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Química Analítica. Sesión 4. Método de Análisis Gravimétrico Ing. María King.
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El análisis gravimétrico : es una de las principales divisiones de la química analítica.
La cantidad de componente en un método gravimétrico : determina por medio de una pesada.
Para esto, la analita se separa físicamente de todos los demás componentes de la mezcla , así como la del solvente.
La precipitación es una técnica muy utilizada para separar la analita de las interferencias, otros métodos importantes de separación
se
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Principios Generales: Un método de análisis gravimétrico por lo general se basa en una reacción química como esta: a A
+ r R
Aa + Rr
En donde : a = Son las moléculas de analita A, que reaccionan con r moléculas de reactivo R.
El producto Aa Rr es por regla general una substancia débilmente soluble, que se puede puede pesar como como tal después después de secarla, secarla, o que se se puede calcinar para formar otro compuesto de composición conocida y después pesarlo.
Para disminuir la solubilidad del precipitado normalmente se añade un exceso de reactivo R.
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Para que un método gravimétrico sea gravimétrico sea satisfactorio , debe cumplir los siguientes requisitos:
1.- El proceso de separación debe ser completo, para que la cantidad de analita que no precipite no sea detectable detectable analíticamente analíticamente ( por lo general , al determinar un componente principal de una muestra macro es de 0.1 mg o menos). 2.- La substancia que se pesa debe tener una composición definida y debe ser puro o casi puro . Si esto, no se cumple se pueden obtener resultados erróneos. Para el analista el segundo requisito es el más m ás difícil de cumplir. cumplir.
Los errores debido a factores tales como la solubilidad del precipitado por lo general se pueden minimizar y rara vez causan un
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Estequiometria: En el procedimiento gravimétrico acostumbrado, se pesa el precipitado y a partir de este valor, se calcula el peso de la analita presente en la muestra analizada.
El porcentaje de analita ( A) es: %
A
Pesode PesodeA A Pesodel Pesodelamu amu estra
100
Pe PesodeA sodeA Pe PesodeP sodeP Fac Facto torgrav rgravimetrico . % A
Pe PesodeP sodeP Fac Facto torgrav rgravimetrico Pe Pesodela sodelamu muestra.
100
El factor gravimétrico aparece en forma natural natural si para resolver el
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Ejercicio 1 : Una muestra de 0.6025g de una sal de de cloro se disolvió en agua y el cloruro se precipitó adicionando un exceso de nitrato de plata . El precipitado de cloruro de plata se filtró, se lavó, se secó y se pesó, obteniéndose obteniéndose 0.7134 g.
Calcule el porcentaje de cloro ( Cl) en la muestra . La reacción es: Ag+ + Cl-
AgCl (s)
Sea g= gramos de Cl en la muestra. Una mol de Cl - da una mol AgCl. AgCl. Moles Cl = Moles AgCl AgCl Igualando las ecuaciones :
g 35.45 g / mol
0.7134 g 143.32 g / mol
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Con la ecuación: Cl
Cl
Peso Pesode delC lCl l Pesod Pesode elamu lamu estra
0.7134 g (35.45 g / mol / 143.32 g / mol ) 0.6025 gdesal gdesal
100
100 29.29.
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Ejercicio 2: Una muestra de 0.4852 g de un mineral de hierro se disolvió en ácido , el hierro se oxido al estado +3 y después se precipito en forma de óxido de hierro hidratado Fe 2O3 . xH2O , El precipitado se filtró, se lavó y se calcinó a Fe 2O3 el cual se encontró que pesaba 0. 2481 g .
Calcule el porcentaje de ( Fe) en la muestra. 2 Fe+3
Fe O . xH O
Fe O
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El % Fe se calcula utilizando la ecuación: A
% Fe
Peso Pesode deP P Fact Factorgrav orgravimetrico Peso Pesode dela lamu mu estra.
(0.2481 g 55.85 g / mol / 159.69 g / mol ) (1 / 2)
100
100 8 941
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Algunos Algu nos factores gravimétricos. Substancia pesada.
Substancia buscada.
AgCl
Cl
Factor.
Cl AgCl AgCl
Fe2O3
Fe
2 Fe
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Ejemplo 3: El fósforo fósforo contenido contenido en una muestra de de roca fosfórica que pesa 0.5428 g se precipita precipita en forma de MgNH 4PO4 .6H2O, y se calcina a Mg2P2O7 . Si el precipitado calcinado pesa 0.2234 g. Calcule:
A.- El porcentaje de P 2O5 en la muestra . B.- El por ciento de pureza expresado como P en lugar lugar de P 2O5. A-Porcentaje de P O
la muestr
esta dado
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Ejercicio 4 : Precipitación del hierro: Calcule la Molaridad del NH
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Formación y propiedades de los precipitados.
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