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

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems .

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Based on our data, we think this problem is relevant for Professor Hopkins' class at LSU.