Graduate
  1. Physical Chemistry  1.1. Thermodynamics  1.1.1. Laws of Thermodynamics  1.1.2. Enthalpy and heat capacity  1.1.3. Entropy and free energy  1.1.4. Phase Equilibrium  1.1.5. Statistical thermodynamics  1.1.6. Thermodynamic cycle  1.1.7. Fugacity and activity  1.2. Quantum Chemistry  1.2.1. Principles of quantum mechanics  1.2.2. Schrödinger Equation  1.2.3. Particle in a box  1.2.4. Operators and eigenvalues  1.2.5. Atomic orbitals  1.2.6. Molecular orbital theory  1.2.7. Perturbation theory  1.2.8. Valence bond theory  1.2.9. Hybridization and chemical bonding  1.3. Chemical kinetics  1.3.1. Rate laws and reaction mechanisms  1.3.2. Collision theory  1.3.3. Transition state theory  1.3.4. Enzyme Kinetics  1.3.5. Chain Reactions and Polymerization  1.3.6. Photochemical reactions  1.4. Statistical mechanics  1.4.1. Partitioning functions  1.4.2. Molecular distribution functions  1.4.3. Boltzmann Distribution  1.4.4. Bose–Einstein and Fermi–Dirac statistics  1.5. Spectroscopy  1.5.1. Rotational Spectroscopy  1.5.2. Vibrational Spectroscopy  1.5.3. Electronic Spectroscopy  1.5.4. Nuclear magnetic resonance spectroscopy  1.5.5. Mass Spectrometry  1.5.6. Raman Spectroscopy  1.5.7. Electron paramagnetic resonance spectroscopy  1.6. Surface and colloidal chemistry  1.6.1. Absorption isotherm  1.6.2. Surface tension and wetting  1.6.3. Colloidal Stability  1.6.4. Catalysis  1.6.5. Emulsions and micelles  1.7. Electrochemistry  1.7.1. Nernst equation  1.7.2. Electrochemical cells  1.7.3. Conductivity and mobility  1.7.4. War  1.7.5. Fuel cells  1.7.6. Electrolysis
  2. Organic chemistry  2.1. Reaction mechanism  2.1.1. Nucleophilic substitution reactions  2.1.2. Electrophilic addition reactions  2.1.3. Elimination reactions  2.1.4. Rearrangement reactions  2.1.5. Radical reactions  2.1.6. Pericyclic reactions  2.2. Spectroscopy and structural determination  2.2.1. UV-Vis Spectroscopy  2.2.2. IR Spectroscopy  2.2.3. NMR Spectroscopy  2.2.4. Mass Spectrometry  2.2.5. X-ray crystallography  2.3. Stereoscopic  2.3.1. Chirality and optical activity  2.3.2. Structural analysis  2.3.3. Geometrical isomerism  2.3.4. Dynamic Stereochemistry  2.4. Organometallic Chemistry  2.4.1. Organolithium and organomagnesium reagents  2.4.2. Palladium-catalyzed cross-coupling reactions  2.4.3. Transition Metal Complexes  2.4.4. Metal–carbon bond  2.5. Polymer chemistry  2.5.1. Polymerization mechanism  2.5.2. Polymer Characteristics  2.5.3. Biodegradable Polymer  2.5.4. Conducting polymer  2.5.5. Supramolecular polymers  2.6. Medicinal chemistry  2.6.1. Drug design and development  2.6.2. Pharmacokinetics and pharmacodynamics  2.6.3. Structure-activity relationships  2.6.4. Molecular docking and drug screening
  3. Inorganic chemistry  3.1. Coordination chemistry  3.1.1. Crystal field theory  3.1.2. Ligand field theory  3.1.3. Spectrochemical Series  3.1.4. Chelation and stability  3.2. Organometallic Chemistry  3.2.1. Metal Carbonyls  3.2.2. Catalysis by organometallic complexes  3.2.3. Metallocenes  3.3. Bio-inorganic chemistry  3.3.1. Metalloproteins and enzymes  3.3.2. The role of metals in biological systems  3.3.3. Metal ion transport and storage  3.4. Solid state chemistry  3.4.1. Crystal Structures  3.4.2. Band theory of solids  3.4.3. Superconductors  3.4.4. Defects in the crystal  3.5. Lanthanides and Actinides  3.5.1. Electronic configuration in lanthanides and actinides  3.5.2. Coordination chemistry of the lanthanides  3.5.3. Magnetic Properties of Lanthanides
  4. Analytical chemistry  4.1. Chromatography  4.1.1. Gas Chromatography  4.1.2. High Performance Liquid Chromatography  4.1.3. Thin Layer Chromatography  4.2. Spectroscopic Techniques  4.2.1. Atomic absorption spectroscopy  4.2.2. X-ray diffraction  4.2.3. Inductively coupled plasma spectroscopy  4.3. Electroanalytical methods  4.3.1. Potentiometry  4.3.2. Voltammetry  4.3.3. Colometry  4.4. Mass Spectrometry  4.4.1. Ionization Technique  4.4.2. Fragmentation Pattern  4.5. Chemometrics  4.5.1. Multidisciplinary analysis  4.5.2. Machine Learning in Chemistry
  5. Theoretical and Computational Chemistry  5.1. Molecular dynamics simulation  5.1.1. Force fields and energy minimization  5.1.2. Monte Carlo simulation in molecular dynamics simulations  5.2. Quantum chemical methods  5.2.1. Hartree–Fock theory  5.2.2. Density functional theory  5.2.3. Semi-empirical methods  5.3. Computational drug design  5.3.1. Molecular Docking  5.3.2. QSAR Modeling  5.3.3. Virtual Screening
  6. Biochemistry  6.1. Enzyme Kinetics  6.1.1. Michaelis-Menten kinetics  6.1.2. Inhibition mechanism  6.2. Metabolism and Bioenergetics  6.2.1. Glycolysis  6.2.2. Citric acid cycle  6.2.3. Electron transport chain  6.3. molecular Biology  6.3.1. DNA replication and repair  6.3.2. Protein synthesis  6.3.3. Gene Regulation  6.4. Structural Biochemistry  6.4.1. Protein Folding  6.4.2. Membrane Biophysics
  7. Environmental Chemistry  7.1. Atmospheric Chemistry  7.1.1. Greenhouse gases  7.1.2. Ozone depletion  7.1.3. Air pollutants and smoke  7.2. Water Chemistry  7.2.1. pH and water hardness  7.2.2. Wastewater treatment  7.2.3. Aquatic Chemistry  7.3. Soil Chemistry  7.3.1. Heavy metal contamination  7.3.2. Soil pH and Buffering  7.3.3. Nutrient cycling  7.4. Toxicology and Chemical Safety  7.4.1. Toxicokinetics  7.4.2. Risk Assessment in Toxicology and Chemical Safety in Environmental Chemistry  7.4.3. Effects of pollutants on the environment

Graduate → Environmental Chemistry → Water Chemistry ↓


Aquatic Chemistry


Introduction

Aquatic chemistry refers to the complex interactions of chemicals in the water environment. It involves understanding the chemical processes and reactions that control water quality in natural and engineered systems. Understanding these interactions is important for maintaining ecological balance and designing processes for water treatment.

Composition of natural waters

Natural water contains a complex mixture of dissolved minerals, gases, and organic matter. The primary components include ions such as sodium (Na +), potassium (K +), calcium (Ca 2+), magnesium (Mg 2+), chloride (Cl -), sulfate (SO 4 2-), and bicarbonate (HCO 3 -).

Water molecule structure

Water is a polar molecule with a bent shape. This structure is essential for its solvent properties. Oxygen is more electronegative than hydrogen and therefore attracts the shared electrons more strongly, creating a dipole moment.

        Höh
           ,
            Hey

pH and acidity of water

The pH scale measures the acidity or alkalinity of water. It is defined as:

        pH = -log[H + ]

For example, pure water has a pH of about 7, which is neutral. Acidic water has a pH less than 7, while alkaline water has a pH greater than 7.

Buffers in aquatic systems

In aquatic systems, buffers play an important role in maintaining pH stability. A common buffer system in natural waters is the carbonate system:

        CO 2 + H 2 O ⇌ H 2 CO 3 ⇌ H + + HCO 3 - ⇌ CO 3 2- + 2H +

This balance helps keep the pH of water within a limited range, even when acids or bases are added to it.

Redox reactions in water

Redox reactions involve the transfer of electrons between species. In aqueous systems, these reactions can affect the solubility of various compounds.

The redox state of water is often identified by its oxidation-reduction potential (ORP). For example, the transformation of iron in water can be represented as:

        Fe2 + ⇌ Fe3 + + e -

Solubility and phase interactions

The solubility of various compounds in water affects their distribution and bioavailability. Solubility is controlled by factors such as temperature, pressure, and the presence of other solutes.

Here's an example of a solubility reaction:

        CaCO 3 (s) ⇌ Ca 2+ (aq) + CO 3 2- (aq)

Complexity in water

Complexation involves the formation of molecules through the coordination of transition metal ions with ligands. This process can significantly affect the solubility and mobility of metal ions in an aqueous environment.

For example, the combination of copper with ammonia can be written as:

        Cu 2+ + 4NH 3 ⇌ [Cu(NH 3 ) 4 ] 2+

Organic chemistry in aqueous systems

Organic matter present in water includes decaying plants and anthropogenic compounds. These can be involved in various reactions, such as erosion and precipitation, that affect the chemistry of the water.

The decomposition of organic matter can be represented as follows:

        C x H y O z + O 2 → CO 2 + H 2 O

Environmental implications

Understanding aquatic chemistry is fundamental to tackling environmental issues such as pollution and eutrophication, which can cause degradation of aquatic ecosystems.

For example, excess nutrients in water bodies can cause algae blooms, which affect oxygen levels:

        NO 3 - + N (this occurs in excessive algae growth)

Conclusion

Aquatic chemistry is an essential field of study for understanding and managing water systems. By exploring concepts such as pH balance, redox reactions, and complexity, scientists and engineers can better predict and mitigate the impacts of human activities on the water environment.


Graduate → 7.2.3


U
username
0%
completed in Graduate

← Prev (7.2.2)
Wastewater treatment
Next (7.3) →
Soil Chemistry

Comments 



Aquatic Chemistry

https://www.chemistryelite.com/g/7.2.3?ceal=en