HBrO(aq) + H2O(l) ⇄ H3O+(aq) + BrO−(aq) Keq=2.8×10−9

The equilibrium reaction in 0.100M HBrO(aq) at equilibrium is represented by the equation above. Based on the magnitude of the equilibrium constant, which of the following correctly compares the equilibrium concentrations of substances involved in the reaction, and why?

answer choices
The equilibrium concentration of BrO− will be much smaller than the equilibrium concentration of H3O+, because H2O is the solvent and is present in the largest amount.

The equilibrium concentration of BrO− will be much smaller than the equilibrium concentration of HBrO, because Keq<<1

The equilibrium concentration of H3O+ will be much smaller than the equilibrium concentration of BrO−, because all the HBrO will react to produce BrO−

The equilibrium concentration of H3O+ will be much larger than the equilibrium concentration of HBrO, because Keq<<1.