Determination of the solubilityproduct constant for a 恒为溶度积测定.pptVIP

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Determination of the solubilityproduct constant for a 恒为溶度积测定.ppt

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Determination of the solubilityproduct constant for a 恒为溶度积测定

Experiment 27 March 9, 2010 Dr. Scott Buzby, Ph.D. Learn to experimentally determine the solubility constant (Ksp) for a salt Practice operation of a spectrophotometer Further explore the use of a calibration graph and Beer-Lambert Law For a true equilibrium to exist between a solid and a solution, the solution must be saturated (i.e. solid material must remain at the bottom of the solution) The solubility of silver carbonate is expressed by the equation: We will use a spectrophotometer to determine the intensity of the color of a solution Described on pages 310 312 in you text Absorbance is related to concentration by the Beer-Lambert Law A – Absorbance of the solution a – Molar absorption coefficient (constant) b – Path length (constant) c - Concentration Prepare a series of solutions of a known concentration Plot absorbance vs. concentration for the known solutions By measuring absorbance of an unknown sample you can determine concentration using your plot (follow red arrows on graph) Procedure on page 311 FOLLOW ALL INSTRUCTIONS PRECISELY!!! Prepare three separate solutions according to the procedure on page 312 Determine the chromate concentration, [CrO42-], using your calibration graph Calculate silver concentration, [Ag+], and Ksp for you solution (see notes on page 313) Next Week – Nothing Enjoy Spring Break! Next Class (3/23/2010) Report Sheet – Pgs. 315-316 Questions – Pgs. 316-317 Calibration Graph – Pg. 318 or print-out Pre-Lab Experiment 28 – Pg. 323