Can anyone please help me with this equilibrium question?

Question

What do you understand by the term equilibrium constant?

How can the idea of an equilibrium constant be used to compare
(i) the strength of acids
(ii) the solubilities of salts

When a mixture of 1.00 mol of ethanoic acid and 1.00 mol of ethanol is allowed to reach equilibrium at room temperature,the equilibrium mixture contains 0.67 mol of ethyl ethanoate. Calculate the equilibrium constant kc at room temperature.

Predict qualitative effect on the amount of ethyl ethanoate in the equilibrium mixture if 2.00mol of ethanol and 1.00mol of ethanoic acid were used initially.

Answer 1

equilibrium constant simply describes which side of the chemical equation is going to be favored at a given temperature (i.e., high k, products are favored and vice versa).

the strength of an acid and the solubility of a salt both have to do with how much of a substance ionizes. this can be described by the chemical equations:

HX+H2O-->H+ + X-
OR
MX+H2O-->M+ + X-

both of these will happen to a certain extent, which can be used to find the equilibrium constant.

to do this, you need figure out the molarity of you mixtures, but then set up the equation

CH3-CH2-OH+HC2H3O2 --> CH3-CH2OOCH2-CH3+H2O

[ethyl ethanoate]
-------------------------
[ethanol][ethanoic acid]

increasing the amount of reactant will push the reaction to the right

Answer 2

It's hard to do a chem problem like this and type it up.
I wish we could post scanned images.


Here is a nice link with formulas. .
For acid strength

http://www.nyu.edu/classes/tuckerman/honors.chem/lectures/lecture_21/node7.html


One for solubility of salts

http://www.ualberta.ca/~jplambec/che/p101/p01191.htm