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Acid and Base Reactions

Acid and Base Reactions. Types of Acid-Base Reactions. Nuetralization reaction – properties of both acid and base are neutralized when they react Acid + Base  Salt + Water Salt – ionic compound (metal + nonmetal). Strong Acid + Strong Base. Strong acids completely ionize

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Acid and Base Reactions

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  1. Acid and Base Reactions

  2. Types of Acid-Base Reactions • Nuetralization reaction – properties of both acid and base are neutralized when they react • Acid + Base  Salt + Water • Salt – ionic compound (metal + nonmetal)

  3. Strong Acid + Strong Base • Strong acids completely ionize • Strong bases completely ionize

  4. Ionic equation – everything (aq) written as ions • Spectator ions • Net ionic equation • NaOH (aq) + HCl (aq)  NaCl(aq) + H2O(l)

  5. H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + H2O(l)

  6. Strong acid + strong base & pH • Hydrogen ion from acid and hydroxide ion from base form water which has a pH of 7

  7. Strong Acid + Weak Base • Weak bases do not completely ionize • 3HBr(aq) + Al(OH)3(s)  AlBr3(aq) + H2O(l)

  8. Bronsted-Lowry Acids & Bases • Acid – H+ donor • Base – H+ acceptor • HC2H3O2 + NH3 NH4+ + C2H3O2-

  9. Conjugate base – formed when acid donates proton • Conjugate acid – formed when base accepts a proton • HC2H3O2 + NH3 NH4+ + C2H3O2-

  10. Identify the acid, base, conjugate acid, and conjugate base in the following: • HCO3-1 + H2O  CO3-2 + H3O +1

  11. Strong Acid + Ammonia • HCl(aq) + NH3(aq)  NH4Cl(aq)

  12. Weak Acid & Strong Base • HC2H3O2(aq) + NaOH NaC2H3O2 + H2O

  13. Applications of Acid-Base Reactions • Buffers regulate pH • Solution that resist changes in pH when moderate amounts of acids or bases are added • Prepared by using a weak acid and its conjugate base or weak base and its salt

  14. Acid-Base Chemistry & Antacids • pH of stomach acid = 2.5 • Stomach is coated with basic mucous to protect it • If stomach becomes too acidic mucous layer breaks down by acid-base neutralization • Antacids are bases

  15. Acid-Base Titrations • Titration – process of determining molarity of an acid or a base through the use of an acid-base reaction • Molarity of one of the reactants is known but the other is unknown • Standard solution – solution whose molarity is known

  16. Standard solution is loaded into a buret • Allows an accurate measurement of the delivery of a given volume of liquid

  17. Using indicators – when solution is neutral you know you have added exactly enough stock solution to react with the unknown solution • endpoint

  18. A 15.0 mL sample of a solution of H2SO4 with unknown molarity is titrated with 32.4 mL of 0.145 M NaOH to the endpoint. What is the molarity of the sulfuric acid solution?

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