’THE OLD, THE NEW, AND THE PRACTICAL
tl.ridation
Oxidatioii
most accepll
past 30 yeii
illustrated tt
By Walter Zabban and Robert Helwil
Chlorination is the most popular treatment for cyanide waste in plating plants. Other treatments such as ozonation. electroly(
oxidation. and biooxidationdeserve considerationfor at least some types of wastes. These and several other treatments are review1
in this paper.
CN- f
CNCl2 CNC
.4 total 0)1
i heoreticallj)
T h e technology of treating cyanide wastes, as is known today,
was developed primarily between 1945 and 1955. An excellent
review of the early literature was published in 1949 by Dodge
and Reams.’ That review, prepared during a project sponsored
by the American Electroplaters’ Society, presented the various
methods of treatment and described the toxicity of cyanide to
aquatic life, bacteria, and other microorganisms in sewage
treatment plants.
Supplemental detailed studies by a handful of researchers
during this period included those by Dobson,’ Pettet,3 and
Dodge and Zabban.4 Since 1955 numerous commercial
applications have been reported.’
Proper methods of analysis are of primary importance for the
control of pollution in industrial waste. This statement is
especially applicable to the determination of cyanides and other
inorganic cyanogen compounds because of the complexity of
the analytical problem. The analytical procedures in use are
described in the manuals published by the American Public
Health Association: ASTM,7 and the U.S. EPA.’
-
ANALYTICAL PROCEDURES FOR TOTAL CYANIDE
A reliable analytical method for total cyanide is necessary to
determine (1) the degree of removal achieved with each
treatment process and (2) compliance with regulatory agencies’
effluent limitations. Yet many of the methods may not yield
desired precise data because of interferences or inherent errors
associated with each type of analytical procedure.
The EPA approved method of analysis for total cyanide is
based on distillation followed by either a colorimetric (pyridinebarbituric acid) or silver nitrate titrimetric procedure. This
method is intended to recover the cyanide from all cyanide
compounds including that from iron cyanide compounds, and
to eliminate or reduce the interferences associated with either
the colorimetric or titrimetric procedures.
The newer ASTM distillation procedure has reintroduced the
use of magnesium chloride in lieu of cuprous chloride to
accelerate the decomposition of certain complex cyanide ions.
Magnesium chloride had been proposed in 1952 in the
distillation procedure developed during two research projects
sponsored by the AES at Yale University and Lehigh
University.’ Cuprous chloride was introduced later in a n effort
to increase the recovery of total cyanide in the distillation
procedure. However, because cuprous chloride did not remove
the interference caused by thiocyanate, magnesium chloride
was readopted. Cyanide recovery with this distillation
procedure is comparable to that obtained with cuprous
chloride.
CYANIDE AMENABLE TO CHLORINATION
There are analytical methods that distinguish cyanide
amenable t o alkaline chlorination, CN(A), from total cyanide.
Because alkaline chlorination of cyanide has been and is still
56
recognized as the main commercially available method
treatment, the term “cyanide amenable to chlorination” w
coined’’ and suitable methods of analysis7 were develop
Since “cyanide amenable to chlorination” typifies those thata
easily decomposable in water and more toxic than others, SOI
of the regulatory agencies have adopted this terminology r
practical way of differentiating between commercially treatat
(amenable to chlorination) and total cyanide.
CN(A) may be determined by two procedures. One adap
the distillation procedure for an aliquot that has k
chlorinated and another that has not. The difference betw
these two measurements is the concentration of CN(1
Although this type of procedure has been accepted by[!
regulatory agencies, it also has several failings, one of which
that it is not reliable for concentrations less than 1 m g / l . .
reported by the ASTM task group for ~ y a n i d e .Anoh
~
problem is that inaccurate
evaluations of the Ch‘O
concentration will result in the presence of ammonia if I’
chlorination step is not conducted properly.
To alleviate some of these difficulties, especially 1’
measurement of low concentrations of CN(A), a colorimelr
method without the distillation step has been proposh
Unfortunately, the method suffers from numerous interferenil
not encountered with the distillation step. Both thiocyanatf
and aldehydes cause interference,’ for example. Efforts 1
resolve these interferences have resulted in the development of
cumbersome method and in unsatisfactory results.
Studies made with a third type of analytical procedurewhg
measures weak, aciddissociable cyanide indicate that it ma! 0
meaningpG!iiiethob. T1LI I-C ..-I..-..
-L*?:--LI-L-..lA
V O I U G b U l J L d I l l d U l C bllUUlU ‘ip‘ylv”’
those of CN(A). This procedure is the Wood River modificallc
of the Jackson and Roberts method. With this method.
sample is distilled in the presence of zinc acetate at a pH:
about 4.5 and the cyanide in the distillate is measured either)
colorimetric, electrometric or titrimetric procedures.
procedure is expected t o be incorporated in the ASS‘
methods.
..-..*AM
TREATMENT METHODS
Methods of treatment that have been in use for years. a‘
some that have been applied more recently, are descrlN
below.
Acidi3cation And Stripping Hydrogen Cyanide
Stripping of hydrogen cyanide is practiced In ’
recirculation of clarified and cooled wastewater to the fluss$
scrubbers in iron blast furnaces. This reduces the amou”:
cyanide
-.
that has t o be treated in effluent from the scrubtx’
1 ne hydrogen cyanide remaining in the flue gas is burn1 l a ”
combustion process in the stoves. This is a normal processin“
steel industry.
Stripping by acidification and volatilization at eletr”
temperature in an open system is no longer practical in 0”
reuse or non-recycle systems because of high enerZ
requirements and restrictions by laws regulating air pOlluti’
PLATING AND SURFACE FINISHI:
6 83 Ib of CI1
the chlorincc
hypochlorit((
\aOCl or I
The actu.,
theoretical ii
cyanide-was;
mmonia, a.
slows the 0)
increased be:
ion
1he oxidai
the carbon
s i t h uncor
complexes. 11
ink olve a 10s;
rhloride is
ioncentratior
increacing PI
c!rnate ion
O,ridation With Chlorine and Hypochlorites
Oxidation with chlorine and hypochlorites has become the
nost acceptable conventional method of treatment during the
30 years. The reactions in this oxidation process are
,lustrated by the following equations4:
-
+
CN- t HOCL CNCl OHCNO- C1- H 2 0
CNCl+ 2 0 H 2 CNCl+ 3 HOC1 + H z 0 5 HCI
-
: method
ination" ha,
e dweloped
those that a r t
others, some
iinology as a
ally treatable
One adapt,
it has been
:nce between
of CN(A)
:pted by t h t
ie of which IS
I I mg/L, as
le.' Another
the CN(A)
monia if the
,pecially t h c
colorimetrl,
n proposed
interference\
thiocyanate,
:. Efforts IO
:lopment of J
S.
cedure which
hat it may he
Ad approach
modification
method, t h r
i at a pH 01
ired either b\
edures. Thi\
the ASTV
3r years, and
ire described
+
-
+ 2 COz + N2
(1)
(2)
(3)
A total of 2.5 moles of available chlorine per mole of C N is
!heoretically required for the overall reaction, equivalent to
83 Ib of Clz per Ib of CN. Available chlorine may be defined as
,he chlorine equivalent of the OC1 radical present in the
j,pochlorite salt. One mole of CI2 is equivalent to 1 mole of
<aOCI or 112 mole of Ca(OC1)2.
The actual c
1
2 requirement is always greater than the
theoretical amount due to the presence of other oxidizable
fianide-waste constituents such a s cuprous ion, nickelous ion,
I"onia, and organic chemicals. The presence of nickel ion
I]OWS the oxidation reaction. The Ch requirement is also
,"creased because some of the nitrogen is converted to nitrate
;on.
The oxidation reaction ( I ) involves a loss of two electrons in
the carbon radical. This is an almost instantaneous reaction
with uncomplexed cyanides and some metallo-cyanide
"plexes. Reaction (2) is a hydrolysis reaction and does not
involve a loss or gain of electrons. The rate at which cyanogen
chloride is converted to cyanate ion is a function of the
ancentration of the hydroxyl ion" and is increased with
pH. Reaction (3) requires only a few min if the
panate ion is treated at pH 6.5, and about I hr a t pH 8.5.
Two steps are recommended for completing the oxidation
reaction: the first at pH 1 1 to oxidize cyanide to cyanate, and
ihe second at p H 6.5 t o oxidize cyanate essentially to nitrogen
ind carbon dioxide.
Improper chlorination of cyanide ion, hydrogen cyanide and
rhiocyanate ion, particularly at pH values below 10, will result
in greater evolution of cyanogen chloride, which is at least as
ioxic as hydrogen cyanide. Although a high pH favors
hydrolysis of cyanogen chloride t o cyanate ion, escape of
qanogen chloride is still possible even if the quantity that
scapes is reduced. Cyanide in combination with nickel, cobalt,
dver and gold is decomposed slowly but still treatable as long
3s proper detention time is provided in the reactors.I2
Cyanogen chloride will persist in the receiving streams for
hours, if not days, because the conditions are not favorable t o a
high rate of hydrolysis. Cyanogen chloride is not detectable by
rnalytical methods for cyanide. Method D in AS'TM D-2036'6 would have to be used. In the appendix to this reference
!here is valuable information on the analysis, treatment, and
:oxicity of simple and complex cyanide compounds plus
qanate and thiocyanate compounds.
Chlorine or hypochlorites have been found by the authors to
iced in t h e
o the flue-@\
ie amount 01
he scrubber$
s burnt in t h r
process in thc
m " i a will react with chlorine and hypochlorites more
rapidly than cyanide, forming chloramines. Monochloramines
formed by reaction of chlorine with ammonia ion will oxidize
?anide and thiocyanate ions but at a slower rate than chlorine.
at elevated
:tical in now
high energ!
air pollution
There is no truth to the often-quoted statement that cyanate
water may revert to cyanide. This information, which filtered
!!!rough =any
reg"1aioi-y agencies liite a n epidemic ij
!Cars ago, was based on erroneous experimentation and
procedures.
w e greater affinity for ammonia than for cyanide; therefore,
Formation of Complex Metallo- Cyanides
As indicated previously, certain complex metal cyanide ions
are either not affected by chlorination or react slowly. Iron
cyanogen complexes, although prone to photodecomposition,
are not readily decomposed by chlorine or hypochlorite
reagents at ambient temperature. It is believed that
complexation of cyanide treatment with iron salts at a n alkaline
pH will not be desirable in the future because all of the cyanide
removed would be converted to insoluble iron ferrocyanide. In
many instances, this product would have to be stored in a secure
landfill, unless it somehow would become immediately
reusable.
Electrolytic Oxidation
Electrolytic oxidation has been used to oxidize relatively high
concentrations (>IO0 mg/ L) of cyanide using a process that is
familiar to electroplaters and less expensive than chlorination
in the high-concentration range. Temperatures in the range of
60 to 82" C (140 t o 180" F) have been used, and carbon, copper,
stainless, and even steel electrodes have been employed. The
reaction produces cyanate, carbonate, and may result in the
recovery of valuable metals. The treated effluent containing
normally less than 100 m g / L of CN can be further treated by
chlorination.
In the recent past, an attempt has been made to apply
electrolysis to dilute solutions using semiconductive beds of
carbon particles and/ or closely spaced electrodes. These
developments increase the efficiency of electrolysis; however, it
is doubtful that cyanide concentrations in all cases could be
reduced t o the limits set by all regulatory agencies for effluent
discharge t o streams.
Reaction with Aldehydes and Peroxygen Compounds
The reaction of formaldehyde with free cyanide to form
glycolonitrile (HOCHXN), as reported in the early literature,'
has been employed t o accelerate the oxidation of cyanide by
peroxygen compounds such as hydrogen peroxide in the
Kastone process." This reaction is enhanced by an increase in
temperature. The products of reaction in the treatment of a
commercial zinc plating solution have been reported as
follows:
20 percent of the cyanide to free ammonia,
33 percent to cyanate, and
34 percent to glycolic acid amide (HOCH2CONH2).
The reaction does not achieve complete oxidation and is
somewhat comparable to the first-stage oxidation with
chlorine. There are also byproducts that have a BOD demand
and contain TOC, unlike the byproducts of complete oxidation
with chlorine.
Oxidation by Ozone
Oxidation with ozonei4 merits additional consideration
particularly now that stringent limits are being imposed on
allowable chlorine residuals in discharges to surface waters,
These requirements would not be applicable to discharges into
sanitary sewers connected t o sewage treatment plants.
Although there has been a great deal of research in the past 30
years, only a few ozonation plants have been installed for the
removal of cyanide.
Additional studies will have to be made to establish whether
the consumption of ozone can be properly controlled. In
addition, it should be determined whether the oxidation of
cyanide proceeds io compietion and to wnat extent beyond the
cyanate state. According to the early l i t e r a t ~ r e ,the
' ~ amount of
ozone required to oxidize CN- to CNO- is I .88 Ib per Ib of CN.
'\
The rate of oxidation of cyanate is roughly one-fifthI6 that of
cyanide. The wide variation of ozone demand (3.05 to 5.94 Ib
O3/lb CNO-) would indicate that the oxidation of cyanate is not
the only ozone reaction occurring.
The more recent literature" indicates that the time required
for the oxidation of cyanide t o cyanate is decreased from 12t o 4
min by increasing the concentration of ozone in the gas feed
from 1 to 2 percent. This effect of concentration of ozone is
confirmed by other i n ~ e s t i g a t o r s . ' ~ ' ' Furthermore,
~'~~
there
appears to be agreement that the oxidation of cyanate is
considerably slower (60 min) than that of cyanide t o cyanate
and that a pH of 6 to 6.5 is beneficial. There is also agreement in
recently published literature that the utilization of ozone is
enhanced by proper injection and dispersion procedures.
From the standpoint of rapidity of treatment, chlorine would
be preferred to ozone. Operating cost comparisons including
amortization of capital investment favor chlorine over ozone in
plating wastes. From a cost-saving standpoint, ozone may be
favored over chlorine for treatment of cyanides in the presence
of ammonia, which does not consume additional n?one but
would consume additional chlorine.
Removal of Cyanide by Ion Exchange
Removal of cyanide by ion exchange is certainly a possibility.
But there may be a problem with the removal of complex
metallo-cyanides present during regeneration of the anionexchange resin or preci itation of the metal cyanide salt on
the cation exchanger.'
This does not present a great
problem when ion exchangers are used in conjunction with
rinses from silver o r gold plating operations. In those cases the
resin can be thermally destroyed and the precious metals are
profitably recovered.
A system developed in the last few years that removes cyanide
as ferrocyanide2*uses a strongly basic macroreticular anionexchange resin with an acrylic matrix and a solution in which
the cyanide ion has been coverted to ferrocyanide by the
addition of a ferrous salt. The resin has selectivity for
ferrocyanides and a capacity of 0.106 to 0.202 meq of CN per
mL of resin (1.2 to 2.3 Ib/ft3). Little loss in capacity has resulted
from 91 cycles in laboratory studies using plant wastewater
when regenerating with 15 percent sodium chloride.
This method, aithough promising, does not appear to have
the desired practicality because of the unpredictability of the
reaction between the ferrous ion and cyanide resulting in either
a n incomplete reaction o r in the formation of insoluble iron
ferrocyanide, plus the possibility of a cyanide leakage in excess
of the regulatory agencies' limitations. In addition, most
leakage would be present as ferrocyanide ion, which would not
be removed by chlorination within a practical length of time.
Reverse Osmosis
Reverse osmosis offers a means for recovering or removing
simple and complex cyanide ions. There are both hollow-fiber
and spiral-wound membranes that operate in a broader p H
range than in the past.23
As in the case of ion exchange, reverse osmosis merely
concentrates the dissolved constituents. Thus it will also
concentrate the impurities which may render some of the
recovered concentrates unsuitable. In some cases. the
concentrates would have t o be treated for destruction of
cyanide prior to the electrolytic recovery of metals such as
copper, zinc and cadmium. It should be remembered that many
applications of reverse osmosis are defeated by chemical
characteristics of the solutions and by inadequate pretreatment.
These problems usually can be resolved by chemical treatment
to remove or complex cations that would precipitate or by
fiitration o i particulate matter.
56
Adsorption on Activated Carbon
The use of activated carbon for the removal of cyanide ha
been tried with and without catalysts by a number
researcher^.'^ However, it does not offer a promising solutio
from a commercial standpoint.
Biooxidat ion
Removal of cyanide by biooxidation has been practiced for;
least 50 yr at a variety of sewage treatment plants. Whetherth
was achieved by design or by accident, it is nevertheless a fea
Although cyanide ion or hydrogen cyanide is considered toxl
to biologically active organisms, this statement is nc
necessarily true when applied to bacteria or microorganism
that have been acclimated to handle certain concentratio
ranges of cyanide. The effluent from a number of byproduc
coke plants is treated biologically for the removal for cyanid
and other compounds containing cyanogen radicals.
Probably the most classical work on activated slude
treatment of cyanide, cyanate, and thiocyanate was perform
' authors reported tha
in 1962 by Ludzack and S ~ h a f f e r . ~The
cyanide, cyanate, and thiocyanate could be effectively degrade1
after two to three weeks of acclimation. A concentration ofC'
greater than 60 mg/ L affected the effectiveness of treatmeni
Biological sludges containing thiocyanate acclimated mor
rapidly than cyanide or cyanate sludges. T h e latter wer
unstable and were affected by changes in condition and loadini
that were acceptable to CN or SCN sludges. Low operatin!
temperatures resulted in lower efficiency and eventual failmt
Biological sludges containing cyanate and thiocyanate were lesi
sensitive to the effects of low temperatures than cyanid:
sludges. Slug dosages of cyanide temporarily disrupted tk
biological process. However, cyanate and thiocyanate slut
dosages had little effect.
Our studies on a laboratory scale using coke-oven wastewale1
indicated that a two-stage biological system was very effem
in reducing cyanide and thiocyanate in the presence of phenok
substances. Phenol and cyanide concentrations were reduced10
the first stage to within I mg/ L in less than 2 days; thiocyanate
concentrations were reduced in the second stage to less than:
mg/L, as CN. This achievement in the laboratory unda
controlled conditions does not mean that the same limits alWa!v
ca:: be attained on a commeicia! jG&. '4 deairab:e fcam
would be to make available provisions for physical-chemic2
treatment of the effluent to remove residual cyanide in Ik
effluent. The treatment would utilize chlorination. Whfl
phenols such as in wastewater from coke-oven plants aR
present, this treatment would be preceded by adsorption O6
activated carbon.
REFERENCES
1. B. F. Dodge and D. C. Reams, Plating, 36, 463 (1949)
2. J. A. Dobson, Sewage Works Journal, 19, 1007 (1947)*,
3. A. E. J. Pettet and G. C. Ware, Chem. & Ind.. p. 12'.
(October 1, 1955).
4. B. F. Dodge and W. Zabban, PZating, 38, 561 (1951).!'
385 (1952).
5. H . S. Skovronek and M. K. Stinson, Plat. and Surf: flll
65, 24 (October 1977).
6. Standard Methods for the Examination of Water 8''.
WurrPwatPr, !4th Ed., .American P~b!ic He~h!! Assr
Washington, D C (1976).
7. Annual Book of ASTM Standards, Part 31- Water, Aa
SOC.for Testing and Materials, Philadelphia, P A ( 1979
p. 619.
8. EPA 625/6-74003, "Methods for Chemical Ana1Ps "
Water and Wastes," U.S. EPA, Washington, DC (J97*'
9. E. J . Serfass, R. B. Freeman. B. F. Dodge. and W. ZabbaP
Plating, 39, 267 (1952).
L Lancy and W. Zabban, Metalloberflache, 13,65 (March
cyanide has
number of
ing solution
1963).
G E. Eden, B. L. Hampson, and A. B. Wheatland, J. SOC.
Chem. Ind., 69, 224 (1950).
L Lancy and W. Zabban, “ASTM Special Tech, Publ. No.
337,” ASTM (1962); p. 32.
B c. Lawes, L. B. Fournier, and 0. B. Mathre, Plating, 60,
~ 0 (1973).
2
(hem. Eng., p. 63 (March 24, 1958).
c A. Walker and W. Zabban, Plating, 40, 77 (1953).
-,E. Sondak and B. F. Dodge, Plating, 48, 173 (1961).
K Stopka, Plat. and Surf: Fin., 67, 77 (May 1980).
F Novak, paper presented at Int’l. Ozone Inst. Conference,
Houston, TX (1979).
1 Bollyky, proc. Int’l. Ozone Inst. Con$, 1, 522 (1975).
G 1. Mathieu, ibid., 533.
c A. Walker and W. Zabban, Fluting, 40, 165 (1953).
Amber-Hi-Lites No. 155, “Ion Exchange Treatment
process for Selective Removal of Cyanide,” Rohm & Haas
LO., Philadelphia, PA (1977).
J K. McNultyandJ. W. Kubarewicz, Proc. 2ndEPAIAES
con& on Adv. Pollution Control, 88 (1979).
F E. Bernardin, person communication (1971).
F J. Ludzack and R. B. Schaffer, JWPCF, 34,320 (1962).
tcticed for at
Whether thl,
heless a feat
idered taxlc
ent is not
roorganismS
incentration
If byproduct
1 for cyanide
11s.
ated sludge
,s performed
eported thar
ely degraded
*ationof Ch
if treatment
nated more
latter were
8 and loading
w operatlng
itual failure
late were less
Tan cyanide
isrupted the
:yanate slug
ZABBAN
i wastewater
‘ery effectibc
e of phenolic
re reduced i n
, thiocyanate
o less than 2
atory under
limits always
rable feature
ical-chemical
anide in the
tion. Where
n plants are
isorption on
HELWICK
LOUTTHE AUTHORS
Walter Zabban is Chief Engineer and Technical Director of
Chester Engineers, 845 Fourth Ave., Coraopolis, P A
108. Mr. Zabban holdsdegrees in chemical engineeringfrom
B
I University o f Louisville and Yale University. H e began his
w r in environmental engineering in 1949 as a n associate on
S Research Project No. 10 a t Yale University. A u t h o r o f 34
blications o n wastewater treatment, Mr. Zabban i s a n
,unct associate professor a t the University o f Pittsburgh.
lobert Helwick is Chief Chemist a n d Manager o f the Concept
partment of The Chester Engineers. H e received a degree in
mistry f r o m the University o f Pittsburgh and i s a Certified
ifersional Chemist a n d a registered Professional Engineer.
has been involved in environmental engineering f o r m o r e
in 12 years and has authored six papers concerning
istewater treatment.
AES ILLUSTRATED LECTURES
Training BookleWColored Slides
24 Gold Electroplating - Part
1 Zinc and Cadmium Plating
I, General Principles
2 Plating on ZincDisCastings
3 Theory and Practice of
25 Chemistry for ElectroplaPhosphating
ters-Part I
26 Selection o f Electrodeposi4 Electrochemistry for Electroplaters
ted Coatings
5 Electroforming with Nickel
27 Chemistry for Electropla6 Metallurgy for Electroplaters-Part II
28 Sulfuric Acid Anodizing of
ters
Aluminum and Its Alloys
7 Cyanide Copper Plating
29 Cleaning and Pickling for
‘8 Modern Methods of SprayElectroplating
ing Paints, Resins and
30 Electropolishing
Coatings
31 Electricity for Electroplaters
9 Degreasing with Trichlor32 Hull Cell Tests for Quality
ethylene
Plating
10 Precious Metal Electro33 Electroless Plating of Metals
deposits
34 Decorative Chromium Plat11 Silver Plating
12 Factors Influencing Plate
ing
35 Treatment of Cyanide and
Distribution
Chromate Rinses
‘14 Fundamentals of Metal
36 Physical Measurements on
Cleaning
Electrodeposits
15 Stop-off Materials and
37 Practical Nickel Plating
Plating Rack Coatings
38 The Art and Science of
16 Bright Acid Sulfate Copper
Plating
17 Chromic Acid Anodizing of
AIuminum
18 C h r o m a t e Conversion
Coatings
19 Hard Chromium Plating
20 Filtration and CarbonTreatment of Plating Solutions
21 Design Precepts for Quality
Plating
22 Principles of Corrosion
*23 Mass Finishing
45. Safety in Plating 81 Finishing Shops
‘Training Booklets not available without slides
taining Memb“23.75
per set
(except “Electroforming wlth
Nickel,” $27.50). AES Student
Members receive 20 per cent
discount; Non-members-$38.75
(except “Electroforming with
Nickel,” $45.00)
Training Booklets Only (Slides
reproducedin biacic-ana-wniiein
text): Members-$4.50 per copy;
Non-member individuals or
companies-$6.00 per copy.
IMPORTANT! Member discounts
good for individual members
only. Companies that are not
Research Sustaining Members
may n o t receive special
discounts by placing orders
through an individual who is an
AES member. Ouantity Dis-
-_..-.-
l.””lllD
-..-:,-ha.-
m.mIIa”IS.
Training Booklets, Including 35
mm Slides: Individual Members,
AES Branches, Research Sus-
ORDER FORM
Please send m e the following lectures (by lecture number):
Enclosed is my check for $
(Please enclose an additional $1 .OO for postage and handling.)
Name
~
t63 (1949).
)07 (1947).
nd., p. 1232
Street
City
l(1951); 39,
-Water, Am.
, PA (1979);
Analysis of
-,-.
UL ( I Y / + l .
r,n7”\
I W. Zabban.
~
PLEASE CHECK AND FILL IN: 0 Master Charge 0 Bank AmericardNisa
IMPORTANT: Copy Account Number from your Charge Card
d Sur$ Fin.,
Water anti
ealth Assn.,
Zip
State
Interested in Authoring a Paper for P&SF?
Those of you interested in authoring an article for
p&SF should send the manuscript, or a request for
an “Instructions to Authors” form, to: Plating &
Surface Finishing, Editorial Dept., 1201 Louisiana
h e . , Winter Park, FL 32789. We accept material of
both piaciicai afid iechiiicai sigfiificafi~eifi all
dlsciplines of surface finishing.
Copy Number above your
Name on Charge Card
My Card
Expires
~
CREDIT CARD ORDERS WITHOUT YOUR SIGNATURE AND EXPIRATION
DATE CANNOT BE PROCESSED
~~-~
~
Mail to: AES Book Department, 1201 Louisiana Avenue,
Winter Park, FL 32789