Final answer:
The pH of a solution during a titration of Ba(OH)2 with HCl is calculated using stoichiometry and the pH formula. It begins as a basic solution and transitions to acidic once the equivalent point is surpassed.
Step-by-step explanation:
Calculating pH for Titration of Ba(OH)2 with HCl
The question involves a titration calculation, which is a common procedure in chemistry to determine the concentration of an unknown solution. In this case, we are asked to calculate the pH of the solution after adding different volumes of 0.544 M HCl to 88.0 mL of 0.136 M Ba(OH)2. As both barium hydroxide and hydrochloric acid are strong electrolytes, they will dissociate completely in the solution.
The pH calculation depends on the stoichiometry of the reaction and the amount of HCl added. Once the equivalent point has been reached, the pH can be found using the excess HCl.
The formula for pH is pH = -log [H+], where [H+] is the concentration of hydrogen ions in the solution. To apply this, we first need to know the moles of both reactants and the remaining concentration of the limiting reactant, if any, after the reaction has occurred.
For example, at the beginning (titrant volume = 0 mL), we only have Ba(OH)2 in solution, and the pH would be >7 due to the presence of OH- ions from Ba(OH)2. As HCl is added, the OH- ions will react with the H+ ions to form water, until the equivalent point is reached. After this point, any additional HCl will cause the pH to drop below 7. The exact values of pH during the process are obtained by applying the stoichiometry of the titration and then using the pH equation.