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OL EH :H E L M U T T OD O T UA S I M A M O RA

BADAN LINGKUNGAN HIDUP, PENELITIAN DAN PENGEMBANGANKABUPATEN SAMOSIR PROVINSI SUMATERA UTARA

BELAJAR TENTANG ANALISIS MENGENAI DAMPAK LINGKUNGAN HIDUP(AMDAL) TENTANG BEBERAPA PARAMETER YANG MEMPENGARUHI

KUALITAS AIR DARI ASUPAN PAKAN KEGIATAN BUDIDAYA PERIKANAN AIR TAWAR

DAN ASUPAN KANDUNGAN ORGANIK DALAM AIR LIMBAH PADA BADAN AIR

PENGUKURAN KANDUNGAN NITRAT

How is Nitrate measured?A common method for nitrate measurement is Method

353.2. Samples are run through a cadmium column to reduce nitrate to nitrite. Nitrites react with an added reagent and generate a red coloured solution whose absorbance is then measured spectrophotometrically at 543 nm. The absorbance of the solution is directly proportional to the concentration of nitrite in the sample. Another method used for the detection of nitrate in water is the nitrate electrode method. This method operates in a similar fashion to a dissolved oxygen meter, where an electric potential of a solution is correlated to the concentration of nitrates in mg/L. Nitrate concentrations can be reported as mg/L NO3 or as mg/L nitrate-nitrogen (NO3-N).

PENGARUH NITRAT

Why is Nitrate important? Nitrogen is a major nutrient for microbial life and is therefore very

important with regards to its effects on the environment. Among nitrogen containing compounds, nitrate is the most common form in water. All other dissolved forms of nitrogen (nitrite, ammonia and organic nitrogen) get oxidized to nitrate over time. Nitrates are found in both ground and surface water, originating from the natural decaying process of biological matter. Many anthropogenic sources also contribute to nitrate levels in the environment such as industrial and municipal wastewater discharge and agricultural runoff containing nitrogen based fertilizers and livestock manure. Nitrate has a high solubility in water and will not be filtered out like other contaminants as it seeps through the soil layers to groundwater level. Measurement of nitrate is important for several applications.

KANDUNGAN NITRAT DALAM LIMBAH

In the drinking water industry, maximum contaminant levels of 50 mg/L NO3 in the EU and 10 mg/L NO3-N in the USA have been established for public safety. When nitrate enters the bloodstream of humans they reduce the ability of red blood cells to carry oxygen, which has serious health effects. This is particularly important for infants under the age of 6 months where excessive levels of nitrates in their bloodstream leads to a health condition known as methemoglobinemia or “blue baby syndrome”. Thus, measuring and removing nitrate from drinking water are important.

Wastewater contains high amounts of nitrates from human sewage and industrial process waste. Monitoring nitrate in wastewater is important to ensure proper removal prior to discharging into the environment.

PEMANTAUAN LEVEL KANDUNGAN NITRAT

From an environmental perspective, monitoring nitrate levels in surface water can indicate the potential for eutrophication or “nutrient pollution”. The influx of nutrients to surface waters can cause accelerated algal growth. When the large algae blooms die out, bacterial action increases expending oxygen levels. Waters may become hypoxic or anoxic, causing stress and possible death of aquatic life. Monitoring nitrate input to surface waters not only protects the health of the water body, but the safety of those who rely on the source.

Measuring Nitrate with UV-VIS technology Measuring nitrates and or/nitrites with UV-VIS technology is a

practical and reagentless solution for real-time monitoring. Nitrate ions have natural absorbance peaks in the 200-220 nm wavelength range in the UV spectrum. As the concentration of nitrates in water or wastewater increases, the absorbance of light in this distinct wavelength range will also increase.

Common interferences with nitrate measurement at 220 nm, such as organic compounds, nitrite, iron (II), hexavalent chromium and turbidity or suspended solids are compensated for by measuring absorbance at additional reference wavelengths in the UV-VIS spectrum where the interfering compounds absorb, but nitrates do not. This multiple wavelength approach ensures a high degree of precision and accuracy.

Where is Nitrate measured? Influent of a drinking water plant from a ground or surface water source After blending of multiple sources to determine reduction Effluent drinking water for compliance assurance Pre and post ion exchange or reverse osmosis for removal efficiency In process for nitrogen removal from wastewater Environmental monitoring stations for contamination events or locating

source pollution

Nitrate test strips are an affordable tool for quickly measuring nitrate (NO3) in soil and water, and can help farmers and crop advisers adjust fertilizer inputs to match the nitrogen (N) needs of various types of crops. There are now a variety of brands of nitrate test strips available, many of which are manufactured for testing the quality of aquarium water, but may also be suitable for soil testing.   All of the brands of test strips are used in a similar fashion: the strip is briefly dipped into an extractant solution (for soil) or in water, and allowed to develop color during a standard interval of time, usually ranging between 30 and 60 seconds.  After color develops on the strip, a color chart, calibrated to either parts per million (ppm) of NO3 or expressed in ppm equivalents of nitrogen (NO3-N), is used to determine the NO3 concentration of the sample. Multiplying Nitrate-N concentration by a factor of 4.43 converts the reading to NO3 concentration.  Because the strips may continue to develop color with time, it is important to always read the strips at a standard time interval, or the measurements will not be accurate or repeatable.  More detailed information on using the nitrate test strips for monitoring soil nitrate levels was presented in several of our past bulletins, newsletters, and blogs.

KANDUNGAN NUTRISI DALAM TANAH

Depending on the soil type and crop nutrient requirements, vegetable farmers need test strips that are accurate for soil NO3-N concentrations ranging between from 5 to 30 ppm, which would roughly correspond to a range of 10 to 60 ppm of NO3 in the nitrate quick test extract solution.  For strawberry production, and other crops that have a slower N uptake rate than vegetables, growers need test strips that are accurate over a narrower range of soil NO3 concentrations (5 to 15 ppm NO3-N in soil).  Past studies have demonstrated that the Merckoquant test strip are accurate for measuring soil NO3-N in the range of 10 to 40 ppm.   Because more brands of test strips have become commercially available in recent years with varying ranges of sensitivity, and the need to identify test strips that are accurate for measuring low concentrations of soil NO3-N (0 to 15 ppm), we evaluated the accuracy and ease of using six commercially available brands of test strips over a range of nitrate concentrations found in commercial agricultural fields.

PROSEDUR

Procedures: A stock solution of a known NO3 concentration was prepared by dissolving a

measured weight of sodium nitrate (NaNO3) into 1 liter of distilled water.  This stock solution was further dilluted with distilled water to standard nitrate concentrations that matched the values of the color chips of the various test strips evaluated in this study.    The NO3 concentration of each standard solution was confirmed by spectrophotometric analysis.

Each brand of strip was evaluated at NO3 concentrations corresponding to the color chips provided by the manufacturer.  The Hach Aquacheck and Lamotte Instatest NO3/NO2 strips differed from the other brands because the color chips were calibrated in  equivalents of  NO3-N rather than NO3.  For convenience of displaying and comparing the data, results for these two brands were converted to NO3 (by multiplying the NO3-N values by 4.43).  The Merckoquant NO3/NO2 test strip was the brand originally tested by UC Cooperative Extension for use with the soil nitrate quick test, and was considered the standard in this evaluation.  This strip measures to a maximum of 500 ppm NO3, but was only evaluated up to 250 ppm NO3 (56 ppm NO3-N) for this test. 

Each brand of test strip was evaluated 4 times for each standard NO3 solution corresponding to the manufacturer's chip color chart.  The procedure that we followed to determine NO3 concentration was to dip the strip briefly in solution, and hold it horizontally after removing it, allowing color to develop for the interval specified by the manufacturer.  Most strip manufacturers recommended a 1-minute time interval between wetting and reading the strip color. 

The manufacturer for API 5-in-1 and LaMotte Instatest 5-Way recommended reading test strips after 30 seconds, but results appeared to be more accurate after a 60 second interval, therefore all results reported for these strips are from readings taken 60 seconds after placing the strip in the test solution.   After waiting the specified interval, the color of the test strip was compared to the color chips provided by the manufacturer.  If the test strip color matched one of the chips, then the value of the chip was recorded. In many cases, the color of the test strip was between 2 of the standard chips, and in these cases an estimate was made based on comparing the intensity of the color development with the 2 closest matching chips.  Because this method relies on visual observations, all tests were made in a room with ample lighting and by one observer. 

HASIL

Results:The mean NO3 values measured using different brands

of test strips were compared to the standard solution values in Table 1.  Some brands of test strips appeared to be accurate at specific ranges of NO3 concentration.  The Merckoquant NO3/NO2 brand was the most accurate for the full range of NO3 concentrations (Table 1).  The next most accurate brand over the entire range of NO3concentrations evaluated was the LaMotte Instatest NO3/NO2. 

The Hach Aquacheck was accurate for the range of 10 to 90 ppm NO3 but measured NO3 lower than the standard solutions at concentrations above 100 ppm NO3.  The remaining brands of test strips, LaMotte  Instatest 5-way, API 5 in 1, Tetra 6 in 1 Easystrips, all measured less NO3 than the standard solutions over the range of 20 to 200 ppm NO3.  These strip brands should probably not be used for the soil nitrate quick test and for assessing nitrate concentration in irrigation water. 

Although the LaMotte Instatest NO3/NO2 also had good accuracy across the range of 20 ppm to 220 ppm NO3, it did not have a standard color chip for evaluating NO3 at low concentrations, and therefore may not be suitable for strawberries and other crops where soil nitrate is typically in the 5 to 15 ppm NO3-N  range.  Both the Merckoquant and Hach brands were accurate for measuring NO3at low concentrations (10 to 40 ppm).  Although the Hach Aquacheck strip had a color standard of 5 ppm NO3, the strip was not able to measure NO3 at a concentration below 10 ppm (Table 1).

TABEL KLASIFIKASI KONSENTRASI NITRAT

Table 1.  Comparison of nitrate-test strip and standard solution values.

TABEL PROPORSI TOKSIK

TABEL FLUKTUASI pH

AMONIA

Ammonia is toxic to fish if allowed to accumulate in fish production systems. When ammonia accumulates to toxic levels, fish can not extract energy from feed efficiently.

If the ammonia concentration gets high enough, the fish will become lethargic and eventually fall into a coma and die. In properly managed fish ponds, ammonia seldom accumulates to lethal concentrations. However, ammonia can have so-called “sublethal” effects—such as reduced growth, poor feed conversion, and reduced disease resistance—at concentrations that are lower than lethal concentrations.

PENGARUH pH

Effects of pH and temperature on ammonia toxicity Ammonia in water is either unionized ammonia (NH3) or the ammonium ion (NH4+). The techniques used to measure ammonia provide a value that is the sum of both forms. The value is reported as “total ammonia” or simply “ammonia.” (In this publication, “ammonia” refers to the sum of both forms; the specific forms will be referred to as appropriate.)

The relative proportion of the two forms present in water is mainly affected by pH. Un-ionized ammonia is the toxic form and predominates when pH is high.

Ammonium ion is relatively nontoxic and predominates when pH is low. In general, less than 10% of ammonia is in the toxic form when pH is less than 8.0. However, this proportion increases dramatically as pH increases.

The proportion of toxic, un-ionized ammonia increases as a function of pH and temperature. To determine the proportion of un-ionized ammonia in a water sample, draw a line from the pH of the water straight up to the line that is closest to the water temperature. From that point, draw a line to the right until it intersects the graph’s vertical axis. That point is an estimate of the percentage of un-ionized ammonia in the water sample. Now, simply multiply that number (divided by 100) by the total ammonia concentration to estimate the un-ionized ammonia concentration.

In ponds, pH fluctuates with the photosynthesis (which increases pH) and respiration (which reduces pH) of pond organisms.

Therefore, the toxic form of ammonia predominates during the late afternoon and early evening and ammonium predominates from before sunrise through early morning. The equilibrium between NH3 and NH4+ is also affected by temperature. At any given pH, more toxic ammonia is present in warmer water than in cooler water.

Ammonia dynamics in fish ponds The measurement of ammonia concentration (and that of many other water quality variables) provides only a snapshot of conditions at the time a water sample is collected. A single measurement provides no insight into the processes that affect ammonia concentrations; it is simply the net result of processes that produce ammonia and processes that remove or transform ammonia.

The relationships among these processes are complex, but the important point is that the rates change differentially throughout the year and result in the measured patterns.

Ammonia sources The main source of ammonia in fish ponds is fish excretion. The rate at which fish excrete ammonia is directly related to the feeding rate and the protein level in feed. As dietary protein is broken down in the body, some of the nitrogen is used to form protein (including muscle), some is used for energy, and some is excreted through the gills as ammonia. Thus, protein in feed is the ultimate source of most ammonia in ponds where fish are fed.

Another main source of ammonia in fish ponds is diffusion from the sediment. Large quantities of organic matter are produced by algae or added to ponds as feed.

Fecal solids excreted by fish and dead algae settle to the pond bottom, where they decompose. The decomposition of this organic matter produces ammonia, which diffuses from the sediment into the water column.

Ammonia sinks There are two main processes that result in the loss or transformation of ammonia. The most important is the uptake of ammonia by algae and other plants. Plants use the nitrogen as a nutrient for growth, “packaging” the nitrogen in an organic form. Algal photosynthesis acts like a “sponge” for ammonia, so anything that increases overall algal growth will increase ammonia uptake. Such factors include sufficient light, warm temperature, abundant nutrient supply, and (to a point) algal density.

The other important process of ammonia transformation in fish ponds is “nitrification.” Bacteria oxidize ammonia in a two-step process, first to nitrite (NO2-) and then to nitrate (NO3 -). The main factors that affect nitrification rate are ammonia concentration, temperature and dissolved oxygen concentration. During summer, ammonia concentration is very low and so nitrification rates are also very low. During winter, low temperature suppresses microbial activity. During spring and fall, ammonia concentration and temperature are intermediate, conditions that favor maximum nitrification rates. Spring and fall peaks of nitrite concentration are commonly seen in fish ponds.

The effect of daily fluctuation in pH on un-ionized ammonia concentration in fish ponds. The top horizontal line indicates a total ammonia concentration of 2.5 mg N/L, which is assumed not to change during the day. The two curved lines indicate daily changes in un-ionized ammonia concentration where the maximum afternoon pH is 9.0 or 9.5. These conditions indicate that fish may be exposed to toxic, un-ionized ammonia concentrations for brief periods during the late afternoon.

Other processes, such as the volatilization of ammonia gas from the pond surface into the air, are responsible for a relatively small and variable amount of ammonia loss from fish ponds.

When is ammonia most likely to be a problem? In fish ponds, it is extremely unlikely that un-ionized ammonia would accumulate to a concentration that would become toxic enough to kill fish. However, unionized ammonia will occasionally accumulate to levels that cause sub-lethal effects.

The following analysis is based on water quality criteria for ammonia developed by the U.S. Environmental Protection Agency (EPA).

The EPA has established three kinds of criteria (one acute and two chronic) for ammonia (expressed as nitrogen), based on the duration of exposure. The acute criterion is a 1-hour average exposure concentration and is a function of pH. One chronic criterion is the 30-day average concentration and is a function of pH and temperature. The other chronic criterion is the highest 4-day average within the 30-day period and is calculated as 2.5 times the 30-day chronic criterion. The EPA criteria help determine when ammonia might be a problem.

During winter It is generally assumed that ammonia is not a problem in the winter because feeding rates are very low. (Fish are fed on only the warmest days of winter, usually when the water temperature is higher than 50 °F.) However, ammonia concentration tends to be greater during winter (2.5 to 4.0 mg/L, or even higher) than during summer (less than 0.5 mg/L) (Fig. 3). The relatively low concentration during summer can be attributed to intense photosynthesis by algae, which removes ammonia. During winter, algae take up little ammonia but the ammonia supply continues, primarily from the decomposition of organic matter that accumulated on pond sediment during the growing season. In general, the magnitude and duration of high ammonia concentrations during the late fall and winter can be related to the total amount of feed added to a pond during the preceding growing season.

PENGARUH MUSIM

The 30-day chronic criterion for ammonia (as nitrogen) in winter ranges from about 1.5 to 3.0 mg/L, depending on pH. Ammonia concentrations during the winter usually exceed this criterion. This may cause stress in fish at a time of year when the fish immune system is suppressed because of low temperature.

After the crash of an algae bloom Some ponds have very dense algae blooms dominated by one or two species. For reasons that are not well understood, these blooms are subject to spectacular collapse, often called a “crash,” where all the algae suddenly die. When this occurs, ammonia concentration increases rapidly because the main mechanism for ammonia removal—algal uptake—has been eliminated.

Rapid decomposition of dead algae reduces the dissolved oxygen concentration and pH and increases ammonia and carbon dioxide concentrations.After the crash of an algae bloom, ammonia concentration can increase to 6 to 8 mg/L and the pH can decline to 7.8 to 8.0. The 4-day chronic criterion, the appropriate criterion to apply. Approximate annual variation of total ammonia concentration in fish ponds. Ammonia concentration is generally lowest during summer and highest during winter.

following the crash of an algae bloom, ranges from about 2.0 mg/L at pH 8.0 to about 3.0 mg/L at pH 7.8. Therefore, ammonia concentration after the crash of an algae bloom may exceed the 4-day chronic criterion.

Occasionally during the late afternoons in late summer or early fall Seasonal variation in ammonia concentration depends on algal density and photosynthesis. When these are high, ammonia concentration is low. Daily variation in the concentration of toxic, un-ionized ammonia depends on changes in pH (from photosynthesis) and, to a much lesser extent, temperature. In the late summer or early fall, ammonia concentration begins to increase but daily changes in pH remain large. In these situations, fish may be exposed to ammonia concentrations that exceed the acute criterion for a few hours each day. If late afternoon pH is about 9.0, the acute criterion is about 1.5 to 2.0 mg/L total ammonia-nitrogen.

Total ammonia-nitrogen concentrations during summer are typically less than 0.5 mg/L, so fish are unlikely to be stressed if the late afternoon pH is less than 9.0. It is difficult to be more precise about the risk of ammonia toxicity because of deficiencies in the methodology used in research.

Nearly all ammonia toxicity tests are conducted in systems that maintain a constant ammonia concentration. These conditions do not reflect the fluctuating concentrations of NH3 in ponds.

Accordingly, one must be careful when applying research results to production situations. For example, in one study, growth of channel catfish exposed to a constant ammonia concentration of 0.52 mg/L NH3 was reduced by 50% relative to unexposed fish.

However, brief (2- to 3-hour) daily exposure to 0.92 mg/L NH3 (such as might occur in ponds) did not affect growth and feed conversion ratio. The fact that many fish can acclimate to repeated exposure to high concentrations of un-ionized ammonia is a further complicating factor.

Ammonia management options On rare occasions ammonia concentration becomes high enough to cause problems. What practical steps can be taken if this occurs? The short answer is—not much. Theoretically, there are several ways to reduce ammonia concentration, but most approaches are impractical for the large ponds used in commercial aquaculture.

Following is a discussion of some options, their practicality and their effectiveness. Stop feeding or reduce feeding rate The primary source of nearly all the ammonia in fish ponds is the protein in feed. When feed protein is completely broken down (metabolized), ammonia is produced within the fish and excreted through the gills into pond water. Therefore, it seems reasonable to conclude that ammonia levels in ponds can be controlled by manipulating feeding rate or feed protein level. This is true to some extent, but it depends on whether you want to control it over the short-run (days) or the long-run (weeks or months). In the short-run, sharp reductions in feeding rate have little immediate effect on ammonia concentration.

The ecological reason for this is based on the complex movement of large amounts of nitrogen from one of the many components of the pond ecosystem to another.

In essence, trying to reduce ammonia levels by withholding feed can be compared with trying to stop a fully loaded freight train running at top speed—it can be done but it takes a long time.

Producers can reduce the risk over the long-run by adjusting both feeding rate and feed protein level. Limit feed to the amount that will be consumed. In midsummer the maximum daily feeding rate should be 100 to 125 pounds per acre. By feeding conservatively, the potential for high ammonia in ponds and the risks associated with sub-lethal exposure (disease, poor feed conversion, slow growth) can be minimized.

Increase aeration The toxic form of ammonia (NH3) is a dissolved gas, so some producers believe pond aeration is one way to get rid of ammonia because it accelerates the diffusion of ammonia gas from pond water to the air. However, research has demonstrated that aeration is ineffective at reducing ammonia concentration because the volume of water affected by aerators is quite small in comparison with the total pond volume and because the concentration of ammonia gas in water is typically fairly low (especially in the morning). Intensive aeration may actually increase ammonia concentration because it suspends pond sediments.

Add lime It has long been thought that liming ponds decreases ammonia concentrations. In fact, using liming agents such as hydrated lime or quick lime could actually make a potentially bad situation much worse by causing an abrupt and large increase in pH. Increasing pH shifts ammonia toward the form that is toxic to fish. In addition, the calcium in lime can react with soluble phosphorus, removing it from water and making it unavailable to algae.

In ponds with similar algal density, daily fluctuations of pH in low alkalinity pond waters are more extreme than those in waters of sufficient alkalinity (greater than 20 mg/L as CaCO3; see SRAC Publication No. 464). Therefore, liming can moderate extreme pH values, particularly those that occur during late afternoon when the fraction of total ammonia that is in the toxic form is highest.

However, this technique is effective only in ponds with low alkalinity. Most fish ponds have sufficient alkalinity. Increasing the alkalinity above 20 mg/L as CaCO3 will not provide additional benefit. Furthermore, liming does not address the root causes of high ammonia concentration; it only shifts the distribution of ammonia from the toxic to the non-toxic form by moderating high pH in the afternoon. Fertilize with phosphorus Most of the ammonia excreted by fish is taken up by algae, so anything that increases algal growth will increase ammonia uptake. This fact is the basis for the idea of fertilizing ponds with phosphorus fertilizer to reduce ammonia levels. However, under “normal” pond conditions, algae blooms in fish ponds are very dense and the rate of algae growth is limited by the availability of light, not nutrients such as phosphorus or nitrogen.

Therefore, adding phosphorus does nothing to reduce ammonia concentration because algae are already growing as fast as possible under the prevailing conditions.

The highest ammonia concentrations in fish ponds occur after the crash of an algae bloom. Fertilization, particularly with phosphorus, may accelerate the re-establishment of the bloom, but most ponds have plenty of dissolved phosphorus (and other nutrients) to support a bloom and do not need more.

Reduce pond depth Algal growth (and therefore the rate of ammonia uptake by algae) in fish ponds is limited by the availability of light. Anything that increases light increases ammonia uptake. Theoretically, dense algae blooms in shallow ponds will remove ammonia more effectively than the same dense blooms in deeper ponds. On balance, however, there are probably more benefits associated with deeper ponds (e.g., ease of fish harvest, water conservation, more stable temperatures, reduced effect of sedimentation on interval between renovations).

Increase pond depth Obviously, deeper ponds contain more water than more shallow ponds. Therefore, at a given feeding rate, deeper ponds should have lower ammonia concentrations because there is more water to dilute the ammonia excreted by fish. In reality, deeper ponds do not usually have enough water to significantly dilute ammonia when compared to the large amounts of ammonia in constant flux between various biotic and abiotic compartments in ponds.

Furthermore, deeper ponds are more likely to stratify and the lower layer of pond water (the hypolimnion) can become enriched with ammonia and depleted of dissolved oxygen.

When this layer of water mixes with surface water in a “turnover,” severe water quality problems may result. Flush the pond with well water Ammonia can be flushed from ponds, although pumping the huge volume of water required to do so in large commercial ponds is costly, time-consuming and unnecessarily wasteful. It is also deceptively ineffective as an ammonia management tool. For

example, assume the ammonia concentration in a full, 10-acre pond is 1 mg/L. The ammonia concentration after pumping 500 gpm continuously for 3 days (equivalent to about 8 inches of water) will be 0.90 mg/L, a drop of only 0.10 mg/L.

Instead of simply running water through a pond as in the example above, now assume that about 8 inches of water is discharged from the pond before refilling with well water. In this case, the decline in ammonia concentration will be slightly greater (to 0.83 mg/L), but even this decrease is not enough in an emergency situation, particularly when the extra time needed to drain the water before refilling is considered. The difference in the two flushing scenarios is related to the blending of pond water with pumped water before discharge in the first case.

Just as paddlewheel aeration creates a zone of sufficient dissolved oxygen concentration, pumping groundwater creates a zone of relatively low ammonia concentration adjacent to the water inflow.

The effectiveness of this practice is questionable because it does not address the root cause of the problem and wastes water. Flushing ponds is not only ineffective, but highly undesirable because of concerns about releasing pond

effluents into the environment. Add bacterial amendments Common aquatic bacteria are an essential

part of the constant cycling of ammonia in a pond ecosystem. Some people believe that ammonia accumulates in ponds because the wrong kind or insufficient numbers of bacteria are present. If this were true, adding concentrated formulations of bacteria would address the problem. However, research with many brands of bacterial amendments has consistently given the same result: Water quality is unaffected by the addition of these supplements.

Standard pond management creates very favorable conditions for bacterial growth. Bacterial growth and activity is limited more by the availability of oxygen and by temperature than by the number of bacterial cells. Also, the most abundant type of bacteria in many amendments (and in pond water and sediment) is responsible for the decomposition of organic matter. Therefore, if bacterial amendments accelerate the decomposition of organic matter, ammonia concentration would actually increase, not decrease.

Another kind of bacteria in amendments oxidizes ammonia to nitrate. Adding them will not reduce the ammonia concentration rapidly because the bacteria must grow for several weeks before there is a large enough population to affect ammonia level.

Add a source of organic carbon If the dissolved oxygen concentration is adequate, adding a source of organic carbon, such as chopped hay, to intensive fish ponds can reduce ammonia concentration.

Many bacteria in fish ponds are “starved” for organic carbon, despite the addition of large amounts of feed. Organic matter in fish ponds (dead algae cells, fish fecal solids, uneaten feed) does not contain the optimum ratio of nutrients for bacterial growth. There is more than enough nitrogen for bacterial growth so the excess is released to the pond water.

Adding organic matter with a high concentration of carbon relative to nitrogen promotes the “fixation” or “immobilization” of the ammonia dissolved in water. Incorporating ammonia into bacterial cells packages the nitrogen into a particulate form that is not toxic to fish. The down side of this approach is that it is hard to apply large amounts of organic matter to large ponds and the effect on ammonia concentration is not rapid. Furthermore, aeration will have to be increased to address the demand for oxygen by large quantities of decomposing organic matter.

Add ion exchange materials Certain naturally occurring materials, called zeolites, can

adsorb ammonia from water. These are practical to use in aquaria or other small-scale, intensive fish-holding systems, but impractical for largevolume fish ponds.

Some shrimp farmers in Southeast Asia have tried making monthly applications of zeolite at 200 to 400 pounds per acre. However, research has demonstrated that this practice is ineffective at reducing ammonia concentration in ponds and it has now been abandoned.

Add acid In theory, adding acid (such as hydrochloric acid) to water will reduce pH. This can shift the ammonia equilibrium to favor the non-toxic form. However, a large amount of acid is necessary to reduce the pH in well-buffered ponds and it would have to be mixed rapidly throughout the pond to prevent “hot spots” that could kill fish. Furthermore, adding acid would destroy much of the buffering capacity (alkalinity) of the pond before any change

in pH could occur. Once the ammonia concentration is lowered, treated ponds might require liming to restore the buffering capacity. Working with strong mineral acids is a safety hazard for farm workers and for fish.

How often should ammonia be measured? From the foregoing discussion, you might assume that

measuring ammonia in ponds is unnecessary. After all, research has indicated that brief daily exposure to

ammonia concentrations far higher than those measured in commercial ponds does not affect fish growth. And, on the rare occasions when ammonia does become a problem, there is nothing you can do about it. However, there are some special circumstances when it is worthwhile to monitor ammonia levels.

In the South, ammonia concentrations in most ponds usually start increasing in September and peak about mid-October, about 5 to 6 weeks after the last stretch of high feeding rates. Then, about 2 to 4 weeks later, nitrite concentrations peak. This is a general pattern. It does not apply to all ponds, and ammonia or nitrite problems can occur with variable intensity at any time, especially between September and March.

Thus, the magnitude of the ammonia elevation in the early fall can indicate the severity of the nitrite spike that will follow. Salt can protect fish against nitrite toxicosis (see SRAC Publication No. 462). If enough salt is added to ponds to achieve chloride levels of 100 to 150 mg/L, there is no reason to measure ammonia even as a predictor of high nitrite concentrations.

Ammonia should be measured every other day after the crash of an algae bloom and weekly in the cooler months of the year to identify ponds that may have a potential problem with nitrite. Other than those times, it is probably not necessary to measure ammonia in fish ponds.

To summarize, fish producers should not be alarmed if ammonia concentration becomes elevated, although a high ammonia level often indicates that nitrite concentrations may soon rise. In this case, farmers should focus on protecting fish from nitrite poisoning by adding salt, rather than on trying to manage the ammonia problem.

Extra vigilance after an algae crash is also probably warranted. Usually, the concentration of ammonia will fall again once the bloom becomes re-established. Because there is little that can be done to correct problems with ammonia once they occur, the key to ammonia management is to use fish culture practices that minimize the likelihood of such problems.

This means stocking fish at a reasonable density, harvesting as often as practical to keep the standing crop from being too large, and using good feeding practices that maximize the proportion of the feed consumed by fish.

NITRAT

Nitrate in Ponds Nitrate, NO3-N,

Nitrate is the final product from the breakdown of ammonia released by the fish.

Nitrate is not especially harmful to freshwater fish but is a potent plant fertilizer and can contribute to the growth of unsightly and unwelcome algae, such as green water or blanketweed. Ideally, the levels of nitrate in the fish pond should be controlled to help reduce the likelihood of these unwelcome algae blooms occurring. It is recommended that a Nitrate Test Kit is used to determine the quantity present in the pond and control the concentration through water changes.

 

Nitrite in Ponds As the ammonia in the water begins to reduce, the secondary break

down product, nitrite will begin to increase and this is also very poisonous to fish.

Nitrite is a skin irritant and will cause the fish to display symptoms of irritability such as rubbing themselves, jumping, or even skimming across the surface of the pond. These symptoms are also commonly associated with parasites and it is sensible to eliminate nitrite as the cause before treating the pond.

Nitrite also has a rather sinister effect on the pond fishes blood, as it will bind very tightly with the red pigment and thereby preventing the blood cells from absorbing vital oxygen from the water. Once the nitrite has become associated with the red pigment, it turns the blood a dull brown color and hence the popular name for nitrite poisoning is "brown blood disease".

A second group of micro-organisms, comprising mostly species of Nitrobacter bacteria are responsible for breaking down the nitrite into nitrate, which is the final breakdown product but in the event of high nitrite levels occurring in the pond, regular partial water changes need to be undertaken to reduce the concentration of this pollutant.

Nitrite is an odorless, colorless substance and its presence can be detected using a Test Kit

Thank You

Dedicated to :1. My loving wife , Hutapea Olga Y.V, dr;2. My loving daughter :a. Simamora Michelle Renata Robertina;b. Simamora Helga Martha Davina;

Also :3. Environment, Research and Development Agency of Samosir Regency Governmentof North Sumatera Province;2. People of Samosir Regency3. All of You

Alumni : PSMIL – Universitas Padjadjaranat Bandung