The electrochemistry of metal complexes reflects the underlying chemical equilibria involved in their formation. A chemist can use the measured electrochemistry to determine the solubility product of a metal-ion complex, or vice versa. Calculate the electrode potential of the following half-cell involving the reduction of the Cu(I)-thiocyanate complex to copper metal, Cu(0).      CuSCN (sat’d), SCN– (0.0300M) | Cu The solubility product, KSP, of CuSCN is 1.77 x 10-11 = [Cu+][SCN–]

Q: What is the value of equilibrium constant, Keq, for the reaction between copper metal and iron (III)…

A: When iron(III) react with copper reaction take place then iron(III) is reduced to iron(II)  and…

Q: To study the effects of a weakly acidic medium on the rate of corrosion of a metal alloy, a student…

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Q: Calculate Eº, Gº, and K at 25 °C for the reaction: 2MnO4 (aq) + 4H+ (aq) + Cl₂(g) (Use: CIO3 to Cl₂…

A: The given reaction is - 4MnO4-aq  +  4H+aq  +  Cl2g   →   2Mn2+aq  +  2ClO3-aq  +  2H2O Oxidation -…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s)+Co2+(aq)↽−−⇀…

A: Given: The concentration of Ti2+ is 0.00180 M.The concentration of Co2+ is 0.813 M.The half-cell…

Q: The free energy change for the following reaction at 25 °C, when [Cr3+] = 4.86×10-3 M and [Cr3+] =…

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Q: Calculate the cell potential at 25°C for the cell             Fe(s) ∣ (Fe2+(0.100 M) ∣∣ Pd2+(1.0 ×…

A: The cell given is Fe(s) ∣ (Fe2+ (0.100 M) ∣∣ Pd2+ (1.0 X 10-5 M) ∣ Pd(s) Since the oxidation half is…

Q: Cobalt(II) ions (Co2*(aq)) react with 6 equivalents of a ligand (L) to from the complex cation…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Given-> [Cr2+] = 0.790 M [Fe2+] = 0.0190 M T = 25°C

Q: 5) Suppose a galvanic cell employs the following half-reactions: Ni²*(aq) + 2é Ni(s) Cr*(aq) + 3é >…

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Q: Balance the redox reaction between acidified potassium tetraoxomanganate and iron (ii)…

A: Balance the redox reaction between acidified potassium tetraoxomanganate and iron (ii)…

Q: (a) Corrosion is essentially an electrochemical phenomenon. Explain the reactions occurring during…

A: The redox reactions are the reactions, which involves the transfer of electrons in the reactants. In…

Q: An unknown metal, x, was placed in a solution of CuCl2(aq) and black solid appeared on the metal.…

A: The reactivity series is a series of metals, in order of reactivity from highest to lowest. It is…

Q: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Cr(s)+Fe+2 (aq )<==>  Cr+2 (aq)+Fe(s) [Cr+2] = 0.768 M [Fe+2] = 0.0170 M

Q: When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M,…

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Q: 99.5 nanomoles of an Os3+ complex are electrochemically Is the reduction product Os²+ or Os+?…

A: One mole of electrons have a charge of 96500 C. Given , moles of Os3+ reduced= 99.5 nano moles…

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.0 M NISO4 solution…

A: A question based on electrochemical cell that is to be accomplished.

Q: Consider Zn+2 (0.056 M) | Zn || TI*3 (9.86 x 102M) I TI* (0.048 M) Pt E° (Zn*2/ Zn) = -0.763 V E°…

A: On the left half of the cell representation there is anode and on the right it is the cathode. Ecell…

Q: Sketch the galvanic element diagram consisting of the following two half-elements Cu2O | Cu, in…

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Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.5 M NISO4 solution…

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Q: A student adds ammonia to a copper half-cell and forms the addition product [Cu(NH3)4]2+ which…

A: Electrochemistry deals with chemical changes and electricity. A galvanic cell contains two…

Q: 28. After electrolyzing a certain concentration of copper sulfate solution with an inert electrode…

A: Given the solution taken for electrolysis is copper sulfate, CuSO4. Moles of [Cu2(OH)2CO3] added to…

Q: oxidation state

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Q: A solution of Cu* is undergoing a redox titration by the addition of Ce**. The standard reduction…

A: Given, Ce4++e-⇌Ce3+              E°=+1.72VCu2++e-⇌Cu+               E°=+0.161 V

Q: Ferrocene is an organometallic complex that contains iron sandwiched between two five-membered…

A: Cyclic voltammetry is an electrochemical technique to find the reduction and oxidation potentials of…

Q: Write a balanced net ionic equation to show why the solubility of Fe(OH)2(s) increases in the…

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Q: Given that standard reduction potentials at 298.15 K are E° Ag+ /Ag = +0.800 V and E° Cu?"/Cu =…

A: When Ag foil is soaked into Cu(NO3)2 solution, for Ag to dissolve the reaction involved would be:…

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.2 M NISO4 solution…

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Q: 1. (a) K₂Cr2O7 reacts with Fe(II) to produce Cr(III) and Fe(III) in acid medium. Write down the…

A: Reduction potential for Chromium system is 1.33 V and for iron it is 0.77 V. So, Cr2O72- will…

Q: Calculate Kf for the iron thiocyanate equilibrium if the concentration of Fe3+ is 0.011M, SCN- ion…

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Q: A Cu electrode is immersed in a solution that is 1.00 Min [Cu(NH3)4]2+ and 1.00 M in NH3. When the…

A: The process is : 2H+(aq)+Cu(s)+NH3(aq)→H2(g)+[Cu(NH3)4]2+ The Nernst equation is,…

Q: Ni content of the steel can be determined by the precipitation gravimetric analysis. For this…

A: The complex of Ni forming is Ni(DMG)2

Q: A Cu electrode is immersed in a solution that is 1.00 M in [Cu(NH3)4]2+ and 1.00 M in NH3. When the…

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Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe"(aq) +…

A: Answer:- This question is answered by using the simple concept of calculation of equilibrium…

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.1 M NiSO4 solution…

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Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co2+(aq) +…

A: Given:  Co2+(aq) + Cu(s)   ------------>  Co(s) + Cu2+(aq)

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s)+Co2+(aq)↽−−⇀…

A: The given red-ox reaction is  Ti(s) + Co2+(aq) Ti2+(aq) + Co(s)Given: The concentration of Ti2+,…

Q: The formation constants at 25°C for Fe(CN)64– and Fe(EDTA)2– are 1.00x1037 and 2.10x1014,…

A: We have Fe^2+(aq) + 6CN^- (aq) => Fe(CN)64-(aq) Kf = 1.00*10^37 Fe^2+(aq) + EDTA^4-(aq) =>…

Q: Write a balanced net ionic equation to show why the solubility of Cu(OH)2(s) increases in the…

A: Cu(OH)2 is a sparingly soluble salt, i.e- it has lower solubility in water.When it is dissolved in…