Acids and Bases
This piece explores acid-base neutralization reactions, where an acid and a base combine to form a salt and water. Highlighting examples such as HCl with NaOH resulting in NaCl and H2O, it emphasizes the necessity for equal concentrations of the acid and base in the reaction. Furthermore, it categorizes strong and weak acids and bases, clarifying their dissociation in water. Key concepts include ionization, double displacement reactions, and the importance of pH levels in differentiating between strong and weak acids and bases.
Acids and Bases
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Presentation Transcript
Acids and Bases Part 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
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
1. Ba(OH)2 + H3PO4 2. HC2H3O2 + NaOH 3. H2SO4 + KOH 4. H2CO3 + NaOH 5. Na2CO3 + HCl
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
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]
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?
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
