Determination of the Solubility Product Constant for Calcium Sulfate: the Effect of Ionic Strengths of Electrolyte Solutions

688 Words3 Pages
Abstract In this experiment, the Ksp for calcium sulfate dihydrate, CaSO4·2H2O, by titrating 4 times a calcium sulfate dihydrate solution with diprotic EDTA, H2(EDTA)2-. For each trial we found the Ksp by means of molarities and activities. The results for the Ksp using only molarities was very different than the Ksp using activities. The average Ksp using molarity only was 2.26 x 10-4 and the average Ksp using activity turned out to be 2.31 x 10-5. The actual Ksp however, is 3.14 x 10-5. A percent error of 26.6 % was calculated.

Introduction

Experimental In this experiment, a saturated calcium sulfate was already made and ready to use. 25.00 mL of this solution was then mixed with 10 mL of an ammonia buffer and 1 drop of
…show more content…
|
|Trial 1 |0.0559 |
|Trial 2 |0.0603 |
|Trial 3 |0.0602 |
|Trial 4 |0.0602 |

| |Activity Coefficient |
|Trial 1 |0.329 |
|Trial 2 |0.315 |
|Trial 3 |0.316 |
|Trial 4 |0.316 |

|

More about Determination of the Solubility Product Constant for Calcium Sulfate: the Effect of Ionic Strengths of Electrolyte Solutions

Open Document