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Chemistry
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13 Dec 2019

Calculate the value of the equilibrium constant (Kc) for thereaction of acetic acid with sodium hydroxide.

Concentration = .83M HC2H3O2 and .5 M NaOH

HC2H3O2 + NaOH --> CH3CO2- + Na+ + H2O

Kc = .83 / (.83)(.5) = 2.0

Is this right and what is the significance of the value of Kc inthis case?

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Lelia Lubowitz
Lelia LubowitzLv2
17 Dec 2019

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Related questions

The equilibrium constant Kc for thereaction

C <---> D + E

is 7.70*10^-5, the initial composition of thereaction mixture is [C] = [D] = [E] = 1.5*10^-3 M. What is theequilibrium concentration of C,D,E?

The value of Kc for the reaction of acetic acid with ethanol is 3.4 at 25∘C:

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Ethyl acetate

Calculate the number of moles of all reactants and products in an equilibrium mixture prepared by mixing 1.00 mol of acetic acid and 10.00 mol of ethanol.

Calculate the pH after 0.014 mole of NaOH is added to 1.00 L of each of the four solutions. (Assume that all solutions are at 25°C.)

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