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CHM152Chapter 15 - 6

Chemistry (MasteringChemistry Series)

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1 1 Chapter 15 - Applications of Aqueous Equilibria Neutralization Reactions Strong acid-strong base HCl (aq) + NaOH (aq) ´ NaCl (aq) + H 2 O (l) What’s in solution? i.e. look at the net ionic equation Weak acid-strong base HA (aq) + NaOH (aq) ´ NaA (aq) + H 2 O (l) What’s in solution? i.e. net ionic equation What will the pH be, roughly? Example: Acetic acid and sodium hydroxide Neutralization Reactions Strong acid-weak base HCl (aq) + NH 3 (aq) ´ NH 4 + (aq) + Cl - (aq) What’s in solution? What will the pH be roughly? What will the pH be, roughly? Weak acid-weak base CH 3 COOH (aq) + NH 3 (aq) Q NH 4 + (aq) + CH 3 COO - (aq) Larger K values than other combinations Reaction 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: HNO 2 and KOH HCl and LiOH HBr and NH 3 The 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 pH This 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 . NaCH 3 CO 2 added to a solution of CH 3 CO 2 H 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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