Unknown Base Titration

The unknown base concentration of a sodium hydroxide solution can be determined by titration potassium hydrogen phthalate (KHP) with an unknown concentration of sodium hydroxide NaOH. The average molarity of NaOH determine by the moles and volume of the KHP and NaOH. (Eq 1).
KHC8H4O4(aq) + NaOH(aq) = H2O(l) + NaKC8H4O4(aq) (Eq 1)
The unknown concentration of white vinegar can be determined by the white vinegar with the known concentration of sodium hydroxide from the previous lab. (Eq 2).
CH3CO2H(aq) + NaOH(aq) = CH3CO2Na(aq) + H2O(l) (Eq 2) The purpose of indicator used to determine the end point of the reaction when both the reactants and product are colorless. The experiment goal of the lab is to determine the concentration of acetic acid (CH3CO2H) in the commercial white vinegar brand.
Procedure and Data Statement The complete experimental procedure is available in the General Chemistry Laboratory Manual for CSU Bakersfield, CHEM 211, pages 60-61, 64-65. Experimental data recored on the attached data pages 62-63, 66-68.
Discussion …show more content…
The average experimental % by mass of acetic acid is 5.607%, it is far away to the percent reported on the vinegar bottle by 0.6070%. The data is higher than the actual real concentration. The total volume of NaOH used suggests the lesser accuracy. In lab one, the titration of primary standard of KHP with the unknown standardization NaOH to determine the concentration of sodium hydroxide by the end point of buret. In the second lab, the pervious lab concentration of NaOH used to titration with the unknown concentration of white vinegar in order to get the concentration of vinegar. The experimental concentration of the sodium hydroxide solution is