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: Multiple Choice For each pair of standard cell potential and electron stoichiometry values below,…

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Q: Saturated Ag/AgCl reference || Ti³+ (0.0850 M), Ti²+ (0.0450 M) || Pt

A: given E Ag/Agcl = 0.199v E; Ti+3/Ti+2 =-0.369V Ti+3=0.0850M Ti+2=0.0450M find Ecell

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…

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Q: Calculate values for the galvanic cells desch (a) Cr³+ (aq) + Cl₂(g) = Cr₂0,2 (aq) + Cl(aq) V (b)…

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Q: The cell potential and the equilibrium.10 :constant at 298.15 K for the cell Pt, H2 (g)|H*(aq)(a =…

A: A Galvanic cell is made up of an anode and a cathode. Reduction reaction occurs at cathode whereas…

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: If the redox process is 3Cu(s) + FeCls(aq) = Fe(s) + 3CUCI(aq) and the (nonideal) solution molality…

A: Fe is getting reduced from +3 to 0 oxidation state (cathode) and Cu is getting oxidized from 0 to +1…

Q: A galvanic cell using Cut/Cu and Zn2+/Zn was set up at 329 K and the non-standard cell potential was…

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Q: (a) Draw the schematic diagram of the Galvanic cell made from the above with appropriate sign…

A: Redox reaction is that type of reaction where oxidation and reduction take place simultaneously.…

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

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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…

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Q: The standard cell potential (E°cei) of the reaction below is +0.126 V. The value of 4G° for the…

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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)|…

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Q: 11.)

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

Q: 10. State the direction in which the reaction proceeds and calculate the cell potential for: 2Cr*…

A: The electrode potential is the ability of an electrode to lose or gain electrons is known as…

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

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Q: Calculate the non-standard cell potential (in V) for the following reaction at 94.68 °C with the…

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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: The cell notation for the Galvanic cell is

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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: The following electrochemical cell was constructed at 298 K. C. Co(s)CoSO4j|NISO4NI(s) E° Co2*Co =…

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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: cell potential

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Q: Consider the voltaic cell with a standard cell potential of 2.89 V: Sr(s)|Sr²+ (1.0 M)||H* (1.0…

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Q: Pt(s) Br (aq) (x M) | Br21) || BrO3¯(aq) (0.43 M), H*(aq) (1.00 M) | Br2(1) | Pt(s)

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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…

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Q: Given the standard reduction potential for Zn2* (aq)/Zn(s) and Ag* (aq)/Ag(s) are -0.79 V and 0.80 V…

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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: A reaction 1 Ag*(aq) + H2 (g) → H* (aq) + Ag(s) Takes place in a cell and the standard cell…

A: Ag+ (aq) + 0.5 H2 (g) ==> H+(aq) + Ag(s)

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…

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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…

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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) +…

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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.