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Hypobromous acid, HBrO, is a weak acid. The following is the equilibrium constant for its reaction...

Hypobromous acid, HBrO, is a weak acid. The following is the equilibrium constant for its reaction with water:

HBrO(aq) + H2O(l) <----------> H3O+(aq) + BrO-(aq)     Ka = 2.5 x 10-9

What is the hydronium ion concentration, [H3O+], in a 1.32 M HBrO solution?

Note: Assume that the ionization of the acid is small enough in comparison to its starting concentration that the concentration of unionized acid is almost as large at equilibrium as it was originally. This will allow you to avoid having to solve the quadratic formula when doing your ICE table calculation. (This approximation technique is discussed in Mr. Robinson's Lecture Notes on "Acid/Base Equilibria".)

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