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13 Dec 2019

Lactic acid, which builds up in muscle tissue upon strenuous exercise, is partially dissociated in aqueous solution:

1. What is the equilibrium constant expression for Kc?

Kc = [C3H6O3]

Kc = 1[H+][C3H5Oâ3]

Kc = [H+][C3H5Oâ3]

Kc = [C3H5Oâ3][C3H6O3]

Kc = [C3H6O3][H+][C3H5Oâ3]

Kc = [H+][C3H5Oâ3][C3H6O3]

Kc = [H+]2[C3H5Oâ3][C3H6O3]

Kc = 1[C3H6O3]

2. What is the value of KC if the extent of dissociation in 0.100 M lactic acid is 3.68 % at 25 âC?

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Reid WolffLv2

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Ok this is a three part questions but I think i correctly answered#1 but i get lost after that..

1. An aqueous solution of ethyl acetate at room temperature has aninitial concentration of 0.15 M. Calculate the equilibriumconcentrations of ethyl acetate (CH3COOC2H5), ethanol (C2H5OH) andacetic acid if the equilibrium constant at this temperature is Kc =3.00.
CH3COOC2H5(aq) + H2O ? CH3COOH(aq) + C2H5OH(aq)

Here I set up an ice table an ice table and got a quadratic ofx^2+3.00x-.45=0
and i got x=.143.

Now here is what I get confused..

2) 2. A solution contains 0.15 M acetic acid and 0.15 ethanol. Ifthe equilibrium constant defined by the reaction in Problem 1 is Kc= 3.00, calculate the equilibrium concentrations of ethyl acetate,acetic acid and ethanol.

Im guessing you just do products/reactants?
so
[0.15 M] x [0.15 M] / [CH3COOC2H5] = 3.00
and CH3COO2H5 = .0075 M.

I think im right up to this point then im not sure what to donext?

then there's

3. A solution contains 0.01 M ethyl acetate, 0.10 M acetic acid and0.10 M ethanol. For the same equilibrium constant of 3.00,calculate the equilibrium concentrations of ethyl acetate, ethanol,and acetic acid in the solution.

orangemoose0

1) During strenuous exercise lactic acid builds up in muscle tissues. in a 1.00 M aquous solution, 2.94 % lactic acid is ionized. What is the value of Ka for lactic acid?

2) A 1.0g sample of solid U3O8 is placed in a rigid 1.500 L flask. 1.007 atm of chlorine gas, Cl2 (g) is added to the flask and is heated to 862 C. The equation for the reaction that takes place is given:

U3O8 + 3 Cl2 = 3 UO2Cl2 + O2

When the system is at equilibrium, what is the particial pressure of O2?

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	Kc = [C3H6O3]
	Kc = 1[H+][C3H5Oâ3]
	Kc = [H+][C3H5Oâ3]
	Kc = [C3H5Oâ3][C3H6O3]
	Kc = [C3H6O3][H+][C3H5Oâ3]
	Kc = [H+][C3H5Oâ3][C3H6O3]
	Kc = [H+]2[C3H5Oâ3][C3H6O3]
	Kc = 1[C3H6O3] 2. What is the value of KC if the extent of dissociation in 0.100 M lactic acid is 3.68 % at 25 âC?