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Acids and Bases

Acids and Bases. Part 2. ACID-BASE NEUTRALISATION. Neutralisation Reaction: Acid + Base  Salt + Water Ex: HCl + NaOH  NaCl + H 2 O The acid and base neutralise each other creating a salt and water Must be equal concentrations of acid and base.

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Acids and Bases

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  1. Acids and Bases Part 2

  2. ACID-BASENEUTRALISATION NeutralisationReaction: Acid + Base  Salt + Water Ex: HCl + NaOH  NaCl + H2O • The acid and base neutralise each other creating a salt and water • Must be equal concentrations of acid and base

  3. Actually a Double Displacement Reaction! acid + base salt + water KNO3 + H2O HNO3 + KOH HF + NaOH NaF + H2O 2 HCl + Ca(OH)2 CaCl2 + H2O 2

  4. 1. Ba(OH)2 + H3PO4 2. HC2H3O2 + NaOH 3. H2SO4 + KOH 4. H2CO3 + NaOH 5. Na2CO3 + HCl 

  5. Strong Acids: 100% ionized (completely dissociated) in water. HCl + H2O  H3O+ + Cl- Strong Acids: Perchloric HClO4 Chloric, HClO3 Hydrobromic, HBr Hydrochloric, HCl Hydroiodic, HI Nitric, HNO3 Sulfuric, H2SO4

  6. What is a strong Base? A base that is completely dissociated in water (highly soluble). NaOH(s)  Na+ + OH- Strong Bases: Group 1A metal hydroxides (LiOH, NaOH, KOH, RbOH, CsOH) Heavy Group 2A metal hydroxides [Ca(OH)2, Sr(OH)2, and Ba(OH)2]

  7. Strong Acids: 100% ionized (completely dissociated) in water. HCl + H2O  H3O+ + Cl- Note the “one way arrow”. Weak Acids: Only a small % ionized in water. HC2H3O2 + H2O H3O+ + C2H3O2- Note the “2-way” arrow. Why are they different?

  8. Key Concepts: Acids and Bases Acid Base Ionization in water undergo produce produce Neutralization gives H + ions OH- ions to form OH- H+ 100% Small % Salt & 100% Small % product Water [H+] x [OH-] Strong acid Weak acid Strong base Weak base is pH

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