Final answer:
Molar concentration is a measure of solute per volume of solution, crucial in titration for determining the amount of titrant needed. To find the molar concentration of LiOH, the moles of titrated HBr are divided by the volume of LiOH to yield approximately 0.0673 M. Accuracy in titration can be affected by several factors, including equipment calibration and experimental conditions.
Step-by-step explanation:
Understanding Molar Concentration in Titration
Molar concentration, often represented by the unit Molar (M), is defined as the number of moles of a solute divided by the volume of the solution in liters. In titration, this measure is crucial as it allows chemists to determine the amount of titrant needed to react completely with the analyte (the substance being analyzed).
Calculating the Molar Concentration of LiOH
The formula for molar concentration is M = moles of solute / liters of solution. To calculate the concentration of LiOH, we first need to know the reaction equation, which is LiOH + HBr → LiBr + H₂O. Since the reaction is 1:1, the moles of LiOH will be equal to the moles of HBr used. We calculate the moles of HBr by multiplying its volume in liters (0.175 L) with its molarity (0.025 M), resulting in 0.004375 moles of HBr. To find the molarity of LiOH, we then divide the moles of HBr by the volume of LiOH in liters (0.065 L), which gives us approximately 0.0673 M of LiOH.
Tips for Accurate Titration
During titration, several steps ensure accuracy: choosing appropriate indicators, calibrating equipment, adding the titrant slowly near the end point, and repeating titrations for consistency. Factors that can affect accuracy include equipment cleanliness, temperature, and human error.