Final Answer:
The titration of the 25ml sample of 0.260M NaOH will require 10.75ml of a 0.650M HCl solution to reach the equivalence point.
Explanation:
To calculate the volume of HCl required for the titration, we can use the equation M1V1 = M2V2, where M1 is the molarity of the NaOH solution, V1 is the volume of NaOH used, M2 is the molarity of the HCl solution, and V2 is the volume of HCl used. Rearranging the equation to solve for V2, we get V2 = (M1V1) / M2. Plugging in the values, V2 = (0.260M * 25ml) / 0.650M = 10.75ml.
In this titration, NaOH reacts with HCl in a 1:1 ratio according to the balanced chemical equation: NaOH + HCl -> NaCl + H2O. This means that for every mole of NaOH, one mole of HCl is required to reach the equivalence point. The molar ratio allows us to directly convert between volumes of the two solutions.
It’s important to note that in a titration, the equivalence point is reached when stoichiometrically equivalent quantities of acid and base have reacted. This calculation assumes ideal conditions and complete reaction between the two solutions.