Laboratorio N°4
Universidad Nacional de Ingeniería
UNIVERSIDAD NACIONAL DE INGENIERÍA FACULTAD DE INGENIERÍA INDUSTRIAL Y DE SISTEMAS QUÌMICA INDUSTRIAL I EQUILIBRIO IONICO EN SOLUCIONES ACUOSAS
Cosquillo Quispe, Mijael 20142502K Garcés Timoteo, Timoteo, Antony 20141067I Huamanyauri Huamán, Renzo 20141033G Lima, junio 1 del 2015
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Laboratorio N°4
Universidad Nacional de Ingeniería
OBJETIVO
-
Realizar el estudio de un aspecto muy importante en el equilibrio heterogéneo; que se refiere a sales poco solubles.
-
Determinar el pH de soluciones acuosas empleando indicadores ácido-básicos y de soluciones que se hidrolizan.
-
Determinar la concentración de ácidos y bases por volumetría.
FUNDAMENTO TEÓRICO
SALES POCO SOLUBLES
Una de las aplicaciones más sencillas en un equilibrio químico es el hallar la concentración de una sal poco soluble. Por ejemplo, si tomamos la disociación del cloruro de plata en un medio acuoso, tenemos lo siguiente:
(−) (+) ⇆() Donde, al ser alcanzado el equilibrio, se llega que se ha disuelto sólo 1,67 x 10-5 mol.
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Laboratorio N°4
Universidad Nacional de Ingeniería
de distintas sales mediante expresiones cuantitativas. Para ello, procederemos a determinar la constante de producto de solubilidad:
[(−))]×[(+))] TITULACIÓN ÁCIDO-BASE Una valoración ácido-base (también llamada volumetría ácido-base, titulación ácido-base o valoración de neutralización) es una técnica o método de análisis cuantitativo muy usada, que permite conocer la concentración desconocida de una disolución de una sustancia que pueda actuar como ácido neutralizada por medio de una base de concentración concentr ación conocida, o bien sea una concentración de base desconocida neutralizada por una solución de ácido conocido .1 Es un tipo de valoración basada en una reacción ácido-base o reacción de neutralización entre el analito (la sustancia cuya concentración queremos conocer) y la sustancia valorante. El nombre volumetría hace referencia a la medida del volumen de las disoluciones empleadas, que nos permite calcular la concentración buscada. Aparte del cálculo de concentraciones, una valoración ácido-base permite conocer el grado de pureza de ciertas sustancias.
VIOLETA DE METILO
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Laboratorio N°4
Universidad Nacional de Ingeniería
En su forma pura, el tetrametilada aparece cristales de color azul-verde como brillantes que se funden a 137 ° C. Violeta de Metilo son solubles en agua, etanol, dietilenglicol y dipropilenglicol. Específicamente, violeta de metilo 6B es soluble en agua a 2,93% y 15: 21% soluble en etanol. Violeta de Metilo no debe confundirse con metilo azul o azul de metileno, otros dos colorantes.
Usos: Violeta de metilo 2B se utiliza como un indicador químico para el pH a prueba pr ueba los intervalos de pH de 0 a 1,0. En el ácido extremo de su rango de medición, toma un color amarillo. En alcalina, se convierte en violeta azulado. Violeta de Metilo puede proporcionarse como papel de prueba de pH, o se puede suministrar en forma de cristales puros y se disuelve en la muestra a ensayar. Violeta cristal se utiliza en el rango de 0 a 1,8, mientras que también se convierte de amarillo a azul. En la medicina, violeta de metilo 10B se conoce como c omo violeta de genciana y es el ingrediente in grediente activo en la tinción de Gram, que se utiliza para clasificar las bacterias. Violeta de genciana destruye las células, y se utiliza en desinfectantes des infectantes intensidad moderada externo. La violeta de
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Laboratorio N°4
Universidad Nacional de Ingeniería
Violeta de metilo también tiene la capacidad de unirse al ADN. Así que en las ciencias biomédicas, que se utiliza para los ensayos de viabilidad celular. La unión al ADN también pueden causar caus ar interrupciones interrup ciones en el proceso de replicación r eplicación de ADN, que pueden conducir a mutaciones y cáncer. Por lo general, se formula para su uso como una gama violeta de metilo como indicador de pH de una solución 0,01-0,05% m / v gama de cristal violeta como una solución de 0,02% w / v en agua.
ANARANJADO DE METILO
Naranja de metilo es un colorante azoderivado, con cambio de color de rojo a naranjaamarillo entre pH 3,1 y 4,4. El nombre del compuesto químico del indicador es sal sódica s ódica de ácido sulfónico de 4-Dimetilaminoazobenceno. Se empezó a usar como indicador químico en 1878. En la actualidad se registran muchas aplicaciones desde preparaciones farmacéuticas, colorante de teñido al 5%, y determinante de la alcalinidad del fango en procedimientos petroleros. También se aplica en citología en conjunto con la solución de Fuschin. También es llamado heliantina.
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Laboratorio N°4
MATERIALES
Experimento N°1
-
2 tubos de ensayo de 12x100.
-
1 Erlenmeyer de 250mL.
-
1 bureta de 25mL.
- NaCl, xM; K 2CrO4, 1M; AgNO3, 0.01N.
Experimento N°2
-
10 tubos de ensayo 13x100
-
1 pipeta de 10mL
-
1 probeta de 25mL
-
HCl, 0.1M
-
Violeta de metilo
-
Anaranjado de metilo
Experimento N°3
-
2 tubos de prueba 13x100
-
1 probeta de 25mL
Universidad Nacional de Ingeniería
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Laboratorio N°4
-
Universidad Nacional de Ingeniería
Anaranjado de metilo
Experimento N°4
-
Erlenmeyer de 250 ml
-
Pipeta
-
Ácido acético, CH3COOH(concentración desconocida)
- NaOH, 0.1 M -
Indicador anaranjado de Metilo
-
Fenoltaleína
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Laboratorio N°4
Universidad Nacional de Ingeniería
PROCEDIMIENTOS
Experimento N°1
-
Vierta 1mL de NaCl, xM, em um tubo de ensayo y 1mL de K 2CrO4 em outro. Anote el color de cada solución, añada unas gotas de AgNO3, 0.01N, a cada solución. Observe cuidadosamente lo ocurrido y tome nota.
-
Con una pipeta, vierta a un Erlenmeyer 10mL de solución de NaCl, xM. Añádale 2 gotas de cromato de potasio (20 gotas es aproximadamente 1cm3) cuya concentración está indicada en el frasco empleado.
-
Coloque en su bureta 10mL de AgNO3, 0.01N, y deje caer lentamente a la solución anterior (gota a gota). Agite convenientemente el tubo de ensayo.
Observará que inicialmente se produce un precipitado blanco. Continúe añadiendo gotas de AgNO3, agitando suavemente el tubo hasta que se produzca un cambio permanente de color; en este momento anote el volumen vo lumen gastado.
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Laboratorio N°4
Universidad Nacional de Ingeniería
Gotas de AgNO3, 0.01N
1mL
1mL
NaCl, xM
K 2CrO4, 1M
10mL AgNO3 0.01N
2 gotas K 2CrO4, 1M
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Laboratorio N°4
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Experimento N°2
-
Tome 5mL de HCl, 0.1M, em um tubo de ensayo de 13x100 que este limpio y seco. Como el ácido flerte se puede suponer completamente ionizado em esta solución diluída. Rotule este tubo como [H+]=0.1M.
-
Prepare 5mL de HCl, 0.01M, para lo cual tome 0.5mL de HCl, 0.1M, y pipetee 4.5mL de H2O destilada. Mezcle perfectamente esta nueva solución y rotule este tubo como [H+]=0.01M,
-
Prepare 5mL de HCl, 0.001M, para lo cual tome 0.5mL de HCl, 0.01M, y pipetee 4.5mL de H2O destilada. Mezcle perfectamente esta nueva solución y rotule este tubo como [H+]=0.001M.
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Prepare 5mL de HCl, 0.0001M, para lo cual tome 0.5mL de HCl, 0.001M, y pipetee 4.5mL de H2O destilada. Mezcle perfectamente esta nueva solución y rotule este tubo como [H+]=0.0001M.
-
Divida en dos partes el contenido de los tubos de concentración 0.1, 0.01, 0.001 y 0.0001 M. A la primera serie añada 2 gotas de violeta de metilo y a los de la segunda serie, añada 2 gotas de anaranjado de metilo.
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Laboratorio N°4
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En el primer tubo de ensayo se coloca 5 ml De HCl a 1 M
En el segundo tubo agregar 0.5 ml de la solucion del anterior tubo, luego pipetear 4.5ml 4.5ml de agua destilada
Realizar el mismo procedimiento para el 3er y 4to tubo
Experimento N°3
-
Mida 5mL de la solución ácida desconocida xM en su probeta.
-
Divídala en partes iguales en dos tubos pequeños.
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Añada 2 gotas de anaranjado de metilo a uno y 2 gotas de violeta de metilo al otro. Compare los colores de estas dos soluciones con los lo s colores de las otras 2 seres series
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Laboratorio N°4
Universidad Nacional de Ingeniería
comparar la solucion acida desconocida con anaranjado de metilo
comparar la solucion acida desconocida con violeta de metilo
observar la intensidad de color
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Laboratorio N°4
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Medir con una pipeta 10ml de CH3COOH xM verterlo en el erlemeyer y agregarle 2 gotas de anrrajando de metilo
Agregar dos gotas de anaranjado de metilo
Llenar en la bureta NaOH 0.1 M y dejarlo cer lentamente en el erlemeyer agitando este hasta que se note un cambio de color permanente.
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Laboratorio N°4
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CÁLCULOS
Experimento N°1 Ecuaciones:
(−) (+) ⇆() 1. 7 ×10− =() 2()+ ⇋ () 2. 2 ×10− Operamos:
[(−)]×[(+)]1.7×10− + − 1. 7 ×10−9………(1)
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Laboratorio N°4
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0.0101×10 0.01 Experimento N°2 Grupo de tubos: A
SUSTANCIA: HCl INDICADOR: VIOLETA DE METILO CONCENTRACIÓN (M) COLOR N° TUBO A1 0.1 Celeste claro 0.01 Azul claro A2 A3 0.001 Lila A4 Lila más claro que 3 0.0001 Grupo de tubos: B
SUSTANCIA: HCl INDICADOR: ANARANJADO DE METILO CONCENTRACIÓN CONCENTRACIÓN (M) (M ) COLOR N° TUBO B1 0.1 Rojo claro B2 0.01 Rojo más claro que 1 Rojo más claro que 2 B3 0.001 0.0001 B4 Naranja claro
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Laboratorio N°4
Universidad Nacional de Ingeniería
Experimento N°3
Tomando en cuenta los colores del contenido de los tubos de ensayo del experimento N°2 planteamos:
Grupo de tubos: A SUSTANCIA: HCl METILO INDICADOR: VIOLETA DE METILO N° TUBO COLOR A5 Entre el tubo A1 y A2
Grupo de tubos: B SUSTANCIA: HCl INDICADOR: ANARANJADO DE METILO N° TUBO
COLOR
B5
Entre el tubo A1 y A2
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Laboratorio N°4
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Grupo de tubos: B N° TUBO
B5 (el tubo del medio)
COLOR Rojo claro
pH 1-2
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Laboratorio N°4
Universidad Nacional de Ingeniería
CH3COOH ↔ H++CH3COOAl inicio
n
Cambio
-x
En el equil.
n-x
---
---
+x
+x
x
x
Donde: Ka=1.8x10-5 (tabla 15.5 (pg. 657)- Raymond Chang)
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Laboratorio N°4
Universidad Nacional de Ingeniería
OBSERVACIONES
Experimento N°1
Sustancia
Color
NaCl
Incoloro
K 2CrO4
Amarillo opáco
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Laboratorio N°4
Universidad Nacional de Ingeniería
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Laboratorio N°4
Universidad Nacional de Ingeniería
Experimento N°2
- Cuando se añade violeta de metilo al tubo de concentración 0.1 M (tubo A1) el color observado es celeste claro; con el tubo de concentración 0.01 M (tubo A2) el color es azul claro; con el tubo de concentración concentr ación 0.001 M (tubo A3) el color co lor es lila; finalmente con el tubo de concentración 0.0001M (tubo A4) el color observado es un lila más claro que el anterior.
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Laboratorio N°4
Universidad Nacional de Ingeniería
Experimento N°4
-
Al añadir gotas de anaranjado de metilo al CH3COOH la solución toma una
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Laboratorio N°4
Universidad Nacional de Ingeniería
5.- El punto final de un indicador no se produce a un pH específico, existe un intervalo de pH en el que se observa el punto final. En la práctica, esto significa que hay un margen en el número de gotas que se puede añadir de NaOH alCH3COOH sin que se afecten los cálculos
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Laboratorio N°4
Universidad Nacional de Ingeniería
=()×[()+ ] 2. 2 ×10− + √ 1.4 8×10−6………(2)
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Laboratorio N°4
Universidad Nacional de Ingeniería
4.- ¿Qué concentración de iones cloruro queda en la solución al momento que empieza a precipitar el
()
?
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Laboratorio N°4
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que solo estamos aumentando solvente, así aumentamos el volumen de la solución y como [] I.P. V, entonces la [] disminuye si el volumen aumenta.
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