The discussion revolves around the dilution process in spectrophotometry, particularly in the context of measuring concentrations during neutralization reactions involving weak acids or bases. Participants explore the implications of water's autoionization on measurement accuracy and the relationship between absorbance and concentration as described by Beer's law.
Participants appear to have differing views on the relevance of concentration measurement versus endpoint detection in titrations, indicating a lack of consensus on the primary focus of the discussion. Additionally, there is uncertainty regarding the impact of water's autoionization on measurement accuracy.
Limitations in the discussion include potential missing assumptions about the significance of autoionization effects, the specific conditions under which measurements are taken, and the definitions of terms like "endpoint" and "concentration" in the context of titration.
Serenie said:when measuring neutralization reaction
After reread and thinking about this again, the description is of two usually very separate things: Spectrophotometer to help measure concentration of some dissolved item which absorbs a specified wavelength of visible light; and neutralization titration between acid and base for which endpoint detection would be either by pH-meter, or acid-base indicator compound. These two ideas are usually not related. Maybe you tell what item is being measured?Serenie said:When using spectrophotometer, to use Rambert-beer's law, we often go through dilution process. Then when measuring neutralization reaction and using week acid or base, then because of water's autoionizaition, i think the results have error.
Is it right?
Serenie said:What i mean is that when doing neutralization titration, we need to measure the concentration.