Why are standard solutions of reductants less often used for titrations than solutions of oxidants?
I think it may be because it is relatively easy to reduce metals/unknowns to their lower/lowest stable state, then oxidize them, than it is to oxidize them to a higher/highest stable state and reduce them. A second reason may be that standard solutions of oxidants generally are more stable than standard solution of reductants (true for cerium solutions but not for permanganate solutions). Then again, I may on the wrong wavelength.
Standard solutions of oxidants are more commonly used for titrations because they provide a more convenient and reliable way to measure the concentration of reducing agents. This is due to a few factors:
1. Stability: Solutions of oxidants tend to be more stable compared to reductant solutions. This stability ensures that the concentration of the oxidant remains constant over time. This is crucial for accurate titration since any variation in concentration can lead to errors in the determination of the analyte's concentration.
2. Safety: Oxidants are generally safer to handle and store compared to reductants. Many reductants are highly reactive and can pose risks of explosion or cause injury if mishandled. In contrast, oxidants are typically more stable and do not pose significant safety hazards.
3. Availability: Standard solutions of oxidants, such as potassium permanganate (KMnO4) or iodine (I2), are readily available commercially in accurate and reliable concentrations. On the other hand, finding commercially available standard solutions of reductants can be more challenging due to their reactivity and instability.
However, this does not mean that standard solutions of reductants are never used in titrations. In certain cases, where the reductant is stable and has appropriate properties, it can be used as a standard solution. However, careful considerations and precautions need to be taken to ensure accurate results and safety while using reductant solutions in titrations.