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The Measurement of Crystal Violet Absorbance at Time Intervals by Determining the Rate Law for the Reaction Between Crystal Violet and Hydroxide The.

Crystal Violet Absorbance

Introduction

Crystal violet reacts with sodium hydroxide and the rate of this reaction is k[CV+]m[OH-]n, where k is the rate constant for the reaction, m and n represent the reaction order for crystal violet, and hydroxide, respectively.1 Because the reaction has a purple color that changes to colorless as the reaction proceeds, a spectrophotometer can be used to monitor the absorbance of crystal violet, and assume that the absorbance is proportional to the concentration of crystal violet. If plotting absorbance vs. time yields a linear graph, the reaction is zero order in respect to crystal violet. If plotting the natural log of absorbance vs. time yields a linear graph, the reaction is first order in respect to crystal violet. If plotting absorbance-1 vs. time yields a linear graph, the reaction is second order in respect to crystal violet. Once the reaction order is determined for crystal violet, it can be determined for hydroxide, and knowing the rate, the value of k for this reaction can be calculated.

Experimental

The spectrophotometer was turned on to allow it to warm up for 15 minutes, and the instrument was set to 565 nm. A beaker was filled with 10.0 mL of 0.020

Crystal Violet Absorbance

Introduction

Crystal violet reacts with sodium hydroxide and the rate of this reaction is k[CV+]m[OH-]n, where k is the rate constant for the reaction, m and n represent the reaction order for crystal violet, and hydroxide, respectively.

Assignment ID
100008638
Discipline
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CREATED ON
17 April 2018
COMPLETED ON
19 April 2018
Price
$28
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