Final answer:
The question involves a titration calculation in chemistry, specifically concerning the titration of a weak base (methylamine) with a strong acid (hydrobromic acid). The calculation requires the use of the molarity and volume of both solutions and the base's dissociation constant. The question details are incomplete for a full answer.
Step-by-step explanation:
The question asks for the determination of various quantities during the titration of a sample of methylamine (CH₃NH₂) with hydrobromic acid (HBr). Methylamine acts as a weak base in this context, and its titration with HBr, a strong acid, proceeds until the equivalence point is reached. To determine specific quantities such as the volume of HBr required, you would typically use the given molarity of the solutions, the volume of CH₃NH₂, and the Kb value provided for methylamine.
An example of such a calculation would be the use of the formula M1V1 = M2V2, where M1 and V1 represent the molarity and volume of the methylamine solution, and M2 and V2 represent the molarity and volume of the HBr solution. However, since the acid is strong and the base is weak, we must also consider the base's dissociation constant (Kb) in the calculation. Unfortunately, the initial question lacks the necessary details, such as the desired quantity (e.g., volume of HBr needed), to provide a complete step-by-step solution, plus appropriate data has not been provided within the question context.