The forum discussion centers on the dilution process in spectrophotometry, particularly in the context of applying Beer-Lambert's Law during neutralization titrations. Participants clarify that while measuring absorbance, the dilution of weak acids or bases can introduce errors due to water's autoionization, which affects concentration. It is established that the primary goal in titration is to detect the endpoint rather than the concentration itself, distinguishing the roles of spectrophotometry and pH indicators in this process.
PREREQUISITESChemistry students, laboratory technicians, and researchers involved in analytical chemistry, particularly those focusing on spectrophotometric methods and titration techniques.
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.