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Help with Chem Extra Credit

Submitted by Anonymous on 24 April 2005 - 9:35pm.

I really need this extrs credit so any help at all would we appreciated.

1.
In aqueous solution, acetic acid and water exist in equilibrium with their conjugate species. Write the balanced chemical equation that fully represents the equilibrium.

2.What is the equilibrium constant expression for the reaction from Question 1?

3.From your Part II data, calculate the value for the equilibrium constant (known as the dissociation constant Ka) for acetic acid, rounded to three significant figures.

Thanks in advance for any help!!

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Submitted by Anonymous on 25 April 2005 - 12:58pm.

1.
In aqueous solution, acetic acid and water exist in equilibrium with their conjugate species. Write the balanced chemical equation that fully represents the equilibrium.

HCH3C00 + H20 ----> CH3C00- + H30+

2.What is the equilibrium constant expression for the reaction from Question 1?

K= ([CH3COO-][H30+])/[HCH3C00]

H20 or solids are never included in K expressions...

3.From your Part II data, calculate the value for the equilibrium constant (known as the dissociation constant Ka) for acetic acid, rounded to three significant figures.

Now, for this, it seems you're not giving us a piece of data that we need. Acetic acid is a weak acid, so it won't ionize fully. You have to use the K expression given above, but we need the starting concentrations.

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