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ACIDS AND BASES

ACIDS AND BASES. Chapter 7 Reactions that form water: Acids and Bases . Objective 4 : To learn the key characteristics of the reactions between strong acids and bases. Properties of Acids. Acids are proton (hydrogen ion, H + ) donors Acids have a pH lower than 7 Acids taste sour

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ACIDS AND BASES

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  1. ACIDS AND BASES

  2. Chapter 7Reactions that form water: Acids and Bases • Objective 4: To learn the key characteristics of the reactions between strong acids and bases

  3. Properties of Acids • Acids are proton (hydrogen ion, H+) donors • Acids have a pH lower than 7 • Acids taste sour • Acids effect indicators • Blue litmus turns red • Methyl orange turns red • Acids react with active metals, producing H2 • Acids react with carbonates • Acids neutralize bases

  4. Acids are Proton (H+ ion) Donors Strong acids are assumed to be 100% ionized in solution (good H+ donors). HCl H2SO4 HNO3 Weak acids are usually less than 5% ionized in solution (poor H+ donors). H3PO4 HC2H3O2 Organic acids

  5. Acids Have a pH less than 7

  6. Acids Effect Indicators Bluelitmus paper turnsredin contact with an acid. Methyl orange turnsredwith addition of an acid

  7. Acids React with Active Metals Acids react with active metals to form salts and hydrogen gas. Mg + 2HCl  MgCl2 + H2(g) Zn + 2HCl  ZnCl2 + H2(g) Mg + H2SO4 MgSO4 + H2(g)

  8. AcidsReact withCarbonates 2HC2H3O2+Na2CO3 2 NaC2H3O2 + H2O + CO2

  9. Effects of Acid Rain on Marble(calcium carbonate) George Washington: BEFORE George Washington: AFTER

  10. Acids Neutralize Bases Neutralization reactions ALWAYSproduce a saltandwater. HCl + NaOH  NaCl+H2O H2SO4 + 2NaOH  Na2SO4+2H2O 2HNO3 + Mg(OH)2 Mg(NO3)2+2H2O

  11. Properties of Bases • Bases are proton (hydrogen ion, H+) acceptors • Bases have a pH greater than 7 • Bases taste bitter • Bases effect indicators • Red litmus turns blue • Phenolphthalein turns purple • Solutions of bases feel slippery • Bases neutralize acids

  12. Bases are Proton (H+ ion) Acceptors • Sodium hydroxide (lye), NaOH • Potassium hydroxide, KOH • Magnesium hydroxide, Mg(OH)2 • Calcium hydroxide (lime), Ca(OH)2 OH-(hydroxide) in base combines with H+in acids to form water H+ + OH- H2O

  13. Bases have a pH greater than 7

  14. Bases Effect Indicators Red litmus paper turns blue in contact with a base. Phenolphthalein turns bright pink in a base.

  15. Bases Neutralize Acids Milk of Magnesia contains magnesium hydroxide, Mg(OH)2, which neutralizes stomach acid, HCl. 2 HCl + Mg(OH)2 MgCl2 + 2 H2O

  16. Mixing Strong Acids and Strong Bases Aqueous hydrochloric acid reacts with aqueous sodium hydroxide HCl(aq) + NaOH(aq) H2O(l) + NaCl (aq) Complete ionic equation: H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) H2O(l) + Na+(aq) + Cl-(aq) Net ionic equation: H+(aq) + OH-(aq) H2O(l)

  17. Mixing Strong Acids and Strong Bases Aqueous hydrobromic acid reacts with aqueous sodium hydroxide HBr(aq) + NaOH(aq) H2O(l) + NaBr (aq) Complete ionic equation: H+(aq) + Br-(aq) + Na+(aq) + OH-(aq) H2O(l) + Na+(aq) + Br-(aq) Net ionic equation: H+(aq) + OH-(aq) H2O(l)

  18. Mixing Strong Acids and Strong Bases Aqueous sulfuric acid reacts with aqueous potassium hydroxide H2SO4(aq) + 2KOH(aq) 2H2O(l) + K2SO4(aq) Complete ionic equation: 2H+(aq) + SO42-(aq) + 2K+(aq) + 2OH-(aq) 2H2O(l) + 2K+(aq) + SO42-(aq) Net ionic equation: H+(aq) + OH-(aq) H2O(l)

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