Course Content
Introduction to Environmental Chemistry
Environmental chemistry is the study of the chemical and biochemical phenomena that occur in nature. It involves the understanding of how the uncontaminated environment works, and which naturally occurring chemicals are present, in what concentrations and with what effects. Environmental chemistry; is the study of sources, reactions, transport, effects and fate of chemical species in water, soil and air environment as well as their effects on human health and natural environment
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Introduction
Origin of the solar System
Cosmology; is the branch of astronomy involving the study of the of the universe and the solar system. Cosmo-chemistry ;( chemical cosmology); is the study of chemical composition of the matter in the universe and the process that led to those compositions The solar system is made up of the sun (a star) with nine planets orbiting around it. These planets together with all the other heavenly bodies moving around or between individual planet form members of the solar system. Other heavenly body include; asteroids, comets, meteors, meteorites and satellites such as moon. The solar system does not include other stars .
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Origin of The Universe and Solar System
Solutions
Solutions are defined as homogeneous mixtures that are mixed so thoroughly that neither component can be observed independently of the other. The major component of the solution is called solvent, and the minor component(s) are called solute.
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Introduction
Solubility of Solutions
Solubility Product
Solution Concentrations
Chemical Equilibria
Chemical equilibrium in the environment refers to the state where the rates of forward and reverse reactions of a chemical reaction reach a balance. In this state, the concentrations of reactants and products remain constant over time, although the reactions continue to occur.
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Introduction
The Concept of Equilibrium
Relation Between Chemical Kinetics and Chemical Equilibrium
Factors Affecting Chemical Equilibrium
Laws of Chemical Equilibria
Phase Interactions
Phase interactions in solutions refer to the behavior and changes that occur when two or more substances (solutes and solvents) mix together to form a homogeneous mixture. These interactions are related to the different phases of matter, such as solids, liquids, and gases, and how they interact and transform during the process of solution formation.
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Introduction
 Phase interactions
Colligative Properties of Solutions
COLLIGATIVE PROPERTIES OF SOLUTIONS Colligative properties are physical properties of solutions that depend on the concentration of solute particles, rather than the specific identity of the solute. The four colligative properties that can be exhibited by a solution are: 1.Boiling point elevation 2.Freezing point depression 3.Relative lowering of vapour pressure 4.Osmotic pressure
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Introduction
Colligative Properties Examples
Introduction To Organic Chemistry
Organic chemistry is the study of carbon containing compounds and their properties. This includes the great majority of chemical compounds on the planet, but some substances such as carbonates and oxides of carbon are considered to be inorganic substances even though they contain carbon.
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Introduction
The IUPAC Naming (nomenclature) 
Alkyl halides, Alkenes and Alkynes
Alcohols , Ethers, Aldehydes and Ketones
Carboxylic Acids, Esters and Amines
Simple Organic Molecules in the Environment
Soil Chemistry and Pollution
soil
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Introduction to Soil Chemistry
Chemical Characteristics of Soil
Biological Characteristics of Soil
Physical Characteristics of Soil
Soil Salinity, Conductivity and Ion Exchange Capacity
Soil Pollution
Water Chemistry and Polution
Water Chemistry
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Water and the Environment
Water Chemistry
Characteristics and Properties of Water
Portable water 
Water pollution
Water Quality Analysis
Biological Oxygen Demand (BOD)
Chemical Oxygen Demand (COD)
Air Quality and Pollution
Air Quality and Pollution
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Air Quality
Testing Air Quality
Biodegradation
Biodegradation
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Biodegradation
Mechanisms of Biodegradation 
Role of Microorganisms in Biodegradation
BioGeoChemical Cycles
BiogeoChemical Cycles
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Biogeochemical cycles
The Water Cycle
The Carbon Cycle
The Nitrogen Cycle
The Phosphorus Cycle
The Sulfur Cycle
Introduction To Environmental Chemistry
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Properties and Characteristics of Water

The chemical characteristics of water refer to the properties and composition of water at a molecular level. Water molecules consist of two hydrogen atoms bonded to one oxygen atom (H2O), giving water its unique chemical properties. Understanding the chemical characteristics of water is important for various applications, including environmental studies, water treatment, industrial processes, and biological systems.

Here are some key chemical characteristics of water:

  1. High Specific Heat Capacity: Water has a high specific heat capacity, meaning it can absorb and store a significant amount of heat energy without a substantial increase in temperature. This property helps regulate Earth’s climate, as water can absorb heat during the day and release it slowly at night, moderating temperature changes in both aquatic and terrestrial environments. It also contributes to the cooling effect of water on organisms and enables water bodies to act as heat sinks.

  2. High Heat of Vaporization: Water has a high heat of vaporization, which means it requires a considerable amount of heat energy to change from a liquid to a vapor state. This property is responsible for the cooling effect of evaporation, where water absorbs heat from the surroundings to evaporate, providing a cooling effect on the surface it evaporates from. This cooling effect is important for temperature regulation in organisms and for processes like sweating in humans.

  3. Universal Solvent: Water is often referred to as the “universal solvent” due to its ability to dissolve a wide range of substances. Its polar nature allows it to interact with and dissolve many ionic and polar compounds. This property is crucial for processes like digestion, transportation of nutrients in living organisms, and chemical reactions in various industries.

  4. Density Anomaly: Water exhibits an anomaly in its density behavior. As water cools from 4 degrees Celsius (39.2 degrees Fahrenheit) to its freezing point, it becomes less dense. This causes ice to float on water instead of sinking. The density anomaly of water is important for the survival of aquatic life during colder seasons, as ice formation on the surface insulates the water below, preventing it from freezing completely and allowing organisms to survive in liquid water.

  5. Cohesion and Adhesion: Water molecules have strong cohesive forces, meaning they tend to stick to each other. This property results in high surface tension, allowing certain organisms to walk or float on water. Water also exhibits adhesion, enabling it to adhere to other polar surfaces. Capillary action, which is the movement of water against gravity through narrow spaces, is a result of water’s cohesion and adhesion properties.

  6. Polar Molecule: Water is a polar molecule, meaning it has a positive charge at one end (hydrogen side) and a negative charge at the other end (oxygen side). This polarity gives water its ability to dissolve many substances and form hydrogen bonds with other water molecules.

  7. Density and Freezing Point: The density of water is highest at around 4 degrees Celsius (39.2 degrees Fahrenheit). As water cools below this temperature, it expands and becomes less dense, leading to the formation of ice. This unique behavior helps to insulate bodies of water, preventing them from freezing solid and allowing aquatic life to survive beneath the ice.

  8. pH Neutrality: Pure water has a pH of 7, which is considered neutral. It is neither acidic (pH below 7) nor alkaline (pH above 7). However, the pH of water can be influenced by dissolved gases, minerals, and other substances present in the water.

  9. Dissociation and Ionization: Water molecules have the ability to dissociate into hydrogen ions (H+) and hydroxide ions (OH-) through a process called self-ionization. This process is responsible for the presence of equal concentrations of H+ and OH- ions in pure water, resulting in a neutral pH.

  10. Buffering Capacity: Water exhibits a buffering capacity, meaning it can resist changes in pH when small amounts of acids or bases are added. This buffering capacity helps to maintain the pH stability of water bodies and biological systems.

  11. Chemical Reactions: Water participates in various chemical reactions, including hydrolysis, condensation, and acid-base reactions. These reactions are vital for biochemical processes, such as digestion, metabolism, and cellular functions.

    It is important to note that the chemical characteristics of water can be influenced by the presence of impurities, contaminants, or dissolved substances. Water quality assessments often involve analyzing parameters such as pH, dissolved oxygen, conductivity, turbidity, and the presence of specific ions or pollutants.

    Understanding the chemical characteristics of water is essential for managing water resources, assessing water quality, designing water treatment processes, and supporting various industrial, agricultural, and biological applications.

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