Omni Solutions provides water treatment systems that use advanced oxidation processes to purify water. Their CBW system uses counter flow mixing, an advanced oxidative gas generator, and UV irradiation lamps to reduce bacteria and other contaminants by 99.9% without chemicals. The system injects oxidative gas generated on-site and exposes the water to UV light to generate hydroxyl radicals that safely and effectively treat the water.

2. OMNI SOLUTIONS
Headquartered in Madison, WI
Charlotte – Atlanta – Dallas – Chicago –
Los Angeles – Hong Kong - Shanghai
Experienced Industry Professionals
National Distribution
Local Support

3. CBW Process Water Treatment System
Water Inlet
Oxidative Gas
Injection Point
Water Outlet
Advanced
Oxidative Gas
Generator
Counter Flow
Mixing Design
Germicidal UV
Irradiation Lamp

4. INSTALLATION SCHEMATIC
Counter Flow
Mixing Design
Advanced Oxidative
Gas UV Generator
Water Outlet
Water Inlet
Venturi Manifold
Oxidative Gas
Injection Point
Germicidal UV
Irradiation Lamp
Ambient Air In
Oxidative Gas Supply Line

5. SYSTEM BENEFITS AND FEATURES
• Best Available Technology
• Modular and Scalable
• 99.9% Bacteria Reduction
• Low Maintenance
• Alarming Functions
• Chemical Free
• On Demand
• No Harmful Byproducts
• Reduction in COD and BOD
• Peace of Mind
• No Chemicals to Store of Ship
• User Friendly
• Green Technology
• Proven Technology Performance

6. ADVANCED OXIDATION GAS
UV GENERATOR SPECS
Patents Pending

7. ADVANCED OXIDATION GAS
GENERATOR BENEFITS
• 187 – 254 nm wave lengths
• Produces O3 (ozone), H2O2
(hydrogen peroxide), OH
(hydroxyl radicals)
• Low power consumption
• Low maintenance
• 8,760 hour lamp life
• Superior Disinfection
Patents Pending

8. UV WATER TREATMENT
SYSTEM SPECS

9. UV WATER TREATMENT
SYSTEM BENEFITS
• Chemical Free
• Addresses broad range of
pathogens
• NSF Standard 55 Class A
Certified
• 254 nm wave length
• Low power consumption
• Low maintenance
• 8,760 hour lamp life

10. ADVANCED OXIDATION PROCESS
Advanced oxidation processes (abbreviation: AOPs), in a broad sense, are a set of chemical
treatment procedures designed to remove organic (and sometimes inorganic) materials in
water and water by oxidation through reactions with hydroxyl radicals (·OH). In real-world
applications of wastewater treatment, however, this term usually refers more specifically to a
subset of such chemical processes that employ ozone (O3), hydrogen peroxide (H2O2) and/or UV
light. One such type of process is called in situ chemical oxidation.
Generally speaking, chemistry in AOPs could be essentially divided into three parts:
1.Formation of ·OH;
2.Initial attacks on target molecules by ·OH and their breakdown to fragments;
3.Subsequent attacks by ·OH until ultimate mineralization.
The mechanism of ·OH production (Part 1) highly depends on the sort of AOP technique that is used. For example, ozonation,
UV/H2O2 and photocatalytic oxidation rely on different mechanisms of ·OH generation:
UV/H2O2:
H2O2 + UV → 2·OH (homolytic bond cleavage of the O-O bond of H2O2 leads to formation of 2·OH radicals)
Ozone based AOP:
O3 + HO− → HO2
− + O2 (reaction between O3 and a hydroxyl ion leads to the formation of H2O2 (in charged form))
O3 + HO2
− → HO2· + O3
−· (a second O3 molecule reacts with the HO2
− to produce the ozonide radical)
O3
−· + H+ → HO3· (this radical gives to ·OH upon protonation)
HO3· → ·OH + O2

11. ADVANCED OXIDATION PROCESS
AOPs hold several advantages that are unparalleled in the field of water treatment:
1. They can effectively eliminate organic compounds in aqueous phase, rather than collecting or
transferring pollutants into another phase.
2. Due to the remarkable reactivity of ·OH, it virtually reacts with almost every aqueous pollutant without
discriminating. AOPs are therefore applicable in many, if not all, scenarios where many organic
contaminants must be removed at the same time.
3. Some heavy metals can also be removed in forms of precipitated M(OH)x.
4. In some AOPs designs, disinfection can also be achieved, which makes these AOPs an integrated
solution to some water quality problems.
5. Since the complete reduction product of ·OH is H2O, AOPs theoretically do not introduce any new
hazardous substances into the water.

12. RELATIVE STRENTH OF OXIDIZERS
OXIDIZING AGENT EOP(Mv) EOP VS CI2
Fluorine 3.06 2.25
Hydroxyl Radical 2.80 2.05
Atomic Oxygen 2.42 1.78
Ozone 2.08 1.52
Hydrogen Peroxide 1.78 1.30
Hypochlorite 1.49 1.10
Chlorine 1.36 1.00
Chlorine Dioxide 1.27 0.93
Oxygen (molecular) 1.23 0.90

13. HYDROXYL RADICALS
Names
IUPAC nameHydroxyl radical
Systematic IUPAC nameOxidanyl
[1]
(substitutive)
Hydridooxygen(•)
[1]
(additive)
Other namesHydroxy
Hydroxyl
λ
1
-Oxidanyl
Identifiers
CAS Number 3352-57-6
ChEBI CHEBI:29191
ChemSpider 138477
Gmelin Reference 105
Jmol 3D model Interactive image
KEGG C16844
PubChem 157350
InChI[show]
SMILES[show]
Properties
Chemical formula HO
Molar mass 17.01 g·mol
−1
Thermochemistry
Std molar
entropy (S
o
298)
183.71 J K
−1
mol
−1
Std enthalpy of
formation (ΔfH
o
298)
38.99 kJ mol
−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C
[77 °F], 100 kPa).
Infobox references

14. HYDROXYL RADICALS
The hydroxyl radical, •OH, is the neutral form of the hydroxide ion (OH−). Hydroxyl
radicals are highly reactive (easily becoming hydroxyl groups) and consequently
short-lived; however, they form an important part of radical chemistry. Most notably
hydroxyl radicals are produced from the decomposition of hydro peroxides (ROOH)
or, in atmospheric chemistry, by the reaction of excited atomic oxygen with water. It is
also an important radical formed in radiation chemistry, since it leads to the formation
of hydrogen peroxide and oxygen, which can enhance corrosion and SCC in coolant
systems subjected to radioactive environments. Hydroxyl radicals are also produced
during UV-light dissociation of H2O2 (suggested in 1879) and likely in Fenton
chemistry, where trace amounts of reduced transition metals catalyze peroxide-
mediated oxidations of organic compounds.

15. HYDROXYL RADICALS
The hydroxyl radical is often referred to as the "detergent" of the troposphere because it
reacts with many pollutants, decomposing them through "cracking", often acting as the first
step to their removal. It also has an important role in eliminating some greenhouse gases like
methane and ozone. The rate of reaction with the hydroxyl radical often determines how long
many pollutants last in the atmosphere, if they do not undergo photolysis or are rained out.
For instance methane, which reacts relatively slowly with hydroxyl radical, has an average
lifetime of >5 years and many CFCs have lifetimes of 50 years or more. Pollutants, such as
larger hydrocarbons, can have very short average lifetimes of less than a few hours.
The first reaction with many volatile organic compounds (VOCs) is the removal of a hydrogen
atom, forming water and an alkyl radical (R•).
•OH + RH → H2O + R•
The alkyl radical will typically react rapidly with oxygen forming a peroxy radical.
R• + O2 → RO•2
The fate of this radical in the troposphere is dependent on factors such as the amount of
sunlight, pollution in the atmosphere and the nature of the alkyl radical that formed it.

16. OZONE
Names
IUPAC nameTrioxygen
Identifiers
CAS Number 10028-15-6
ChEBI CHEBI:25812
ChemSpider 23208
EC Number 233–069–2
Gmelin Reference 1101
IUPHAR/BPS 6297
Jmol 3D model Interactive image
Interactive image
MeSH Ozone
PubChem 24823
RTECS number RS8225000
UNII 66H7ZZK23N
InChI[show]
SMILES[show]
Properties
Chemical formula O3
Molar mass 48.00 g·mol
−1
Appearance colorless to pale blue gas
[1]
Odor pungent
[1]
Density 2.144 mg cm
−3
(at 0 °C)
Melting point −192.2 °C; −313.9 °F; 81.0 K
Boiling point −112 °C; −170 °F; 161 K
Solubility in water 1.05 g L
−1
(at 0 °C)
Solubility very soluble in CCl4, sulfuric acid
Vapor pressure >1 atm (20 °C)
[1]
Refractive index(nD) 1.2226 (liquid), 1.00052 (gas, STP,
546 nm — note high dispersion)
[2]
Structure
Space group C2v
Coordination geometry Digonal
Molecular shape Dihedral
Hybridisation sp
2
for O1
Dipole moment 0.53 D

17. OZONE
Ozone (systematically named 1λ1,3λ1-
trioxidane and catena-trioxygen), or trioxygen, is an
inorganic molecule with the chemical formula O
3. It is a pale blue gas with a distinctively pungent smell. It is
an allotrope of oxygen that is much less stable than
the diatomic allotrope O2, breaking down in the lower
atmosphere to normal dioxygen. Ozone is formed from
dioxygen by the action of ultraviolet light and also
atmospheric electrical discharges, and is present in low
concentrations throughout the Earth's
atmosphere (stratosphere). In total, ozone makes up
only 0.6 ppm of the atmosphere.

18. OZONE
• OZONE IS THREE OXYGEN MOLECULES : O3
• IT IS 150% STRONGER THAN CHLORINE,
REACTS OVER 3,000 TIMES FASTER
• LEAVES NO HARMFUL BYPRODUCTS
• OVER 90% OF BOTTLED WATER IS PURIFIED
WITH OZONE
• BEEN USED FOR OVER 100 YEARS IN WATER
TREATMENT

19. OZONE
Oxidation
Because of its high oxidation potential ozone can precipitate a variety of
organic and inorganic contaminants from pool water via direct filtration
including iron, manganese, sulfides, metals, body oils, sweat and saliva
among others.
Disinfection
Ozone kills bacteria, cysts and viruses up to 3,125 times faster than
chlorine which is one reason it it used to purify municipal drinking water
and bottled water worldwide.
Taste and Odor Control
Ozone oxidizes organic chemicals responsible for 90% of
taste/odor/color related problems
Kills Algae Spores
Ozone effectively kills algae spores in the contact system, but an
additional algaecide, like PhosFee from Natural Chemistry, Inc., is
needed to control algae in pools treated exclusively with ozone.

20. OZONE
Oxidation
Because of its high oxidation potential ozone can precipitate a variety of
organic and inorganic contaminants from pool water via direct filtration
including iron, manganese, sulfides, metals, body oils, sweat and saliva
among others.
Disinfection
Ozone kills bacteria, cysts and viruses up to 3,125 times faster than
chlorine which is one reason it it used to purify municipal drinking water
and bottled water worldwide.
Taste and Odor Control
Ozone oxidizes organic chemicals responsible for 90% of
taste/odor/color related problems
Kills Algae Spores
Ozone effectively kills algae spores in the contact system, but an
additional algaecide, like PhosFee from Natural Chemistry, Inc., is
needed to control algae in pools treated exclusively with ozone.

21. OZONEUltraviolet Light Ozone Production
UV ozone generators, or vacuum-ultraviolet (VUV) ozone generators, employ a light source
that generates a narrow-band ultraviolet light, a subset of that produced by the Sun. The Sun's
UV sustains the ozone layer in the stratosphere of Earth.
While standard UV ozone generators tend to be less expensive, they usually produce ozone
with a concentration of about 0.5% or lower. Another disadvantage of this method is that it
requires the air (oxygen) to be exposed to the UV source for a longer amount of time, and any
gas that is not exposed to the UV source will not be treated. This makes UV generators
impractical for use in situations that deal with rapidly moving air or water streams (in-duct
air sterilization, for example). Production of ozone is one of the potential dangers of ultraviolet
germicidal irradiation.
VUV ozone generators are used in swimming pool and spa applications ranging to millions of
gallons of water. VUV ozone generators, unlike corona discharge generators, do not produce
harmful nitrogen by-products and also unlike corona discharge systems, VUV ozone
generators work extremely well in humid air environments. There is also not normally a need
for expensive off-gas mechanisms, and no need for air driers or oxygen concentrators which
require extra costs and maintenance.

22. HYDROGEN PEROXIDE
Names
IUPAC namehydrogen peroxide
Other namesDioxidane
Oxidanyl
Identifiers
CAS Number 7722-84-1
ChEBI CHEBI:16240
ChEMBL ChEMBL71595
ChemSpider 763
EC Number 231-765-0
IUPHAR/BPS 2448
Jmol 3D model Interactive image
KEGG D00008
PubChem 784
RTECS number MX0900000 (>90% soln.)
MX0887000 (>30% soln.)
UNII BBX060AN9V
UN number 2015 (>60% soln.)
2014 (20–60% soln.)
2984 (8–20% soln.)
Properties
Chemical formula H2O2
Molar mass 34.0147 g/mol
Appearance Very light blue color; colorless in
solution
Odor slightly sharp
Density 1.11 g/cm
3
(20 °C, 30% (w/w)
solution )
[1]
1.450 g/cm
3
(20 °C, pure)
Melting point −0.43 °C (31.23 °F; 272.72 K)
Boiling point 150.2 °C (302.4 °F; 423.3 K)
(decomposes)
Solubility in water Miscible
Solubility soluble in ether, alcohol
insoluble in petroleum ether
Vapor pressure 5 mmHg (30 °C)
[2]
Acidity (pKa) 11.75
Refractive index(nD) 1.4061
Viscosity 1.245 cP (20 °C)
Dipole moment 2.26 D

23. HYDROGEN PEROXIDE
Hydrogen peroxide is a chemical compound with the formula H2O2. In its pure form, it is a
colorless liquid, slightly more viscous than water; however, for safety reasons it is normally
used as a solution. Hydrogen peroxide is the simplest peroxide (a compound with an oxygen–
oxygen single bond) and finds use as a weak oxidizer, bleaching agent and disinfectant.
Concentrated hydrogen peroxide, or "high-test peroxide", is a reactive oxygen species and has
been used as a propellant in rocketry.
Hydrogen peroxide is often described as being "water but with one more oxygen atom", a
description that can give the incorrect impression of significant chemical similarity between the
two compounds. While they have a similar melting point and appearance, pure hydrogen
peroxide will explode if heated to boiling, will cause serious contact burns to the skin and can
set materials alight on contact. For these reasons it is usually handled as a dilute solution
(household grades are typically 3–6% in the U.S. and somewhat higher in Europe). Its
chemistry is dominated by the nature of its unstable peroxide bond.

24. HYDROGEN PEROXIDE
Hydrogen peroxide was first described in 1818 by Louis Jacques Thénard, who produced it
by treating barium peroxide with nitric acid. An improved version of this process used
hydrochloric acid, followed by addition of sulfuric acid to precipitate the barium
sulfate byproduct. Thénard's process was used from the end of the 19th century until the
middle of the 20th century.
Pure hydrogen peroxide was long believed to be unstable, as early attempts to separate it
from the water, which is present during synthesis, all failed. This instability was due to traces
of impurities (transition-metal salts), which catalyze the decomposition of the hydrogen
peroxide. Pure hydrogen peroxide was first obtained in 1894 — almost 80 years after its
discovery — by Richard Wolffenstein, who produced it by vacuum distillation.
Determination of the molecular structure of hydrogen peroxide proved to be very difficult. In
1892 the Italian physical chemist Giacomo Carrara (1864–1925) determined its molecular
mass by freezing-point depression, which confirmed that its molecular formula is H2O2. At
least half a dozen hypothetical molecular structures seemed to be consistent with the
available evidence. In 1934, the English mathematical physicist William Penney and the
Scottish physicist Gordon Sutherland proposed a molecular structure for hydrogen peroxide
that was very similar to the presently accepted one.

25. HYDROGEN PEROXIDE
Today, hydrogen peroxide is manufactured almost exclusively by the anthraquinone process,
which was formalized in 1936 and patented in 1939. It begins with the reduction of an
anthraquinone (such as 2-ethylanthraquinone or the 2-amyl derivative) to the corresponding
anthrahydroquinone, typically by hydrogenation on a palladium catalyst; the anthrahydroquinone
then undergoes to autoxidation to regenerate the starting anthraquinone, with hydrogen peroxide
being produced as a by-product. Most commercial processes achieve oxidation by bubbling
compressed air through a solution of the derivatized anthracene, whereby the oxygen present in
the air reacts with the labile hydrogen atoms (of the hydroxy group), giving hydrogen peroxide and
regenerating the anthraquinone. Hydrogen peroxide is then extracted, and the anthraquinone
derivative is reduced back to the dihydroxy (anthracene) compound using hydrogen gas in the
presence of a metal catalyst. The cycle then repeats itself.
The simplified overall equation for the process is deceptively simple:
H2 + O2 → H2O2
The economics of the process depend heavily on effective recycling of the quinone
(which is expensive) and extraction solvents, and of the hydrogenation catalyst.

26. POTABLE WATER STANDARDS
According to the EPA and the World Health Organization,
Ultraviolet Light and ozone generation is the ‘best available
technology’ to meet the worlds most demanding health issues.
For water to be considered potable (drinkable) water, the Safe
Drinking Water Act requires the Maximum Contaminant Level of
microorganisms to be below 200 MCL

27. TESTING RESULTS
Testing was completed by Minnesota Valley Testing Laboratories, Inc. The first
group of test results demonstrate the bacteria reduction in the water
recirculation loop on the CBW. In the report #1 Water is the post treatment
result on the first CBW machine, #2 Water is pre treatment water sample. In
this case we have a 99.92% reduction in bacteria. The test was repeated and
demonstrated, #3 Water is post treatment sample and #4 Water is pre
treatment sample. In this case we have a 99.89% reduction in bacteria.

28. TESTING RESULTS
Post treatment

29. TESTING RESULTS
Pre treatment
Pre treatment
Post treatment

30. TESTING RESULTS
A second round of testing was completed to ensure disinfection was being
maintained throughout the entire water recirculation loop. Samples were
drawn just before treatment and directly after treatment to demonstrate a
continuous disinfected water recirculation loop.

31. TESTING RESULTS

32. OMNI SOLUTIONS
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