b) In the development of a method for the determination of formic acid by neutralization volumetry, the pH was calculated as a function of the addition of NaOH for the titration of 25.00 mL of 0.1280 mol/L formic acid with NaOH standardized with concentration of 0.0670 mol/L. With reference to this titration curve, determine the pH of the solution after the addition of 5.00 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two places after the comma and show your calculations. c) Based on the table below, indicate which indicators could be used to determine the end point of this titration. TABELA 14-1Alguns Indicadores Ácido/Base ImportantesNome ComumAzul de timolFaixa de Transição de pHMudança de CortTipo de Indicador;1,2-2,81,65§8,96$V-A8,0-9,62,9 4,0A-AzAmarelo de metilaAlaranjado de metilaVerde de bromocresolV-A3,1-4,43,8-5,44,2-6,35,2-6,86,2-7,63,4654,66$5,00$6,1257,10$7,81$V-LA-AzV-AA-PVermelho de metilaPúrpura de bromocresolAzul de bromotimolA-AzA-VVermelho fenol6,8-8,47,6-9,28,3–10,09,3-10,510-12Púrpura de cresolFenolftaleinaA-P-VI-AzI-ATimolftaleinaAmarelo de alizarina GG*Em força iõnica de 0,1.1Az = azul; I = incolor; L = laranja; P = púrpura; V = vermelho; A = amarelo.(1) Tipo ácido: HIn + H,0 = H,0* + In-: (2) Tipo básico: In + H,0 = InH* + OH-.SPara a reação InH* + H,0 = H,0* + In.Para uma discussão desses efeitos, ver H. A. Latinen e W. E. Harris, Chemical Analysis, 2. ed., p. 48-51. Nova York: McGraw-Hill, 1975.

Answer- Ka=1.70x10-4. for Formic acid.

Answered: determination of formic acid by…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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b) In the development of a method for the determination of formic acid by neutralization volumetry, the pH was calculated as a function of the addition of NaOH for the titration of 25.00 mL of 0.1280 mol/L formic acid with NaOH standardized with concentration of 0.0670 mol/L. With reference to this titration curve, determine the pH of the solution after the addition of 5.00 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two places after the comma and show your calculations. c) Based on the table below, indicate which indicators could be used to determine the end point of this titration.

TABELA 14-1
Alguns Indicadores Ácido/Base Importantes
Nome Comum
Azul de timol
Faixa de Transição de pH
Mudança de Cort
Tipo de Indicador;
1,2-2,8
1,65§
8,96$
V-A
8,0-9,6
2,9 4,0
A-Az
Amarelo de metila
Alaranjado de metila
Verde de bromocresol
V-A
3,1-4,4
3,8-5,4
4,2-6,3
5,2-6,8
6,2-7,6
3,465
4,66$
5,00$
6,125
7,10$
7,81$
V-L
A-Az
V-A
A-P
Vermelho de metila
Púrpura de bromocresol
Azul de bromotimol
A-Az
A-V
Vermelho fenol
6,8-8,4
7,6-9,2
8,3–10,0
9,3-10,5
10-12
Púrpura de cresol
Fenolftaleina
A-P
-V
I-Az
I-A
Timolftaleina
Amarelo de alizarina GG
*Em força iõnica de 0,1.
1Az = azul; I = incolor; L = laranja; P = púrpura; V = vermelho; A = amarelo.
(1) Tipo ácido: HIn + H,0 = H,0* + In-: (2) Tipo básico: In + H,0 = InH* + OH-.
SPara a reação InH* + H,0 = H,0* + In.
Para uma discussão desses efeitos, ver H. A. Latinen e W. E. Harris, Chemical Analysis, 2. ed., p. 48-51. Nova York: McGraw-Hill, 1975.

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