What is the rate law for crystal violet and NaOH?
Upon reaction with NaOH the conjugation gets disrupted and the color is lost. The rate law for reaction (1) is of the form: rate = k [CV+]m[OH–]n, where k is the rate constant for the reaction m is the order with respect to crystal violet (CV+) n is the order with respect to the hydroxide ion.
What happens when crystal violet reacts with hydroxide?
When crystal violet reacts with a base (−OH), the conjugation is disrupted and the color is lost. Note that in the reaction product, the three rings are no longer in conjugation with one another, and hence the material is colorless.
What is the effect of adding the sodium hydroxide solution to the crystal violet solution?
Crystal violet solutions may cause skin and eye irritation. Sodium hydroxide solutions are caustic and will cause skin burns. Any skin contact with either chemical should be immediately washed. Safety goggles must be worn in the lab at all times.
What happens to the color of crystal violet as the reaction proceeds with excess sodium hydroxide?
What happens as the reaction proceeds? The purple color of the solution fades as the concentration fo the crystal violet cation decreases. Measure the absorbance of the crystal violet/hydroxide ion solution at time intervals after the reactants are mixed.
What is the purpose of the crystal violet lab?
The purpose of this advanced inquiry lab activity is to use spectroscopy and graphical analysis to determine the rate law for the color-fading reaction of crystal violet with sodium hydroxide.
Why is crystal violet intense color?
The colour of the dye depends on the acidity of the solution. At a pH of +1.0, the dye is green with absorption maxima at 420 nm and 620 nm, while in a strongly acidic solution (pH −1.0), the dye is yellow with an absorption maximum at 420 nm.
Who Made Beer’s law?
August Beer
Formulated by German mathematician and chemist August Beer in 1852, it states that the absorptive capacity of a dissolved substance is directly proportional to its concentration in a solution.