The Nernst Equation Write the Nernst equation2 for the reaction Cu2+ (aq) + Zn (s)  Zn2+ (aq) + Cu (s) Let activity of Cu2+ equal to 1 and change the activity of Zn2+ such that Q is in the range  0.001 to +0.001. Select different values of Q and for each calculate Ecell. Plot E_"cell" -E_"cell" ^ө vs ln Q. What is the effect of Q (that is the activity) on E_"cell" -E_"cell" ^ө ? Is the effect the same at higher and lower values of Q? what is the largest value of the absolute difference between cell potential and standard cell potential, |E_"cell" -E_"cell" ^ө |? What do you expect the graph will look like for different number of electron transferred ( )? And why?

Q: Use the nernst equation to calculate the cell potentials of the following cells at 298K:…

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Q: How much time in minutes would it take to deposit 4.77 grams of X (MW = 41.53 g/mol) on a cathode in…

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Q: Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: 2Cr³+…

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Q: The cell potential of the following electrochemical cell depends on the gold concentration in the…

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Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr2* (aq) is…

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Q: Using the Nernst equation calculate the cell voltage for: Fe(s) + Cd²+(aq) → Fe2+(aq) + Cd(s) when…

A: Given- [Fe2+] = 0.19 M [Cd2+] = 2.0 M E°cell = -0.44 V E°cell = -0.40 V

Q: A concentration cell similar to the one shown is composed of two Mn electrodes and solutions of…

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Q: 1. Use the calculation of E° to determine which of the following reaction is spontaneous under…

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Q: <Electrochemistry For Practice 20.7 - Enhanced - with Feedback E° ( V) Au3+ (aq) +3e-Au(s) 1.50 Ag+…

A: First calculate the standard electrode potential and use that value to calculate the equilibrium…

Q: Calculate Ecell for an electrochemical cell at room temperature (298K) based on the two…

A: Nernst expression correlates temperature, concentration and cell potential together. These are…

Q: Select the correct cell notation for the following reaction, which is setup as a cell with a…

A: Oxidation (loss of electrons) occurs at anode and reduction (gain of electrons) takes place at…

Q: To calculate the cell potential of electrochemical cells under nondtandard conditions, Nernst…

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Q: Write the Nernst equation2 for the reaction Cu2+ (aq) + Zn (s) ® Zn2+ (aq) + Cu (s)

A: Nernst equation is used to determine the emf of the cell. Nernst equation:

Q: Half-Reaction Mg²+ + 2e¯ → Mg Nat+eNa E°(V) -2.37 -2.71 2Na+ (aq) + Mg(s) = 2Na(s) + Mg²+ (aq)…

A: Given that, a reaction is 2Na+ aq + Mg s ⇌ 2Na s + Mg2+ aq. And, Half-reaction E0(V) Mg2+ +…

Q: Ell -0.201 V for the reaction 3Pt(s)+12C1 (aq) + 2NO₁ (aq) +8H(aq) → 3PtCl(aq) + 2NO(g) + 4H₂O(1)…

A: From E°cell we can calculate individual half cell potentials.

Q: 4) For the Zn|Zn²*(1M)||Cu²*(1M)|Cu battery discussed in class (6°=1.1V), answer the following…

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Q: Calculate the pH of the cathode compartment for the following reaction given & cell = 3.01 V when…

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Q: What is the potential (in V) of the following electrochemical cell? Sn(s) | Sn²+(1.00 M) ||…

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Q: Calculate the pH ôf thể cathode compartment for the following reaction given Ecell = 3.01 V when Cr*…

A: In a given question , we have to find out the pH of a solution in a cathode compartment.

Q: The  Eocell for the following reaction is 0.96V. Given this, what is the voltage of a cell that…

A: To find the voltage of the given cell, we can use the Nernst equation:   Ecell = E°cell - (RT/nF)…

Q: Calculate the value of the potential for the following electrochemical cell under the conditions…

A: Answer:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

Q: Calculate the value of Eºcell for the following reaction as written: HINT: Identify what is being…

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Q: Calculate the cell potential for the following concentration cell at 25 °C.…

A: Given Concentration cell Ni(s)|Ni(NO3)2(0.00522 M)|| Ni(NO3)2(3.07 M)| Ni(s)              Ni…

Q: Example 9. In an electrolysis experiment, a current was passed for 5 hours through two cells…

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Q: 31. Assuming SATP conditions, (a) calculate the standard cell potential of an aluminum-nickel(II)…

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Q: Given the following galvanic cell shown with initial concentrations at 25°C, calculate Ecell after…

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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.