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Understanding Acids, Bases, and pH Scales in Chemistry

Learn about acids, bases, and the pH scale, their properties, and importance. Explore examples, buffering systems, and the impact of pH on chemical reactions. Discover how slight pH changes can affect our body functions.

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Understanding Acids, Bases, and pH Scales in Chemistry

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  1. Acids and Bases

  2. Acid • A molecule that has more hydrogen (hydronium) ions than hydroxide ions • Usually donates H+ to solution • Less than 7.0 on pH scale • Ex)

  3. Base • Molecule that has more hydroxide (OH-) ions than hydrogen ions • Tends to remove H+ from solution creating water • Higher than 7.0 on pH scale • Ex)

  4. Pure Water • Neither acidic or alkaline • Same amount of H+ and OH- • 7.0 or neutral on pH scale

  5. pH scale • Scale to measure the concentration of hydrogen ions in solution • Logarithmic

  6. Examples of pH’s • Gastric juice • Urine • Saliva • Milk • Tears • Blood • Pancreatic Juice

  7. Most cellular fluids range from 6-8 on the pH scale • Ave is 7.4 • Slight changes in pH can change chemical reactions!!

  8. The pH of blood is 7.4 if it decreases as little as 6.95 the nervous system is unresponsive • Coma and death soon follow

  9. We don’t hear in the news about people dieing of acid/base toxicity why?

  10. Buffers • Capable of neutralizing small amounts of acids and bases by easily donating hydrogen or hydroxide ions

  11. Carbonic acid/bicarbonate • Human buffer system • Know this for the test!! • Carbon dioxide combines with water to make carbonic acid H2CO3 (neutralizing bases)

  12. Carbonic acid can break down into a hydrogen ion and a bicarbonate ion HCO3- (neutralizing acids)

  13. When no longer needed bicarbonate then reacts with a hydrogen ion to create H2O and CO2

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