The Ksp of Magnesium Oxalate

THE Ksp of Magnesium Oxalate ABSTRACT INTRODUCTION In this experiment the solubility product constant of the salt magnesium oxalate (MgC2O4)will be determined. The system of interest exists as a solid in equilibrium: Precipitation reaction of EXPERIMENTAL METHODS Preparation of the 0.15M Potassium Permanganate (KMnO4) solution {text:list-item} B. Prepare precipitation mixtures 1. Obtain three labeled 20-mL vials from the cart. 2. Burets are set up in the lab with 0.250 M MgSO4 and 0.250 M Na2C2O4. Refer to Table 1, and add the appropriate volume of each solution to the numbered vials. Table 1. Precipitation reactant volumes Standardize the Permanganate Solution {text:list-item} {text:list-item} {text:list-item} {text:list-item} {text:list-item} {text:list-item} {text:list-item} {text:list-item} Titrate the Oxalate equilibrium mixtures {text:list-item} {text:list-item} {text:list-item} {text:list-item} {text:list-item} DATA *Table 2.* Precipitation reactant volumes Molarity of Permanganate solution: RESULTS ICE Reaction Tables Table 5. Vial #2 ICE TABLE Table 6. Vial #3 ICE TABLE Average Ksp* from the 3 experimental vials is *1.11 x 10*-3*. DISCUSSION The Ksp of the different reactions of the vials should be similar if not the same. In experiment vial 3 the Kspwas slightly different than the other two results. This variation could be due to temperature differences of the titration of oxalate, the vials not mixing well sitting and coming to equilibrium for the week it sat in the vial, or a contaminant might have made its way in the reaction. Bibliography References [1.] Ebbing · Gammon, General Chemistry, Ch. 13

References: [1.] Ebbing · Gammon, General Chemistry, Ch. 13 (2009)