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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 AHIKayleigh (2.3k points)

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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 EdytheEwk100 (2.6k 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 LuzMccrary7 (2.5k points)

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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 TwylaArledge (1.6k 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 Lizzie32E683 (1.8k points)

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1 answer 47 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 Feb 3 in Chemical reactions by Beatris09Q13 (1.9k points)

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1 answer 46 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 Feb 3 in Chemical reactions by LeeAlder0448 (1.5k points)

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1 answer 49 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 EmilySulman6 (2.0k points)

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1 answer 47 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 JaneAlbrecht (1.9k points)

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1 answer 51 views

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 MorrisMcGahe (1.7k points)

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1 answer 53 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 LorenaReinha (1.8k points)

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1 answer 46 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 DarylBottoml (2.0k points)

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1 answer 10 views

Calculate the percent composition of phosphoric acid, H3PO4.

asked Feb 3 in Inorganic Chemistry by KrystleDHage (2.0k points)

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

asked Feb 3 in Inorganic Chemistry by OctavioDyaso (2.3k points)

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1 answer 57 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 Juliana93U49 (2.3k points)

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1 answer 54 views

Calculate the partition function for a system of 10 molecules of a monoatomic gas confined to a 1-dimensional box of length 1 nm at a temperature of 300 K using the classical and quantum mechanical methods. Then, compare the results obtained and explain the discrepancies observed.

asked Feb 3 in Physical Chemistry by ChloeBodnar (2.0k points)

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1 answer 45 views

Calculate the partition function (q) and the Helmholtz free energy (A) of an ideal gas containing 2 moles of particles at a temperature of 300 K, assuming the gas is in the canonical ensemble.

asked Feb 3 in Physical Chemistry by JanniePeek84 (2.0k points)

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1 answer 55 views

Calculate the overpotential of an electrochemical cell where Zinc metal is used as an anode and Copper metal as a cathode. The concentration of Zinc ions in the half-cell is 1 M and Copper ions in the half-cell is 0.1 M. The temperature of the system is 25°C. (Given: Standard Reduction Potentials - Zn²⁺ + 2e⁻ → Zn(s) = -0.76 V and Cu²⁺ + 2e⁻ → Cu(s) = +0.34 V)

asked Feb 3 in ElectroChemistry by jozzpfdeimmyapm (2.0k points)

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1 answer 39 views

Calculate the overpotential of a lead electrode in contact with a solution containing [Pb2+] = 0.001 M when the temperature is 298 K. Given that the standard potential of the Pb2+ / Pb electrode is -0.13 V and the exchange current density is 0.015 A/m2.

asked Feb 3 in ElectroChemistry by CletaF793120 (2.8k points)

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Calculate the overpotential for the reduction reaction of Ag+ to Ag on a silver electrode at 25°C with a current density of 0.5 A/cm2. The standard reduction potential of Ag+ to Ag is 0.799 V vs. the standard hydrogen electrode. The activation energy for this reaction is 65.0 kJ/mol, the transfer coefficient is 0.4 and the reaction order is 1.5.

asked Feb 3 in ElectroChemistry by MerissaGxv8 (1.7k points)

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