Acid/Base fun (not really)
The molecular weight of a monoprotic acid HX was to be determined. A sample of 15.126 grams of HX was dissolved in distilled water and the volume brought to exactly 250.00 mL. Several 50.00 mL portions of this sol'n were titrated against NaOH sol'n, requiring an average of 38.21 mL of NaOH.
The NaOH sol'n was standardized against oxalic acid dihydrate (H2C204x2H20 mole.wt: 126.066) The volume of NaOH sol'n required to neutralize 1.2596 g of oxalic acid was 41.24 mL.
a)Calculate the molarity of the NaOH sol'n
b)Calculate the number of moles of HX in a 50.00 mL portion used for titration
c)Calculate the molecular weight of HX
d)Discuss the effect of the calculate molecular weight of HX if the sample of oxalic acid dihydrate contained a nonacidic impurity.
That's all. I know, it's pretty ugly, but any help would be appreciated =)