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Rate Law Determination of the Crystal Violet Reaction

Experiment #30 from Chemistry with Vernier

Education Level
High School
Subject
Chemistry

Introduction

In this experiment, you will observe the reaction between crystal violet and sodium hydroxide. One objective is to study the relationship between concentration of crystal violet and the time elapsed during the reaction. A simplified version of the equation is:

{\text{C}}{{\text{V}}^{\text{ + }}}{\text{(aq) + O}}{{\text{H}}^{\text{ - }}}{\text{(aq)}} \to {\text{CVOH(aq)}}

The rate law for this reaction is in 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+), and n is the order with respect to the hydroxide ion. Because the hydroxide ion concentration is more than 1000 times as large as the concentration of crystal violet, [OH–] will not change appreciably during this experiment. Thus, you will find the order with respect to crystal violet (m), but not the order with respect to hydroxide (n).

As the reaction proceeds, a violet-colored reactant will be slowly changing to a colorless product. You will measure the color change with a Vernier Colorimeter or a Vernier Spectrometer. The crystal violet solution used in this experiment has a violet color, of course, thus the Colorimeter users will be instructed to use the 565 nm (green) LED. Spectrometer users will determine an appropriate wavelength based on the absorbance spectrum of the solution. We will assume that absorbance is proportional to the concentration of crystal violet (Beer’s law). Absorbance will be used in place of concentration in plotting the following three graphs:

  • Absorbance vs. time: A linear plot indicates a zero order reaction (k = –slope).
  • ln Absorbance vs. time: A linear plot indicates a first order reaction (k = –slope).
  • 1/Absorbance vs. time: A linear plot indicates a second order reaction (k = slope).

Once the order with respect to crystal violet has been determined, you will also be finding the rate constant, k, and the half-life for this reaction.

Objectives

In this experiment, you will

  • Observe the reaction between crystal violet and sodium hydroxide.
  • Monitor the absorbance of the crystal violet solution with time.
  • Graph Absorbance vs. time, ln Absorbance vs. time, and 1/Absorbance vs. time.
  • Determine the order of the reaction.
  • Determine the rate constant, k, and the half-life for this reaction.

Sensors and Equipment

This experiment features the following sensors and equipment. Additional equipment may be required.

Option 1

Go Direct® Colorimeter

Option 2

Go Direct® SpectroVis® Plus Spectrophotometer

Option 3

Colorimeter

Option 4

Go Direct® Visible Spectrophotometer

Correlations

Teaching to an educational standard? This experiment supports the standards below.

International Baccalaureate (IB) 2025/Chemistry
Reactivity 2.2.11—The rate constant, k, is temperature dependent and its units are determined from the overall order of the reaction.

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Purchase the Lab Book

This experiment is #30 of Chemistry with Vernier. The experiment in the book includes student instructions as well as instructor information for set up, helpful hints, and sample graphs and data.

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<i>Chemistry with Vernier</i>
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