Ácido nítrico - Godetti - 08

ÁCIDO NÍTRICO ALUMNO: EZEQUIEL GODETTI PROFESOR: JUAN PABLO COLOTTA

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HISTORIA DEL CIDO NÍTRICO Se cuenta que los antiguos egipcios ya conocían el

ácido nítrico y que a partir del siglo VIII era usada por los alquimistas con el nombre de “aqua fortis” para separar la plata del oro. Hacia el año 1200 se fabricaba por calcinación del salitre (KNO3), o por tratamiento de dicha sal con vitriolos (mezclas de sulfatos), como alumbre y sulfato de cobre. En 1648, Glauber obtuvo ácido nítrico destilando nitrato de potasio con ácido sulfúrico. En 1776, Lavoisier demostró que contenía oxígeno. En 1784, Cavendish determinó su composición, que fue finalmente establecida por Gay Lussac en 1816.

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FÓRMULA Y ESTRUTURAS

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PROPIEDADES FÍSICAS DEL ÁCIDO NÍTRICO FÓRMULA: HNO3 ► ESTADO DE AGREGACIÓN (A PRESIÓN NORMAL Y  TEMPERATURA AMBIENTE): LÍQUIDO ► PUNTO DE FUSIÓN: -43 ºC ► PUNTO DE EBULLICIÓN: 86 ºC ► DENSIDAD: VARÍA SEGÚN LA CONCENTRACIÓN. A 70% m/m ES DE 1,41 g/cm3. SOLUBILIDAD EN AGUA: MISCIBLE EN TODAS ►

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PROPIEDADES QUÍMICAS 

ES UN ÁCIDO POCO ESTABLE, QUE SE DESCOMPONE SEGÚN LA SIGUIENTE REACCIÓN:

4 HNO3 

ES UN ÁCIDO MONOPRÓTICO FUERTE:

HNO3  

4 NO2 + O2 + 2H2O H+ + NO3-

ES UN FUERTE OXIDANTE. DISUELVE METALES COMO EL COBRE Y LA PLATA: 4

HNO3 + Cu

2 NO2 + Cu(NO3)2 +

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ESTADO NATURAL EL ÁCIDO NÍTRICO SE HALLA EN LA ATMÓSFERA LUEGO DE LAS TORMENTAS ELÉCTRICAS. SE ENCUENTRA EN LA NATURALEZA SOLAMENTE EN

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USOS GENERALES • •

SE UTILIZA EN LA FABRICACIÓN DE EXPLOSIVOS, PLÁSTICOS Y PINTURAS. SE EMPLEA TAMBIÉN PARA LA FABRICACIÓN DE ABONOS COMO POR

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CÓDIGO DE RIESGO

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ALMACENAMIENTO EL ÁCIDO NÍTRICO SE

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. NÍTRICO EN EL LABORATORIO SE HACE REACCIONAR NITRATO DE SODIO CON ÁCIDO SULFÚRICO CONCENTRADO, OBTENIÉNDOSE EL ÁCIDO NÍTRICO Y SULFATO DE SODIO:

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BTEN I N INDUSTRIAL SE UTILIZA EL MÉTODO DE OSTWALD (OXIDACIÓN DEL AMONÍACO). SE PUEDE DIVIDIR EL PROCESO

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DIAGRAMAS DE FLUJO

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ELABORACIÓN DE HNO3

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COMBUSTIÓN DEL AMONÍACO

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ABSORCIÓN ÁCIDA

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ABSORCIÓN ALCALINA

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