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Chapter 17: Q11P (page 428)

A solution of Sn²⁺is to be electrolyzed to reduce the Sn²⁺to Sn(s). Calculate the cathode potential (versus S.H.E.) needed to reduce $[{Sn}^{2 +}]$ to $1.0 脳 10^{- 8} M$ if no concentration polarization occurs. What would be the potential versus S.C.E. instead of S.H.E? Would the potential be more positive or more negative if concentration polarization occurred?

Short Answer

Expert verified

The potential of cathode versus S.H.E is $E (cathode) = - 0.378 V$

The potential of cathode versus S.C.E. is $E = - 0.619 V$

Step by step solution

01

Electrogravimetric Analysis

Separation along with the quantification of metals are mainly observed in electrogravimetric analysis.
Electrolysis of the analyte solution is done during this procedure.

02

Determine the lead lactate

The reaction of cathode

${Sn}^{2 +} + 2 e^{-} 鈬� Sn$

The standard reduction potential is $E 掳 = - 0.141 V$

The potential of cathode versus S.H.E is

$E (cathode) = E 掳 - \frac{0.05916}{2} 路 \log (\frac{1}{[{Sn}^{2 +}]}) E (cathode) = - 0.141 V - \frac{0.05916}{2} 路 \log (\frac{1}{1 脳 10^{- 8} M}) E (cathode) = - 0.378 V$

The potential of cathode versus S.C.E. is

$E = E (cathode) - E (S . C . E .) E = - 0.378 V - 0.241 V E = - 0.619 V$

The potential would be more negative if concentration polarization occurred.

The potential of cathode versus S.H.E is $E (cathode) = - 0.378 V$

The potential of cathode versus S.C.E. is $E = - 0.619 V$

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Most popular questions from this chapter

In a coulometric Karl Fischer water analysis, 25.00 mL of pure "dry" methanol required 4.23 C to generate enough I₂ to react with residual H₂O in the methanol. A suspension of 0.8476 g of finely ground polymeric material in 25.00 mL of the same "dry" methanol required 63.16 C. Find the wt %H₂O in the polymer.

$T i^{3 +}$ is to be generated in $0.10 M H C l O_{4}$ for coulometric reduction of azobenzene.

$\begin{aligned} {TiO}^{2 +} + 2 H^{+} + e^{鈭�} 鈬� {Ti}^{3 +} + H_{2} O E^{0} = 0 .100 V \\ 4 {Ti}^{3 +} + C_{6} H_{5} N = {NC}_{6} H_{5} + 4 H_{2} O 鈫� 2 C_{6} H_{5} {NH}_{2} + 4 {TiO}^{2 +} + 4 H^{+} \end{aligned}$

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 $1.00 c m^{2}$ . The rate of reduction of the azobenzene is 25.9nmol/s , and the resistance of the solution between the generator electrodes is $52.4 惟$ .

Calculate the current density $(A / m^{2})$ at the electrode surface. Use Table 17-1 to estimate the overpotential for $O_{2}$ liberation.
Calculate the cathode potential (versus S.H.E.) assuming that role="math" localid="1668356673323" $[Ti {O^{2 +}}_{surface}] = {[{TiO}^{2 +}]}_{bulk} = 0.050 M$ and $[T i^{3 +}]_{s u r f a c e} = 0.10 M$ .
Calculate the anode potential (versus S.H.E.).
What should the applied voltage be?

(a) How does the amperometric glucose monitor in Figure 7-12 work? b) Why is a mediator advantageous in the glucose monitor? c) How does the coulometric glucose monitor in Figure 17-14 work? (d) Why does the signal in the amperometric measurement depend on the temperature of the blood sample, whereas the signal in coulometry is independent of temperature? Do you expect the signal to increase or decrease with increasing temperature in amperometry?

(e) Glucose $(C_{6} H_{12} O_{6} $, F M 180.16)$ is present in normal human blood at a concentration near 1g/L How many microcoulombs are required for complete oxidation of glucose in 0.300 $渭 L$ of blood in a home glucose monitor if the concentration is 1.00g/L ?

Consider the cyclic voltammogram of the ${Co}^{3 +}$ compoundrole="math" localid="1663646447735" $Co {(B_{9} C_{2} H_{11})}_{2}^{-}$ . 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" $Co {(B_{9} C_{2} H_{11})}_{2}^{-}$ . [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.]

In $1 MN {NH}_{3} / 1 M {NH}_{4} CI$ solution, ${Cu}^{2 +}$ is reduced to ${Cu}^{+}$ near -0.3V(versus S.C.E.), and ${Cu}^{+}$ is reduced to $Cu (inHg)$ near 0.6V.

(a) Sketch a qualitative sampled current polarogram for a solution of ${Cu}^{+}$ .

(b) Sketch a polarogram for a solution of ${Cu}^{2 +}$ .

(c) Suppose that Pt, instead of Hg, were used as the working electrode. Which, if any, reduction potential would you expect to change?

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