Review: Predict the products of the following acid base reactions, write net ionic equations for each, and identify whether the resulting pH will be greater.

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Presentation transcript:

Review: Predict the products of the following acid base reactions, write net ionic equations for each, and identify whether the resulting pH will be greater or less than 7 and WHY. NaOH + HClO  HNO3 + KH2PO4 

Acids, Bases and Equilibrium, Oh My!!!

pH and Concentrations Calculations: For pH calculations of acids, bases and salts, it is important to know which situations are equilibrium and which are not! Equilibrium Not Equilibrium 1. Weak acids/bases dissociating in water 1. Strong acids/bases dissociating in water 2. Most acid-base rxn’s

Weak acid or base solutions: Since these only dissociate partially, eqm is established Use ICE tables and K expressions to solve … Example: A 0.10 M aqueous solution of lactic acid, CH3CHOHCO2H, has a pH of 2.43. What is the value of Ka for lactic acid?

Strong Acid or Base solutions: Since these dissociate completely, reactions go to completion Use stoichiometry to solve … What is the pH of a 0.5 M HCl solution?

Practice: Example: Calculate the pH of a 0.020 M solution of benzoic acid (C6H5CO2H) if the Ka = 6.3x10-5

For polyprotic acids: How would this process work for a polyprotic acid such as H3PO4 that has multiple dissociations? 1. H3PO4 + H2O ↔ H2PO4- + H3O+ Ka=7.5x10-3 2. H2PO4- + H2O ↔ HPO4-2 + H3O+ Ka=6.2x10-8 3. HPO4-2 + H2O ↔ PO4-3 + H3O+ Ka=3.6x10-13

For polyprotic acids: For most polyprotic acids, the pH only depends on the amount of H3O+ generated in the first step! The other reactions are so reactant favored, that they barely produce any H3O+ at all Practice: Calculate the pH of 0.020M solution of Phosphoric acid.

Acids and Bases