T H E J C I I - K A I A . i LOF I-YDL-STRI.4L qAI-DE.I-.GI.YEERI.YG
300
with moderate amounts of vanadium present the characteristic chromium color is but slightly changed, but the results are high as shown by Table I . The samples were compared against a 0.30 per cent. chromium standard t h a t contained no vanadium. TABLEI Sample no.
P er cent. vanadium present
Per cent. chromium present
Per cent. chromium obtained
Per cent error
0.23 1 0.10 0.20 +0.03 0.30 0.31 t o 01 2 0.10 0.30 0.33 t0.05 3 0 15 0 30 0.34 + 0 04 4 0 15 0.37(a) 5 0.20 0 30 +0.07 (a) Difficulty in comparing. owing t o the solutions being of different shade.
The results in Table I1 also show the influence of vanadium on the determination of the chromium. The samples were compared against a 0.2 j per cent. chromium standard t h a t contained 0 . I 5 per cent. vanadium. I t will be noted t h a t the samples containing more than 0.15 per cent vanadium mere high, while those containing less than this amount \\-ere lon-. TABLEI1 Sample no. 6
7 8 9 10 11 12 13
'
Per cent. vanadium present 0 0 0 0 0 0 0 0
10 10 10 10 20 20 20 20
Per cent. chromium present 0 20 0 20 0 25 0 30 0 20 0 20 0 25 0 30
Per cent. chromium obtained 0.18 0 1s 0 23 0 24 0 22 0 21 0 28 0 34
Error -0
02
-n
02 02 06 02 01 03 01
-0 -0 -0 -0 +0 +0
The color due t o vanadium is only obtained in acid solutions of the pentavalent compounds, and is quite characteristic. As a matter of fact, a few experiments made with pure vanadate solutions indicate t h a t the reaction is quantitative, and is almost as sensitive as the well-known hydrogen peroxide test for this element. The addition of the reagent t o slightly acid solutions of quadrivalent titanium gives brick-red colors t h a t are destroyed by adding hydrofluoric acid, or strongly acidifying with mineral acids. Concentrated sulfuric acid solutions of titanium, however, give pink colored solutlcns. The reaction for titanium is much more sensitive than the hydrogen peroxide test, but the percentage of free acid present has a very marked influence on the color, and i t is not thought that a reliable quantitative method could be developed, owing t o this fact. Titanium would not interfere v-ith the chromium determination in the method as given, of course, as any titanium present would be precipitated and removed by filtration. The writer does not think t h a t the method given above is more advantageous for determining large percentages of chromium in steel (say over 0.60 per cent.) than Galbraith's or some such modification, but it seems t o be particularly suited for small percentages of this element in steel. Table I11 shows some results obtained by the new method. The result on sample N o . 14 was obtained by making an ether separation of the ferric chloride solution, a n d then replacing the hydrochloric acid with sul-
i"E-III\'TRl-
Vol.
j,
So. 4
TABLE111 \Veight of steel Sample taken no.
Grams
14 15
2 0 0.4 0.4 0.4 0.2 0.2 0.2 0 2 0 2 0.2 0.2 0.4 0 4 0.4 0 4 0 4 0.4 0.4 0.4
16 17 IS 19 20 21 22 23 24 25 26 27 28 29 30 31 32
Per cent.
Per cent. molyb-
present
present
.. ..
5.5 5 5 20.0 20 0 I
O
5.0 10.0 10.0
Per cent chromium
Per cent
chromium
taken
obtained
0.012 0.03 0.06 0.09 0 15 0 20 0.30 0 50 0.70 1.10 1 40 0.20 0.30 0.20 0 25 0 20 0 30 0.20 0.25
0. 013 0.03 0.06 0.09 0.15 0.20 0.31 0.49 0.70 1.10 1 .38 0.20 0.29 0.20 0.24 0.18 0.29 0.18 0.25
Error -0.001 none none none none none + 0 01 -0.01 none none -0 02 none -0.01 none -0.01 -0.02 -0.01 -0.02 none
furic acid. The chromium was then oxidized with sodium peroxide in an alkaline solution, and the small amount of ferric hydroxide removed by filtration. The solution of sodium chromate was then acidified with sulfuric acid, the chromium reagent added, and the color matched against a pure solution of potassium bichromate in sulfuric acid. By taking larger quantities of steel, as in the case of sample No. 14, there is no difficulty in determining 0.001 per cent. chromium. Such a minute quantity of chromium in steel has no metallurgical significance whatever; of course, b u t the analyst is often called upon t o look for very small quantities of metals, and i t is a pleasure t o have a method t h a t will detect them without difficulty. The writer is indebted t o his assistant, Mr. D. J. Giles, for performing much of the experimental work leading up t o the perfection of this method. FIRTH-STERLING STEEL Co. MCKEESPORT,PA.
WATERS OF THE BREITENBUSH HOT SPRINGS, OREGON' By
\\-ALTON
VAN \ \ - I X K L E ~
Received January 16, 1913
Breitenbush Hot Springs are near Breitenbush Creek on the west slope of the Cascade Mountains in Marion County. Oregon. Their exact elevation is unknoim. but it is probably somewhat more than 2 0 0 0 feet above sea level. The valley of the Breitenbush is narrow and the formations exposed are lavas of the Cascade Range series. Faults a t the springs TTere not observed by MI-. Finkbiner, though possibly the waters issue from a fault. More than 60 hot springs, in three general groups, lie along both sides of the stream for almost a third of a mile. A few cold springs, entirely different in character, are within the limits of the groups, but as they are normal for the region they are unimportant. All the hot springs have nearly the same temperature and the manner of their grouping suggests a common origin. Reputed curative properties have been assigned t o the various springs, and a crude "health resort" has been con1 Published by permission of the director of the U. S . Geological Survey, dated January 4, 1913. 2 Field work by N. M . Finkbiner.
i structed. Many patients take the waters each year. and if the place were more readily accessible it would undoubtedly enjoy a large patronage. In September, 1 9 1 2 , Mr. N. M. Finkbiner. of the laboratory of the U. S. Geological Survey a t Salem, Oregon, described 23 of the springs. and made field determinations of the temperature and alkalinity of each. He also collected from nine of these, from one cold spring, and from Breitenbush Creek above and below the springs, samples of water, which were analyzed conjointly at Salem by the writer, N. 11. Finkbiner, and S. C. Dinsmore, state chemist of Sevada. The accompanying table gives results of both field and laboratory tests of these samples; the other 14 springs, field tests of which were made but are not reported, furnish mater of similar character. .kSALSSES O F THE TVATERS O F
I1 E .\-G-I-\-EE R I -1-G ‘i H E -1I I.\’ TR I
30 i
or through these rocks v-ould be heated, the bicarbonates in them would thereby be decomposed, and the maters would be relieved of part of their charge of iron, aluminum, alkaline earths, and carbonates, Alkaline salts with perhaps a slight residuum, of calcium. and even less magnesium, would remain in solution. The calcic carbonate and the magnesia deposited would remain behind in the rock, and the water would move on without them. The carbonic acid set free as gas would react with rock silicates, decomposing them and depositing alkaline earth carbonates, the alkalies and part of the silica entering into solution. Thus a large part of the carbonic acid would be lost from the solution. The waters, percolating still further into the heated zone. would become further heated, and would be subjected to
BREITENBUSH HOTS P R I N G S ,
OREGON
(Parts per million unless otherwise designated’)
.i
B
C
D
E
F
G
S O z .. . . . . . . . . . . . . . . . . Fe. . . . . . . . . . . . . . . . Ca . . . . . . . . . . . . . . . . . . . . Mg.. . . . . . . . . . . . . . . . . . .
14 1 134 142 138 144 141 0 35 0.10 0.17 0 20 0 10 0.10 99 93 59 90 56 95 1 5 1.2 I S 1 5 1 5 1 7 S a . .. . . . . . . . . . . . . . . . . . 735 .. ... 73 3 . . ... K ..................... 41 41 . . cos. . . . . . . . . . . . . . . . . 0 0 0 0 0.0 0 0 0.0 0 0 HC03., . . . . . . . . . . . . . . . 154 116 128 127 125 141 so4... . . . . . . . . . . . . . . . . . 143 13; 138 137 137 135 C1. . . . . . . . . . . . . . . . . . . . 1.133 1.128 1.135 1,120 1,133 1.115 ... ... ... tr. 180°.
. . . . . . . . . . . . . . 2,470
T em perat ure, degrees C.
67
2,380 59
2,408 73
2,379 73.5
2.42.3 73
411 samples collected S e p t . 27, 1912. A. S pri ng near right bank of creek a t X E end of group. Flows from crevice in rock. Flow about “size of wrist.” B. “Arsenic spring” (no arsenic present) near left bank of creek d i o u t 600 feet SXV from A . Flow one-half t h a t of .I. C. Spring 4 3 feet from B a n d 84’ X E of A. Flow same as 1. D. S pri ng 5 8 feet f r om B a t 8 7 ’ N E . Flows same as A . E. S pri ng about I50 feet f r om B and d u e west. Flow one-fourth size of wrist.
H
15 I 0.30 93
0 10 97
o s
1. o
J
I
147
142 0 05 96
. .
...
0 0 128 139 1 , 14.3
6 0 146 137 1 . 145
. . 133’ I , 120
. .
41 0 0
13 3 137 1.131 tr.
5.2 2.4
24 0.01 4 4 1 1
8.7
6 9
0.iO
73Y
...
...
L
24
I .4
, . .
...
K
142 0.27 93
0.0
0.1)
27 1.2 2.3 0.26
24 2 .i 2 0 tr.
2.396 2,412 2,43.j 2 434 67 54 69 83 66 70 13 ... F. Spring 17.5 feet from E and about 95’ VW. G. Spring a b o u t I50 feet from F and 64’ h3V. H. Spring a t S W end of group. I . Spring in main b a t h house. Difficult of access. J. Average of analyses 4 t o I inclusive. K . Cold “ I r o n ” spring on right bank of creek 2 5 0 feet above mouth of .Mangfield Creek. L. Composite sample from Breitenbush River.
2,384 69
I
The figures show t h a t the several hot springs are merely separate outflows from a common source. The water is sodic chloride in character, but it contains small amounts o f silica, calcium. bicarbonates, and sulfates. Minimum medicinal doses of both sulfates and carbonates might be obtained by drinking about 4 liters of the mater,’ but the disagreeable and even nauseating taste of the chlorides mould make the drinking of t h a t amount in one day an Herculean feat. I t is certain t h a t any curative properties a t tributable t o the mineral content are psychologic rather t h a n physiologic. The water is interesting to geologists, as it is an excellent example of a type encountered in many regions of recent volcanic activity. Hot springs in volcanic regions may be placed in several general divisions, such as sulfate springs, carbon dioxide, or “soda” springs, chloride springs, and the like. The origin of the waters of many of the types can easily be explained, but no adequate explanation of the presence of the large quantities of sodium chloride in the waters of the third type has yet been advanced, so far as known to the writer. The lavas of the Cascade Range have been erupted
through, and nom overlie. the older sedimentaries of the continental floor. At the great depth to which the sediments have been buried, the adjoining lava is still hot. This heat has also been communicated t o some extent to the sediments so t h a t these are a t high temperatures. As any waters. percolating into increasingly great pressures. They would become more strongly concentrated, because of these and other physical conditions, and would finally be forced to the surface under combined static and thermal pressure. Any carbon dioxide still held in solution would cause small amounts of calcium, encountered en route, to be dissolved, and the springs would then deliver a sodic chloride, calcic bicarbonated and sulfated water, containing appreciable amounts of dissolved silica. This explanation avoids the necessity of considering the action of magnatic, or “juvenile” waters, and, being based entirely on well-known chemical reactions. has the merit of simplicity, and freedom from speculative hypotheses.
Cf. R . B. Dole, “Concentration of Mineral W a t e r in Relation t o Therapeutic hctivity.” in .Mineval Resources of the United States f o r 1911. C . S . Geol. Survey, 1912.
Received February 5 , 1913
L-.S . GEOLOGICAL SURVEY SALEM. OREGOS
PHOSPHATES IN SURFACE WATERS B y GEORGES.
The
well-known
JAMIESON
colorimetric-molybdate
method
