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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 Feb 3 in ElectroChemistry by Alyce51K2334 (550 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 Feb 3 in ElectroChemistry by TomasKersey7 (530 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 Feb 3 in ElectroChemistry by TrishaSutton (430 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 Feb 3 in ElectroChemistry by MohammadVazq (470 points)

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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 Feb 3 in ElectroChemistry by MargeneT1167 (410 points)

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

asked Feb 3 in Chemical reactions by KassieNewbig (390 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 Feb 3 in Chemical reactions by Valeria6199 (370 points)

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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 Feb 3 in Chemical reactions by LazaroR32061 (270 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 Feb 3 in Chemical reactions by YongSheehy6 (550 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 Feb 3 in Chemical reactions by StacyMaple9 (590 points)

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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 Feb 3 in Chemical reactions by JerroldRayfo (530 points)

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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 Feb 3 in Chemical reactions by EdwinCamidge (410 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 Feb 3 in Inorganic Chemistry by MamieGreenwe (350 points)

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1 answer 33 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 Feb 3 in Chemical reactions by NganCollocot (310 points)

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

asked Feb 3 in Chemical reactions by CarltonMunz3 (210 points)

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1 answer 38 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 Feb 3 in Chemical reactions by SallyLarocqu (450 points)

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1 answer 34 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 Feb 3 in Chemical equilibrium by LonnaGatlin5 (540 points)

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1 answer 7 views

Calculate the percent composition of phosphoric acid, H3PO4.

asked Feb 3 in Inorganic Chemistry by DesireePitt (390 points)

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1 answer 30 views

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

asked Feb 3 in Inorganic Chemistry by JennaCottle (310 points)

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1 answer 38 views

Calculate the partition function for a system of 300 molecules occupying an energy level of 10 J at a temperature of 300 K using the classical harmonic oscillator model.

asked Feb 3 in Physical Chemistry by ValorieDemar (310 points)

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