UNITED STATES ENVIRONMENTAL PROTECTION AGENCY 

WASHINGTON D.C., 20460 

OFFICE OF CHEMICAL SAFETY 

AND POLLUTION PREVENTION 

September 24, 2012 

MEMORANDUM 

SUBJECT: 

FROM: 

THRU: 

TO: 

Product Chemistry, Environmental Fate, and Ecological Effects Scoping 

Document in Support of Registration Review of Ammonium Bromide 

PC Code: 000352 DP Barcode: 401471 

Decision No.: 464378 Registration Nos.: See Table 1 

Petition No(s).: NA Regulatory Action: Ecological 

Environmental Scoping Document 

for Registration Review 

Risk Assessment Type: Single chemical Case No.: 5002 

TXRNo.:NA CAS No.: 12124-97-9 

MRID Nos.: See Tables 7, 8, & 9 and 40 CFR: None 

pages 4, 11, and 15 

Srinivas Gowda, M.S. Microbiologist/~c~ce Coordinator Sa--l~"~~ 

William Erickson, Ph.D., Biologis~/i/~ 

Najm Shamim, Ph.D., Chemist 1\fJ /l[aA .. ..,.... . Risk Assessment and Science Support Branch (RASSB) 

Antimicrobials Division (7 51 OP) 

Donna 

Steven 

Randall, 

Weiss, Acting 

M.S. Ecological 

Branch Chief 

Risk Assessment 

;iit' ~ Team Leader 

Risk Assessment and Science Support Branch (RASSB) 

Aritimicrobials Division (751 OP) 

Rebecca von dem Hagen, Chemical Review Manager 

Regulatory Management Branch II 

Antimicrobials Division (7 51 OP) 

Page 1 of 16 
Executive Summary 

Ammonium bromide is registered for use as an algicide, bactericide, microbicide and 

slimicide for treating industrial process and water systems such as recirculating cooling towers 

and pulp and papermills, and wastewater treatment systems. End use products of ammonium 

bromide are used in conjunction with an oxidant such as sodium hypochlorite (12.5%) or 

chlorine gas (99.9%) under controlled conditions within an approved feeder/delivery system to 

produce monochloramine biocide in situ. The monochloramine biocide is added to the water to 

be treated immediately as it is formed to control algal, bacterial and fungal slimes. 

Ammonium bromide has no pesticidal activity per se. Rather, it dissociates in water to 

ammonium anion (NH/) and bromide cation (Br-; bromine is in a -1 oxidation state here). 

However, ammonium bromide converts to a hypobromite cation (BrO-; bromine is in the+ 1 

oxidation state) and monochloramine (NH2Cl) when mixed with sodium hypochlorite or chlorine 

gas, which act as the disinfectants. 

Ammonium bromide was initially registered as a pesticide in the United States in January 

1999 for use as a bacteriocide and slimicide in recirculating cooling water systems and pulp and 

paper mills. Currently it is used in five active products, two of which are technical chemicals. 

All product chemistry data requirements have been satisfied for this active ingredient ammonium 

bromide. 

Conventional fate data for ammonium bromide, monochloramine, and hypobromite is not 

required because these are inorganic compounds for which this type of data is not applicable. 

The Agency has evaluated the existing chemical information and properties on these compounds, 

their reaction products and ammonium bromide use patterns and has determined that no 

additional data are required for reregistration review. The environmental fate of these 

compounds is complex but is known based on inorganic and oxidation/reduction chemistry. 

Hypobromite is a bleaching agent and germicide. The hypobromite cation is not stable and 

converts into bromide ultimately; conditions in these systems are not considered favorable for 

the conversion to bromate. More recent data indicates that monochloramine is not stable in 

aquatic medium and it is biodegradable in water, and in sediments and possibly in soils. For the 

given ammonia bromide uses, resulting monochloramine residuals are not expected to persist 

long enough in industrial water systems to reach the aquatic environment. 

Technical-grade ammonium bromide is practically nontoxic to birds. However, when 

ammonium bromide is combined with sodium hypochlorite, the resultant monochloramine is 

highly to very highly acutely toxic to freshwater and estuarine/marine organisms. No additional 

ecological effects data are needed for these chemicals. Monochloramine is not expected to reach 

the aquatic environment. Therefore, an ecological risk assessment will not be conducted for the 

current uses of ammonium bromide. The Agency anticipates the registered uses will have "no 

effect" on endangered or threatened terrestrial or aquatic species, or their designated critical 

habitats, as listed by the USFWS and the NOAA. 

Page 2 of 16 
Introduction 

Ammonium bromide is an inorganic nitrogen and bromine compound registered for use 

as an algicide, bactericide, microbicide and slimicide for treating industrial process and water 

systems such as recirculating cooling towers and pulp and papermills, which includes their 

wastewater treatment systems. Ammonium bromide is used in conjunction with an oxidant such 

as sodium hypochlorite (12.5%) or chlorine gas (99.9%) to produce monochloramine biocide 

within an approved Fuzzicide®feeder/delivery system. 

Ammonium bromide was initially registered as a pesticide in the United States in January 

1999 for use as a bacteriocide and slimicide in industrial process waters of recirculating cooling 

towers and pulp and paper mills. Currently it is used in five active products, two of which are 

technical products and three which are end-use products. Technical grade products are solid 

materials and have declared active ingredient content of 99%. Two of the three end use products 

are solids with declared ammonium bromide content of 99%, the other end use product is a 

ready-to-use solution with a declared active ingredient content of 35%. Summary information 

about these products is listed in Table 1. Ammonia bromide is currently registered for use as a 

bacteriocide and slimicide in industrial process waters of recirculating cooling towers and pulp 

and paper mills, which includes their sewage and wastewater treatment systems (Table 2). 

No ecological risk assessment was previously been performed for ammonium bromide. A 

Reregistration Eligibility Decision (RED) has not been issued by the Agency for ammonium 

bromide because the initial registration date was after the November 1984, the federally 

mandated cutoff for initiation of the RED process. 

Table 1. Registered Products of Ammonium Bromide 

Registration # Registration Name Company Name Formulation Type %of Active 

Ingredient 

8622-58 Fuzzicide-Comp ICL-IP America, Inc. Soluble Concentrate 99 

8622-59 Ammonium Bromide-Comp ICL-IP America, Inc. Technical Chemical 99 

8622-64 Fuzzicide Solution ICL-IP America, Inc. Ready-to-Use 35 Solution 

8622-75 Ammonium Bromide-SP ICL-IP America, Inc. Technical Chemical 99 

8622-76 Fuzzicide-SP (Ammonium ICL-IP America, Inc. Soluble 99 Bromide) Concentrate/Solid 

Page 3 of 16 
Table 2 - Ammonia Bromide Antimicrobial Use Summary 

Use Site (Treatment Site) Application Application Rate Notes Method 

Industrial Process Systems 

Recirculating cooling systems: 

Industrial cooling towers, 

evaporative condensers, heat 

exchange water towers, influent 0.3-5.0 ppm of 

systems such as flow through Metering residual Nonauthorized, filters, industrial water scrubbing (Enclosed feeder/ monochloramine nontrained personnel systems, brewery pasteurizers, delivery system) expressed as total cannot operate system sewage systems (septic tanks, leach chlorine in process 

fields, tank lines, sewers, lagoons, system' 

and sewage effluent water), 

industrial air-washing systems 

equipped with a mist eliminator 

PulQ and PaQer Mills (Pulp and 

paper mill fresh and sea water 0.3-10.0 ppm of influent systems, and associated residual cooling water systems and Metering monochloramine Nonauthorized, 

wastewater treatment systems, pulp, (Enclosed feeder/ expressed as total nontrained personnel 

paper and paper board mill systems, delivery system) chlorine in process cannot operate system 

nonpotable water systems, starch system' slurries, and other process water 

that may contact food) 

1 While the amount of ammonia bromide end use product and sodium hypochlorite or chloride gas aqueous solution 

to add to the feeder box is listed on the label, the amount actually applied per a given volume of process water is not 

specifically designated-operator adds sufficient dosage to maintain a designated residual (unreacted) 

monochloramine in the process water. 

A. Product Chemistry Summary of Ammonium bromide (100% TGAI) 

Chemical identity and the physical and chemical properties of the ammonia bromide 

technical grade active ingredient (TGAI) are provided in Tables 3 and 4, respectively. The 

primary source of information for this assessment was MRID Nos. 44711101 and 44683601. All 

product chemistry data requirements have been satisfied for the active ingredients sodium 

bromide. 

Table 3. Chemical Identity 

Chemical Name Ammonium bromide 

Common Name Ammonium bromide 

Classification Inorganic 

PC Code 000352 

CAS No. 12124-97-9 

Molecular Formula NHJ3r 

Page 4 of 16 
Molecular Weight 97.95 g/mole 

H 

(±) I s.S 

Molecular Structure: I ,, / ~ .i";'H 

H H 

Table 4. Product Chemistry Data Summary of Ammonium bromide (99% TGAI) 

OPPTS Physical and Chemical Value 

Guideline No. Properties 

830.1550 Product identity and Refer to Table 3. composition 

830.1800 Enforcement analytical Potentiometric titration. 

method HPLC with U.V. detection at 320 nm. 

830.6302 Color White 

830.6303 Physical State Granular powder hygroscopic; solid. 

830.6304 Odor Odorless 

Stability to sunlight, normal Stable following storage at 54 oc for 14 days, exposure 

to artificial daylight for 28 days, had no exothermic 830.6313 and elevated temperature, reaction or weight loss upon exposure to air at 150- metals/metal ions 160°C, no reaction with 10% iron, tin, or aluminum. 

Product has no oxidizing or reducing potential, based on 

830.6314 Oxidation/Reduction: results of exposure to water, monoammonium 

Chemical Incompatibility phosphate, iron powder, hydrogen peroxide, and 

kerosene. 

830.6315 Flammability-Flash point Non-flammable. Flash Points: Not applicable. 

830.6316 Explodability Product is not explosive (exposure to heat, mechanical 

shock, or friction did not cause the product to explode). 

830.6317 Storage Stability Stable following storage for about 12 months. 

830.6319 Miscibility Not apj>licable:_Q_roduct is a solid. 

830.6320 Corrosion Characteristics Stable for at least 3 months. Not corrosive to packaging 

following storage for about 12 months. 

830.6321 Dielectric breakdown Not applicable: product is a solid and is not intended for 

voltage use around electrical equipment. 

830.7000 pH 6.62 at 19.8°C (for I% aqueous solution). 

830.7050 UV Nisible Absorption Not expected to absorb at A> 300 nm 

830.7100 Viscosity Not applicable: product is a solid. 

830.7200 Melting point >370°C (metal block method). 

830.7220 Boiling point Not applicable: product is a solid. 

830.7300 Density 2.429 g/cmj ; 2.4550 g/mL 

It dissociates in water to ammonium and bromide ions. 

830.7370 Dissociation constant Ammonium bromide is a weak acid with a pKa of -5 in 

water. 

Page 5 of 16 
OPPTS Physical and Chemical Value 

Guideline No. Properties 

830.7550 Partition coefficient (n- Not applicable since NH4Br is inorganic salt. octanoVwater) 

830.7840 Solubility in water 97 g /100 mL at 25°C in water. 

830.7860 Solubility in organic Soluble in organic solvents - alcohol, acetone, ether, 

solvents ammonia. 

830.7950 Vapor pressure 9.8 X 10-7 mmHg 

Henry's law constant 1.3 X 10-13(Calculated) 

Physical and Chemical Properties of Monochloramine 

End use products of ammonium bromide are used in conjunction with an oxidant such as 

sodium hypochlorite or chlorine gas to produce monochloramine biocide in situ. Inorganic 

chloramines represent the stoichiometric reaction products resulting from the reaction of chlorine 

and ammonia in water; namely monochloramine, dichloramine, and trichloramine (Figure 1). 

Monochloramine (NH2Cl), dichloramine (NHCh) and trichloramine (NCh) are produced by 

either adding chlorine to a solution containing ammonia, by adding ammonia to a solution 

containing free residual chlorine or by adding premixed solutions of ammonia and chlorine to 

water. However, the production of monochloramine versus dichloramine and trichloramine is 

highly dependent upon pH, the ratio of chlorine to ammonia-nitrogen and, to a lesser extent, 

temperature and contact time. A pH between approximately 7.5 and 9.0 is optimum for the 

formation of monochloramine; the ideal pH is 8.3. 

,,,N, 

H'''''J 'CI 

H 

Monochloramine (NH2Cl) 

,,,N, 

H'''''J 'CI 

Cl 

Dichloramine (NHC/2) 

_......N •• c1" \·····c1 

Cl 

Trichloramine (NC/3) 

Figure 1. Chemical Structures of Inorganic Chloramines 

When ammonium bromide in the end use product reacts in a 1: 1 molar ratio sodium 

hypochlorite, a 12.5% aqueous solution of sodium hypochlorite under controlled conditions 

forms a 12.5% solution of monochloramine. Monochloramine is the preferred form of 

chloramine in the industrial process system use for microbiocidal purposes. Summary of 

chemical and physical properties of monochloramine is presented in Table 5 (Source: Toxnet). 

Table 5. Summary of Chemical and Physical Properties of Inorganic Monochloramine 

CHEMICAL VALUES 

PARAME1ER 

CAS# 10599-90-3 

Molecular Formula NH2Cl 

Molecular Weight 51.48 

Page 6 of 16 
CHEMICAL VALUES 

PARAMETER 

Solid form: Colorless crystals 

Color/Physical State Liquid form: Yellow liquid 

Aqueous form: Colorless liquid 

Odor No data available 

Melting Point -66°C 

It may decompose violently above -66 deg °C 

Boiling Point No data available 

Water Solubility Soluble 

Other solubilities ETOH, ether, 

CC14, benzene 

pH ----

Density -----

Partition coefficients -1.19 

Vapor pressure 1.16E-009 mm Hg at 25 °C (source: EPI Suite version 4.0) 

Henry's Law constant 7 .857E-O 17 atm-m3 /mole (source: EPI Suite version 4.0) 

Monochloramine is oxidized by ozone faster than ammonia 

Other 

Chemical/Physical Ultraviolet light depletes only free chlorine, whereas chloramines seem to be quite stable in 

Properties sunlight. Chloramine decay has been suggested to be at most 0.2 mg/litre per sunlight hour 

between 10 a.m. and 2 p.m. (latitude 30-40°N). 

B. Environmental Fate Summary 

A review of labels indicate that in pulp and paper mills application of ammonium 

bromide as a disinfectant is done in a closed system, when 12.5% NaOCl or Clz (one label: EPA 

Registration Number 8622-76 indicates this process) is mixed with ammonium bromide. In this 

mixture solution there will be three reactants: bromide anions (BO, hypochlorite anions (OCr) 

and ammonium cations (N~ +). An understanding of basic chemical reactions of ammonium 

bromide, ammonium, and bromine will help in understanding the unique environmental fate and 

transport of ammonium bromide. The stoichiometric reactions of ammonium bromide in the 

closed system feeder/delivery system in industrial process water systems is described below in 

two sections. One section examines the reactions of bromine contained within ammonium 

bromide and the other the ammonium ion in the presence of hypochlorous acid. 

Page 7 of 16 
Stoichiometric Reactions of Bromine from Ammonium Bromide Use 

The following chemical information is provided to understand the aqueous chemical processes. 

Ammonium bromide is an inorganic and an ionic chemical, and it undergoes very rapid 

reactions in the presence of other inorganic species. Inorganic ionic reactions are much faster 

than organic reactions, and understanding of these reactions is critical for the environmental fate 

processes. 

Ammonium bromide readily dissociates in water into the respective ammonium cations 

and bromide anions (bromine is in a -1 oxidation state): 

Awunonium d~ 

NH + 4 Equation 1 

The bromide ion in the presence of chlorine gas (Ch) in solution readily undergoes a 

reaction to form bromine gas (bromine is in a zero oxidation state1) and chloride anions: 

+ Cl2 (aqueous) ~ + Br2 (aqueous) Equation 2 ·o idt> a-nio n Chlo rid;; ar.~ion 

Bromine gas in an aqueous solution reacts with the water releasing bromide anions 

(bromine in -1 oxidation state) and hypobromite (bromine in +1 oxidation state): 

Br2 (aqueous) + H2 0 

Hy pobr o m it;; io ~tl Eko1nids ion 

Equation 3 

Alternatively in the presence of hypochlorite released from sodium hypochlorite in 

solution rather than from Ch, bromide anions (bromine in -1 oxidation state) released from 

ammonium bromide form hypobromite (bromine in +1 oxidation state) and chloride anions: 

Bromide ant on Hypoch lo r i tB a-nion Hypobromitt> ~ai ot~ 

Equation4 

Chi oTid'g anao·n 

In an aqueous solution hypobromite is in equilibrium with hypobromous acid or bromic 

acid (Equation provided below) which is a weak, unstable acid. Hypobromous acid has 

properties very similar to hypochlorous acid, and is used like hypochlorous acid as a bleach, an 

oxidizer, a deodorant, and a disinfectant. The percent bromine as the hypobromite anion versus 

hypobromous acid (HOBr) is a function of pH as listed in Table 6. 

HypobT om o ·us o r Brom i c acid H y d1•ogen i o n Hy pobr om ite ion 

Equation 5 

1 Oxidation state is a measure of the degree of oxidation of an atom which in turn represents the tendency to lose 

electrons present in the valence orbitals 

Page 8 of 16 
Table 6. Percent hypobromite in solution as a function of pH 

pH % Bromine as Bro- % Bromine as HOBr 

6.0 0.0 100 

6.5 0.6 99.4 

7.0 2.0 98.0 

7.5 6.0 94.0 

8.0 17.0 83.0 

8.5 43.0 57.0 . . . . Source: http://www .lenntech.cornlprocesses/dtsmfecttonlchemtcalldtsmfects-bromme.htm 

Table 6 indicates that if the is pH> 8 (alkaline medium) it makes the availability of 

hypobromite optimum, and also shifts the equilibrium toward hypobromite as it gets used up 

during a disinfection process. It also helps in determining which pH will produce highest 

reactivity of hypobromite ion or hypobromous aicd 

Hypobromite (bromine in +1 oxidation state) can further decompose where one mole of 

hypobromite reacts with two electrons to form bromide (bromine in -1 oxidation state). 

2e- + = Equation 6 

Ammonium ions in the presence of hypobromite (BrO-) may form monobromamine: 

Equation 7 

If this reaction is not controlled, the formation of dibromamine, and tribromamine occurs. 

NH2Br + HOBr ~ MHBr2 + H 20 Equation 8 

M on ob1•om a€ne Hypolnr o-mous Gci d Di,b r o mGmin-e W a t e·>" 

NHBr2 + HOGl ----7 NBr3 + H20 Equation 9 

Dibr omamin ll Hyp ochlorous aci d Trib·r omaminli W B t 8'1' 

Alternatively, in a strongly alkaline solution (pH> 10 up to 14) the hypobromite anions 

can further undergo oxidation to form bromate anions (bromine in + 7 oxidation state) and 

bromide anions, bromate is a strong oxidizing agent similar to chlorate: 

BrOs:- + Equation 10 

Hyp obrcm its- anio ns Eilr o n'l.ate ani oms BJ•om i de a n i o-ns 

Given the application method and controlled conditions, formation of bromate ions is 

considered unlikely for the registered uses of ammonium bromide. Released hypobromite in the 

system under consideration is expected to act as an oxidant releasing bromide ions. 

Page 9 of 16 
This is supported by two studies conducted with bromide compounds, which while not 

using ammonium bromide, still provide some insight into the formation of bromate from 

bromide in solution. One study provides insight under different pH conditions and excess 

bromide, and the other excess bromide and sunlight in the presence of hypochlorite. These 

consist of a laboratory study conducted by the United States Navy (A Memo from Timothy 

Leighton to Mark Hartman: Nov.3, 2005: Sodium Bromide: Sodium Bromide: Residential and 

Dietary Antimicrobial Uses (Pools, Spas, Sugar Beets, and Fruit & Vegetable Wash). DP 

Barcode 321793)) with polybrominated trimethylbenzylammonium column, and the second 

study was a swimming pool monitoring study conducted with sodium bromide, respectively. 

A lab study conducted by registrants and submitted as a 6(a)(2) (Same memo of Timothy 

Leighton cited above) showed that in the pH range of 4 to 7.5 and buffered conditions bromide in 

the concentration range of 0.5, 2 reacted in the following way: 

• No bromate was detected over the pH range of 4-6 for 5 days at any of the 

bromide concentrations. 

• However at pH 7 at the bromide level of 5 ppm, bromate started forming from day 

1 (6.7 11g bromate/L). At day 4 bromate concentrations reached 9.1!-lg/L, and 

remained at this level on day 5 (9.1!-lg/L). Thus a steady state was achieved on 

day 4. This shows that even in the absence of an oxidant and sunlight there is a 

possibility of bromate formation under the right condition (acidic and neutral pH, 

constant temp, and high buffer concentration). However, the bromate level 

reached (9.1!-lg/L or 0.0091 mg!L) represents a 0.002 fold conversion from the 

bromide to the bromated form which represents a very small conversion. 

The second study was conducted in the presence of calcium hypochlorite (Ca(OCl)z), 

sunlight, and a very high concentration of sodium bromide (250 mg!L versus 6 mg!L, which is a 

permissible concentration for available bromine for swimming pool scenario) the conversion to 

bromate was as high as 3 ppm. It is clear that the formation of higher amounts of bromate 

occurred under highly exaggerated conditions. 

Stoichiometric Reactions of Ammonium from Ammonium Bromide Use 

In the presence of hypochlorite (ClO-) released from aqueous solutions of hypochlorous 

acid, the ammonium ion released from ammonium bromide (Equation 1) undergoes the 

following reaction: 

NH + 4 + Equation 11 

If this reaction is not controlled, the formation of dichloramine, and trichloramine occurs. 

M on o chlo r am in e H y po chl o-t•ous acid Dichl-o lt·am i n e W ater 

Equation 12 

Page 10 of 16 
NHC12 + HOC'l 

Equation 13 

Dicldorami.11-111 Hypochlorous acid T-rich lora-mine Water 

The controlled conditions of the system used for paper and pulp (pH> 8, constant 

temperature, and molar ratios of ammonium ions and hypochlorite, will not likely produce 

dichloro and trichloroamines. 

Environmental Fate of Ammonia Bromide Reaction Products 

Hypobromite and monobromamine have a similar capability to act as mild disinfectants 

like hypochlorite and monochloramine; so theoretically in the closed system of ammonium 

bromide and sodium hypochlorite, at an appropriate pH, many disinfecting moieties are likely be 

present. The three most likely chemicals formed in the feeder/delivery system under controlled 

conditions are: hypochlorous acid (or hypochlorite), hypobromous acid (or hypobromite ion), 

and monochloramine. These chemicals are inorganics so conventional fate studies do not apply. 

These chemicals have a tendency to form various intermediates depending on the pH of the 

system and the concentration of the various species involved. Unlike reactions with organics, 

typically inorganic reactions are much faster, and therefore not easy to keep tract of the 

intermediates. These intermediates cannot be classified as degradates in the classical sense. 

A study in simulated natural waters (MRID #452052-03) was conducted in lieu of the 

conventional hydrolysis study in simulated natural water at different pHs. The study was based 

on the OECD Test Guideline 111, and included the following modifications: 

• Secondary effluent collected from a wastewater treatment facility was used; 

• The study was conducted at pH 7.7; and 

• Monochloramine was used as a reference material instead of another substance 

(aspirin) suggested in the test guidelines. 

Ammonium bromide formed HOBr, and its decay as well as the decay of chloramines 

was followed at two temperatures: 25 and 35 °C and also two concentrations of Fuzzicide were 

selected: expressed as 5.0 milligrams of chlorine residual per liter (mg Ch/L) and 0.50 mg Ch/L; 

a first order kinetics was assumed in both cases. Maximum half life of Fuzzicide was 48 hours 

(2 days) and maximum half life for chloramine was 155 hours(> 6 days). Hence both of them 

degrade fast in the simulated natural water systems. 

The study did not mention the formation and likely presence of Bro-. However, 

ammonium bromide or its active moieties formed during the use and application are not stable 

and convert into other moieties and perhaps mineralize. However, this study shows that 

monochloramine under environmental conditions is not stable and undergoes rapid degradation 

in natural waters. 

For chloramine taking into account the physicochemical properties, and environmental 

fate parameters the source primarily from EPI Suite (version 4.0) a screening level 

environmental fate assessment summarized as follows: 

Page 11 of 16 
• Monochloramine is highly soluble in water and its vapor pressure and Henry's 

Law Constant are both low. Therefore, it is not expected to volatilize from water 

surfaces quickly. 

• Its low Koc indicates that it is mobile in soils and sediments. 

• Its half-life in aqueous media varies from a fraction of a day to about 40 days. 

(Health Canada, 1998), depending upon temperature, pH, and salinity. This study 

and other Canadian studies for aqueous medium decay of chloramines show that 

in deionized water and seawater mixtures the half life varied from 0.68 days to 

0.98 days. However, see below for a more recent observation. 

• A Canadian study on the sediment of Grand River, in North Saskatchewan River 

and Downes Creek showed the half life of 1.4, 2.5 and 0.05 days. 

• No concrete studies are known that provides data on the dissipation rate of 

chloramines from soil surfaces. 

• Monochloramine has been in use as a secondary disinfectant in the U.S. and 

internationally for over fifty years. Compared to hypochlorite ion, it degrades 

slowly and, hence, its disinfecting power in aqueous media is higher than 

hypochlorite. 

• All EPI Suite BioWIN (EPI Suite 4.0) models estimate that monochloramine is 

quickly biodegraded and it can be classified as readily biodegradable. (EPI suite 

classifies it fast biodegradation, which is less than a day) 

• PMRA in its most recent Proposed Registration Decision (March 2012)21 on 

Ammonium bromide (Fuzzicide) has shown that monochloramine (referred to as 

bromide activated chloramine(BAC)) hydrolyses in water quickly and at pH 5 the 

half life is 15.9 minutes, while at pH 9, the half life was measured at 184 hours 

(12 days). 

• Pulp and paper use of ammonium bromide (and monochloramine) as the active is 

used in a closed system, and the waste from this process is kept in holding ponds 

(in some registered labels). Thus the release waste to the wastewater streams is 

not likely to contain monochloramine keeping in view of the physical/chemical 

characteristics of monochloramine (short hydrolytic half life, readily 

biodegradable etc.) 

• Similarly from the recirculating cooling tower process, the waste is not likely to 

contain monochloramine. 

Chloramine in Drinking Water: 

Since it is used as a secondary disinfectant for waste water treatment, chloramine is likely 

to be found as a contaminant in drinking water. EPA has set a maximum Drinking Water Limit 

for a number of contaminants in surface water (and in drinking water) regardless of the source. 

The maximum contaminant limit goal (MCLG) for chloramines is 4.0 ppm and the maximum 

residual disinfectant level goal (MRDLG) is also 4.0 ppm. Thus most of the water utilities are 

required to keep the level of chloramines at this level for residential drinking water. 

2 Pmra.publications@hc-sc.gc.ca 

Page 12 of 16 
Water Quality 

Ammonium bromide is not identified as a cause of impairment for any water bodies listed 

as impaired under section 303(d) of the Clean Water Act, based on information provided at the 

Agency's National Pesticides Cause of Impairment of Waters website (searched August 27, 

2012l In addition, no Total Maximum Daily Loads (TMDL) have been developed for 

ammonium bromide, based on information provided at the Agency's National Pesticide TMDL 

web site (searched August 27, 2012)4. More information on impaired water bodies and TMDLs 

can be found at http://www.epa.gov/owow/tmdl/. The Agency invites submission of water 

quality data for this pesticide. To the extent possible, data should conform to the quality 

standards in Appendix A of the OPP Standard Operating Procedure: Inclusion of Impaired 

Water Body and Other Water Quality Data in OPP's Registration Review Risk Assessment and 

Management Process (see: http://www.epa.gov/oppfeadl/cb/ppdc/2006/november06/session1-

sop.pdf ), in order to ensure they can be used quantitatively or qualitatively in pesticide risk 

assessments. 

C. Ecological Effects Summary 

All of the major oxidants formed in the registered application method of ammonia 

bromide would be measured as chlorine residual: chloramines, bromamines, hypochlorite, 

hypobromite. The Ambient Water Quality Criteria for Chlorine- 1984 document contains a 

review of public literature on effects of chlorine (total residual chlorine) and based on the data 

derives freshwater and saltwater organism acute and chronic water quality criteria as total 

chlorine residual. Current ambient water quality criteria for chlorine or total chlorine residual 

are based on the data in the 1984 document and the method for deriving water quality standards 

discussed in a 1986 Water Quality Document (USEPA, 1986). 

• Freshwater Criterion Maximum Concentration= 19 J.lg/L; 

• Freshwater Criterion Continuous Concentration = 11 J.lg/L; 

• Saltwater Criterion Maximum Concentration= 13 J.lg/L; and 

• Saltwater Criterion Continuous Concentration= 7.5 J.lg/L 

A review of toxicity effects data for ammonium bromide and for monochloramine is 

summarized in the following sections. 

No ecological risk assessment has previously been performed for ammonium bromide. 

a. Toxicity to Terrestrial Animals 

The available toxicity studies submitted by the registrant categorize ammonium bromide 

TGAI as being practically nontoxic to birds (Table 7). Mammalian toxicity data are presented in 

the Human Health scoping document. No additional data are required for terrestrial animals. 

3 . http://iaspub.epa.gov/tmdl waters 10/attains nation cy.cause detail 303d?p cause group id=885 4 

http://iaspub.epa.gov/tmdl waterslO/attains nation.tmdl pollutant detail?p pollutant group id=885&p pollutant 

group name=PESTICIDES 

Page 13 of 16 
Table 7. Summary of the Endpoints from Submitted Terrestrial Ecotoxicity Studies for the 

TGAI 

Study Type Species Test material Toxicity Toxicity MRID& 

Classification Status 

Acute- Mallard Ammonium bromide LD50: >2000 Practically 447213-01 Avian Oral (Anas mg/kg-bw/day 

850.2100 platyrhynchos) (98.5% ai) nontoxic Acceptable 

AcuteAvian Mallard Ammonium bromide LC50: >5000 ppm Practically 447213-02 

Dietary (98.5% ai) nontoxic Acceptable 

850.2200 

b. Toxicity to Aquatic Animals 

The available toxicity studies submitted by the registrant categorize monochloramine 

(generated from ammonium bromide mixed with sodium hypochlorite) as being acutely highly to 

very highly toxic to freshwater and estuarine/marine animals (Table 8). No additional acute 

toxicity data are needed. Because monochloramine is so acutely toxic, sublethal reproductive 

effects are not expected. Chronic toxicity data are not required. 

Table 8. Summary of Endpoints from Submitted Fish and Aquatic Invertebrate 

Ecotoxicity Studies for Monochloramine. 

Study Type Species Test material Toxicity Value Toxicity 

Classification 

Rainbow trout Very highly (Oncorhynchus Ammonium 96-hr LC50: 58 jlg Cl2/L 

my kiss) bromide toxic 

AcuteFreshwater Fish (99.9% ai) 

850.1075 Bluegill sunfish in 10% 

(Lepomis hypochlorite 96-hr LC5o: 290 jlg Ch/L Highly toxic 

macrochirus) solution with 

carbonate buffer 

Acute- Sheepshead 

Estuarine/marine minnow Highly toxic Fish ( Cyprinodon 96-hr LC50: 360 jlg Cl2/L 

850.1075 variegatus) 

AcuteFreshwater Water flea 48-hr EC5a: 23 jlg Ch/L Very highly 

Invertebrate toxic 

850.1010 

Acute- Mysid Estuarine/marine Very highly 

Invertebrate (Mysidopsis 96-h LC5o: 36 jlg Ch/L toxic 

850.1035 bahia) 

Acute- Eastern oyster Estuarine/marine Very highly 

Invertebrate ( Crassostrea 96-h EC50: 18 jlg Cl2/L toxic 

850.1025 virginica) 

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MRID& 

Status 

447213-13 

Acceptable 

447213-12 

Acceptable 

447213-16 

Acceptable 

447213-14 

Acceptable 

447213-15 

Acceptable 

447213-17 

Acceptable 
c. Toxicity to Aquatic Plants 

A summary of acute aquatic ecotoxicity data endpoints from two registrant-submitted 

studies is provided in Table 9. 

Table 9. Summary of the Endpoints from Submitted Aquatic Plant Ecotoxicity Studies for 

Monochloramine. 

Study Type Species Test material Toxicity Toxicity MRID& 

Classification Status 

Aquatic 

Plants- Duckweed Ammonium bromide 7-day EC5o: 680 Jlg nla 452052-02 

Vascular (Lemna gibba) (99.9% ai) Cl2/L Acceptable 

850.4400 

Aquatic in 3% hypochlorite 

Plants- Green algae solution with 452052-01 

Nonvascular (Pseudokirchneriella carbonate buffer 72-h EC50: 28 Jlg Clz/L nla Acceptable 

850.5400 subcapitata) 

d. Aerobic Microbial Inhibition 

An Activated Sludge Respiration Inhibition (ASRI) (MRID# 452052-04) study was 

conducted using OECD Test Guideline 209 with an activated sludge obtained from a domestic 

waste site. The study serves two purposes: 

a) a screen to determine if the pesticide will adversely affect aerobic microbial 

treatment plants; 

b) determine the level of non-inhibitory concentration of the pesticide which in turn 

can be used for a biodegradability test. 

Test solutions were made by mixing ammonium bromide and sodium hypochlorite along 

with the reference material (3,5-dichlorophenol). A log plot of sample concentrations versus 

the oxygen consumption yielded an ICso value of 16 mg/L, which was well within the 5 to 30 

mg/L value. This limit indicates that the actives do not adversely affect the microbial 

population in the wastewater system. 

Environmental Fate and Ecotoxicity Data Gaps and Anticipated Work 

There are no ecological effects data gaps for ammonium bromide or its reaction product, 

monochloramine. For environmental fate, a hydrolysis study in open literature was identified 

for monochloramine. The Agency requires registrants to formally submit the hydrolysis study to 

the Agency; therefore, the Agency anticipates the need to call-in a hydrolysis study. The Agency 

has concluded that environmental exposure from these chemical substances is not likely to occur 

in the aquatic environment due to registered uses as labeled. Therefore, an ecological risk 

assessment is not anticipated to be needed. 

835.2120- Hydrolysis 

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Endangered Species Determination 

Based on the ammonium bromide use pattern, rapid and complete formation of 

monochloramine under controlled application conditions, the rapid hydrolysis and 

biodegradation of monochloramine in industrial water systems, including their waste systems, 

the Agency anticipates the registered uses will have "no effect" on endangered or threatened 

terrestrial or aquatic species, or their designated critical habitats, as listed by the USFWS and the 

NOAA. However, the Agency will review any comments made by the public on this document 

and will conduct an environmental risk assessment if new information warrants such action. An 

ecological risk assessment planned during registration review allows the Agency to determine 

whether an antimicrobial pesticide's use has "no effect" or "may affect" federally listed 

threatened or endangered species (listed species) or their designated critical habitats. When an 

assessment concludes that a pesticide's use "may affect" a listed species or its designated critical 

habitat, the Agency will consult with the U.S. Fish and Wildlife Service and/or National Marine 

Fisheries Service (the Services), as appropriate. 

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