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➢ ➢ ➢ ➢ ➢
INTRODUCCIÓN HISTORIA DEFINICIÓN DE DIAGRAMA DE POURBAIX CARACTERÍSTICAS CARACTERÍST ICAS DE LOS DIAGRAMAS DE POURBAIX USOS DE LOS DIAGRAMAS DE POURBAIX
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Los diagramas de Pourbaix (Eh pH) se presenta como una herramienta muy importante para el estudio termodinámico de la hidrometalurgia, en general, y de la precipitación de metales, en particular. Se discuten los principios termodinámicos en los que se basa la construcción de los diagramas, –
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Fue creado por un químico Ruso llamado Marcel Pourbaix (1904-1998) honorario de la universidad ➢ Profesor Libr Li bree de Br Brus usel elas as Director honorario del ➢ Administrador Centro Belga de Estudios de la corrosión CEBELCOR CEBEL COR Brus Bruselaselas-Bélg Bélgica. ica. ➢ A este le encantaba encantaba leer mucho mucho sobre los diagramas de fase y por esto decidió ➢
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Un diagrama de Pourbaix es una representación gráfica del potencial (ordenada) función del pH (abscisa) para un metal dado bajo condiciones termodinámicas standard (usualmente agua a 25 ºC). ❑ El diagrama tiene en cuenta los equilibrios químicos y electroquímicos y define el dominio de estabilidad para el electrólito (normalmente agua), el metal y los compuestos relacionados, por ejemplo, óxidos, hidr hi dróx óxid idos os e hi hidr drur uros os.. ❑
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❑ ❑
❑ ❑
Disolu Diso luci ción ón me metá táli lica ca----> -> di dife fere rent ntes es re reac acci cion ones es en entr tree el metal y el electrolito. Si ocurre por formación de oxido o hidróxido, el potten po enci cia al de eq equi uili libr brio io co corr rres espo pon ndi dien ente te de depe pen nde del pH de la solución. Prod Pr oduc ucto toss so solu lubl bles es fa favo vore rece ce la di diso solu luci ción ón me metá táli lica ca.. Productos insolubles protegen el metal pasivandolos.
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Hay tres tipos generales de líneas en los diagramas de Pourbaix, cada una representa un equilibrio entre dos
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Este se lee en los ejes de X ,Y: En Y, se encuentra el potencial, el cual calculamos con la
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ECUACION DE EQUILIBRIO EQUILIB RIO DE REACCIONES QUÍMICAS SIN IONES H + (m = 0)
i M i = 0
i log( M i ) = log
K
a log( A) + b log( B )
=
log
K
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REACCIONES QUÍMICAS CON IONES H + (m i log( M i ) = log
K
a log( A) + b log( B) = log K + mpH A - Equ Equilil ib ibri ri o hom h omog ogéneo éneo
H CO
HCO
−
H
+
0)
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LEYES DEL EQUILIBRIO ELECTROQ EL ECTROQUIMICO UIMICO Se ha definido una reacción electroquímica electroquímica como aquella aquella en la que intervienen sustancias químicas Mi (moléculas neutras y/o iones), y cargas eléctricas libres o electrones.
−
i i + ne = 0 Esta ecuación expresa la condición de equilibrio termodinámico, la cual,
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REACCIONES ELECTROQUÍMICAS SIN IONES H + (m = 0)
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