Calculate the standard cell potential for the reaction below and note whether the reaction is spontaneous under standard standard standard state conditions (6 points) Mg(s) + Ni²+ (aq) = Mg² + (aq) + Ni(s) Ni²+ (aq) + 2e- = Ni(s) -0.257V Mg²+ (aq) + 2e- = mg(s) -2.372V Provide answers in the following order: Substance being oxidized  Substance being reduced Calculated cell potential  Is the reaction spontaneous or non-spontaneous

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: Dear student, according to Bartleby guidelines, we can only solve the first question if multiple…

Q: A galvanic cell Cr(s)|Cr2+(aq) || Sn2+(aq)|Sn(s) is constructed using a completely immersed Cr…

A: Cr(s) is undergoing oxidation to Cr2+(aq) and Sn2+(aq) undergoing reduction to Sn(s) half-reactions…

Q: A galvanic cell consists of an Mg electrode in 1 M Mg(NO3)2 solution, and an Ag electrode in 1 M…

A:

Q: The II, III, and IV oxidation states of Mn are related thermodynamically by these equilibria in acid…

A: Given:Determine the standard electrode potential of the couple.The standard electrode potential…

Q: 1 Using these metal ion/metal standard reduction potentials: Cd2+ (aq)|Cd(s): -0.38 V: Zn2+…

A: Given, Cu2+(aq) + Cd(s) ➝ Cd2+(aq) + Cu(s) Standard cell potential (E°cell) = ? Standard reduction…

Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A:

Q: Consider the following reaction and standard cell potential: N2H4(aq) + O2(g) → N2(g) + 2H2O(I)…

A: N2H4(aq) + O2(g) -----> N2(g) + 2H2O(l) Standard cell potential (E°cell) = 1.56 V = 1.56…

Q: The standard cell potential for the reaction provided below is-2.431V, calculate the cell potential…

A:

Q: Calculate the cell potential, at 298 K, for the following reaction under the conditions given. Pb(s)…

A: The cell reaction taking place is given as, => Pb (s) + Fe2+ (aq, 0.0100 M) ------> Pb2+ (aq,…

Q: Calculate the value of the cell potential, Ecell, for this reactión at 29 [1"] = 0.0050 M, and [Br2]…

A: In the given cell reaction, iodine is reduced and bromine is oxidized. The standard oxidation…

Q: Consider these metal ion/metal standard reduction potentials Cd2+(aq)|Cd(s): -0.40 V;…

A: ->The species which has high reduction potential that tends to reduce itself and oxidize other…

Q: Consider these metal ion/metal standard reduction potentials Cd2+ (aq)| Cd(s): -0.40 V; Zn2+ (aq)|…

A:

Q: 11.)

A: We have given that From representation of the cell reaction  Oxidation half reaction :  Zn(s)…

Q: For the cell shown, the measured cell potential, Ecell, is –0.3669 V at 25 °C. Pt(s) | H, (g, 0.713…

A:

Q: Calculate the standard cell potential, Ecell, for this reaction at 298 K. 12 (s) + 2 Br (aq) --> 21…

A: Equilibrium constant (Kc) = 1.1 × 10-18  Temperature (T) = 298 k  Standard cell potential (E°) = ? •…

Q: a. Ba (s) + Mn²+ (aq) -> Ba²+ (aq) + Mn (s) b. Pb (s) + Cu²+ (aq) → Pb²+ (aq) + Cu (s) c. 2Ce4+ (aq)…

A: To determine standard cell potential (E°cell) following formula is used :  E°cell = (E°RP) cathode -…

Q: onsider the following half-cells:    (1)  AgCl(s) | Ag(s), Cl–(aq)                      E°red =…

A: The given half cells are:    (1)  AgCl(s) | Ag(s), Cl–(aq)                       E°red = +0.22 V…

Q: Calculate the potential (emf) of a working galvanic cell that is based on these two half cells and…

A: Given: Cr3+(aq)  →  Cr2+(aq)       E°(Cr3+/Cr2+) = −0.40 V IO−(aq)  →  I2(aq)            E°(…

Q: Determine the standard cell potential, E° cell, for a galvanic cell that employs the half-reactions…

A: Given: Reduction potential of MnO4-/Mn2+ half reaction is 1.506 V. Reduction potential of…

Q: Pt(s) Sn2+ (0.0016 M), Sn+ (0.10 M) Fe+ (0.11 M), Fe2+ (0.0065 M) Pt(s) E "Sn+/Sn² = 0.154 V EreT =…

A: Given: The reaction at cathode Fe3++e-→Fe2+.............E0Fe3+Fe2+=0.771 V The reaction at anode…

Q: 9. If a redox reaction has oxidation potential of 1.5V and reduction potential of -0.5V, will the…

A: 9) Given :- Oxidation potential = E0oxidation = 1.5 V  Reduction potential = E0reduction = -0.5 V…

Q: What is the cell potential, Ecell, at 298K for the following cell under non-standard conditions when…

A:

Q: Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard…

A: The process of breaking the electrolyte by applying an electric charge to its constituent ions is…

Q: Zn cation has 0.76 V as it's standard reduction potential.the cell potential is measured for the…

A: 0.0203 mol/L

Q: Determine the Cell potential (volts, V) of a spontaneous galvanic cell rxn under the conditions; 2…

A:

Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A: Nernst equation is used to calculate so many entities, like the solubility product, pH , equilibrium…

Q: Use the appropriate standard reduction potentials below to determine the equilibrium constant at 206…

A:

Q: Given the following standard electrode potentals: Ag°(aq) + e¯ = Ag(s) N,(g) + 5H°(aq) + 4e° =…

A: Consider the given values as; Ag+ aq + e- ⇌ Ag s…

Q: Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F°(aq) 2.870V 2+ Pb"(aq) +…

A:

Q: Consider the following half-cells:    (1)  AgCl(s) | Ag(s), Cl–(aq)                E°red = +0.22 V…

A: In this question, we will Identify which combination produces Highest voltage.  How we can identify…

Q: What is the expected standard cell potential for the following unbalanced reaction under basic…

A: In the given cell reaction, ferrous ion is oxidized to ferric ion. The oxidation state of iron…

Q: Chemistry 19.10.-Calculate the standard potential, „E°, for this reaction from its AG° value.…

A: Given, X(s) + Y4+(aq) → X4+(aq) + Y(s)  ∆Go = 31.0 KJ = 31000 J

Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.