ANALISIS QUIMICO CUANTITATIVO TITULACIONES DE NEUTRALIZACION
OSNAIDER BERRÍO RAMOS HOREMY GONZALEZ HERRERA
PRESENTADO A: HANNAEL MODESTO OJEDA MORENO
LABORATORIO DE QUÍMICA ANALÍTICA QUÍMICAY FARMACIA UNIVERSIDAD DEL ATLÁNTICO BARRANQUILLA / ATLANTICO 2011
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CONTENIDO
1. INTRODUCCION 2. OBJETIVOS 2.1 OBJETIVO GENERAL 2.2 OBJETIVO ESPECIFICO 3. METODOLOGIA 3.1 MUESTREO 3.1.1 MUESTREO GLOBAL 3.1.2 MUESTRA DE LABORATORIO 3.1.3 PORCIONES DE PRUEBA 3.2 PROCEDIMIENTO PARA LA RECOLECCION DE DATOS 3.3 PROCESAMIENTO Y ANALISIS DE DATOS 3.3.1 PROCESAMIENTO DE DATOS 3.3.2 ANALISIS Y RESULTADOS 4. CONCLUSION 5. BIBLIOGRAFIA 6. ANEXOS
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1.
INTRODUCCION
El ácido clorhídrico HCl se usa frecuentemente en los análisis volumétricos de neutralización porque sus soluciones diluidas son estables y porque se puede utilizar en presencia de la mayoría de los cationes sin que ocurran reacciones de precipitación; se usa ampliamente para valoraciones de bases, las disoluciones diluidas son estables por tiempos definidos y no dan lugares a reacciones de precipitación con muchos cationes. Hay 2 tipos de valorizaciones:
1. Según tipo de reacción 2. Según tipo de valorización (directa e indirecta) La primera a su vez se subdivide en:
Protometría
Red/ox
Precipitación
Formación de complejos
Las reacciones de Protometría también presentan presentan subdivisiones, alcalimetría y acidimetría.
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2.
OBJETIVOS
2.1 OBJETIVO GENERAL:
Analizar e identificar mezclas de carbonatos o bases fuertes.
2.2 OBJETIVOS ESPECIFICOS
Conocer los componentes de cada una de las muestras tomadas para estandarizar. Realizar los cálculos estadísticos para cada una de las muestras analizadas. Obtener habilidad en la obtención de titulaciones y determinación de la alcalinidad.
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3
METODOLOGIA
3.1 Muestreo
3.1.1 Muestreo global Preparación de la solución patrón de HCl. 0.1M Estandarización de la solución de HCl 0.1M con Na 2CO3 Análisis de mezclas de carbonatos y bases fuertes. 3.1.2 Muestra de laboratorio: Alícuotas de 25 mL que se tomaron para ser estandarizadas. 5 muestras problemas 3.1.3 Porciones de prueba muestras problemas Fenolftaleína Naranja de metilo.
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3.2 PROCEDIMIENTO PARA LA L A RECOLECCION DE DATOS.
DETERMINACION DE LA ALCALINIDAD EN MEZCLAS DE CARBONATO
Estandarización de solución de HCl 0.1 M
Calculo de la concentración del HCL
Se tomaron alícuotas de 25 mL de cada una de las muestras
Se pasaron a Erlenmeyer para ser valoradas.
Se agregaron 3 gotas del indicador fenolftaleina a cada muestra y se titulo con la solución de HCl 0.1M hasta el viraje de fucsia a incoloro.
Luego a esta misma muestra se agregaron 3 gotas del indicador
Se siguió titulando con HCl 0.1 M hasta el viraje de amarillo a naranja – rojizo.
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3.3 PROCESAMIENTO Y ANALISIS DE DATOS.
3.3.1PROCESAMIENTO DE DATOS:
Se nos es entregado cinco muestras diferentes a las cuales se le deben realizar ciertas pruebas para así determinar los componentes de estas, para esto nos basamos en los siguientes criterios con los cuales se llegara al objetivo:
SOLUCION
CRITERIO
NaOH Na2CO3 NaHCO3 NaOH + Na2CO3 Na2CO3 + NaHCO3
VFEN > VNAR ≈ 0 VFEN ≈ VNAR VFEN ≈ 0 < VNAR VFEN > VNAR VFEN < VNAR
NOTA: en cualquier disolución no pueden existir más que dos de estos componentes en concentraciones apreciables, ya que tendrá lugar a una reacción para eliminar el tercero.
COMPOSICION DE CADA UNA DE LAS MUESTRAS:
WARDER
Muestra 1:
Volumen gastado 1(fenolftaleína) = 18.5mL Volumen gastado 2 (naranja de metil) = 10.2mL
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Muestra 4 :
Volumen gastado 1 (fenolftaleína) = 9.3mL Volumen gastado 2 (naranja de metil) = 30.3mL Como V1 < V2 entonces la muestra 4es: Na 2CO3 + NaHCO3
Muestra 5:
Volumen gastado 1 (fenolftaleína) = 19.1mL Volumen gastado 2 (naranja de metil) = 0mL Como V1 > V2 ≈ 0 entonces la muestra 5 es: NaOH WINKLER
Muestra 6:
Volumen gastado 1 (fenolftaleína) = 8.7mL Volumen gastado 2 (naranja de metil) = 27.6mL
Muestra 7:
Volumen gastado 1 (fenolftaleína) = 27.1mL Volumen gastado 2 (naranja de metil) = 31.0mL
PREPARACION DE LA SOLUCION PATRON DE HCl
Concentración inicial del HCl:
37% p/p
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25 mL x 25 mL x
̅
M -4 S = 4.95x10 CV = 0.3764
CALCULOS DE LAS CONCENTRACIONES DE LAS MUESTRAS
Muestra 1: NaOH + Na2CO3
8.3mL HCl
10.2 mL HCl Fen; 18.5 ml
NaOH
10.2 mL HCl Nm; 10.2ml
= (V1 – V2) = 18.5 mL – 10.2 mL = 8.3 mL
PM =
40g / mol
X 100% =0.1746% NaOH Na2CO3 =
2 (V2) = 2 (22mL) = 44 mL
PM = 106g / mol.
=0.5687%p/v Na CO
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Muestra 3: NaHCO 3
HCl 23.1mL
= 1,0206%p/v NaHCO3
Muestra 4 : Na 2CO3 + NaHCO3
HCl
HCl
Fen: 9.3mL Na2CO3
HCl nm: 30.3mL
= (V2 – V1) = 30.3mL – 9.3mL = 21mL.
PM =
106g / mol.
=0.2593%p/v Na2CO3
NaHCO3=
2(V1) = 2(9.3) = 18.6mL.
PM =
84 g / mol.
=0.8218%p/v NaHCO3
Muestra 5 : NaOH
HCl, Fen :19.1mL
nm: 0mL
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[ ] MUESTRA 1 GRUPO
[ ]MUESTRA2
[ ]MUESTRA3
[ ] MUESTRA 4
[ ]MUESTRA5
M NaOH
M Na2CO3
M Na2CO3
M NaHCO3
M Na2CO3
M NaHCO3
M NaOH
1
0,05220
0,05080
0,05100
0,1289
0,0244
0,1123
0,09817
3
0,0391
0,0492
0,0475
0,1170
0,0220
0,1012
0,1888
7
0,0436
0,0536
0,0478
0,1215
0,0244
0,1104
0,1004
9
0,0413 0, 0413
0,0541
0,0491
0,1221
0,02376
0,0689
0,09932
APLICACIÓN DE DE LA ESTADISTICA ESTADISTICA PARA LA MUESTRA MUESTRA 1 SOLO NaOH NaOH Para hallar la media se procede de la siguiente manera:
= ∑
MEDIA
=0.04405
Para hallar la desviación estándar (S), y el coeficiente de variación (Cv), se realiza el siguiente procedimiento: Desviación estándar (S) es igual a:
∑ S = √
S = 0.0057
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= 0,0519
Desviación estándar (S) es igual a:
∑ S = √
S = 0,00232 RSD =
RSD = O.044 CV= RSD * 100
Cv= 4.4
APLICACIÓN DE DE LA ESTADISTICA ESTADISTICA PARA LA MUESTRA MUESTRA 2: Na2CO3 Para hallar la media se procede de la siguiente manera:
= ∑
MEDIA
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∑ S = √
S = 0.0016 RSD =
RSD = 0.013 Cv= RSD * 100
Cv= 1.3
APLICACIÓN DE DE LA ESTADISTICA ESTADISTICA LA MUESTRA 4 SOLO Na2CO3 Para hallar la media se procede de la siguiente manera:
= ∑
MEDIA
=0.02364
La mediana (Me) es igual a: 0,7708
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Desviación estándar (S) es igual a:
∑ S = √
S = 0.00113 RSD =
= DESVIACIÓN ESTÁNDAR RELATIVA
RSD = 0.011 Cv= RSD * 100
Cv= 1.1
APLICACIÓN DE DE LA PRUEBA DE DE DIXON PARA LA MUESTRA MUESTRA 5 NaOH Para hallar la media se procede de la siguiente manera:
= ∑
=0.0992
MEDIA
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CONCLUSION
De la practica ya concluida queda claro que antes de llevar a cabo una titulación hay que tener en cuenta todas las clases de errores que se puede generar durante la realización de la misma, para así minimizarlos y obtener los mejores resultados en el análisis, ya que por este método de titulación volumétrica se pude conocer de manera sencilla rápida y práctica la concentración del analito, con ayuda de distintos indicadores ácido-base que permiten la aplicación de este método, siendo posible ver el cambio de color en el punto final final de la reacción, de esta manera gracias gracias a este método de valoración se pudo comprobar experimentalmente el porcentaje de alcalinidad de ciertas muestras que se nos fue entregado en el laboratorio.
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BIBLIOGRAFIA
SKOOG, Douglas; WEST; Donald; HOLLER; James. Química Analítica. Sexta Edición. Ed. McGraw – Hill. Pág. 52 – 94
Diccionario de Química. DAINTITH, John. Edit. Norma 1985.