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Acid-Base Reactions: Understanding pH and Neutralization

Explore the fundamentals of acids, bases, pH scale, and neutralization reactions. Learn how pH impacts living organisms and their environments. Discover the significance of buffers in maintaining stable pH levels in blood.

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Acid-Base Reactions: Understanding pH and Neutralization

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  1. Acid - Base Reactions

  2. Acid - substance that releases H+ when add to H2O HCl + H2O H+ + Cl- + H2O Base - substance that releases OH- when added to H2O NaOH + H2O Na+ + OH- + H2O

  3. Acids Bases HCl -hydrochloric acid H2SO4 - sulfuric acid H2CO3 - carbonic HC2H3O2 - acetic HNO3 - nitric NaOH - sodium hydroxide KOH - potassium hydroxide Ca(OH)2 - calcium hydroxide

  4. pH scale 0 1 2 3 4 5 678 9 10 11 12 13 14 neutral measures whether a solution is acidic or basic STRONG weak weakSTRONG BASE ACID

  5. ACIDS - pH less than 7 BASES - pH greater than 7 Neutral - pH = 7 (distilled water)

  6. Other characteristic of acids 1. Sour taste 2. Reacts w/ carbonate (CO3) 3. Litmus paper turns red 4. React w/ most metals

  7. Other characteristic of bases 1. Bitter taste 2. Feels slippery 3. Litmus paper turns blue

  8. pH and living things • Most complex chem. rxn. in organisms- Only occur when pH is between 6.5 to 7.5 Transport of CO2 & O2 by red blood cells

  9. some organisms require habitat at specific pH Cranberries, carnivorous plants (venus-fly trap & pitcher plants) pH - 3.5 to 5.5

  10. Neutralization reaction a salt + H2O ACID + BASE  pH < 7 pH >7 pH=7 General formula:

  11. H+ (from acid) & OH- (from the base) combine to make water Need equal amount of each to get neutralization (pH=7)

  12. Buffers Substance able to resist pH change

  13. Blood, Buffers, & pH • pH of blood 7.35 - 7.45 • blood contains buffers to keep w/in this range If base added H2CO3 + OH- (base) HCO3- + H2O If acid added HCO3 + H+ (acid) H2CO3 + H2O

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