A 30.00ml sample of 0.1234 M hypobromous acid (HBrO) is titrated with a 0.2555 M KOH solution. The Ka for HBrO is 2.5*10^-9

Calculate the pH of the titration mixture at the equivalence point.

You must recognize what you have at the equivalence point. In this titration, the HBrO has been neutralized with KOH to produce the salt KBrO. The salt will be hydrolyzed. Set up an ICE chart, substitute into Kb for the salt (Kb = Kw/Ka) and solve.

k;j

To calculate the pH of the titration mixture at the equivalence point, we need to determine the moles of HBrO and OH- at the equivalence point, and then calculate the resulting concentration of each species to find the resulting pH.

1. Determine the moles of HBrO in the 30.00 ml sample:
Moles of HBrO = Volume (in liters) x Concentration
Moles of HBrO = 0.03000 L x 0.1234 M

2. Calculate the moles of OH- at the equivalence point:
Since HBrO reacts with KOH in a 1:1 stoichiometric ratio, the moles of OH- at the equivalence point will be equal to the moles of HBrO.

3. Calculate the total volume of the titration mixture at the equivalence point:
Since the volume of HBrO solution is given as 30.00 ml, this will be the same as the total volume at the equivalence point.

4. Calculate the concentration of OH- at the equivalence point:
Concentration of OH- = Moles of OH- / Total volume (in liters)
Concentration of OH- = Moles of HBrO / Total volume (in liters)

5. Calculate the pOH of the titration mixture at the equivalence point:
pOH = -log10(OH- concentration)

6. Finally, calculate the pH of the titration mixture at the equivalence point using the pOH value and the equation:
pH + pOH = 14

Substituting the values obtained from calculations into the respective equations will give you the pH of the titration mixture at the equivalence point.