9.5
Potenciales de unión en células galvánicas
La ecuación de Nernst, derivada bajo la suposición de equilibrio termodinámico, calcula la fuerza electromotriz (fem) como la suma de diferencias de p…
La ecuación de Nernst predice el potencial de la celda bajo condiciones no estándar.
Sin embargo, en muchas celdas galvánicas, el potencial medido suele diferir del valor predicho por la ecuación de Nernst.
Para entender esto, consideremos una celda galvánica que contiene dos medias celdas con diferentes soluciones electrolíticas. Cuando entran en contacto, los iones comienzan a difundirse a través del límite. Como los iones tienen diferentes movilidades, se desplazan a distintas velocidades.
Este movimiento desigual de iones crea una pequeña separación de carga en la interfaz entre ambas soluciones. Esto desarrolla un potencial adicional llamado potencial de unión líquida, EJ.
Como resultado, la fem medida incluye tanto el potencial de Nernst como el potencial de unión.
Para reducir este efecto, se utiliza un puente salino. El puente salino suele contener gel de agar mezclado con un cloruro de potasio concentrado similar a un electrolito.
Como los iones potasio y cloruro tienen movilidades similares, se difunden a velocidades similares. Su difusión ayuda a minimizar el potencial de unión y mejora la precisión de las mediciones.
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Q1: Why does the measured potential in a galvanic cell differ from the Nernst equation prediction?
The measured potential differs because ions in the two half-cell electrolyte solutions have different mobilities and diffuse at unequal rates across the boundary. This creates a charge separation at the interface, generating an additional potential called the liquid junction potential. The total measured emf includes both the Nernst potential and this junction potential.
Q2: What is a liquid junction potential and how does it form?
A liquid junction potential is a small potential difference that develops at the interface between two electrolyte solutions due to different ion diffusion rates. Since ions have different mobilities, they move at different speeds across the boundary, creating unequal charge separation. This additional potential must be accounted for in accurate electrochemical measurements.
Q3: How does a salt bridge minimize junction potential in galvanic cells?
A salt bridge contains agar gel mixed with an electrolyte like concentrated potassium chloride. Potassium and chloride ions have similar mobilities, so they diffuse at comparable rates. This balanced diffusion minimizes the junction potential at both ends of the salt bridge, causing them to largely cancel each other out and improve measurement accuracy.
Q4: Can salt bridges completely eliminate liquid junction potentials?
No, salt bridges can minimize but not eliminate liquid junction potentials. Although the junction potentials at both ends of the salt bridge largely cancel each other due to similar ion mobilities, a small residual potential remains. This is why junction potentials are considered significant for accurate electrochemical work.
Q5: What role do ion mobilities play in creating junction potentials?
Ion mobilities determine the diffusion rates of ions across electrolyte solution boundaries. When ions have different mobilities, they move at unequal speeds, creating uneven charge distribution at the interface. This charge separation generates the liquid junction potential. Selecting ions with similar mobilities, as in salt bridges, reduces this effect.
Q6: How does the total emf of a cell with a liquid junction relate to the Nernst equation?
The total emf of a cell with a liquid junction equals the sum of the Nernst potential and the liquid junction potential. The Nernst equation calculates the potential under thermodynamic equilibrium conditions without a junction. Adding the junction potential accounts for the real-world charge separation that occurs when different electrolyte solutions meet.
Q7: Why are junction potentials important in electrochemical measurements?
Junction potentials are important because they contribute to the total measured emf and can introduce significant errors in electrochemical work. Although small, they affect measurement accuracy in applications of emf measurements. Understanding and minimizing junction potentials through salt bridges ensures reliable and precise electrochemical data.