Note: Descriptions are shown in the official language in which they were submitted.
~ 3 r~
STABLE COMPOSITIONS FOR USE AS
CORROSION INHIBITORS
Technical Field
The present invention is related to zinc-containing cor-
rosion inhibitor treatment compositions. The ability of zinc to
inhibit the corrosion of ferrous metals is, indeed, well known.
Accordingly, soluble zinc salts are vital ingredients of many cor-
rosion treatment programs. For example, U.S. 4,089,796 to Harris
et al discloses a corrosion inhibiting composition comprising zinc
and hydrolyzed polymaleic anhydride or soluble salt thereof and
benzotriazole. Other exemplary patents disclosing such zinc
containing treatments are U.S. 3,432,428 to Wirth et al and U.S.
4,1ZO,655 to Crambes et al.
<
An art-recognized major problem encountered with zinc-
containing treatments, particularly in cooling water, is the un-
controlled preclpitation of zinc salts; because, to be effective,
the z~nc must reach the surfaces to be protected in a soluble form.
For example, the use of orthophosphate in combination with zinc as
a cooling water treatment is well known as evidenced by U.S.
2,900,222 to Kahler et al wherein phosphate, chromate and zinc
are used in combination. The orthophosphate can be provided as
20 an actual addition, or as a reversion product from any one of
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.
.
: . . . . .
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. .
-2-
complex inorganic phosphate, organic phosphate or organic phos-
phonate. When orthophosphate and zinc are both present in the
water, zinc phosphate precipitation becomes a concern. Whether
or not orthophosphate is present, the zinc could precipitate in
other forms, for example, as zinc hydroxide or zinc silicate. The
solubility of the various salts, that is, the retention of the
respective salt constituents in ionic form, depends on such factors
as water temperature and pH and ion concentrations. Wirth et al
states that although water temperatures can vary from 32 to 200F,
lower temperatures of 32 to 80F are preferred because "zinc tends
to remain in solution better in cooler waters." This patent further
states that alkaline waters, particularly above about pH 7.5, are
relatively undesirable because "the dissolved zinc tends to deposit
out or drop out much more rapidly in alkaline water." Similarly,
Crambes et al points out that zinc salts are unstable in neutral or
alkaline water and will precipitate with phosphates. Thus, if any
of these conditions are present, the aqueous medium becomes prone
to zinc precipitation. Because of the formation of this zinc scale,
many of the surfaces in contact with the aqueous medium will foul
and the amount of effective (soluble) corosion inhibitor present
in the aqueous medium can be significantly reduced.
Although the present invention is considered to have
general applicability to any aqueous system where zinc precipitation
is a problem, it is particularly useful in cooling water systems.
Accordingly~ the invention will hereinafter be described as it re-
lates to cooling water systems.
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Description of the Invention
There has existed for a long time the need for a zinc-
containing corrosion inhibitor treatment which overcomes the above-
noted problems, and the present invention is considered to fulfill
that need.
According to the present invention, a corrosion in-
hibitor treatment for metal surfaces exposed to an aqueous medium
comprises (i) water-soluble zinc compound and (ii) a particular
type of water-soluble polymer composed essentially of moieties -
derived from acrylic acid or derivatives thereof and hydroxylated
lower alkyl acrylate moieties (HAA). The treatment could addi-
tionally comprise (iii) orthophosphate. It was discovered that,
although the polymer demonstrated no significant activity alone
as a corrosion inhibitor, when it was combined with a zinc-contain-
ing treatment the various ionic constituents of the treatment wereunexpectedly retained in their soluble form and a corresponding
increase in corrosion inhibiting activity was observed.
The Polymer
The polymers according to the present invention are
those effective for the purpose which contain essentially
moieties derived from an acrylic acid compound (AA), i.e.,
' ~
--4--
~ CH2-- t ( I )
C =O
Rl
where R is hydrogen or a lower alkyl of from 1 to 3 carbon atoms
and R1 = OH, NH2 or OM, where M is a water-soluble cation, e.g.,
NH4, alkali metal (K, Na), etc; and moieties of an hydroxylated
lower alkyl (C2-C6~ acrylate (HAA) as represented, for example,
by the formula:
IR3 ' I I
--CH2--C--
C = O (II)
I
O
R2 - OH
where R3 is H or lower alkyl of from 1 to 3 carbon atoms, and R2
is a lower alkyl having from about 2 to 6 carbon atoms.
In terms of mole ratios, the polymers are considered,
most broadly, to have a mole ratio of M :HAA of from about 1:4 to
36:1. This mole ratio is preferably about 1:1 to 11:1, and most
preferably about 1:1 to 5:1. The only criteria that is considered
to be of importance with respect to mole ratios is that it is
des1rable to have a copolymer which is water-soluble. As the
proport10n of hydroxylated alkyl acrylate moieties increases, the
solubil~ty of the copolymer decreases. It is noted that, from an
efficacy point of view, the polymers having a mole ratio of AA:HAA
of 1:1 to 5:1 were considered the best.
'
C~
--5--
The polymers could have a molecular weight of from about
1,000 to about 50,000 with from about 2,000 to about 6,000 being
preferred.
The polymers utilized in accordance with the invention can
be prepared by vinyl addition polymerization or by treatment of an
acrylic acid or salt polymer. ~ore specifically, acrylic acid or
derivatives thereof or their water soluble salts, e.g., sodium, pot-
assium, ammonium, etc. can be copolymerized with the hydroxy alkyl
acrylate under standard copolymerization conditions utilizing free
radical initiators such as benzoyl peroxide, azobisisobutyronitrile
or redox initiators such as ferrous sulfate and ammoniu~ persulfate.
The molecular weights of the resulting copolymer can be controlled
utilizing standard chain control agents such as secondary alcohols
(isopropanol), mercaptans, halocarbons, etc. Copolymers falling
within the scope of the invention are commercially available from,
for example, National Starch Company.
The hydroxy alkyl acrylate can be prepared by the addition
reaction between the acrylic acid or its derivatives or water solu- -
ble salts and the oxide of the alkyl derivative desired. For ex-
ample, the preferred monomer of the present invention is the propyl
derivative. Accordingly, to obtain the hydroxylated monomer, acry-
lic ac1d is reacted with propylene oxide to provide the hydroxy-
propyl acrylate monomer.
The polymers of the invention may also be prepared by re-
acting a polyacrylic acid or derivatives thereof with an appropriateamount of an alkylene oxide having from 2 to 6 carbon atoms such as
ethylene oxide, propylene oxide and the like. The reaction takes
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35~1
-6--
place at the COOH or COM group of the moieties to provide the hydro-
xylated alkyl acrylate moiety.
The polymer prepared either by copolymerization of M with
hydroxy propyl acrylate (HPA) or reaction of AA with propylene oxide
would be composed of units or moieties having the structural
formulas:
_ - CH2 - C - - and CH2 C -
Cl = O C = O
10 0 ~H2
where M is as earlier defined.
The Zinc Compounds
Illustrative water-soluble zinc compounds which are
considered to be suitable for use in accordance with the present
invention are zinc oxide, zinc acetate, zinc chloride, zinc
formate, zinc nitrate, zinc sulphate, zinc borate, zinc chromate,
zinc dichromate, etc.
9~
--7--
The Orthophosphate Compounds
As already noted above, the treatment could further com-
prise orthophosphate. Indeed, the use of zinc and orthophosphate
together as a corrosion inhibition treatment is well known. It has
also already been noted that the orthophosphate could be provided as
an actual addition product, e.g., sodium orthophosphate, or as a
precursor compound such as complex inorganic phosphates, organic
phosphates or organic phosphonates which revert to orthophosphate in
the water.
Illustrative examples of orthophosphate as an actual addi- -
tion are monosodium phosphate, and monopotassium phosphate. Any
other water-soluble orthophosphate or phosphoric acid would also be
considered to be suitable.
The complex inorganic phosphates are exemplified by sodium
pyrophosphate, sodium tripolyphosphate, sodium tetraphosphate,
sodium septaphosphate, sodium decaphosphate and sodium hexameta-
phosphate. Either the corresponding potassium or ammonlum salts or
the corresponding molecularly dehydrated phosphoric acids such as
metaphosphoric acid or pyrophosphoric acid are considered to be
2~ suitable.
The organic phosphonates are exemplified by aminotri-
methylene phosphonic acid, hydroxyethylidene diphosphonic acid and
the water-soluble salts thereof.
Organic phosphates are exemplified in U.S. 3,510,436.
: .
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The amount of each constituent added to the cooling water
will, of course, be an effective amount for the purpose and will
depend on such factors as the nature and severity of the corrosion
problem being treated, the temperature and pH of the cooling water
and the type and amount of precipitation-prone ions present in the
water.
In terms of active zinc ion, as little as about 0.5 parts
of zinc per million parts (ppm) of cooling water are believed to
be effective in certain instances, with about 2 ppm being preferred.
Based on economic considerations, the amount of zinc ion added could
be as high as about 25 ppm, with about 10 ppm representing the pre-
ferred maximum.
In terms of active polymer, as little as about 0.5 ppm
polymer is considered to be effective, while about 2 ppm is the
preferred minimum. Based on economic considerations, the polymer
could be fed in amounts as high as about 200 ppm, with about 50 ppm
representing the preferred maximum.
In terms of active product added, the orthophosphate or
precursor compound thereof could be fed in an amount as low as about
1 ppm, with about 2 ppm representing the preferred minimum. Based
on economic considerations, the maximum amount is considered to be
about 200 ppm. However, about 50 ppm is considered to be the pre-
ferred maximum.
Methods for feeding corrosion inhibitors to cooling water
are well known in the art such that details thereof are not consid-
.
,
-9-
ered necessary. However, due to rather severe stability problems
experienced when the polymer was stored at high concentrations with
the remaining components, a two or three-barrel treatment is recom-
mended.
Compositions according to the present invention could com-
prise on a weight basis:
(i) about 1 to about 95% of water-soluble zinc compound,
and
(ii) about 5 to 99% AA/HAA polymer of the total amount of
zinc compound and polymer. The preferred relative proportions are
about 5 to 85% water-soluble zinc compound and about 15 to 95% poly-
mer; while it is most preferred that the compositions comprise about
4 to 70% zinc compound and about 30 to 96% polymer.
In those instances where orthophosphate is also present,
compositions according to the present invention could comprise on a
we1ght basis:
(i) about 1 to 95~ water-soluble zinc compound
(ii) about 5 to 99% AA/HAA po1ymer, and
(iii) abo~t 1 to 95% orthophosphate (or precursor there-
of) of the total amount of zinc compound, polymer and orthophos-
phate.
.
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.
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-10-
The preferred relative proportions are about 5 to 85% zinc com-
pound, about 15 to 95% polymer and about 5 to 85% orthophosphate.
The most preferred relative proportions are about 10 to 60% zinc
compound, about 15 to 80% polymer and about 10 to 60% ortho-
phosphate.
The cooling water preferably will have a pH of about
6.5 to about 9.5. Since zinc precipitation problems most commonly
occur at pH's above about 7.5, the most preferred pH range is from
about 7.5 to about 9.5.
i
EXAMPLES
Illustration of Zinc Precipitation Problem
Example 1
As noted above, an art-recognized major problem encoun-
tered with zinc-containing treatments, particularly in cooling
water, is the uncontrolled precipitation of zinc salts from the
water. Even in the absence of orthophosphate in the water, the
zinc can form precipitates such as zinc hydroxide.
This point is illustrated by the zinc-solubility results
of several tests conducted in water containing no orthophosphate.
The tests were conducted, inter alia, to determine the solubility
of zinc in the test water as a function of pH.
;
:
The following aqueous test solutions were first prepared:
Solution A: 1,000 ppm Zn++ obtained from
0.27 gram Zn-S04 H20/100 ml
SCW7: 170 ppm Ca as CaC03,
110 ppm Mg as CaC03
15 ppm SiO2 :
The tests were conducted using the following procedure:
1. Prepare SCW7 (detailed in Example 5 below) and adiust
its pH to 4 with concentrated HCl.
2. To 2,000 ml of the above solution, add the required
amount of Solution A with stirring.
3. Add 100 ml of the solution from step 2 to a bottle and
agitate.
4. Slowly adjust the pH to the desired value with dilute
NaOH solution and record pH.
5. Place the samples in an oven at the required temper-
rature for 24 hours, after which time, filter through a 0.2 micron
millipore filter.
6. Analyze the filtrate for soluble zinc and record final
pH.
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.
The results of these tests are reported below in Tables 1 ~.
and 2 in terms of soluble zinc (ppm) remaining after 24 hours at
various final pH values.
' TABLE 1
ZINC PRECIPITATION AS FUNCTION OF pH
Conditions: Initial Zinc = 2 ppm as Zn+~
T = 120F
Time = 24 hours :
pH soluble zinc (ppm)
7.62 0.8
7.70 0.5
7.92 0.5
8.12 0.2 `
8.21 0.1
8.35 0.2
8.42 0.1
8.76 o.Q
.
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TABLE 2
ZINC PRECIPITATION AS FUNCTION OF pH
Conditions: Initial Zinc = 10 ppm as Zn++ ~:
T = 120F
Time = 24 hours
pH soluble zinc (ppm)
7.15 8.2
7.25 7.8
7.36 8.2
7.46 8.0
7.50 7.8
7.56 5.4
7.67 1.8
7.70 1.6
8.05 0.4
8.10 0.2
8.22 0.4
8.65 0.2
9.06 0.0
.
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-14-
Example 2
The problem of zinc precipitation in cooling water is
further illustrated by the zinc-solubility results of additional
tests similar to those in Example 1, but conducted in water con-
taining both zinc ions and orthophosphate ions.
The following aqueous test so1utions were first prepared:
Solution A: 1,000 ppm P04~3, obtained from
0.400 gram Na3P04~12H20/100 ml
Solution B: 1,000 ppm Zn+2, obtained from
0.27 gram ZnS04 H20/100 ml
SCW7: Same as Example 1
The following procedure was used:
1. Prepare SCW7 and adjust its pH to 4 with HCl
solution.
2. To 2,000 ml of the above solution, add the appro-
priate amount of Solution A, followed by the
appropriate amount of Solution B with agitation.
3. Add 100 ml of the solution from step 2 to a bottle
and adjust the pH to 7.5 with dilute NaOH with
agitation.
,. . . . ......
5~
-15-
4. Place the samples in an oven for 24 hours at the
appropriate temperature.
5. After the 24 hour period, filter the solution through
a 0.2 micron millipore filter.
6. Analyze the filtrate for zn+2 and P04~3.
The results of these tests are reported below in Tables 3
and 4 in terms of ppm soluble zinc and ppm soluble phosphate remain-
ing after 24 hours at various final pH values.
TABLE 3
ZINC PRECIPITATION AS FUNCTION OF pH
Conditions: Initial Zinc = 5 ppm as Zn++
Initial o-P04 = 10 ppm
T = 120F
Time = 24 hours
pH soluble zinc (ppm) soluble PO4 (ppm~
7.0 3 6
7.5 0.5 5
8.0 0.1 3.7
8.5 0.1 2.4
9.0 0.1 1.2
.
. .
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-16-
TABLE 4
ZINC PRECIPITATION AS FUNCTION OF pH
. Conditions: Initial Zinc = 10 ppm as Zn++
Initial o-P04 = 5 ppm
T = 120F
Time = 24 hours
pH soluble zinc (ppm) soluble P04 (ppm)
7,5 3.3 0.8
B.O 0.2 0.7
9.0 0.1 0.1
EFFICACY IN RETAINING SOLUBLE ZINC-CONTAINING TREATMENTS
Example 3
A series of tests were conducted to determine the efficacy
of various materials in retaining zinc-containing corrosion inhib-
ition treatments in a soluble form. After all, the corrosion in-
hibition efficacy of such treatments will, for the most part, depend
on the constituents remaining soluble.
The test water contained both zinc and orthophosphate
10ns, and the test procedures were the same as in Example 2 but
for a few different steps as follows:
$~ :
-17-
1. Solution C comprising 1,000 ppm of active treatment
was also used.
3. Add 100 ml of solution from step 2 to a bottle, add
the appropriate quantity of treatment solution
(1 ml = 10 pp0), and adjust pH to appropriate value
with dilute NaOH with agitation.
The results of the tests were calculated in terms of ~O in-
crease in retention of soluble zinc ions and soluble phosphate ions
vs. an untreated solution using the following equation:
~ Retention =
100 x Sol.POa at T=24 hrs-Sol. PO4 in control at T=24 hrs.
Sol. PO4 in control at T=O hrs-Sol. PO4 in control at T=24 hrs.,
where Sol. PO4 = soluble PO4 in ppm. Of course, a similar
equation was used for zinc calculations.
The results of these tests are reported below in Tables 5
and 6 In addition to testing various M /HPA copol~ymers in accordance
with the present invention, various commercial polyacrylic acids
(P M ) were also tested.
.
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Example 4
A further series of tests were conducted to demonstrate
the efficacy of various M /HPA polymers in retaining soluble zinc
in an aqueous medium. The tests were the same as those of Example
3 except for the absence of orthophosphate from the test solutions.
The results of these tests are reported below in Tables
7-13 in terms of ppm soluble zinc retained in solution. For pur-
poses of comparison with untreated test solution, Table 7 should
be compared with the results of Table 1 and Tables 8-13 should be -
compared with the results of Table 2.
Visual comparisons of Table 7 with Table 1 and Tables 8-13
with Table 2 are provided in the accompanying drawing.
!, ~
In Fig. 1 are presented a series of graphs which con-
tain comparisons of Table 7 with Table 1 in terms of soluble zinc
remaining in solution after 24 hours vs. pH of the test water. As
can be seen from the figure, the lowermost graph represents a no
treatment test wherein the zinc readily precipitates. In compari-
son, the higher graphs represent various test solutions to which
have been added the noted AA/HPA polymers. The polymers were all
considered to be efficacious in retaining soluble zinc in solution.
Remaining Figs. 2-7 provide visual comparisons of respec-
t1ve ones of Tables 8-13 with Table 2. Fig. 2 compares Table 8,
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-24-
Fig. 3 compares Table 9, F;g. 4 compares Table 10, Fig. S compares
Table 11, Fig. 6 compares Table 12, and Fig. 7 compares Table 13,
all with Table 2 in terms of plots of soluble zinc remaining in
solution after 24 hours vs. pH at various indicated treatment
levels. The line marked "No Treatment" in each figure represents
the results of Table 2.
i :
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TABLE 7
ZINC RETAINED AS COMPARED T0 TABLE 1
Conditions: Initial Zinc = 2 ppm as Zn++
T = 120F
Time = 24 hours
Treatment = AA/HPA
Dosage = 5 ppm actives
:. :
Mole Ratio Molecular Water Soluble Zinc
AA:HPA Weight pH Retained (ppm)
101.8:1 6,000 8.27 1.8
" " 8.42 1.7
" " 8.78 1.8 :
" " 8.86 1.7
" " 9.10 0.9
159.9:16,000-10,000 ~.59 1.7
" " 7.85 1.7
7.95 1.7
" " 8.00 1.8
" " 8.4~ 1.6
20 " " 8.72 1.6
" " 8.94 1.5
3:1 6,000 7.50 1.8
" " 7.85 1.8
" " 8.21 1.9
25 " " 8.54 1.8
" " 8.67 1.6
" " 8.94 1.5
" " 9.06 1.2
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-26-
TABLE 7 (Continued)
Mole Ratio Molecular Water Soluble Zinc
AA:HPA Weight pH Retained (ppm~
9.9:1 1,000-2,000 7.68 1.9
" " 8.06 1.8
" " 8.21 1.7
" " 8.38 1.8
" " 8.51 1.5
" " 8.88 1.7
1019.8:1 2,000-6,000 7.79 1.7
" " 7.92 1.8
" " 8.25 1.4
" " 8.50 1.4
" " 8.67 1.1
" " 8.92 0.7
36:1 2,000-6,000 7.84 1.7
" " 8.05 1.8
" " 8.65 1.7
" " 8.88 1.6
" " 8.95 1.6
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-27-
TABLE 8
ZINC RETAINED AS COMPARED TO TABLE 2
Conditions: Initial Zinc = 10 ppm as Zn++
T = 120F
Time = 24 hours
Treatment = AA/HPA, Mole Ratio M :HPA = 1.8:1,
Molecular Weight = 6,000
WaterTreatment Dosage Soluble Zinc
pH (ppm actives) _Retained (ppm)
10 7.50 5 8.6
7.60 5 10.0
7.75 5 5.4
7 79 5 6.6
7.92 5 5.0
15 7.g6 5 4.4
8.26 5 0.2
8.30 5 0.6
8.42 5 0 4
8.48 5 1.6
20 8.60 5 0.8
7.61 10 8.0
7.70 10 8.4
7.90 10 8.0
::
-28-
TABLE 8 (Continued)
-
Water Treatment Dosage Soluble Zinc
pH Ippm actives) Retained (ppm)
8.00 10 8.2
5 8.27 10 8.4
8.75 10 8.0
8.90 10 8.6
9.02 10 7.4
9.18 10 6.8 :
109.23 10 3.4
8.82 20 9.4 -
8.88 20 9.8
9.13 20 10.0 .
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-29- :
TABLE 9
ZINC RETAINED AS COMPARED TO TABLE 2
Conditions: Initial Zinc = 10 ppm as Zn++
T = 120F
Time = 24 hours
Treatment = AA/HPA, Mole Ratio M :HPA = 3
Molecular Weight = 6,000
Water Treatment Dosage Soluble Zinc
pH (ppm actives) Retained (ppm)
107.27 5 10
7.54 5 10
7,77 5 10
8.02 5 8.4
8.08 5 8.0
158.20 5 0.8
8.37 5 2.0
8.45 5 0.8 `~
8.55 5 0.0
7.62 10 7.8
207.90 10 7.6
8.00 10 8.0
8.29 10 7.0
8.34 10 8.4
,
,
:
59~
-30-
TABLE 9 (Continued)
.~
Water Treatment Dosage Soluble Zinc
pH (ppm acti~es) Retained (ppm) .
8.41 10 7.4
8.56 10 7.2
8.60 10 8.4
8.97 10 6.6
9.14 10 7.0
9.30 10 4.8
8.58 20 9.0
8.80 20 9.4
9.31 20 8.8
., . . ~, ..
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:. ~
~ 3r~ 3
TABLE 10
ZINC RETAINED AS COMPARED T0 TABLE 2
Conditions: Initial Zinc = 10 ppm as Zn++
T = 120F
Time = 24 hours
Treatment = AA/HPA, Mole Ratio M:HPA = 9.9:1,
Molecular Weight = 1,000-2,000
~,
WaterTreatment Dosage Soluble Zinc
pH(ppm actives) Retained (ppm)
107.60 5 8.6
7.72 5 8.0
7.80 5 6.6
7.93 5 5.0
8.04 5 3.2
158.27 5 1.2
8.35 5 1.0
7.53 10 9.0
7.75 10 10.0
7.97 10 10.0
208.15 10 9,4
8.30 10 6.6
8.48 10 8.4
8.65 10 6.8
- : .
1859`0
-32- :
TABLE 10 (Continued)
.:
Water Treatment DosageSoluble Zinc
pH (pDm actives) Retained (ppm) ~ -
8.72 10 : 5.6 :
8.92 10 6.0
9.10 10 5.0
9.25 10 4.4
8.65 20 7.6
8.90 20 7.2 '~
9.10 20 7.6
9.30 20 3.2
.
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... . .. . ...
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. . , . ' ,;; ' ~
.:, : . . .
. :, . , , , :
... . . . . . ~ . -
. , . .. , ,, ... . , . . . - . .
,... :. -., .. : ., , : .
,. i. . ;
3.~
TABLE 11
ZINC RETAINED AS COMPARED T0 TABLE 2
Conditions: Initial Zinc = 10 ppm as Zn++
T = 120F
Time = 24 hours
Treatment = AA/HPA, Mole Ratio M :HPA = 9.9:1,
Molecular Weight = 6,000-10,000
WaterTreatment Dosage Soluble Zinc
pH (ppm actives) Retained (ppm)
107.50 5 7.6
7.68 5 8.2
7.74 S 2.4
7.80 5 2.0
7.86 5 2.8 :-
157.88 5 0.8
8.20 5 0.6
8.27 5 0.2
8.58 5 0.2
8.10 10 8.4
208.13 10 8.4
8.20 10 8.2
8.25 10 8.6
8.50 10 7.2
"
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.
: ,.
-34-
TABLE 11 (Continued)
Water Treatment Dosage Soluble Zinc
pH (ppm actiYes) Retained (ppm)
8.74 10 6.0
9.01 10 7.4
9 . 14 10 7 . 6
9.32 10 - 3.8
~, ,.
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- '
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- ~ .:,. - . ::
~8~59
-35
TABLE 12
ZINC RETAINED AS COMPARED TO TABLE 2
Conditions: Initial Zinc = 10 ppm as Zn++
T = 120F
Time = 24 hours
Treatment = AA/HPA, Mole Ratio M :HPA = 19.8:1,
Molecular Weight = 2,000-6,000
.
Water Treatment Dosage Soluble Zinc
pH _ (ppm actives) Retained (ppm)
:
107.80 10 2.4
7.83 10 2.4
7.95 10 1.2
8.08 10 1.0
8.12 10 1.2
158.25 10 1.2
8.35 10 1.4
8.15 20 4.6
8.35 20 4.8
8.52 20 5.2
208.78 20 4.0
8.62 30 8.4
8.83 30 8.6
8.88 30 8.2
8.95 30 8.4
9.02 30 7-4
9.11 30 5.2
, ~
.. ..
TABLE 13
ZINC RETAINED AS COMPARED T0 TABLE 2
Conditions: Initial Zinc = 10 ppm as Zn++
T = 120F
Time = 24 hours
Treatment = AA/HPA, Mole Ratio M :HPA = 36:1, :
Molecular Weight = 2,000-6,000 ~
- - :
Water Treatment Dosage Soluble Zinc
pH (ppm actives) Retained (ppm) ~:
107.75 5 5.8
7,79 5 2.6
8.02 5 1.0
8.34 5 0.2
8.66 5 -
158.27 10 7.0
8.40 10 5.8
8.50 10 7.6
8.62 10 6.6 ~:
8.87 10 6.6
208.90 10 7.2
9.03 10 7.8
9.40 10 5.2
8.79 20 9.0
, , ' ~ ' ,
, .
,
. ' ' '
: '1,
,
. .
TABLE 13 (Continued)
_
Water Treatment Dosage Soluble Zinc
pH (ppm actives) Retained (ppm)
8.95 20 8.6
59.0~ 20 8.6
9.11 20 7.0
9.21 20 7.8
9.23 20 7.2
EFFICACY AS CORROSION INHIBITOR
:.
Example 5
Having already demonstrated both the zinc precipitation
problem related to zinc-containing corrosion inhibitor treatments
in aqueous mediums and the resolution of this problem by combining
the treatment with M/HM polymer, the following test results are
presented to demonstrate, from a corrosion inhibition point of view,
the benefits of the combined treatments.
The tests were each conducted with two non-pretreated low
carbon steel coupons which were immersed and rotated in aerated
synthet1c cool~ng water for a 3 or 4 day period. The water was ad-
~usted to the desired pH and readjusted after one day if necessary;
,
, . .;
,:
~859~) ~
:- `
-38-
no further adjustments were made. Water temperature was 120F.
Rotational speed was maintained to give a water velocity of 1.3
feet per second past the coupons. The total volume of water was
17 liters. Cooling water was manufactured to give the following
conditions:
SCW7 (pH=7) SCWg (pH=8)
ppm Ca as CaC03 170 170
ppm Mg as CaC03 110 110
ppm SiO2 15 15
ppm Na2C03 0 100
Corrosion rate measurement was determined by weight loss
measurement. Prior to immersion, coupons were scrubbed with a mix-
ture of trisodium phosphate-pumice, rinsed with water, rinsed with ~;
~sopropyl alcohol and then air dried. Weight measurement to the
nearest milligram was made. At the end of one day, a weighed coupon
was removed and cleaned. Cleaning consisted of immersion into a 50
solution of HCl for approximately 20 seconds, rinsing with tap
water, scrubbing with a mixture of trisodium-pumice until clean,
then rinsing with tap water and isopropyl alcohol. When dry, a
second weight measurement to the nearest milligram was made. At the
termination of the tests, the remaining coupon was removed, cleaned
and weighed.
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-39-
Corrosion rates were computed by differential weight loss
according to the following equation:
. Nth Da Wei ht Loss - lSt Day Weight Loss
5 Corroslon Rate ~ Y 9 N-1
where N = 3 or 4.
The cooling water was prepared by first preparing the
fo11owing stock solutions:
Solution A - 212.4 9 CaC12 2H20/l
Solution B - 229.9 9 MgS04 7H20/1
Solution C - 25.5 9 NaSiO3~9H20/1
Solution D - 85 9 Na2C03/1
Treatment Solutions - 1.7% solutions (1.7 9/100 ml)
Then, these solutions were combined using the following order of
addition:
1. To 17 1 of de-ionized water add, with stirring,
(a1 20 ml of Solution A, (b) 20 ml of Solution B and (c) 20 ml
of Solution C.
2. Adjust pH to 6.
3. With stirring add treatment (except Zn+2).
~ ~ .
, ~ , . --
35~
-40-
4. Add o-P04 Solution (if used).
S. Adjust pH to 7.0 if necessary.
6. Add zn+2 Solution (if used).
7. (a) For SCW7 adjust pH to 7Ø
5 (b) For SCWg add 20 ml of Solution D and adjust
pH to 8Ø
The results of these tests are reported below in Table
14 in terms of corrosion rates in mils per year (mpy).
. .
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-41 -
O Q CO 1
O ~_~
~7
Z +
J z E
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-
~o E I I o o u~ u~ ~ I I I I I u~ u~
O1 CL
~ 1 o 8 o o o o o o
~n O O I o I o o I o ) o o I o o I o o
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~, E m o I m I u~ ~n o o I Ln u7 1 !n Ln
o_ Z
91~)
-42-
While the comparative test results were not so pronounced
at pH = 7, the comparative results at pH = 8 were considered to be
rather dramatic, Even though the M /HPA polymer alone demonstrated
little, if any, efficacy as a corrosion inhibitor, when combined
with the zinc-containing treatments, the combined treatments
demonstrated significantly enhanced results as corrosion inhibitors.
For example, at pH = 8, the corrosion inhibition efficacy of 30 ppm
active polymer alone (86 mpy) and lO ppm zn+2 alone (84 mpy)
appeared to be non-existent as compared to the untreated system (82
mpy); however, when only 5 ppm polymer were combined with only 5 ppm
Zn~2, the corrosion rate decreased to 13.6 mpy.
Illustrative examples of stable aqueous compositions made
in accordance with the present invention are presented in Table 15
in terms of relative proportions (in weight percent) of the various
constituents. In these compositions, the water-soluble zinc com-
pound was ZnS04 H20 and the orthophosphate was Na3P04 12H20.
Since calculations were rounded-off to two places, not all composi-
tions added up to 100%. Stability is defined in terms of soluble
constituents in solution after 24 hours at 120F.
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-43-
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-44-
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