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Understanding the Unique Properties of Water: Polarity, Bonding, and pH

Water is a remarkable compound that exists naturally as a liquid and is essential for life. Its polarity arises from the unequal sharing of electrons between oxygen and hydrogen, creating slight charges that enable hydrogen bonding. This bonding leads to significant properties such as cohesion, adhesion, and high heat capacity. As the universal solvent, water can dissolve various substances, forming solutions and suspensions critical in biological processes. Additionally, water's pH scale, ranging from 0 to 14, reveals its acid-base properties, vital for maintaining the body's homeostasis.

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Understanding the Unique Properties of Water: Polarity, Bonding, and pH

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  1. 2-2 Properties of Water Federoff

  2. The Water Molecule • Water is one of the only few compounds that naturally occur as a liquid • Polarity • Oxygen’s 8 protons vs. Hydrogen’s 1 proton = Oxygen with a greater pull on electrons • So, the Oxygen end is slightly negative and Hydrogen slightly positive • “Polar” molecules behave like poles of magnets

  3. The Water Molecule • Hydrogen Bonding - The attraction between a hydrogen atom on one molecule and the oxygen atom of another • Because water is a polar molecule, it is able to form multiple hydrogen bonds, which account for many of water’s special properties.

  4. The Water Molecule • Cohesion – an attraction between molecules of the same substance. • Ex: Surface Tension • Adhesion – an attraction between molecules of different substances. • Ex: Water meniscus • Ex: Capillary Action

  5. The Water Molecule • Heat Capacity • It takes a large amount of energy to have water molecules move faster to raise the temperature of water • Ex: Ocean temperature • Ex: Cell Processes

  6. Solutions and Suspensions • Mixture – is a material composed of two or more elements or compounds that are physically mixed together but not chemically combined. • Ex: Saline Solutions

  7. Solutions and Suspensions • Solutions – a mixture in which all materials are evenly distributed throughout the solution. • Solute – The substance dissolved • Solvent – The substance in which the solute dissolves • Water’s polarity gives it the ability to dissolve both ionic compounds and other polar molecules. • Water is the universal solvent with some limitations • Ex: Salt Water

  8. Solutions and Suspensions • Suspensions – mixtures of water and non-dissolved material • Ex: Human Blood

  9. Acid, Base, pH • Water does split apart into ions every 1 in 550 million molecules • Remember though, the number of H+ ions is equal to OH- ions therefore water is neutral

  10. Acid, Base, pH • The pH Scale – a system of measurement that indicates the concentration of H+ ions in a solution. • Ranges from 0-14 • 7 is neutral (equal H+ and OH-) • <7 Acidic (more H+ than OH-) • >7 Basic (more OH- than H+) • Each step represents a factor of 10

  11. Acid, Base, pH • Acid – a compound that forms H+ ions in a solution. • Ex: Hydrochloric acid for stomach digestion • Base – a compound that produces hydroxide (OH-) ions in a solution. • Ex: Lye (NaOH – Sodium Hydroxide) for soap making

  12. Acid, Base, pH • Buffer – a weak acid or base that can react with strong acids or bases to prevent sharp, sudden changes in pH. • The human body needs to maintain a pH of a 6.5 to 7.5 to maintain homeostasis • Buffers dissolved in life’s fluids play and important role in maintain homeostasis in organisms.

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