1. 51.2 g of NaClO (pKa of HClO is 7.50) and 25.3 g of KF (pKa of of HF is 3.17) were combined in enough water to make 0.250 L of solution. Determine the pH of the mixture. Determine the equilibrium concentrations of HF and HClO in the solution.

*

*

*

Explanation:

Hello,

At first, the molarities of NaClO and KF are computed as shown below:

Now, since both NaClO and KF are ionic, one proposes the dissociation reactions as:

In such a way, by writing the formation of HClO and HF respectively, due to the action of water, we obtain:

Now, the presence of OH⁻ immediately implies that Kb for both NaClO and KF must be known as follows:

In such a way, the law of mass action for each case is:

Now, by solving for the change for both the ClO⁻ and F⁻ equilibriums, we obtain:

Such results equal the concentrations of OH⁻ in each equilibrium, thus, the total concentration of OH⁻ result:

With which the pOH is:

And the pH:

In addition, the equilibrium concentrations of HClO and HF equals the change for each equilibrium as:

Best regards.