11Chapter 15 - Applications of Aqueous EquilibriaNeutralization Reactions•Strong acid-strong baseHCl(aq)+ NaOH(aq)´NaCl(aq) + H2O (l)What’s in solution? i.e. look at the net ionic equation•Weak acid-strong baseHA (aq) + NaOH(aq) ´NaA(aq) + H2O (l)What’s in solution? i.e. net ionic equationWhat will the pH be, roughly?Example: Acetic acid and sodium hydroxideNeutralization Reactions•Strong acid-weak baseHCl(aq)+ NH3 (aq) ´NH4+(aq) + Cl-(aq)What’s in solution?What will the pH be roughly?What will the pH be, roughly?•Weak acid-weak baseCH3COOH (aq)+ NH3 (aq) QNH4+(aq)+ CH3COO-(aq) Larger K values than other combinationsReaction does not proceed as far toward completion as previous 3 reactions.Neutralization Reactions•Predict whether the pH after neutralization will be greater than, less than, or equal to 7 for the following combinations:•HNO2and KOH•HCl and LiOH•HBr and NH3The Common Ion Effect•Metal ions or salts containing a conjugate weak acid or base can shift the pH of a solution.•This is the mechanism that controls the pHThis is the mechanism that controls the pH of your blood and other biological systems. The Common Ion Effect•If we add a conjugate acid (base) to a solution of a weak base (acid), the pH will shift. This is called the Common Ion Effect. •NaCH3CO2added to a solution of CH3CO2H will make the solution more basic. Why?•A common ion will shift a chemical equilibrium in such a direction as to get rid of some of the added ion. (think Le Chatelier’s principle)
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