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Understanding Acids, Bases, and pH: Properties and Interactions

This overview explores the characteristics and roles of acids, bases, and the pH scale. Acids, known for their sour taste and conductivity, are found between 0 and 7 on the pH scale, releasing H+ ions in solution. Conversely, bases taste bitter and feel slippery, ranging from 7 to 14 pH, and release OH- ions. This guide also covers the neutralization process where acids and bases react to form water and salts, highlighting the significance of pH in maintaining homeostasis through buffers.

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Understanding Acids, Bases, and pH: Properties and Interactions

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  1. 2-2 Acids, Bases and pHI. Acids • Latin acere = sour • Properties: • Taste sour • Reacts with some metals to release hydrogen gas • Become less acidic when mixed with bases • Are located between 0 and 7 on the pH scale (Stronger acids = lower numbers) • Conduct electricity

  2. C. All acids contain Hydrogen, and when they are dissolved in H2O will release H+ ions in solution. Example: HCl + H2O H+ (aq) + Cl- (aq) (aq) = aqueous or “in water”

  3. II. Bases • Used to be called Alkalies • Properties: • Taste bitter (think aspirin) • Feel slimey or slippery • Are located between 7 and 14 on the pH scale (strong bases = high numbers) • Can be very dangerous because they are extremely reactive • Conduct electricity

  4. All bases contain OH (hydroxide) and will release OH- ions when dissolved in water Example: NaOH + H2O  Na+ (aq) + OH- (aq) (aq) = aqueous or “in water”

  5. III. pH • Measures the number of H+ ions in a solution. • Many H+ ions means the pH is very low or acidic (stomach acid, vinegar) • Few H+ ions means pH is very high or basic (bleach, soap) • Same number of each ion = neutral 7 (water, blood)

  6. That’s basically it….(get it?)

  7. Acids + bases will neutralize each other H+(aq) + OH-(aq) H20 • An acid + a base will always produce water and a salt Acid Base Water Salt HCl +  NaOH  H2O + NaCl (hydrochloric acid + sodium hydroxide = water and salt)

  8. F. Buffers – keep pH from sharply increasing or decreasing = homeostasis

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