When acetic acid is dissolved in water, if reacts to form hydronium and acetate

Question

When acetic acid is dissolved in water, if reacts to form hydronium and acetate anions. This reaction will reach equilibrium, which favors heavily the left side of this equation. a) What can be said about the ration of acetic acid to acetate of equilibrium? b) If you were to add NaOH (sodium hydroxide) to this solution, how would this affect the equilibium and the proportion of acetic acid and acetate? c) If the concentration of acetic acid at equilibrium is determined to be 1. 0 M and the concentratyion of acetate and hydronium is 0. 010 M, what is the equilibrium constan tat 27 mdegreeC. (The concentration of water is ignored in this calculation!)

Explanation / Answer

a)

acetic acid is lareger compared to acetat, since

HA <-> H+ + A-

and it favours HA

b)

Yes it will, since H+ react with OH-, it will form omre acetate, HA lowers

c)

K = [H+][A-]/[HA]

K = (0.01)(0.01)/(1) = 0.0001

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