Problem: 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 × 10–9What is the hydronium ion concentration, [H3O+], in a 1.32 M HBrO solution?a) 2.6 x 10-8 Mb) 7.2 x 10-6 Mc) 5.7 x 10-5 Md) 1.3 x 10-4 Me) 4.9 x 10-3 M

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FREE Expert Solution

We are being asked to calculate the hydronium ion concentration, [H3O+], in a 1.32 M HBrO solution.

We're given the following equilibrium reaction:

HBrO(aq) + H2O(l) ⇋ H3O+(aq) + BrO(aq)        Ka = 2.5 × 109


Since HBrO is a weak acid. We need to construct an ICE chart.

85% (86 ratings)
Problem Details

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 × 109

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

a) 2.6 x 10-8 M

b) 7.2 x 10-6 M

c) 5.7 x 10-5 M

d) 1.3 x 10-4 M

e) 4.9 x 10-3 M

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