18 Questions
According to the Nernst equation, what is the relationship between the electrode potential (E) and the molar concentration of metal ions [M+n]?
E is directly proportional to the logarithm of [M+n]
How does the increase in hydrogen ion concentration ([H+]) affect the oxidation potential of oxygenated systems?
Increases the oxidation potential
At what pH value will both iodide (I-) and bromide (Br-) ions be oxidized to their respective halogens (I2 and Br2)?
pH = 3
What is the effect of adding mercuric chloride (HgCl2) to the I2/I- redox system?
It increases the ratio of [I2] / [I-], thereby increasing the electrode potential
How does the common ion effect affect the ratio of [MnO4-] / [Mn2+] in a MnSO4 solution?
It decreases the ratio, thereby decreasing the oxidation potential
What is the purpose of increasing the difference in oxidation potential between the MnO4-/Mn2+ redox couple?
To improve the endpoint detection in the titration of Mn2+ with MnO4-
What happens to the ratio [Fe3+]/[Fe2+] when F- or PO43- is added to the Fe3+/Fe2+ system?
Decrease
What effect does Ferrocyanide have on the oxidation potential of the Ferri/Ferro system?
Increase
What type of charge may a Pt electrode acquire when the system is reducing?
Negative charge
What do F ions do when added to the Fe/Fe system?
Complex with Fe2+; decrease oxidation potential
Which factor affects the oxidation potential according to the Common ion effect?
$H_2SO_4$
What does the Zimmerman reagent contain?
$KNO_3, H_2SO_4, HCl$
What is the relationship between an oxidizing agent and its conjugate reducing agent?
The stronger the oxidizing agent, the weaker its conjugate reducing agent, and vice versa.
When a platinum (Pt) electrode is placed in a redox system like Fe³⁺/Fe²⁺, what does a positive charge on the electrode indicate?
The system is oxidizing because it gains electrons from the Pt electrode.
What is the relationship between the oxidation potential (E) and the concentrations of the oxidized and reduced species in a redox system?
When [oxidized] = [reduced], E = E°.
What is the significance of the standard oxidation potential (E°) in a redox system?
It represents the oxidation potential when the concentrations of the oxidized and reduced species are equal.
Which statement best describes the order of oxidizing and reducing agents based on their oxidation potentials?
The most powerful oxidizing agents have the highest positive oxidation potentials, and the most powerful reducing agents have the lowest negative oxidation potentials.
What is the purpose of using a reference electrode, such as the Normal Hydrogen Electrode (NHE), in a redox system?
To measure the relative potential of the redox system against a known reference.
Learn about oxidation potential in an analytical chemistry system containing oxidants and reductants. Understand the relationship between oxidants and their conjugate reductants, as well as the concept of equilibrium in redox reactions.
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