Exploring Fundamental Concepts in Aqueous Solution Conductivity: A General Chemistry Laboratory Exercise

Nyasulu, Frazier; Stevanov, Kelly; Barlag, Rebecca

doi:10.1021/ed100385s

Cited by 9 publications

(14 citation statements)

References 6 publications

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“…For example, a 1 °C error in temperature is associated to a conductivity variation of ~3% for NaCl. 3 These errors are acceptable for an undergraduate laboratory experiment and are similar to those obtained using more concentrated solutions and the use of the Kohlrausch equation, as reported by Eslek and Tulpar. …”

Section: Strong Electrolytessupporting

confidence: 82%

“…The study of the conductivity of electrolyte solutions is important for the development of electrochemical devices, 1,2 for the characterization of the dissociation equilibrium of weak electrolytes, [2][3][4] and for the fundamental understanding of charge transport by ions. 5 Therefore, experiments in general chemistry and physical chemistry laboratories are widespread in undergraduate chemistry courses, and are subject to many educational developments, from the development of conductivity measuring apparatus to the preparation and study of specific electrolytes.…”

Section: Introductionmentioning

confidence: 99%

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Measuring the Conductivity of Very Dilute Electrolyte Solutions, Drop by Drop

Martı́nez¹

2018

Quim. Nova

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Undergraduate experiments on ionic conductivity are common practice in general chemistry and advanced physical chemistry laboratories. Often, the conductivities are measured for solutions prepared for various salts, in a range of concentrations, and the relationship between solution conductivity and concentration is interpreted in terms of the Kohlrausch law. Contaminations can dominate the conductivity of the solutions such that students might obtain unsatisfactory results for analysis. Here, the experience of using a simple experimental procedure to obtain the concentration dependence of ionic conductivities for very dilute (sub-millimolar) electrolyte solutions in undergraduate laboratories is described. The experiment consists of measuring the conductivity of solutions of increasing concentration prepared by dropping the electrolyte solution into an initial vessel of deionized water. The range of concentrations achieved is one in which the conductivities vary linearly with the concentrations, such that the molar conductivities can be obtained directly without the use of the Kohlrausch equation. The simplicity of the experimental procedure leads the students to obtain good quality results using minimal amounts of materials. Examples are presented for the conductivities of strong electrolytes, and for the weak acetic acid electrolyte, for which the conductivity is dependent on the degree of dissociation also for dilute solutions.

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Section: Strong Electrolytessupporting

confidence: 82%

Section: Introductionmentioning

confidence: 99%

Measuring the Conductivity of Very Dilute Electrolyte Solutions, Drop by Drop

Martı́nez¹

2018

Quim. Nova

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“…Binding to larger structures will also affect ionic mobility. Conductivity can also be affected by the viscosity of the solution, which could be different in the more complex DMEM/F12 . However, the viscosities of each solution were measured and there were no significant differences in viscosity between the solutions before adding Mg metal (SI Table S1).…”

Section: Resultsmentioning

confidence: 99%

“…To enable detection of Mg corrosion products in physiologically appropriate solutions in vitro, we explored the use of a conductivity sensor that essentially detects the ionic components in a solution . Conductivity, the ability of an electrolyte solution to pass an electric current, is concentration dependent as it varies with the sum of dissolved ion concentrations in water.…”

Section: Introductionmentioning

confidence: 99%

Conductivity Sensor for Real‐time Monitoring of Magnesium Corrosion under Cell Culture Conditions

et al. 2016

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1Introduction tested whether ac onductivity sensor could be used to monitor Mg degradation by detecting changes in ionic strength in real time,i nt hree physiologically appropriate fluids (a sodium chloride solution, phosphate buffered saline and ac ell culture medium maintained under the standard conditionsu sed for mammalian cell culture).Here we demonstrate that an electrochemical conductivity sensor, in combination with ap Hs ensor,r ecorded very different patternso fr eal-timec hanges in the ionice nvironmentc reated by Mg immersion and degradation in the three modele lectrolyte solutions,o ver a4 8-hour time period.

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“…The molar conductivity at infinite dilution can be decomposed into the contributions of each ion, (3) where λ + and λare the ionic conductivities of the positive and negative ions, respectively, and ν + and νare their stoichiometric coefficients in the salt molecular formula. From the concentration dependence of the molar conductivity of each salt, it is possible to obtain the molar conductivities at infinite dilution through Equation 1.…”

Section: Introductionmentioning

confidence: 99%

Measuring the conductivity of very dilute electrolyte solutions, drop by drop

Martı́nez¹

2017

Preprint

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<div>The study conductivity of electrolyte solutions is important for practical applications and for the understanding of ion mobility. Because of that, undergraduate experiments on ionic conductivity are common practice in first year general chemistry or more advanced physical chemistry laboratories.</div><div>Often, the conductivities are measured for solutions prepared for various salts, in a range of concentrations, and the relationship between solution conductivity and concentration is interpreted in terms of the Kohlrausch law. Extrapolation of the molar conductivities to infinite dilution allows the study of the individual ionic conductivities. In practice, the preparation of dilute solutions for these</div><div>experiments can be cumbersome, because small electrolyte contaminations can dominate the conductivity of the solutions. Additionally, significant amounts of reactants, particularly deionized water, must be used. Here, a simple experimental procedure is proposed to obtain the concentration dependence of ionic conductivities for very dilute (sub-millimolar) electrolyte solutions. The experiment</div><div>consists in measuring the conductivity of solutions of increasing concentration prepared by dropping the electrolyte solution into a single initial vessel of deionized water. The range of concentrations achieved is one in which the conductivities vary linearly with the concentrations, such that the molar conductivities can be obtained directly without the use of the Kohlrausch equation. The simplicity of the experimental procedure leads the students to obtain very good quality results using minimal amounts of materials. Examples are presented for the conductivities of various strong electrolytes, and for the weak acetic acid electrolyte, for which the conductivity is dependent on the dissociation rate even at very low concentrations.</div>

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Exploring Fundamental Concepts in Aqueous Solution Conductivity: A General Chemistry Laboratory Exercise

Cited by 9 publications

References 6 publications

Measuring the Conductivity of Very Dilute Electrolyte Solutions, Drop by Drop

Measuring the Conductivity of Very Dilute Electrolyte Solutions, Drop by Drop

Conductivity Sensor for Real‐time Monitoring of Magnesium Corrosion under Cell Culture Conditions

Measuring the conductivity of very dilute electrolyte solutions, drop by drop

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