Polkadot JAM Slides - Token2049 - By Dr. Gavin Wood
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2008 newwa annual conference in burlington vt chloramine talk
1. The Use of Chloramines
as a Secondary Disinfectant:
Is Your Chemistry Good Enough?
David G. Miller, P.E.
Water Supply Engineer
Manchester, NH Water Works
Voice: (603) 624-6842 E-mail: dmiller@manchesternh.gov
and
James P. Malley, Jr., Ph.D.
Professor of Civil/Environmental Engineering
University of New Hampshire (UNH)
Voice: (603) 862-1449 E-mail: jim.malley@unh.edu
NEWWA 127th Annual Conference
September 14-17, 2008 Burlington, VT
2. Acknowledgements
⢠NEWWA Disinfection Committee
⢠Manchester, NH Water Works
⢠UNH - Environmental Research Group
⢠U.S. Army Corp. of Engineers
⢠Information presented by WASA
⢠Information presented by WSSC
⢠USEPA Reports
⢠Phillippe Boissonneault, Portland Water District
⢠Cynthia Klevens, NHDES
⢠Professor Gregory Harrington, University of
Wisconsin â Madison
3. Take Home Messages
⢠Chloramines Reduce DBP Risks to Public Health
⢠Chloramines Reduce Microbial Regrowth and Risk in
Distribution Systems and in Hospitals
⢠Chloramines WILL Change the Water Quality Conditions
in a Distribution System (especially the ORP)
⢠Chloramines alone DO NOT cause Corrosion Problems
⢠The Decision to Switch to Chloramines Requires:
â An Experienced Team Effort
â Careful Planning Including Public Education
â Careful Implementation of Switching to Chloramines
â System Monitoring of Key Water Quality Parameters
{e.g., pH; Cl2 to NH4-N Mass Ratio; Lead and Copper;
Microbes, Ammonia, Nitrite and Nitrate} is Needed
4. Outline
⢠Chloramine Chemistry Basics
â We want to form Monochloramine (NH2Cl)
â Importance of the Chlorine to Ammonia-
Nitrogen Mass Ratio
â Importance of pH Effects on Chloramine
Species
â Issues with Nitrification
⢠Chloramines and Lead in Washington, D.C.
The Chemistry Explains/Solves the Problem
5. Chloramine Formation Equations
⢠Monochloramine (NH2Cl):
HOCl + NH3 â NH2Cl + H2O
⢠Dichloramine (NHCl2):
HOCl + NH2Cl â NHCl2 + H2O
⢠Trichloramine (NCl3):
HOCl + NHCl2 â NCl3 + H2O
⢠Organochloramines:
HOCl + Organic Amines â Organochloramines + H2O
============================================
We select for Monochloramine since it is a stronger
Disinfectant, is more stable and has less taste and odor issues
pH and Cl2 to NH4 -N mass ratio are the key factors to control
6. The Famous Breakpoint Curve
8
Chlorine Residual
mg Cl/mg NH-N
6
4
NHCl2
4
HOCl + OCl-
2
2
NH2Cl NCl3
0
0 2 4 6 8 10 12 14 16
Chlorine Dose, mg Cl2/mg NH4-N
Target Ratio in Practice is 3:1 to 5:1 mg Cl2 / mg NH4-N
BE CAREFUL! In practice, poor blending/mixing can cause
ratios as high as 12:1 which will have negative impacts
7. 100
80
Monochloramine
Total Combined Chlorine (%)
60
40
20 Dichloramine
Nitrogen
Trichloride
3 5 6 7 8
pH
pH 8.3 to 8.4 is commonly
used as the optimum target for monochloramine
formation at a Cl2:NH4 -N mass ratio of 3:1 â 5:1
8. Potential for Nitrification
⢠When the Cl2:NH4-N mass ratio is too low or for
some other reason excess levels of NH4-N persist
in the distribution system, there is strong potential
for nitrification events especially in warmer water
⢠Nitrification â the two step microbial conversion of
ammonia to nitrite and then to nitrate
NH3 Nitrosomonas NO2 Nitrobacter NO3
⢠Factors that Effect the Potential:
â Free NH4-N Concentration
â Temperature
â pH range â 7.5 to 8.5 is where it occurs fastest
9. Impacts of Nitrification
⢠Degrades chloramine residual
⢠Consumes dissolved oxygen
⢠Consumes alkalinity
⢠Can increase potential for corrosion
either due to lower ORP (REDOX)
potential in the system and/or lower pH
⢠Increases HPC counts and can
indirectly lead to coliform rule violations
⢠Increases nitrite and nitrate levels
⢠Can result in taste and odor complaints
10. Control of Nitrification
⢠Increase Monitoring of HPCs, Nitrite and Nitrate to
Understand Where and Why it is Occurring
⢠Conversion to Free Chlorine For Short Periods â
{often termed a chlorine burn}
⢠Spot Chlorination âTea-Baggingâ of Water Towers
⢠Increase Chloramine Residual
⢠Increase Chlorine to Ammonia Nitrogen Mass Ratio
⢠Set pH for Optimum Monochloramine Formation
⢠Increase Flushing especially for dead ends
⢠Reduce Water Age
11. The Washington, D.C. Case Study
History
Water Source is the Potomac River
The U.S. Army Corp. of Engineers â Washington Aqueduct
Operates Reservoirs and Two Conventional Treatment Plants:
Dalecarlia and McMillan Producing about 180 MGD Total
The treatment plants use chlorine for disinfection and in November
2000 switched to Chloramines in the distribution system to control
DBPs for lead and copper rule compliance the plants add Lime to
maintain a positive Langelier Index and favorable Stability Index
Washington Water and Sewer Authority (WASA) â Provides water to
130,000 Service Connections (23,000 Lead Services) in the 8 Wards
of Washington, D.C. - 725 Square Miles and 1,300 miles of piping.
12. Lead Problems in Washington, D.C.
Fall 2001 â Spring 2003
53 Homes Exceed 0.015 mg/L
(Lead Levels Up to 0.600 mg/L
Documented)
Spring 2002 to October 2003
5000 Homes Exceed Lead Limit
February 2, 2004 Washington
Post Article Exposes the Lead
Problem â âThe Lead Hits the
Fanâ A Media Feeding Frenzy
Results
March 2004 Two Congressional
Hearings; USEPA Criticizes
Map of Lead services in DCWASA
13. Lead Problems in Washington, D.C.
March 2004 WASA Convenes
Panel of Corrosion Experts
April 7, Senators introduce the
Lead-Free Drinking Water Act of
2004, S. 2733
April 8, WASA Completes the
Shipment of 23,000 Filters to
Homes with Lead Service Lines
May 2004 Washington Post and
Times Magazine Articles Decree
that Chloramines are Cause of
the Lead Problem Noting Switch
Back to Chlorine as Problem
Solution Between April 2 and
Map of Major Lead Levels in DCWASA
May 8, 2004
14. Lead Problems in Washington, D.C.
June 2004 Washington
Aqueduct Begins Pilot Test of
Orthophosphate (Zinc Free)
July 17, WASA and USEPA
Enter a Multiphase Agreement
to Address the Lead Problem
August 23, Washington
Aqueduct Begins Feeding
Orthophosphate (Zinc Free)
System Wide
September 2004, Lead Levels
Continuing to Drop, Class
Actions Lawsuits Beginning
and Legal Websites Popping
Map of Lead Service Replacements in DCWASA Up All Over The Area
15. Lead Problems in Washington, D.C.
2004 to 2006, chloramines
were given a black eye and
their use has been questioned
by some citizens and groups
Present Day - we have
learned from the Washington,
D.C. case and have paid close
attention to corrosion issues
when changing distribution
system water quality
Present Day â chloramine
use continues to grow but
carefully and with increased
attention to potential for
Map of Lead Service Replacements in DCWASA corrosion issues
16. What Happened in Washington, D.C. ?
Were Things Done Incorrectly ? - Yes
Could this happen to a New England Water Utility ? - Yes
Did the Switch to Chloramines Cause the Problem ? - Yes
Were Chloramines the Primary Cause ? â No
Do We Understand the Science ? - Mostly Yes
Can Chloramines Be Used Safely ? - Yes
17. What Happened in Washington, D.C. ?
⢠For over 20 years, Lead Service Line Replacement has
been recommended in D.C. â its costs prevented it
⢠For over 20 years, Corrosion Control Issues have been
raised in D.C. â little was done except Lime addition
⢠After switching to Chloramines in 2000, Corrosion problems
were noted almost immediately especially in the form of
pinhole leaks in copper services both at WASA and at its
neighbor WSSC. WASA lead monitoring results in early
2001 showed increasing lead levels
⢠Chloramines changed the water chemistry resulting in
higher lead leaching primarily from lead service lines and to
a smaller degree from in-line brass fixtures - this put a
system with a history of corrosion issues and lead risk over
the top â with serious public consequences for us all
18. The Chloramine Chemistry Involved
⢠As we noted earlier, chloramine use normally depends
on the formation of monochloramine as follows:
HOCl + NH3 ď¨ NH2Cl + H2O
Two important differences between chlorine (HOCl) and
monochloramine (NH2Cl) of importance to corrosion are:
⢠Chlorine is a much stronger oxidizing agent and will insure more
oxidizing conditions (higher ORP) in the distribution system than
monochloramine
⢠Monochloramine introduces amines or ammonia into the
distribution system and this nitrogen source can result in
Nitrification which can further lower the ORP and in some systems
lower the pH (this has been well proven in distribution systems
especially those which have a long retention time and are in
warmer climates).
19. Nitrificationâs Impacts
⢠Nitrification is the conversion of ammonia to nitrate by
naturally occurring microorganisms under aerobic
conditions. It follows the general reaction:
NH3 + 2 O2 + Nitrifying Microbes ď¨ NO3- + H+ + H2O
This reaction causes two very significant problems for
corrosion control in distribution systems:
⢠It consumes oxygen making for more reducing conditions in the
distribution system which leads to greater metals (lead and
copper) solubility/leaching.
⢠It produces acid (H+) lowering the pH or at least the buffering of
the system which also leads to greater metals leaching (not a
major factor in Washington, D.C.)
⢠In the Washington D.C. case the water buffering was
adequate to prevent any lowering of pH
20. Review of Lead Chemistry
2Pb(s) + O2 (g) ď¨ 2PbO(s) Lead Oxide
2PbO(s) + 2HOCl ď¨ 2PbO2(s) + 2H+ + 2Cl â
2PbO2(s) Lead Dioxide
Lead dioxide is a critical intermediate in the leaching of lead
and is very subject to water quality changes
Effect of Lowering pH
2PbO2(s) + 4H+ ď¨ 2Pb++ + 2H2O
Effect of Removing Oxygen â A Reducing Environment
NH3 + 2O2 + Nitrifying Microbes ď¨ NO3- + H+ + H2O
2PbO2(s) ď¨ 2Pb++ + 2O2 + 4e -
========================================================
++ - + -
21. B (0.008 mg/L)
(0.045 mg/L)
C
N
(0.600 mg/L)
Chemical Equilibrium of Lead Levels
B â Before Change to Chloramines
C â After Change to Chloramines
N â Effects if Nitrification Occurs and
Lowers pH and ORP
22. Steps to Resolve the Problem (1/3)
⢠Switch Back to Free Chlorine
â Would help insure the PbO2 (s) Form Dominated
So the Lead Levels in the DS Would Drop
â Would eliminate the reducing environment and
prevent Nitrification
â Return to the Health Risk Concerns of High
DBPs at the Consumerâs Tap
â Return to the Health Risk Concerns of
Regrowth in the DS and No Residual
Disinfectant Protection
23. Steps to Resolve the Problem (2/3)
⢠Remove the Sources of Lead
â Replace the Lead Service Lines
â Impose Tougher Standards for âLead Freeâ
Brass (currently allow 8% lead by weight)
â This is a costly effort and will take years to
accomplish (it has begun in many Water
Systems and will eventually be accomplished)
â It may be impossible to identify and remove all
sources of lead from the DS plumbing
24. Steps to Resolve the Problem (3/3)
⢠Apply A Different Corrosion Control Strategy
and Keep Chloramines
â Improve Distribution System Flushing and
Maintenance Procedures
â Use an Extended Free Chlorine Residual Flush or
Do Twice per Year (to prevent Nitrification)
â Switch to an Orthophosphate Corrosion Inhibitor
and Work to Optimize System-wide pH Control
â Increase monitoring and data analysis and then
communication between all parties
25. Orthophosphate for Corrosion Control
Orthophosphate â Food grade phosphoric acid H3PO4;
Trisodium orthophosphate Na3(PO4); and Zinc
orthophosphate Zn3(PO4)2 are all used by water utilities to
control corrosion. The later two are not used if Sodium is an
issue (e.g., in MA) or if Zinc becomes a wastewater
treatment issue as in the case of WASA. Typically 3 ppm is
added at first and then the dose is optimized often to the 0.5
to 2 ppm range The phosphate ion can then react with the
pipe (metal) material that is corroding to form a protective
phosphate solid coating ( Pb3(PO4)2(s) ):
2H3PO4 + ď¨ 6H+ + 2PO43 â
3PbO2(s) + 6H+ ď¨ 3Pb++ + 3H2O
==================================
26. Corrosion Control is Complex
⢠Much success with corrosion control has been achieved
in drinking water and much has been learned by
researchers but there are cases where the chemistry of
the water and the distribution system are complex and
corrosion control strategies are unsuccessful.
⢠Careful control of pH and system ORP is very important
as is careful selection and application of corrosion
control chemicals. Good monitoring is vital
⢠A thorough understanding other factors such as water
treatment plant processes; nature and role of organic
matter (TOC) in the system; electrochemical aspects
such as mixing of pipe materials; electrical grounding;
and biofilm aspects may all be important
27. DC WASA Pledge in USEPA Agreement
Twelve Point Plan of What WASA is Actually Implementing:
⢠Significantly accelerate the replacement of all District public space lead service
lines compared to EPAâs requirements.
⢠Work in partnership with a local financial institution to create a means tested
loan program to help customers finance the replacement of lead service line
pipes on private property.
⢠Continue to work with District government agencies to identify public grant funds
to help District residents with lead service line pipe replacements.
⢠Appoint a Lead Service Coordinator reporting directly to the General Manager to
manage all day-to-day WASA activities regarding lead service line
replacements, community outreach, communications and water testing.
⢠Launch a Mobile Community Response Unit to more readily address customers
concerns.
⢠Work closely with WASA stakeholders, including elected officials, faith-based,
community and civic organizations, and others to ensure communications are
clear and reach audiences appropriately, including those that donât speak
English.
28. DC WASA Pledge in USEPA Agreement
Twelve Point Plan (continued):
⢠Measure communication effectiveness in a quantitative manner.
⢠Strengthen its partnership with the D.C. Department of Health to address any
health concerns of D.C. residents regarding lead leeching.
⢠Work closer with the Washington Aqueduct regarding production of water
provided to D.C. residents. System-wide Orthophosphate Now in Use
⢠Further develop corporate partnerships to benefit resident and rate payers
which will specifically address the further distribution of water filters and the
availability of bank loans to residents in order to finance lead service line
replacements on private residential property.
⢠Work with the D.C. Department of Health and experts from the George
Washington University School of Public Health to more fully understand and
communicate to residents information now available from local research and
analysis regarding the health effects of water-based lead exposure.
⢠Convene a National Water Authority Peer Group Workshop so experts,
scientists and health professionals can discuss and explore the D.C.
experience with other utilities in an effort to better frame future policy
discussions for the nation and our policymakers.
29. Take Home Messages
⢠Chloramines Reduce DBP Risks to Public Health
⢠Chloramines Reduce Microbial Regrowth and Risk in
Distribution Systems and in Hospitals
⢠Chloramines WILL Change the Water Quality Conditions
in a Distribution System (especially the ORP)
⢠Chloramines alone DO NOT cause Corrosion Problems
⢠The Decision to Switch to Chloramines Requires:
â An Experienced Team Effort
â Careful Planning Including Public Education
â Careful Implementation of Switching to Chloramines
â System Monitoring of Key Water Quality Parameters
{e.g., pH; Cl2 to NH4-N Mass Ratio; Lead and Copper;
Microbes, Ammonia, Nitrite and Nitrate} is Needed
30. The Use of Chloramines
as a Secondary Disinfectant:
Is Your Chemistry Good Enough?
David G. Miller, P.E.
Water Supply Engineer
Manchester, NH Water Works
Voice: (603) 624-6842 E-mail: dmiller@manchesternh.gov
and
James P. Malley, Jr., Ph.D.
Professor of Civil/Environmental Engineering
University of New Hampshire (UNH)
Voice: (603) 862-1449 E-mail: jim.malley@unh.edu
TI O NS!
FO RQ UES
T IME
Hinweis der Redaktion
Chloramines reduce DBP risk : The primary benefit a utility will receive when switching from free chlorine to chloramines is a dramatic reduction in DBP formation. Chloramines simply donât react with natural organics to form DBPs as readily as free chlorine. In Manchester, NH, TTHMs have dropped form the 60-80 ug/L range to about 5 or 6. HAAs have also dropped into the single digits. Chloramines are less powerful and slower acting than free chlorine, but can be more effective at penetrating and inactivating biofilms in the distribution system. Chloramines will change water quality conditions in the distribution system, for example: excess free ammonia is food for nitrifying bacteria. This may result from a low Cl2:NH3 ratio or simply the natural decay of the chloramine residual over time. Chloramines can reduce ORP which can have a profound impact on corrosion chemistryâŚWeâll take a close look at the Washington DC story that erupted in early 2004 to illustrate this and weâll see that changing to chloramines alone DOES NOT directly cause corrosion problems. The final take home message is that a decision to switch to chloramines requires careful planning over several months to a year (or perhaps more), it should be accomplished by a team of experienced professionals, involve lots of public notification, and a comprehensive water quality monitoring plan following the switch to avoid potential problems.
Before we get to the Washington DC nightmare, letâs quickly review some basic chloramine chemistry The goal is to form a monochloramine residual by adding chlorine and ammonia at a carefully controlled and monitored ratio We need to understand how pH impacts the predominance of chloramine species We also need an understanding of conditions that may lead to nitrification in the distribution system and how to interpret system water quality data to avoid or mitigate the problem And finally, understanding the chemistry will help us understand what happened in Washington, DC
Adding ammonia to water containing free chlorine results in the formation of chloramine species. The species formed is primarily a function of the chlorine to ammonia ratio and pH. Temperature and the presence of other compounds are also factors. The equations for the three chloramine species are listed here Monochloramine is desired because it is a more powerful disinfectant than di- and tri-chloramine and it is more stable and has much less detectable taste and odor in water Keeping the chlorine to ammonia ratio between 3 and 5:1 at a pH above 7.5 favors the formation of the desirable monochloramine species As the ratio increases beyond 5:1, the formation of undesirable di- and tri-chloramine species predominates
Here is The Famous Breakpoint Curve The Y-axis shows the measured chlorine residual and the X-axis is the chlorine dose. Both in mg Cl2 / mg NH4-N As the chlorine dose increases from 0 to 7 mg Cl2 per 1 mg ammonia monochloramine is the predominant species present, with some dichloramine formation between 5 and 7. This plot illustrates nicely that keeping the chlorine to ammonia ratio between 3 and 5:1 forms almost exclusively the desired monochloramine residual and does so at levels that are detectable and will persist in the distribution system As the ratio goes beyond 5:1, undesirable dichloramine begins to form, AND the measured residual begins to drop until it is completely lost somewhere between 7 & 8. This phenomena is referred to as the âbreakpointâ where all of the mono and dichloramine has been oxidized. As the chlorine dose and corresponding ratio increases further, trichloramine and free chlorine predominate and the phone begins to ring with lots of taste and odor complaints! Chlorine and ammonia react very quickly together, so if either or both are poorly mixed in the treatment process the actual applied ratio can vary dramatically from what is intended. The bottom line: good mixing and monitoring is crucial
Here are two graphs showing the impact of pH on chloramine species formation The graph on the left shows percentage of combined chlorine as a function of pH. Following the dashed green line clearly illustrates that monochloramine formation is favored over di- & trichloramine at a pHâs beyond 7âŚand maintaining the pH between 8 and 8.5 is a common practice for plants practicing chloramination The graph on the right illustrates that the rate of monochloramine formation is also a function of pHâŚand that the rate peaks at a pH of 8.4
Adding ammonia, a source of nitrogen, to water can potentially lead to nitrification. Nitrification can occur if excess ammonia is available in the system. This will happen if the chlorine to ammonia ratio is too low or simply through autodecomposition of the monochloramine residual over time, especially in warm water conditions. Two groups of nitrifying bacteria are responsible for nitrification nitrosomonas feed on the excess available nitrogen oxidizing it to nitrite. Nitrobacter in turn feed on nitrite converting it to nitrate The factors that impact nitrification potential are The amount of free ammonia as nitrogen available Water temperature pH (the rate is highest at pH 7.5 to 8.5) And residence time
Nitrification can lead to: Loss of disinfectant residual can lead to an increase in HPCs and total coliform bacteria levels Nitrifying bacteria consume dissolved oxygen as they convert ammonia to nitrite and nitrate Consumption of alkalinity can reduce the buffering capacity of the water, lower the pH and make the water less pH stable Corrosion potential can be increased due to a lower oxidation-reduction potential (ORP) and/or lower pHâŚthe Washington, DC story will focus more on this impact. Nitrifying bacteria will cause nitrite and nitrate levels to increase Taste and odor complaints may increase
To control nitrification you have to monitor your system very carefully: increases total coliforms, HPCs, nitrite and nitrate levels, and loss of residual are key indicators. Knowing your system and understanding where the greatest potential may exist (storage tank, dead ends, places where water age is an issue) will help to control nitrification. If nitrification occurs, or to pre-empt it from occurring, some utilities convert to free chlorine residual for short periods. Be warned that doing so will likely create taste and odor problems due to shifting chlorine to ammonia ratios and localized production of di- & trichloramine Spot chlorination of water tanks and/or other parts of your system where water age is a concern may help Increasing chloramine residual, particularly in warmer months will help Increasing the chlorine to ammonia ratio closer to 5:1 will reduce free ammonia levels in the systemâŚminimizing the food source for nitrifying bacteria Controlling the distribution system pH at 8.4 promotes optimum monochloramine formation System flushing and water age reduction strategies will also help considerably
LCR compliance monitoring began to show levels in the system above the 90 percentile 15ppb action level beginning in July 2000. The number of homes exceeding the action level grew rapidly in each of the next several LCR monitoring cycles until in February, 2004 when the Washington Post ran the story âThe Lead Hits the Fanâ. The next month two congressional hearings focused on WASAâs lead problem and EPA offered some heavy criticism leading to the resignation of the WASA Director.
DCâs lead problem was the most intensely covered national drinking water story in recent years. In 2004 & 2005 More than 230 articles appeared in the Washington Post More than 120 stories on local TV and radio Corrosion experts were consulted In April 2004 the senate introduced the Lead-Free Drinking Water Act and WASA ships 23,000 filters to homes with lead service lines In May the Post and Time Magazine decree that chloramine is the smoking gun and cause of the lead problem
WASA, USEPA, and a Technical Expert Work Group conducted a series of studies to address, reduce, and control lead levels at the consumer tap. In June 2004, WASA began zinc-free orthophosphate addition in a portion of their system and based on the favorable results, began full system application in August. So finally, after about four years of increasing lead levels, and lots of public scrutiny and outrage, the levels began to drop To add insult to injury, right about that time, the legal system began a massive class action lawsuit advertising campaign
The problem in Washington, DC gave chloramines a severe black eye and their use continues to be questioned by some citizens and groups as the folks from right here in Burlington, VT can attest â for reasons other than corrosion. Chloramine use continues to grow today to enable utilities to comply with more stringent DBP Rules The big lesson learned from the Washington experience is that careful evaluation and attention must be devoted to corrosion issues when changing water quality in the distribution system.
The Washington experience raised many questions in the effort to determine what really happened. Were things done incorrectly and could this happen in New England? Absolutely. Did the switch to chloramines cause the problem? Yes, but it could have been avoided. Were chloramines the primary cause? No! Do we fully understand the science, the chemistry? For the most part yes. Is chloramine disinfection safe? When it use is carefully planned and monitoredâŚyes.
Reviewing the history of what happened in Washington reveals a troubling, but not that surprising or uncommon set of circumstances. For decades, lead service line replacement had been debated and recommended but the price tag was too high. There are over 28,000 identified lead service lines in this densely populated city. Corrosion control issues had been raised over the same time period with little being done to address these concerns. Almost immediately following the switch to chloramines in 2000, lead and copper corrosion problems began to appear in the form of pinhole leaks in copper services and elevated lead levels at consumer taps. Chloramines altered the corrosion chemistry and accelerated lead leeching from service lines. The already dubious corrosion control strategies and history of lead risk were pushed to the brink and, as they say, all hell broke loose! The consequences and public outcry were devastating not just for Washington, DC, but for all of us in the water business.
Looking back at chloramine chemistry again, two important differences are noted between chlorine (HOCl) and monochloramine reactions and their impact on corrosion: Free chlorine is a much more powerful oxidizer and will establish a higher ORP in the distribution system than monochloramine. As I described earlier, monochloramine adds a nitrogen source that can, through the nitrification process, further lower the ORP and the pH in some cases. ORP and pH play a crucial role in lead and copper corrosion chemistry
Another look at nitrificationâs impacts: Nitrification, as described earlier, is the conversion of ammonia to nitrate by nitrifying bacteria under aerobic conditions. The reaction impacts corrosion chemistry because