Question
In: Chemistry
5. For the titration of 50.00 mL of 0.0500 M Ce4+ with 0.1000 M Fe2+ in...
5. For the titration of 50.00 mL of 0.0500 M Ce4+ with 0.1000 M Fe2+ in the presence of 1 M H2SO4, please calculate the system potential while 3.00 mL of Fe2+ is added.
Ce4+ + e <==> Ce3+, E0 = + 1.44 V (in 1 M H2SO4)
Fe3+ + e <==> Fe2+, E0 = + 0.68 V (in 1 M H2SO4).
Answer is 1.49 V
5b) In the above titration, what's the electrode potential after 28.90 mL of Fe2+ is added?
Answer is 0.73 V.
Just wondering, how they got that?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
19. a. For the titration of 50.00 mL of 0.0500 M Fe2+ with 0.1000 M Ce4+...
19. a. For the titration of 50.00 mL of 0.0500 M Fe2+ with
0.1000 M Ce4+ in the presence of 1 M H2SO4, please calculate the
system potential after 2.25 mL of Ce4+ is added .
Ce4+ + e ÍÎ Ce3+, E0 = + 1.44 V (in 1M H2SO4)
Fe3+ + e ÍÎ Fe2+, E0 = + 0.68 V (in 1M H2SO4).
They got Esystem = 0.62 V.
b) For the same titration as in question (a), what’s
the system potential...
For the titration of 50.00 mL of a 0.1000 M solution of compound H2SO4 with a...
For the titration of 50.00 mL of
a 0.1000 M solution of compound H2SO4 with a
0.2000
M solution of compound NaOH in the following table.
For each titration, calculate the pH after the addition
of 0.00, 20.00, 25.00, 37.50,
50.00, and 60.00 mL of com-
pound NaOH.
Please explain all the steps.
For the titration of 50.00 mL of a 0.1000 M solution of compound ethylenediamine with a...
For the titration of 50.00 mL of
a 0.1000 M solution of compound ethylenediamine with a 0.2000
M solution of compound HCl in the following table.
For each titration, calculate the pH after the addition
of 0.00, 20.00, 25.00, 37.50,
50.00, and 60.00 mL of com-
pound HCl.
Please explain all the steps.
Do the calculations for the titration of 50.00 mL of a 0.1000 M solution of H2SO3...
Do the calculations for the titration of 50.00 mL of a 0.1000 M
solution of H2SO3 with a 0.2000 M solution of
NaOH. Calculate the pH after the addition of 0.00, 12.50, 25.00,
37.50, 50.00, and 60.00 mL of NaOH. Provide the answers in the
blanks below.
Ka1(H2SO3)=1.23×10-2;
Ka2(HSO3-)=6.60×10-8.
Consider the titration of 50.0 mL of 0.0500 M Cu+ with 0.1000 M Fe3+ to give...
Consider the titration of 50.0 mL of 0.0500 M Cu+ with 0.1000 M
Fe3+ to give Cu2+ and Fe2+ using Pt and standard H+/H2 reference
electrode to find the end point. The standard electrode potentials
are E0Cu+/Cu2+=0.161 V and E0Fe2+/Fe3+=0.767 V. Calculate the
actual electrode potential, E, at the following volumes of Cu2+ (i)
15, (ii) 25, and (iii) 26 mL
Question 7. Suppose titration of 100 ml 0.2 M Fe2+ with 0.5 M Ce4+ and indicator...
Question 7. Suppose titration of 100 ml 0.2 M
Fe2+ with 0.5 M Ce4+ and
indicator electrode is saturated calomel electrode
Formal potential for Fe3+ reduction:0.767, formal
potential for reduction of Ce4+: 1.70, potential for
saturated calomel electrode: 0.241
(3 pts) Write a balanced titration
reaction
(3 pts) Write two different half reactions for
the indicator electrode
(3 pts) Write two different Nernst equation
for the cell voltage
(3 pts) Calculate the E for the addition of 20
ml Ce4+...
5. In the titration of 15.00 mL of a 0.1000 M acetic acid solution by a...
5. In the titration of 15.00 mL of a 0.1000 M acetic acid
solution by a 0.1000 M NaOH solution, find the pH of the solution
being titrated when
a) 0.00 mL of NaOH has been added
b) 5.00 mL of NaOH has been added
c) 7.50 mL of NaOH has been added
d) 14.90 mL of NaOH has been added
e) 15.00 mL of NaOH has been added
f) 30.00 mL of NaOH has been added
For the titration of 25.00 mL of 0.1000 M HCl with 0.1000 M NaOH, calculate the...
For the titration of 25.00 mL of 0.1000 M HCl with 0.1000 M
NaOH, calculate the pH of the reaction mixture after each of the
following total volumes of base have been added to the original
solution. (Remember to take into account the change in total
volume.) Select a graph showing the titration curve for this
experiment. (a) 0 mL (b) 10.00 mL (c) 24.90 mL (d) 24.99 mL (e)
25.00 mL (f) 25.01 mL (g) 25.10 mL (h) 26.00...
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M...
Calculate the pH during the titration of 30.00 mL of 0.1000 M
KOH with 0.1000 M HBr solution after the following additions of
acid: (a) 5.00 mL (b) 29.50 mL (c) 36.00 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M...
Calculate the pH during the titration of 30.00 mL of 0.1000
M KOH with 0.1000 M HBr solution after the
following additions of acid:
(a) 8.00 mL
pH =
(b) 29.80 mL
pH =
(c) 38.00 mL
pH =
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