Final answer:
The statement is true; a concentration of KIO3 greater than 0.01M is typically used for standardizing Na2S2O3 solutions to produce a measurable amount of I3- for accurate titration.
Step-by-step explanation:
The statement that the concentration of KIO3 used for standardizing the solution of Na2S2O3 is somewhat greater than 0.01M is True. In a typical redox titration process, a known concentration of KIO3 is used to standardize Na2S2O3 solutions due to its stability and purity as a primary standard. When standardizing the Na2S2O3 solution, a sufficient quantity of KIO3 is dissolved in an acidic medium containing an excess of KI. The iodate (IO3-) reacts with iodide (I-) to release iodine (I3-), which is then titrated with thiosulfate in the presence of starch as an indicator until the endpoint is reached.
The actual concentration of KIO3 used for standardization purposes typically exceeds 0.01M to ensure that an accurate and detectable amount of I3- is produced for the titration with Na2S2O3. The slight excess concentration ensures that there is a measurable iodine release for accurate titration and analysis.