Standardization of NaOH Solution Part 2: Standardization of NaOH Solution In thi

Question

Standardization of NaOH Solution

Part 2: Standardization of NaOH Solution In this part of the lab experiment you will standardize a solution against a primary standard. Specifically, you will titrate a known amount of potassium hydrogen phthalate (KHP), which will serve as the primary standard, with a solution of NaOH that is approximately 0.10 M in order to determine its concentration more accurately - standardize it. This is a technique that will be used throughout this semester. Fill a clean vial with pure KHP. Weigh out, by difference, 0.5000 g KHP into each of four Erlenmeyer flasks. mass of KHP. Add 25 mL of DI water to each flask. Do not worry if the mass is not exactly 0.5000 g, but be sure to record the exact Fill your buret with the 0.1 M NaOH solution. Be sure to rinse the buret with this solution before filling it. Record the initial volume of NaOH in the buret in your lab notebook. Remember: do not waste tume attempting to bring the liquid level in the buret up to 0.00 m.L. Add 3 drops of phenolphthalein indicator solution to the analyte solution in the flask. Page | 2

Explanation / Answer

the reaction of KHP with NaOH is

KHC8H4O4(aq) + NaOH(aq) --> KNaC8H4O4(aq) + H2O(l)

1 mole of KHP requires 1 mole of NaOH as per the stoichiometry of the reaction

Hence moles of KHP = 0.533g/204.22g = 0.00261 moles

hence 0.00261 moles of KHP requries 0.00261 moles of NaOH.

Molarity= moles/ Volume in L= 0.00261 *1000/24.8   M=0.105 M

(data is taken based on consecutive readings in your result)

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