Titration and Oxidization. See attached file for full problem description.
The standard electrode potential (abbreviated Eo) is the measure of individual potential of any electrode at standard ambient conditions (temperature 298K, solutes at 1 M and gases at 1 bar).
The value of Eo is related to the equilibrium constant for the reaction. A positive value indicates that the equilibrium constant K is greater than 1, while a negative value of Eo says that it is less than 1. These potentials are widely used to predict the feasibility of redox processes. In general if the electrode potential for the reaction is positive, it is regarded as being feasible. However, it is not fool-proof for two reasons. Firstly, it is valid only under standard conditions, and second, it does not say anything about the rate of the reaction.
Remember that an oxidizing agent takes electrons (i.e. is reduced) and a reducing agent gives electrons (i.e. is oxidized). A good way to remember this is
LEO the lion goes GER
loss of electrons = oxidation
gain of electrons = reduction
For acids, the strength of the bond holding H to the molecule determines its strength. When that bond breaks, it breaks heterolytically. That means that ...
Using standard electrode potentials, arranging substances in order of decreasing oxidizing and reducing strength.