A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated wi

Question

A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated cylinder to obtain approximately 0.6 M HCl. This solution was titrated with the original NaOH solution. The student calculated the concentration of NaOH from the experiment to be 0.099 M. In which experiment should the student be more confident of the concentration of the NaOH solution? Why?

Explanation / Answer

Well writing it out may help. Titration: determining the unknown concentration of a chemical. M is molecular measurement. NaOH + .347g KHP= .110 M NaOH + 6 M HCL= .099 M Which experiment better determines the concentration of NaOH? So Hydrochloric acid (HCL) vs. Potassium hydrogen phthalate (KHP) Hmmm...Yeah, still stumped. Here, this link discusses NaOH and KHP and HCL. Edit* From what I read here, KHP is more reliable because it has a higher moler mass. I don't know how to explain in more detail, but hope that helps :)

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