A Simplified Undergraduate Laboratory Experiment To Evaluate the Effect of the Ionic Strength on the Equilibrium Concentration Quotient of the Bromcresol Green Dye

Abstract

A modified laboratory experiment for undergraduate students is presented to evaluate the effects of the ionic strength, I, on the equilibrium concentration quotient, K c, of the acid–base indicator bromcresol green (BCG). The two-step deprotonation of the acidic form of the dye (sultone form), as it is dissolved in water, yields suitable hydronium concentration in the solution to carry out the experiment successfully and avoids the use of any buffer solution to fix the hydronium concentration of the media. The 95% confidence interval for the slope parameter (−2.08 ± 0.13), obtained from the linear fit of pK c versus √I/ (1 + 2.30·√I) plot, contains the theoretical value of −2.04 predicted by the Debye–Hückel extended law. From the intercept, a value for the equilibrium dissociation constant of BCG, pK = (4.91 ± 0.02), is obtained, showing a reasonable agreement with literature data. The simplification makes it possible for students to complete the experiment in the course of an ordinary 3-h laboratory session.

Universal pH Indicator as a Colorimetric Reagent for Differentiating Inorganic Anions

“…This observation may be attributed to an increase in ionic strength of halide solutions which caused a shift in the color of the indicator. This behavior has also been noted by Rodriguez and Mirenda 16 in which an increase in salt concentration led to a shift of the pH indicator towards the basic form. Thus, it is important to compare anions with the same concentration and under dilute conditions.…”