Determinants of Water Quality. 1) Biological 2) Physical 3) Chemical Basic Types of Pollution.
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Transcript of Determinants of Water Quality. 1) Biological 2) Physical 3) Chemical Basic Types of Pollution.
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Determinants of Water Quality
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1) Biological
2) Physical
3) Chemical
Basic Types of Pollution
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Develops from microorganisms and their activities.
Biological Water Pollution
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Physical Pollutants
Heat½ of water withdrawn in the U.S.
Thermal Shock to organismsReduction in O2 content.
Sediment
Turbidity limits light penetrationParticles carry contaminants
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Chemical Pollutants
NutrientsPesticides
MetalsSalts
Synthetic Organics
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Two Basic Avenues of Water Pollution
Point source pollution Specific entry pointIndustrial dischargesSewage treatment plantsLandfills
Non-point source pollution
Diffuse sourcesDifficult to trace, regulateAgriculture, Urban Runoff
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Point and Non-Point Pollution
Example
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Superior
Michigan
Erie
OntarioHuron
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Shallowest of the Great Lakesaverage depth = 62 feet
agriculture
Largest population density of Great Lakes
Detroit
Cleveland
Buffalo
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Heavy Metals
Point and Non-Point Source Pollution
Industrial Chemicals
Petroleum
Nutrients
Pesticides
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Non-point Source Pollution
Blue-green algaephytoplankton
Nitrogen and Phosphorus
Agriculture, Wastewater Discharge, Urban Runoff
Stimulation of Primary Productivity
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Point Sources
lip papillomas
PetroleumOrganic ChemicalsHeavy MetalsPesticides
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Cuyahoga River Fire (1969)
Petrochemicals
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Clean Water Act: 1972
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Determining Water Quality
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Major Determinants of Water Qualityand the Impact or Availability of Water Pollutants
OrganismsSolubilityOxygen
pH
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Microorganisms
Pathogenic – harmful
Non-pathogenic - benign
Determinants of Water Quality
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Autotrophic: produce complex organic compounds from simple inorganic molecules and an external source of energy.
The Earliest Organisms
Chemoautotrophs, Cyanobacteria, Plants
Organic = Carbon-containing
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Autotrophs – Plants, Algae, Cyanobacteria
Produce complex organic compounds fromcarbon dioxide using energy from light.
6CO2 + 6H2O C6H12O6 + 6O2
light
simple inorganic molecule complex organic compound
energy
Primary producers – base of the food chain
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Heterotrophic Organisms
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Heterotrophs
Derive energy from consumption of complex organic compounds produced by autotrophs
Autotrophs store energy from the sun in carbon compounds (C6H12O6)
Heterotrophs consume these complex carbon compounds for energy
carbon compounds (C6H12O6)
autotrophs Heterotrophs
ConsumersProducers
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Heterotrophic Organisms
Two Basic Types Related to Oxygen Status
Anaerobic
low-oxygen environments
Anaerobic heterotrophs
Aerobic
high oxygen environments
Aerobic heterotrophs
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Autotrophs store energy from the sun in carbon compounds (C6H12O6)
Heterotrophs consume these complex carbon compounds for energy
There are two types of heterotrophic organisms: aerobic and anaerobic
Aerobic: high oxygen environments, Anaerobic: low oxygen environments
Summary
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Extra Credit:
2. ________consume complex carbon compounds for energy
1. Organisms that live in high oxygen environments are ____
3. Organisms that are directly harmful to health are called ___
4. Organisms that produce complex organic compounds from simple inorganic molecules and an external source of energy are called ______________________________
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Aerobic Heterotrophs and Anaerobic Heterotrophs
Heterotrophic Organisms
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Aerobic Heterotrophic Organisms
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Aerobic Heterotrophs
Obtain the energy stored in complex organiccompounds by combining them with oxygen
C6H12O6 + Oxygen = energy
Live in high-oxygen environmentsConsume organic compounds for energy
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C6H12O6 + 6O2 → 6CO2 + 6H2O
Aerobic Respiration
+ energy
organisms
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C6H12O6 + 6O2 → 6CO2 + 6H2O
Electron poor
Electron rich Electron poor
Electron rich
The energy is obtained by exchanging electrons between carbon and oxygen.
2880 kJ of energy is produced
Aerobic respiration is very efficient, yielding high amounts of energy
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Anaerobic Heterotrophic Organisms
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Anaerobic Heterotrophic Organisms
Can use energy stored in complex carbon compounds in the absence of free oxygen
The energy is obtained by exchangingelectrons with elements other than oxygen.
Nitrogen (NO3-)
Sulfur (SO42-)
Iron (Fe3+)
Live in low-oxygen environmentsConsume organic compounds for energy
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C6H12O6 + 3NO3- + 3H2O = 6HCO3
- + 3NH4+
Anaerobic respiration
C6H12O6 + 6O2 → 6CO2 + 6H2O
Electron poor
Electron rich Electron poor
Electron rich
Aerobic Respiration
Electron rich
Electron poor
Electron poor
Electron rich
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Becoming Anaerobic
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The oxygen status of water determines and is determined by the type of organisms
aerobic or anaerobic
High-oxygen Low-oxygen
Oxygen status also impacts availability and toxicity of some pollutants
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Solubility: 0.043 g/L(20oC)
Oxygen is Water Soluble
O2
O2
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Diffusion of O2 through the water andfrom the atmosphere into water is generally slow
Oxygen enters water from the atmosphereand from aquatic photosynthetic organisms
Oxygen
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Diffusion of O2 in water is generally slow
Heterotrophic organisms together with inputs of organic materials (food sources) control the oxygen status of waters.
C6H12O6 + 6O2 → 6CO2 + 6H2O
Accelerated metabolic activity of aerobic heterotrophsdue to an abundance of organic materials (food source)can significantly reduce the amount of dissolved oxygen
Lower dissolved oxygen levels impact species diversityincluding a shift to a dominance of anaerobic microorganisms
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Reduced Oxygen Levels
Oxygen is being used by aerobic heterotrophsat rate faster than it can be replaced
Oxygen
Slow diffusion
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SO4-2 HS-
O2
NO3-
SO4-2
Respiration and Still Ponds
C6H12O6 + 3SO42- + 3H+ = 6HCO3
- + 3HS-
Heterotrophic Organisms
oxygen
Aerobic heterotrophsconsume oxygen
Anaerobic heterotrophsUse nitrate instead of O2
Anaerobic heterotrophsUse sulfate instead of O2
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C6H12O6 + 3NO3- + 3H2O = 6HCO3
- + 3NH4+ 1796 kJ
C6H12O6 + 3SO42- + 3H+ = 6HCO3
- + 3HS- 453 kJ
C6H12O6 + 6O2 → 6CO2 + 6H2O 2880 kJ
Anaerobic respiration also is less efficient andproduces less energy than aerobic respiration
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Carboniferous Period
About 350 million years ago
First land plants: 480 mya.
Primitive bark-bearing trees (lignin)
Anaerobic respiration is less efficient, slower, andproduces less energy than aerobic respiration
anaerobic
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End of lecture 22
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Solubility
The ease with which substances dissolve in water
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NaCl Na+ + Cl-Na+
Sodium Chloride is extremely soluble in water
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The solubility of other ionic salts varies
KCl solubleCaCO3 somewhat solubleHgCl2 solublePbCO3 poorly solubleFePO4 poorly soluble
The degree to which contaminants can existin water is often determined by their solubility
Solubility also can be influenced strongly by factors such as pH and oxygen content
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Many toxic organic pollutants includingpesticides, and industrial productsare extremely insoluble in water.
DDTDioxinsPCBs
Ironically their insolubility in water is partly responsibleFor their persistence in the environment.
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Oxygen is also water SolubleIn natural systems, oxygen diffusing from the atmosphere
and from plant photosynthesis dissolves in water
Diffusion of O2 from the atmosphere is generally slow
Oxygen
Slow diffusion
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Temperature and Oxygen
The solubility of oxygen in water is highly temperature dependent.
Saturated Oxygen Content
10.1 mg/L 8.3 mg/L
15oC 25oC
Affects species diversity
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Cold water species: 5-6 mg/L TroutCool water species: 4 mg/L PikeWarm water species: 2-3 mg/L Bass, Catfish, Bluegill
Fish Species
Minimum Oxygen Tolerances
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Warm WaterHigh biotic activityHigh demand on oxygenDecreased oxygen content
Slow diffusion of oxygen
Oxygen contents can affect the form, solubility, or toxicity of important contaminants
Heat also increases Biological activity
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Oxygen
Oxygen is water soluble, but its solubility is temperature-dependent.In the atmosphere, about one out of 5 molecules is oxygen; in water, about one out of every 100,000 molecules is oxygen.
Oxygen enters the water body from the atmosphere (slowly)and from photosynthesis near the surface
Oxygen leaves the water column principally by organism respiration.
Higher temperatures increase biotic activity, decreasing oxygen
Higher temperatures decrease the ability of water to hold or contain O2.
Oxygen status affects microbial populations and other species diversityas well as the availability or toxicity of important water contaminants.
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pH
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pH (hydrogen)
H+ ion
Ions are stable forms of elements that result from gaining or losing electrons in chemical reactions
Cations have lost electrons and are positively charged
Anions have gained electrons and are negatively charged
H+, Na+, K+, Ca2+, NH4+, Mg+2
Cl-, F-, NO3-, CO3
2-, SO42-
Elements have equal numbers of protons (+) and electrons (-)
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pH is based on the abundance of hydrogen ions in water
When elemental hydrogen loses its electronit becomes a positively charged ion.
Nucleus1 Proton (+)
1 Electron (-)
Hydrogen ions participate in enormousnumbers of environmental reactions
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Common Acids
Hydrochloric Acid HClSulfuric Acid H2SO4
Nitric Acid HNO3
Carbonic Acid H2CO3
Acetic Acid HC2H3O2
Ammonium NH4+
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HCl H+ + Cl-
HNO3 H+ + NO3-
H2SO4 H+ + HSO4-
Dissociation of acids
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pH
A measure of the amount of Hydrogen ions in water
- Log (H+)
Low pH = High amount of Hydrogen ions in waterHigh pH = Low amount of Hydrogen ions in water
Low pH: acidic
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pH (hydrogen)
Low pH = High H+
H+
pH 2 = 0.01 g H+/ LpH 4 = 0.0001 g H+/ L
Acid: any substance whichincreases the hydrogen ionconcentration in water.
- Log (H+)
Natural rainfall has a pH of 5.6
There is 100 times more H+ in water at pH 2 compared to pH 4
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CaHPO4 + H+ = Ca2+ + H2PO4-
Availability and Form of Nutrients
NH4+ NH3
Low pH High pHHigh H+ conc. low H+ conc.
Solid(unavailable)
Dissolved (available)
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Solid(unavailable)
dissolved(available)
Availability and Form of Metals
Dissolution of metals increases their mobility
PbCO3 + H+ Pb2+ + HCO3-
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There are approximately 420,000 abandoned mines in the states of California, Arizona and Nevada
Mine Tailings
FeS2 2H2SO4
oxygen
water
Direct toxicity plus dissolution of associated metal contaminants such as arsenic, lead, and cadmium
Cd, Pb, Zn,Cr, Cu, Al
PbCO3 + H+ Pb2+ + HCO3-
solid soluble
2H+ + SO42-
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pH and Acid Rainfall
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Natural rainfall is acidic: pH 5.6
CO2 + H2O = H2CO3
H2CO3 => H+ + HCO3-
Acid
Pollution by sulfur dioxide and nitrogen oxidescontributes additional acidity to rainfall.
SO2 + H2O → H2SO4
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The Canadian government has estimated that 14,000 lakes in eastern Canada are acidic.
National Surface Water Survey (EPA)
Investigated the effects of acidic deposition in over 1,000 lakes
Acid rain caused acidity in 75 percent of the acidiclakes and about 50 percent of the acidic streams
Adirondacks and Catskill Mountains mid-Appalachian highlands
Little Echo Pond has a pH of 4.2.
Most lakes and streams have a pH between 6 and 8.In the Northeast U.S. many lakes have pH less than 5.
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Acid tolerances
Increasing acidityfood
As acid rain flows through soils in a watershed, aluminum is released
Low pH can be directly toxic to fish and other species
Low pH and increased aluminum levels cause chronic stress thatmay not kill individual fish, but leads to lower body weight and
smaller size and makes fish less able to compete for food and habitat.
At pH 5, most fish eggs cannot hatch