Respuesta :
In the titration of acetic acid and NaOH using an indicator, the reported mass percent of acetic acid is higher.
To indicate the color shift, a small amount of base is applied to the indicator. This yields the titration end point. It should be emphasized that this tiny surplus of base is used by the indication rather than the titre. This indicates that titration has already been finished, and the added base helps elevate pH, causing the indicator to change hue.
[tex]M_{acid} V_{acid} = M_{base} V_{base}[/tex]
[tex]V_{base}[/tex] will be somewhat higher, resulting in a slightly higher estimated value of [tex]M_{acid}[/tex].
[tex]M_{acid} = M_{base} V_{base} / V_{acid}[/tex]
This mistake is insignificant since very little excess is required for the indicator to change color.
During the titration of NaOH versus [tex]CH_3COOH[/tex] using indicator, the number of [tex]OH^-[/tex] ions required to reach the end point equals the number of [tex]H^+[/tex] ions from the analyte, [tex]CH_3COOH[/tex] plus the number of [tex]H^+[/tex] ions from the indicator, resulting in a slightly higher calculated molarity of acetic acid and a higher reported mass percent of acetic acid.
Learn more about Titration here:
https://brainly.com/question/12708635
#SPJ4
