The potential of platinum versus saturated calomel electrode when polarized cathodically in deaerated H,SO4, pH-1.0 at 0.01 A/cm is-0.334 V and at 0.1 A/cm? it is – 0.364 V. Calculate B and io for discharge of H' on platinum in this solution.

Q: For the cell shown, the measured cell potential, Ecell, is -0.3507 V at 25 °C. Pt(s) | H, (g. 0.817…

A: Given cell notation is : Pt (s) |H2 (g, 0.817 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd (s)…

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A: (a) Given that a current of 7.5×104 A was flowed for a period of 24 h.

Q: Calculate the pH of cathode half-cell solution if the cell emf at 298 K is measured to be +0.684 V…

A: Given: Temperature  = 298 K Cell potential = +0.684 V Concentration of Zn2+      = 0.30 M Pressure…

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A: The chemical reaction corresponding to electroplating of Chromium is given as:Cr2O72- (aq) + 14 H+…

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Q: Enter your answer in the provided box. Consider the following electrochemical cell in, for which E°…

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Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

A: Anode half cell reaction: Cathode Half reaction: Overall reaction taking place is as follows:

Q: Consider the half reactions shown below with their associated standard reduction potentials at 25 ∘C…

A: First of all we have to calculate the cell potential of the overall reaction.

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Q: The standard oxidation potential of Ni/Ni2+ electrode is 0.3 V. If this is combined with a hydrogen…

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A: In Electrolytic cell , Oxidation takes place at anode and reduction takes place at cathode.

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Q: What is the pH of the solution in the cathode half-cell inFigure when PH2 = 1.0 atm, [Zn2+] in the…

A: SOLUTION: Step 1: The anodic half-reaction and cathodic half-reaction that occurred in the…

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A: To find: the percentage of copper, iron and silver in crude copper.

Q: A galvanic cell consists of Mg anode in a 1.0 M Mg(NO,), and Al cathode in a 1.0 M AI(NO,), solution…

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Q: calculate the potential of platinum elctrode emersed in a solution 0.0613 M in k4Fe(CN)6 and…

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Q: For the cell shown, the measured cell potential, ?cellEcell, is −0.3669 V at 25 °C.   Pt(s) |…

A:

Q: For the cell shown, the measured cell potential, ?cell, is −0.3723 V at 25 °C. Pt(s) | H2(g,0.773…

A: [ H+] = 0.091 M

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A: Introduction : given : Current=3 A  Volume = 0.50 L  Molarity=0.010M

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A:

Q: Question is attached

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Q: For the cell shown, the measured cell potential, Ecet, is -0.3715 V at 25 °C. P(s) | H,(g.0.857 atm)…

A: Given- Ecell =-0.3715V  PH2=0.857atm Concentration of Cd2+=1.00M

Q: An electrode Is prepared fromm liquid mercury in contct willh a salurated solution o mercury(1)…

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Q: Calculate the cell potential at 25 °C for the cell: A(s) I A²^(0.100 M) II B²^(1.0 x 10-5 M) I B(s)…

A: We have to tell which option is correct by finding Ecell

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A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A salt of each of the ions in Table is dissolvedin water. A Pt electrode is immersed in each…

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Q: For the cell shown, the measured cell potential, Ecell, is -0.3521 V at 25 °C. Pt(s) | H,(g, 0.785…

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Q: A cell consisting of a saturated calomel electrode and a lead ion electrode developed a potential of…

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Q: Calculate the theoretical potential at 25°C needed to initiate the deposition of copper from a…

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Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

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Q: Consider the following voltaic cell at 25°C: |3+ Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) |…

A: This problem is based on Nerst Equation For which, first we need to calculate the E°cell E°cell =…

Q: If the Standard Potential cell for the following AgI/Ag and I/I Was -0.152vand o, suv respectillery.…

A:

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Q: Given that standard reduction potentials at 298.15 K are E° Mg*2 /Mg = -2.37 V and E° Sn2*/Sn =…

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Q: 2H+(aq)+2e- -> H2(g) under standard conditions (pH=0.00, PH2=1 atm) this standard hydrogen…

A: SHE is the universal reference for reporting relative half-cell potentials. It can also be used as…

Q: For the cell shown, the measured cell potential, Ecell, is −0.3627 V at 25 °C. Pt(s) | H2(g,0.735…

A:

Q: Given the hypothetical metal samples a, B. and y were placed in an electrochemical cell as…

A: E°alpha = ? E°gamma = -2.38 V

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.