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Equilibrium Constant of an Ionic Compound
The idea of the reversibility of chemical reactions was first stated by C. Berthollet in 1799. He noted deposits of sodium carbonate in certain salt lakes in Egypt and concluded that they were produced by the high concentration of sodium chloride and dissolved calcium carbonate. This is the reverse of the standard laboratory procedure in which calcium carbonate is produced from the reaction on sodium carbonate and calcium chloride. A standard curve will be established for the absorbance of a colored species and the used to determine the concentrations of unknown solutions. The results will allow us to determine the equilibrium constant for the formation of the colored species.
Kit Includes:
- Iron (III) Nitrate, 0.2M - 500 ml x 1 Bottle
- Potassium Thiocyanate, 0.002M - 100 ml x 2 Bottles
- Nitric Acid, 0.5M UN2031 - 100 ml x 1 Bottle
Materials needed but not supplied:
- (# 6108-36) Volumetric Flasks 100 ml - 5 pcs
- (# 3871-23, -24) Volumetric Pipette Set 1 ml - 5 ml - 1 Set
- (# 6108-37) Volumetric Flask 250 ml - 1 pc
- (# 6135-3) Test Tube 13 x 100 mm - 75 pcs
- Volumetric Pipettes 0.5, 1.0, 1.5, 2.0, 2.5 ml - 30 pcs each
- Spectrophotometer w/ 1 cm Cuvettes
Please note that the pictures may show items not included in this kit, the pictures are there to show kit functionality. Please refer to the product details above for more information on the contents of this kit.
DOT: UN2031, Nitric acid, 8, PG II
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Equilibrium Constant of an Ionic Compound AP Chemistry