Question

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

Answer 1

Answer: The equilibrium concentration of $BrO^-$ will be much smaller than the equilibrium concentration of $HBrO$, because Keq<<1

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as $K_{eq}$

K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For the given chemical reaction:

$HBrO(aq)+H_2O(l)\rightarrow H_3O^+(aq)+BrO^-(aq)$

The expression for $K_{eq}$ is written as:

$K=\frac{[H_3O^+]\times [BrO^-]}{[HBrO]}$

Concentration of pure solids and liquids is taken as 1.

$K=2.8\times 10^{-9}$

Thus as $K_{eq}$ , That means the concentration of products is less as the reaction does not proceed much towards the forward direction.