values are given in molarity units for convenience. |
|
|
|
||||||||
|
As a result of a variable liquid-junction potential, the measured pH may be expected to differ |
|
|
|
|||||||
seriously from the p |
a H determined from cells without a liquid junction in solutions of high acidity |
|
|
||||||||
or high alkalinity. Merely to affirm the proper functioning of the glass electrode at the extreme ends |
|
|
|||||||||
of the pH scale, two secondary standards are included in Table 8.14. In addition, values for a 0.1 |
|
|
m |
||||||||
solution of HCl are given |
to extend |
the pH |
scale up to |
275 |
|
C |
[see R. S. Greeley, |
Anal. |
Chem. |
||
32: |
1717 (1960)]: |
|
|
|
|
|
|
|
|
|
|
|
t, C: |
25 |
60 |
90 |
125 |
150 |
175 |
200 |
225– 275 |
|
|
|
pH: |
1.10 |
1.11 |
1.12 |
1.13 |
1.14 |
1.15 |
1.16 |
1.2 |
|
|
Uncertainties in the values are |
0.03 pH unit from 25 to 90 |
|
C, 0.05 pH unit from 125 to 200 |
C, |
|||||||
and 0.1 pH unit from 225 to 275 |
C. |
|
|
|
|
|
|
|
TABLE 8.14 |
National Bureau |
of Standards (U.S.) Reference pH Buffer Solutions |
|
|
|
|
|
|
|
|
|
|
|
|
|
|||||||
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Secondary |
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
standard |
|
|
|
|
|
|
0.025 |
M |
0.0087 |
M |
|
|
0.025 |
M |
|
|
|
|
|
|
|
|
0.05 |
M |
|
|
0.05 |
M |
0.05 M |
KH 2PO 4 , |
KH 2PO 4 , |
|
|
NaHCO |
3 , |
Secondary |
|
|||
Temperature |
|
|
|
K |
KH tartrate |
|
|
KH |
2 |
KH |
0.025 |
M |
0.0302 |
M |
0.01 |
M |
0.025 |
M |
standard Ca(OH) |
2 |
||
|
C |
|
|
|
tetraoxalate |
(saturated at 25 |
C) |
|
citrate |
phthalate |
Na 2HPO |
4 |
Na 2HPO |
4 |
Na 2B |
4 O 7 |
Na 2CO |
3 |
(saturated at 25 |
C) |
||
|
0 |
|
|
|
1.666 |
|
|
|
3.860 |
|
4.003 |
6.984 |
|
7.534 |
|
9.464 |
|
10.317 |
|
13.423 |
|
|
|
5 |
|
|
|
1.668 |
|
|
|
3.840 |
|
3.999 |
6.951 |
|
7.500 |
|
9.395 |
|
10.245 |
|
13.207 |
|
|
|
10 |
|
|
|
1.638 |
|
|
3.820 |
|
3.997 |
6.923 |
|
7.472 |
|
9.332 |
|
10.179 |
|
13.003 |
|
||
|
15 |
|
|
|
1.642 |
|
|
|
3.802 |
3.998 |
6.900 |
|
7.448 |
|
9.276 |
|
10.118 |
|
12.810 |
|
||
|
20 |
|
|
|
1.644 |
|
|
3.788 |
|
4.002 |
6.881 |
|
7.429 |
|
9.225 |
|
10.062 |
|
12.627 |
|
||
|
25 |
|
|
|
1.646 |
3.557 |
|
3.776 |
|
4.005 |
6.865 |
|
7.413 |
|
9.180 |
|
10.012 |
|
12.454 |
|
||
|
30 |
|
|
|
1.648 |
3.552 |
|
3.766 |
|
4.011 |
6.853 |
|
7.400 |
|
9.139 |
|
9.966 |
|
12.289 |
|
||
|
35 |
|
|
|
|
|
3.549 |
|
3.759 |
|
4.018 |
6.844 |
|
7.389 |
|
9.102 |
|
9.925 |
|
12.133 |
|
|
|
38 |
|
|
|
1.649 |
3.548 |
|
3.756 |
|
4.030 |
6.840 |
|
7.384 |
|
9.088 |
|
9.910 |
|
12.043 |
|
||
|
40 |
|
|
|
1.650 |
3.547 |
|
3.753 |
|
4.035 |
6.838 |
|
7.380 |
|
9.068 |
|
9.889 |
|
11.984 |
|
||
|
45 |
|
|
|
|
|
3.547 |
|
|
|
|
4.047 |
6.834 |
|
7.373 |
|
9.038 |
|
|
|
11.841 |
|
|
50 |
|
|
|
1.653 |
3.549 |
|
3.749 |
|
4.050 |
6.833 |
|
7.367 |
|
9.011 |
|
9.828 |
|
11.705 |
|
||
|
55 |
|
|
|
|
|
3.554 |
|
|
|
|
4.075 |
6.834 |
|
|
|
8.985 |
|
|
|
11.574 |
|
|
60 |
|
|
|
1.660 |
3.560 |
|
|
|
|
4.081 |
6.836 |
|
|
|
8.962 |
|
|
|
11.449 |
|
|
|
70 |
|
|
|
1.671 |
3.580 |
|
|
|
|
4.116 |
6.845 |
|
|
|
8.921 |
|
|
|
|
||
|
80 |
|
|
|
1.689 |
3.609 |
|
|
|
|
4.164 |
6.859 |
|
|
|
8.885 |
|
|
|
|
||
|
90 |
|
|
|
1.72 |
3.650 |
|
|
|
|
4.205 |
6.877 |
|
|
|
8.850 |
|
|
|
|
|
|
|
95 |
|
|
|
1.73 |
3.674 |
|
|
|
|
4.227 |
6.886 |
|
|
8.833 |
|
|
|
|
|
||
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
Dilution |
value |
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
pH |
1/2 |
|
|
|
0.186 |
0.049 |
|
0.024 |
|
0.052 |
0.080 |
0.070 |
|
0.01 |
0.079 |
|
0.28 |
|
||||
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
||||||
Source: |
R. G. Bates, |
J. Res. Natl. Bur. Stand. (U.S.), |
66A: 179 (1962) and B. R. Staples and R. G. Bates, |
J. Res. Natl. Bur. |
|
|
|
|
|
|
|
|
||||||||||
Stand. (U.S.), |
73A: |
37 (1969). |
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|||
Note: |
The uncertainty is |
0.003 in pH in the range 0–50 |
C, rising to |
0.02 above 70 C. |
|
|
|
|
|
|
|
|
|
|
105.8