Consider the following reaction of Fe2+ with KMnO4. This is a classic potentiometric titration that was highlighted in t
Posted: Mon May 02, 2022 6:01 pm
Consider the following reaction of Fe2+ with KMnO4. This is
a classic potentiometric titration that was highlighted in the
text.
MnO4- +5Fe2+ +8H+ →Mn2+ +5Fe3+ +4H2O
400.0 mL of 3.75 mM Fe2+ were titrated with 20.0 mM
MnO4- at a fixed pH of 0.00 in 1 M H2SO4. A Pt indicating
electrode was used to measure cell potential using a calomel
reference electrode (E- = 0.241 V for the calomel
reference).
Given the following half reactions and standard reduction
potentials, calculate the cell voltage at titrant volumes of
1.0, and 16.0 mL of added 20.0 mM MnO4-.
MnO4- + 8 H+ + 5 e- → Mn2+ + 4 H2O
E◦ = 1.507 V in 1 M H2SO4
Fe3+ + e- → 5 Fe2+
E◦ = 0.68 V in
1 M H2SO4
a classic potentiometric titration that was highlighted in the
text.
MnO4- +5Fe2+ +8H+ →Mn2+ +5Fe3+ +4H2O
400.0 mL of 3.75 mM Fe2+ were titrated with 20.0 mM
MnO4- at a fixed pH of 0.00 in 1 M H2SO4. A Pt indicating
electrode was used to measure cell potential using a calomel
reference electrode (E- = 0.241 V for the calomel
reference).
Given the following half reactions and standard reduction
potentials, calculate the cell voltage at titrant volumes of
1.0, and 16.0 mL of added 20.0 mM MnO4-.
MnO4- + 8 H+ + 5 e- → Mn2+ + 4 H2O
E◦ = 1.507 V in 1 M H2SO4
Fe3+ + e- → 5 Fe2+
E◦ = 0.68 V in
1 M H2SO4