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2. Examples of Acids

2. Examples of Acids. nitric (HNO 3 ) HNO 3  H + + NO 3 – makes fertilizers hydrochloric ( HCl ) HCl  H + + Cl - stomach acid sulfuric (H 2 SO 4 ) H 2 SO 4  2H + + SO 4 - car batteries. acetic (CH 3 COOH )

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2. Examples of Acids

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  1. 2. Examples of Acids • nitric (HNO3 ) HNO3 H+ + NO3 – makes fertilizers • hydrochloric (HCl) HCl H+ + Cl- stomach acid • sulfuric (H2SO4 ) H2SO4 2H+ + SO4- car batteries

  2. acetic (CH3COOH ) CH3COOH  H+ + CH3COO- food preservation • Carbonic (H2CO3) H2CO3 H+ + HCO3- carbonated drinks

  3. extent to which the acid dissociates determines its strength Polar water allows for acids to dissolve Strong Acid - Dissociates completely in a solvent Weak Acid - Releases few hydrogen ions in the solution. ** Lower the pH the stronger the acid** 3. Strength of Acids

  4. strong acids almost completely dissociate 10 H2SO4 18 H+ + 9 SO4-2 + 1 H2SO4 10 HCl 9 H+ + 9 Cl- + 1 HCl weak acids only partially dissociate 10 H2CO3 2 H+ + 2 HCO3-2 + 8 H2CO3 18 CH3COOH 3 H+ + 3 CH3COO- + 7 CH3COOH

  5. Often confused Strength (strong or weak) tells how acid dissociates Concentration (dilute or concentrated) tells amount of acid dissolved in the solution. It is possible to have a dilute solution of a strong acid! 4. Strength vs. concentration

  6. Streams become more acidic and removes minerals from the rocks. Water contains more Pb, As, and Hg Kills aquatic life 5. Acid Mine Drainage (AMD)

  7. 4 FeS2 + 15 O2 + 14 H2O  4 Fe(OH)3 + 8 H2SO4 “yellow boy” (iron hydroxide) yellow-orange solid Pyrite (mineral) sulfuric acid fool’s gold

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