Recent questions in Chemistry

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Calculate the polarization resistance of a copper electrode in a 0.1 M copper sulfate solution at 25°C, given that the current density is 10 mA/cm² and the exchange current density is 0.1 mA/cm². The Tafel slope is 30 mV/decade.

asked 5 days ago in ElectroChemistry by MauricioMaj (630 points)

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Calculate the polarization potential in an electrochemical cell if the concentration of zinc ions in the anode compartment is 0.5 M, the concentration of copper(II) ions in the cathode compartment is 1.0 M, and the voltage of the cell is 1.1 V. The standard reduction potential of copper(II) ions is +0.34 V and the standard reduction potential of zinc ions is -0.76 V.

asked 5 days ago in ElectroChemistry by Ethel40B2651 (690 points)

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Calculate the polarization of a copper-silver galvanic cell in which the concentration of copper ions is 0.5 M, the concentration of silver ions is 0.1 M, and the cell is operating at a temperature of 25°C. The potential difference of the cell is measured to be 0.75 V.

asked 5 days ago in ElectroChemistry by TUOCaitlyn4 (490 points)

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Calculate the polarization of a copper electrode immersed in a 0.1 M CuSO4 solution at 25°C when it is coupled to a hydrogen electrode with a hydrogen pressure of 1 atm. Given that the standard reduction potential of Cu2+|Cu electrode is 0.34 V and the standard reduction potential of H+|H2 electrode is 0 V at 25°C.

asked 5 days ago in ElectroChemistry by EldonHyman82 (490 points)

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Calculate the polarization of a cell having an anode made of copper metal immersed in a 1.0 M Cu(NO3)2 solution and a cathode made of silver metal in a 1.0 M AgNO3 solution. Given that the potential of the copper electrode is -0.34 V and that of the silver electrode is 0.80 V. Also, assume that the current density is 0.1 A/cm² and that the temperature is 298 K.

asked 5 days ago in ElectroChemistry by Wally645704 (350 points)

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1 answer 34 views

Calculate the polarization in an electrochemical cell consisting of a zinc electrode and a copper electrode. The electrode potentials of zinc and copper are -0.76 V and +0.34 V, respectively. The resistance of the electrolyte solution between the electrodes is 10 ohms, and the current flowing through the cell is 0.5 A.

asked 5 days ago in ElectroChemistry by GabriellaJai (250 points)

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1 answer 37 views

Calculate the pH of a solution with a concentration of 0.01 M HCl.

asked 5 days ago in Chemical reactions by JuliMighell (410 points)

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1 answer 23 views

Calculate the pH of a buffer solution that contains 0.2 moles of acetic acid (CH3COOH) and 0.1 moles of sodium acetate (NaCH3COO) dissolved in one liter of solution. The dissociation constant of acetic acid is 1.8 x 10^-5.

asked 5 days ago in Chemical reactions by Genevieve973 (350 points)

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1 answer 25 views

Calculate the pH of a buffer solution made by combining equal volumes of 0.1 M acetic acid and 0.1 M sodium acetate. The dissociation constant of acetic acid is 1.8 × 10^-5.

asked 5 days ago in Chemical reactions by JaneenZepps (370 points)

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1 answer 30 views

Calculate the pH of a buffer solution consisting of 0.1 M acetic acid and 0.1 M sodium acetate, given that the dissociation constant (Ka) of acetic acid is 1.8x10^-5.

asked 5 days ago in Chemical reactions by SilkeVelasqu (450 points)

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Calculate the pH of a 0.2 M solution of acetic acid (Ka = 1.8 x 10^-5) at 25°C.

asked 5 days ago in Chemical reactions by MckinleyAlba (430 points)

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1 answer 32 views

Calculate the pH of a 0.2 M solution of acetic acid (CH3COOH) if the acid dissociation constant (Ka) of acetic acid is 1.8 × 10^-5.

asked 5 days ago in Chemical reactions by Hai18V559862 (450 points)

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1 answer 35 views

Calculate the pH of a 0.1 M solution of hydrochloric acid assuming complete dissociation. The acid dissociation constant (Ka) for HCl is 1.3 × 10^-6 at 25°C.

asked 5 days ago in Chemical reactions by DwightSparro (570 points)

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1 answer 30 views

Calculate the pH of a 0.1 M solution of hydrochloric acid (HCl) assuming complete dissociation of the acid in water, and identify if the solution is acidic, basic or neutral.

asked 5 days ago in Inorganic Chemistry by KeeshaSwaffo (470 points)

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1 answer 32 views

Calculate the pH of a 0.1 M solution of acetic acid with a dissociation constant (Ka) of 1.8 x 10^-5.

asked 5 days ago in Chemical reactions by Xavier496923 (230 points)

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1 answer 33 views

Calculate the pH of a 0.1 M solution of acetic acid (Ka = 1.8 x 10^-5).

asked 5 days ago in Chemical reactions by Newton78P742 (530 points)

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1 answer 37 views

Calculate the pH of a 0.1 M solution of acetic acid (CH3COOH) given that its dissociation constant Ka is 1.8x10^-5.

asked 5 days ago in Chemical reactions by TawnyaMorgan (350 points)

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1 answer 33 views

Calculate the percentage change in the concentration of reactants and products in a chemical equilibrium when the concentration of a common ion is increased by 0.1M. The equilibrium constant for the reaction is Kc = 1.5 x 10^-5 M at a certain temperature.

asked 5 days ago in Chemical equilibrium by GiselleRoot (530 points)

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1 answer 6 views

Calculate the percent composition of phosphoric acid, H3PO4.

asked 5 days ago in Inorganic Chemistry by MadgeLemberg (310 points)

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1 answer 29 views

Calculate the percent composition of copper sulfate pentahydrate (CuSO4 • 5H2O).

asked 5 days ago in Inorganic Chemistry by RoccoPreece (370 points)

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