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Understanding Acid-Base Neutralization and Titration Principles

This overview explains the process of acid-base neutralization, where acids and bases react to form water and salts, neutralizing potentially dangerous solutions. It discusses the equivalence point in titration, where complete neutralization occurs. Examples of reactions are provided, including those that produce gases and calculations to determine concentrations of unknown acids or bases. The properties of strong and weak acids/bases are contrasted, highlighting the importance of concentration in determining safety. Additionally, concepts of amphoteric substances and proton donation in acids are addressed.

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Understanding Acid-Base Neutralization and Titration Principles

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  1. Neutralization of an acid or base.

  2. Mixing acids and bases • ~creates water • H3O+ + OH- 2 H2O • this is called neutralizing the solution • a neutralized solution is no longer dangerous. • The point where neutralization is complete is called the equivalence point

  3. Salts • ~the byproduct of an acid and a base. • NaOH + HCl  H2O + NaCl • (base) (acid) (water) (salt) • there are several more than just table salt. • HNO3 + NH4OH  H2O + NH4NO3 • Acid Base water salt

  4. Gases can be created • this depends on the reactants (not all will) • sodium bicarbonate (baking soda) will pretty much always release a gas • NaHCO3 + H2SO4H2O + NaHSO4 +CO2 Salt Gas

  5. Titration • ~mixing an acid and base perfectly to make a neutral solution. • You normally need some kind of indicator for this. • Phenolphthalein- when in solution turns red if basic and is clear if acidic. • You can also use a pH probe

  6. Graph of titration equivalence point pH Volume strong base added

  7. Using math • To neutralize a solution you will need to add an equal amount of H3O+ / OH- to what was already present. • so that • mol H3O+ = mol OH- • This is used if and only if you are at the equivalence point (completely neutral solution)!

  8. Problem • If 94 mL of 4.0 M NaOH neutralizes 6.0 L of an unknown strong acid, what was the H3O+concentration of the unknown? • 4 M NaOH x .094 L = .376 mol NaOH • .376 mol H3O+/ 6.0 L = .063 M H3O+

  9. Another problem • If 127 mL of 2.0 M NaOH neutralizes 4.1 L of an unknown acid, what is the initial concentration of the acid? • 2.0M(.127 L) = .254 mol NaOH • =.254 mol OH- = .254 mol H3O+ • 4.1 L • =.062 M

  10. Strong acids and bases • The strong acids and bases completely dissociate in water. • Most acids or bases will only react to a certain extent • Strong acids/bases make the most amount of hydronium or hydroxide that they possibly can.

  11. Strong acids

  12. Strong Bases these make a lightning bolt on the periodic table!

  13. Danger!!! • Strong and Weak acids and bases do NOT necessarily tell you how dangerous they are. • Concentration is the most important factor for determining danger. • Ammonia is a weak base, if it is highly concentrated it can burn you. • Dilute hydrochloric acid (less than 1 M) is not particularly dangerous

  14. What is water • Water is either an acid or base depending on the situation. • Anything that is either an acid or a base is called amphoteric. • Several things are amphoteric, like parts of you.

  15. Donating Protons • Hydrochloric acid (HCl) can donate 1 proton, so it is called a monoprotic acid. • Sulfuric acid (H2SO4) can donate 2 protons, so it is called a diprotic acid. • Phosphoric acid (H3PO4) can donate 3 protons, so it is called a triprotic acid.

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