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Acids

Acids. Substances that donate hydrogen ions (H + ) to water to form H 3 O + Called the hydronium ion Examples of Acids HCl hydrochloric acid used in pools H 2 SO 4 sulfuric acid- battery acid HC 2 H 3 O 2 acetic acid- vinegar HC 6 H 7 O 7 citric acid- lemons, limes. Properties of acids.

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Acids

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  1. Acids • Substances that donate hydrogen ions (H+) to water to form H3O+ • Called the hydronium ion • Examples of Acids • HCl hydrochloric acid used in pools • H2SO4 sulfuric acid- battery acid • HC2H3O2 acetic acid- vinegar • HC6H7O7 citric acid- lemons, limes

  2. Properties of acids • Taste Sour • Conduct electricity • strong electrolytes - will conduct a lot • weak electrolytes- will conduct only a little • React with metals to form hydrogen gas • Change indicators (BAR) • Blue litmus in Acid turns Red • React with hydroxides to form water and a salt

  3. Acids • ones in food are dilute • Concentrated acids - dangerous • They can burn skin and eyes • Strong acids ionize completely • All the H’s make hydronium • HCl + H2O  Cl- + H3O+ • Makes lots of ions • Are dangerous

  4. Acids • Weak acids only partially ionize • Only a few H’s attach to water • HC2H3O2+ H2O C2H3O2- + H3O+ • Can be dangerous if concentrated

  5. Bases • Increases the amount of OH- in solution • Either has OH- in it or takes an H off of water • Examples of bases • KOH - in drain cleaner • NaOH - in drain cleaner • NH3- ammonia

  6. Properties of bases • Taste bitter. • Feel slippery • Can be strong or weak electrolytes. • Change indicators (RBB). • Red litmus paper in Base turns Blue • React with acids to form water and a salt

  7. Bases • KOH  K+ + OH- • Strong bases ionize completely • Make lots of ions • Are dangerous • NH3 + H2O NH4+ + OH- • Weak bases only make a few ions • Are dangerous if concentrated

  8. 0 7 14 Acidic Neutral Basic How Acidic? • More H3O+ is more acidic • Measured with pH • Lower pH is more acidic • As H3O+ goes down, OH- goes up • Higher pH more basic • pH of 7 is neutral

  9. pH • French origin “Pouivier Hydrogene” – means “power of hydrogen” • Measures hydronium ion concentration • Every 1 unit less of pH is 10 times more hydronium • A pH of 2 is 100 times more H3O+ ions than a pH of 4 • pH is number of places after the decimal point • pH of 2 is 0.01 Molar H3O+ • pH of 4 is 0.0001 Molar H3O+ • pH of 9 is 0.000000001 Molar H3O+

  10. pH • Low pH is acid (pH 1,2,3,4,5,6) • Lots of H3O+ • Little OH- • High pH is base (pH 8,9,10,11,12,13,14) • Little H3O+ • Lots of OH-

  11. Neutralization Reactions • Acids and bases react and neutralize each other • Strong acids make lots of ions • HCl + H2O  H3O+ + Cl- • Strong bases make lots of ions • NaOH  Na+ + OH- • and • H3O+ + OH-  2H2O

  12. Neutralization Reactions • Put acids and bases together • H3O+ + Cl- + Na+ + OH- Cl- +Na+ +2H2O • The Na+ and Cl- make salt which is neutral • Water is neutral • Will be neutral if the right amounts of strong acids and bases are added

  13. Neutralization Reactions • Weak bases will neutralize a strong acid, but not as well. • You need to add more of them • If you add enough, it will make the solution basic • Same works for weak acids and strong bases • As you add acid to a base the pH drops • As you add base to and acid the pH rises

  14. Household Uses • Antacids- Weak bases that neutralize excess stomach acid • Shampoo- made from detergents • Need to keep pH between 5 and 8 or it will make the hair dull • Citric acid keeps fruit from browning • Acidic marinades tenderize meats • Drain cleaners are strong bases

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