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Consider the cyclic voltammogram of the Co3+compoundrole="math" localid="1663646447735" Co(B9C2H11)2- . Suggest a chemical reaction to account for each wave. Are the reactions reversible? How many electrons are involved in each step? Sketch the sampled current and square wave polarograms expected for this compound.

Cyclic voltammogramofrole="math" localid="1663646461802" Co(B9C2H11)2- . [Data from W. E. Geiger, Jr., W. L. Bowden, and N. El Murr, "An Electrochemical Study of the Protonation Site of the Cobaltocene Anion and of Cyclopentadienylcobalt(I) Dicarbollides," Inorg. Chem. 1979,18,2358.]

Short Answer

Expert verified

The chemical process was linked to waves in a cobalt ion cyclic voltammogram. Cobalt ion cyclic polarograms were sketched.

Step by step solution

01

Definition of Cyclic voltammetry

Cyclic voltammetry can be used to determine the redox behaviour of substances as well as the kinetics of electrode reactions. The cathodic wave dominates the upper section of a cyclic voltammogram. Anodic wave dominates the lowest section of the cyclic voltammogram.

02

Chemical reaction relates to waves in cyclic voltammogram of cobalt

Reaction sequence occurred in cyclic voltammetry is given as

CoIIIB9C2H112-CoIIB9C2H1122-CoIB9C2H1123-

From EpaandEpcit is obvious that two reduction reactions took place, as depicted above.

The reactions are reversiblebecause the anodic and cathodic peaks are the same. The current sampled is presented as


Figure 1

The polarogram of square wave is drawn as

Figure 2

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Most popular questions from this chapter

Ti3+ is to be generated in 0.10MHClO4 for coulometric reduction of azobenzene.

TiO2++2H++eTi3++H2OE0=0.100V4Ti3++C6H5N=NC6H5+4H2O2C6H5NH2+4TiO2++4H+

At the counter electrode, water is oxidized, and \(\mathrm{O}_{2}\) is liberated at a pressure of \(0.20\) bar. Both electrodes are made of smooth Pt, and each has a total surface area of 1.00cm2. The rate of reduction of the azobenzene is 25.9nmol/s , and the resistance of the solution between the generator electrodes is 52.4Ω.

  1. Calculate the current density (A/m2)at the electrode surface. Use Table 17-1 to estimate the overpotential for O2liberation.
  2. Calculate the cathode potential (versus S.H.E.) assuming that role="math" localid="1668356673323" [TiO2+surface]=[TiO2+]bulk=0.050Mand [Ti3+]surface=0.10M.
  3. Calculate the anode potential (versus S.H.E.).
  4. What should the applied voltage be?

The figure shows the behavior of Ptand Ag cathodes at whichreduction ofH3O+toH2(g)occurs. Explain why the two curves arenot superimposed.

Current versus voltage forPtand Agelectrodes in O2 -free, aqueous H2SO4

Adjusted topH3.2.

Explain how amperometric end-point detection in Figure17-9 operates.

What are the advantages of using a microelectrode for

voltametric measurements?

Coulometric titration of sulfite in wine. Sulfur dioxide is added to many foods as a preservative. In aqueous solution, the following species are in equilibrium:

Bisulfite reacts with aldehydes in food near neutral pH:


Sulfite is released from the adduct in 2MNaOH and can be analyzed by its reaction with I3- to give I-and sulfate. ExcessI3- must be present for quantitative reaction.

Here is a coulometric procedure for analysis of total sulfite in white wine. Total sulfite means all species in Reaction and the adduct in Reaction . We use white wine so that we can see the color of a starch-iodine end point.

1. Mix 9.00 mL of wine plus 0.8gNaOH and dilute to 10.00mL. The releases sulfite from its organic adducts.

2. Generate I3-at the working electrode (the anode) by passing a known current for a known time through the cell in Figure 17 - 10. The cell containsofacetate buffer () plus. In the cathode compartment, is reduced to H2+OH-. The frit retards diffusion of into the main compartment, where it would react with I3- to giveIO-.

3. Generate I3- at the anode with a current of for.

4. Inject 2.000mL of the wine/ solution into the cell, where the sulfite reacts with leaving excess.

5. Add of thiosulfate to consume by Reaction and leave excess thiosulfate.

6. Add starch indicator to the cell and generate freshI3- with a constant current of 10.0mA. A time of 131s was required to consume excess thiosulfate and reach the starch end point.

(a) In what pH range is each form of sulfurous acid predominant?

(b) Write balanced half-reactions for the anode and cathode.

(c) At pH 3.7, the dominant form of sulfurous acid isand the dominant form of sulfuric acid is HSO42-. Write balanced reactions between andand between I3-and HSO3-thiosulfate.

(d) Find the concentration of total sulfite in undiluted wine.

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