CHEM 1332 1st Edition Lecture 15 Outline of Last Lecture - Arrhenius acids and bases- Bronstel and Lowry - Conjugate pairs- Relationship with KOutline of Current Lecture - pH and pOH levels - Types of Acids- Types of BasesCurrent Lecture- In every aqueous solution you have +¿H3O¿ −¿O H¿-+¿ eqH3O¿ −¿ eq=kwO H¿-pH+ pOH = pKw=14- At 25 ℃ pH+ pOH =14- In pure water:+¿eqH3O¿ −¿ eq pH = pOH=7O H¿- The acidic solution +¿eq>¿H3O¿ −¿ eq pH < pOH pH <7O H¿because –log- In basic solution +¿eqH3O¿ −¿ eq pH > pOH pH >7 pOH <7¿O H¿- Neutral solution +¿ eqH3O¿ −¿ eq pH = pOH=7¿O H¿- Types of Acids (HnX ¿ X is the selected nonmetals- Strong acids HCl(aq), HBr(aq), HI (aq)- Weak acids HF(aq), H2O(aq), H2S , P H3-−¿ pseudo halides−¿ N3¿HCN , H N3CN¿-+¿−¿+H¿X −H ⇄ X¿ conjugate basesThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- Strength of an acid depends upon willingness of X to accept that electron- Strength depend on X: In the Periodic Table as it goes right across it increases based on electronegativity down the group it increases as well as size increases- Oxyacid (tenory) (HnX Om¿- Strong acids H2S O4, HN O3, HCl O4- Weak acids HN O2, H3PO4, HCl O3, HCl O2, HClO , HBr O3-+¿−¿+ H¿X −O+H ⇌ X−O¿- Nonmetal hydroxides- Even though extra −¿e¿ always goes on an O, the electronegativity of oxygen depends on what else bonds to it-X −O X electronegativity increases across the period in a group it increases in electronegativity up a group- Number of O increases so acid strength increases- Carboxylic acids also known as organic acids- All of these acids are weakHC O2H ,C H3COOH ,C F3COOH ,CC l3COOH , CC l2CHOOH-C H3COOH <CC l2CHOOH <CC l3COOH<C F3COOH- Types of bases are metal hydrides, hydroxides, organic bases –amines, anions (−¿A¿ - conjugate bases of HAKey TermsPseudo halides- are the anions of corresponding pseudohalogen
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