A 15.0-mL sample of 0.100 M Ba(OH)2 is titrated with 0.125 M HCl. Calculate the pH for at least five different points throughout the titration curve and sketch the curve. Indicate the volume at the equivalence point on your graph.

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant (a solution of known concentration) to a sample solution until the reaction reaches its equivalence point, where the amount of titrant equals the amount of substance in the sample. Understanding the titration process is essential for calculating pH changes at various points during the titration.

The equivalence point in a titration is the stage at which the amount of titrant added is stoichiometrically equivalent to the amount of substance present in the sample solution. For the titration of Ba(OH)2 with HCl, this point occurs when all the barium hydroxide has reacted with hydrochloric acid, resulting in a neutralization reaction. Identifying the equivalence point is crucial for determining the pH and understanding the overall titration curve.

pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. During a titration, pH changes can be calculated at various points by considering the concentrations of the reactants and products formed. For strong acid-strong base titrations, the pH at the equivalence point is typically around 7, while before and after this point, the pH will vary significantly, reflecting the dominance of either the acid or base.