Final answer:
The molarity of the NaOH titrant can be accurately calculated if the concentration of the KHP analyte solution is known. This allows for precise stoichiometric calculations in titrations. Additionally, osmolality can be used to determine the relative concentrations of solutions based on the moles of solute per kilogram of solvent.
Step-by-step explanation:
The question asks whether the concentration of a KHP analyte solution must be known to calculate the molarity of an NaOH titrant. The answer is true. For example, when a 0.3420-g sample of KHP (potassium hydrogen phthalate) reacts with NaOH in a titration, knowing the exact mass of KHP is crucial to determine the molarity of the NaOH solution. During titration, the moles of KHP are stoichiometrically equivalent to the moles of NaOH. Therefore, by accurately measuring the mass of the KHP and the volume of the NaOH solution that reacted with KHP, the calculation of the molar concentration of the NaOH solution is possible.
When performing titrations, it is necessary to prepare the NaOH solution with a precise concentration. If a student measures a correct mass of NaOH pellets and dissolves it in exactly 200 cm³ of pure water, this does not guarantee the NaOH solution will have the correct concentration without confirming the actual solubility and any potential loss during transfer or dissolving.
In another example, the osmolality of a solution indicates its concentration by measuring the moles of solute per kilogram of solvent. If Solution A has a higher osmolality compared to Solution B, then Solution A is more concentrated. This explains how osmolality is used to determine the strength of a solution.