Wetland Network '16up'  

About the project

Wetland network - a project which will try to get an answer to the crucial question: "Is our wetland feeling well?"  The  answer to that question you'll get within a couple of hours and with a minimum of equipment, but you have the opportunity to add and report other analyses than those you find in the guideline below. 

Before you start to carry out the testing if your wetland is feeling well choose basic level or advanced. Then please read Guidelines and Materials needed.

Choose Level: Basic (click here) or Advanced (below)

Guidelines

1. Read the manual
2. Find a wetland area close to your school.
3. Start the investigation.
4. Sum up results and report your investigation directly on a mobile phone (http://www.schoolweb.se/wetland/phone.htm) or print the form (click here) and report later to the database. You get an opinion about the health of the area by adding plus (+) and minus (-)
5. Then compare information with similar areas around the globe - over the Internet.

Materials

  • Outside
    • Manual
    • Guide to plants and animals 
    • Spade
    • Ruler
    • Thermometer take the temperature immediately after collecting the sample
    • Measure 20m
    • Plastic bag to bring samples from soil or vegetation back to school., 
    • Plastic or glass bottle to bring water-samples back to school. Rinse the bottle with the wetland water. Don't use any detergent or washing up liquid. Then fill the bottle to the top (no air at the top).  
    • secchi-disc or similar 
      White metallic disc designed for the measurement of the clarity of a body of water. The disc is lowered into the water on a graduated line. The depth at which the disc is no longer visible is recorded - a rough limit of the visibility.
    • aqua-scope for secchi-disc readings and aquatic plant and animal observations ( see Fig above, it's just a plastic pipe or similar)
    • plankton net
      Useful in many aquatic areas - to collect micro-organisms in water

      If you can't find a plankton net in your school try to make one yourself (see Figure)

      1. Small plastic jar  - put a stone inside the jar (easier for the net to get under the water surface
      2. rubber band
      3. fine-meshed net 'nylon stockings'
      4. plastic strings
  • In lab
    • pH-paper
    • destilled water ( you'll find it in a petrol station) 
    • filtrerpapper
    • funnel
    • conductometer
    • indicator solution (bromcresol green-methyl)
    • burette
    • hydrochloric solution 0,02 mol/dm3

 

Field activity

  • The approach to the sampling site must be easy and safe.
  • Samples must not be collected from stagnant water 
  • Note date and time of sampling.
  • Observe and record the surroundings around the site of sampling.
    • Vegetation and animals in the water and on land.
    • Human activity around (fishing, drinking, boating, washing....)
    • Bedrock and soil surface on land.
    • Water - colour, odour etc
  • Give the site of sampling a name.
  • Samples should be taken a bit from the 'landedge' (for example tie a bottle to the end of a long stick

I.   Address of wetland

 

 

 Country 
  State (US only) otherwise leave empty
  Name of your city or village
  Name of your school
  Your email-address  (just for registration; will not be published)

II.  Month of research 

 

  Month of research  

III. Description of wetland

  Name of wetland area  
  Type of wetland area
(stream, river, mere, lake)		  
     
  General observations of the sampling area (weather, air temperature, bottom material, soil around, water flow, borders, colours, salinity, how is the wetland used) 
     
  Temperature  
 


Variations in water temperature profoundly affects the aquatic life. At higher temperatures gases like oxygen dissolve to a lower extent than in cool water. Aquatic animals are affected by this as they are weakened by the less availability of oxygen. Plants on the other hand grow better with raise in temperature.
The water temperature can get raised due to both natural and human factors.
This test has to be done immediately after collecting the sample. Keep the thermometer dipped for sufficient time before constant at a reading.

   
  Most characteristic field-plants around your wetland  
  Field vegetation is more dynamic than trees. 
Reproductive maturity is reached earlier, the life span is shorter and the dependence on environmental factors 
(such as pH and nitrate) seems to be grater.
Death of herbaceous vegetation beneath affected trees is a warning sign.
    
  Birds observed    
     
  Benthic fauna (insects on water surface)   
     
  Pollution degree
Estimating the degree of pollution includes a study of the fauna because it indicates how stable or strained the ecosystem is.
 

A
Clean and pure water
if you find these moni-beasts


Mayfly nymph


Stonefly nymph

B
Slightly polluted water 
if you find these moni-beasts nut none from A


Caddisfly larva


Freshwater shrimp

C
Moderate polluted water 
if you find these moni-beasts nut none from A or B


Water louse


Bloodworm

D
Filthy water
if you find these mini-beasts nut none from A, B or C


Sludgeworm


Rat-tailed maggot

E
Heavily polluted water with no life at all
if you find no mini-beasts at all

No life

 

     
  Water pH  
  This indicates how acid or alkaline the water is. pH is defined as the logarithm of the hydrogen ion (H+) expressed in moles per liter. An acid solution has a pH value less than 7 and a hydrogen concentration above 10-7 mol/dm3. An alkaline solution has a value of more than 7 and a hydrogen concentration lower than 10-7 mol/dm3.

A solution of pH 5  is 10 times more acid than a solution of pH 6.

Some natural waters range from pH 4 up to pH 9 and are often slightly basic due to the presence of carbonates and bicarbonates. A major deviation from the normal pH for a given water indicates the intrusion of strongly acidic or strongly basic industrial wastes.

pH can range widely due to addition of wastes from industries and cities but also from the photosyntetic activity in the water itself. During the assimilation period (daytime) carbondioxide is consumed and water pH is slightly increased. Nighttime, when assimilation is null, organisms are breathing. Carbondoioxide is produced and pH is lowered.

 

Technique (choose one alternative) 

  • pH paper
    • Take a sample from the water and pour it into a suitable clean container
    • With dry hands tear a strip from a pH paper roll and dip one end of the strip into the water briefly. Then compare the colour developed on the wet portion of the strip with the colour shart printed on the cover of the paper roll.
  • Universal indicator - a mixture of pH indicators, used to gauge the acidity or alkalinity of a solution. Each component changes colour at a different pH value, and so the indicator is capable of displaying a range of colours, according to the pH of the test solution, from red (at pH 1, strong acid) through green (neutral) to purple (at pH 13, strong alkali).
    • Take 8 ml of a sample water in a test tube. Add 2 drips of the indicator. Shake the test-tube and compare
    • Strong acid = red; Weak acid = orange/yellow; Neutral = green; Weak alkali = turquoise/bkue; Strong alkali = = deep blue/purple
  • Electronic pH-meter. There are many meters on the market, follow the instructions of the meter you use.
     
  Alkalinity mmol bicarbonate per litre  
 

Alkalinity is a measure of the capacity of water to neutralize acids. It's due to the presence of bicarbonate (HCO3-), carbonate(CO32-) and hydroxide ions(OH-).  Bicarbonate is the major form of alkalinity. Carbonate and hydroxide may be significant when algal activity is high and in certain water and wastewater, such as boiler water. 
Total alkalinity is determined by titration to a pH of 5,4 depending on the amount of carbon dioxide present.
At pH=5,4 Alkalinity is null
If acids are added to a water with pH<5,4 the pH of the water is lowered.
If acids are added to a water with pH>5,4 then the pH will stay constant but the amount of bicarbonate will be lowered.

 

Technique (without pH-meter)

  1. Put a 50 ml sample in a beaker (or similar). Add 3 drops of a mixed indicator solution (bromcresol green-methyl red for a distinct point colour change) to the sample.
  2. Fill a burette with 0,02 M HCl and clamp it so that the acid can be run into the sample.
  3. Add HCl from burette and stir the sample until the indicator get the colour of pink.
  4. Note the added amount of acid v ml and count the alkalinity or the concentration of bicarbonate.

    Alkalinity = 0,02 * v / 50
Tecnique (using pH-meter)


Instead of adding indicator - put a pH-electrode in the beaker. Clamp it gently in position; if you are using a magnetic stirrer, make sure that the electrode is in such a position that it cannot be struck by the stirrer bar when the stirrer is switched on. Note the pH of the sample.

Switch on the magnetic stirrer and run the acid into the sample slowly, noting the pH after each addition, until you get the pH value 5,4.  Then you stop the addition of acid, note the added amount of acid v ml and count the alkalinity
 
  Alkalinity  Acidity
  < 0,16 mmol bicarbonate per litre a High risk
  0,17-0,49 mmol bicarbonate per litre a Some risk
  > 0,50 mmol bicarbonate per litre a No risk

     
  Suspended solids  
  Solids may affect the water quality adversely in a number of ways. Outside sources that can affect the natural balance of total solids include urban runoff like fertilizers from residential agricultural use (mainly phosphates and nitrates). Sources that can affect the level of suspended solids are leaves and other plant material, suspended sediments (clay particles) from urban runoff and soil erosion and decayed plants and aimal matter.
High concentration of suspended solids reduces water clarity, contributes to decrease in photosynthesis; binds with toxic compounds and heavy metals; and leads to increase in water temperature through greater absorption of sunlight by surface water.

No
residue

Low
residue

High
residue

Very high residue

 Method
 1. Filter 100 ml sample through a funnel lined with a filter paper (Whatman No. 1)
 2. Allow the filter paper to dry
 3. Unfold the dry filter paper and observe it for any retained solid.
 4. Record the observation

     
  Conductivity (mS/m)  
  Conductivity is a measure of the ability of water to pass an electrical current. Conductivity in water is affected by the presence of inorganic dissolved solids such as chloride, nitrate, sulfate, and phosphate anions (ions that carry a negative charge) or sodium, magnesium, calcium, iron, and aluminum cations (ions that carry a positive charge). Organic compounds like oil, phenol, alcohol, and sugar do not conduct electrical current very well and therefore have a low conductivity when in water. Conductivity is also affected by temperature: the warmer the water, the higher the conductivity. For this reason, conductivity is reported as conductivity at 25 degrees Celsius (+25o C).

Conductivity in a streaming water is affected primarily by the geology of the area through which the water flows. Streams that run through areas with granite bedrock tend to have lower conductivity because granite is composed of more inert materials that do not ionize (dissolve into ionic components) when washed into the water. On the other hand, streams that run through areas with clay soils tend to have higher conductivity because of the presence of materials that ionize when washed into the water. Ground water inflows can have the same effects depending on the bedrock they flow through.

Discharges to streams can change the conductivity depending on their make-up. A failing sewage system would raise the conductivity because of the presence of chloride, phosphate, and nitrate; an oil spill would lower the conductivity.

The basic unit of measurement of conductivity is the mho or siemens. Conductivity is measured in micromhos per centimeter (µmhos/cm) or microsiemens per centimeter (µs/cm). Distilled water has a conductivity in the range of 0,5 to 3 µmhos/cm. The conductivity of rivers generally ranges from 50 to 1500 µmhos/cm. Studies of inland fresh waters indicate that streams supporting good mixed fisheries have a range between 150 and 500 µhos/cm. Conductivity outside this range could indicate that the water is not suitable for certain species of fish or macroinvertebrates. Industrial waters can range as high as 10,000 µmhos/cm.

     
  Turbidity  
 

This is the result of fine solids in the water. Thes solids can be in form of sand, industrial wastes and sewage contributed by soil, industrial and urban discherges.

Oil which does not settle down and floats on the surface as a milky white film cuts the sunlight reaching the water body. Thus turbidity decreases the light penetrating into the water, which in turn reduces the photosynthetic ativity of plants. Heavy solid particles settle down and smother organisms at the river bottom.

The turbidity is measured with help of a turbidmeter. A Secchi disk, based on the visibility of an object in water is an approximation. The Secchi disk is made of any hard and heavy material such as iron. The metal piece can be cut either in circular or rectangular shape. The disk is tied with a string at the center and coloured white. 

Procedure
Lower the Secchi disk into water until it disappears from view. Mark the string length that has gone under the water. The length of the string is referred to as the secchi disc transparency.

     
  Smell
     
  True colour (ocular inspection)  
     
  Other analyses (i.e. content of oxygen, hardness, content of phosphate....)  

© Hans Willstedt, Vaxjo Katedralskola, Sweden. Revised: 09 02, 2005