In aqueous solution, the hydrogen sulfate ion, HSO4–(aq), reacts with the hypochlorite ion ClO–(aq).
At equilibrium, are products or reactants favoured? Explain your reasoning
To determine whether products or reactants are favored at equilibrium, we need to examine the reaction and the respective concentrations of the reactants and products.
The balanced equation for the reaction between the hydrogen sulfate ion (HSO4–) and the hypochlorite ion (ClO–) in aqueous solution can be represented as:
HSO4–(aq) + ClO–(aq) ⇌ HClO(aq) + SO4^2–(aq)
In this case, the hydrogen sulfate ion (HSO4–) and the hypochlorite ion (ClO–) are both reactants, while the hypochlorous acid (HClO) and the sulfate ion (SO4^2–) are the products.
To determine which side of the reaction is favored at equilibrium, we need to consider the equilibrium constant expression (K) for the reaction:
K = [HClO] / [HSO4–][ClO–]
If the value of the equilibrium constant (K) is greater than 1, it indicates that the products are favored at equilibrium. Conversely, if the value of K is less than 1, it indicates that the reactants are favored at equilibrium.
Without specific information about the concentrations of the reactants and products, we cannot calculate the exact value of K or determine whether it is greater or less than 1. However, we can make some general observations:
1. The hydrogen sulfate ion (HSO4–) is a weak acid, while the hypochlorite ion (ClO–) is a strong base. Therefore, HSO4– can partially dissociate to produce H+ ions in the solution, while ClO– will be fully dissociated into Cl– ions. The resulting increase in H+ ions can shift the equilibrium towards the products.
2. The formation of hypochlorous acid (HClO) is an acid-base reaction that can also increase the concentration of H+ ions, favoring the products.
Based on these general observations, it is reasonable to conclude that at equilibrium, the products (HClO and SO4^2–) are likely to be favored. However, without specific information about the concentrations and the value of K, a definitive conclusion cannot be drawn.