  # 20. For each of the following equilibrium reactions and their associated K value, determine what species will be predominate at equilibrium.a. HC2H3O2(aq) + H2O(l) ⇄ H3O1+(aq) + C2H3O21-(aq) K=1.8x10-5b. Hydrochloric acid reacts with water to form the hydronium ion and the chloride ion. The K value is 1.8x1060c. Water reacts with water to form the hydronium ion and the hydroxide ion. The K value is 1.0x10-14d. NaC2H3O2(s) ⇄ Na1+(aq) + C2H3O21-(aq) K=2.5x1045

Question

20. For each of the following equilibrium reactions and their associated K value, determine what species
will be predominate at equilibrium.
a. HC2H3O2(aq) + H2O(l) ⇄ H3O1+
(aq) + C2H3O2
1-
(aq) K=1.8x10-5
b. Hydrochloric acid reacts with water to form the hydronium ion and the chloride ion. The K value
is 1.8x1060
c. Water reacts with water to form the hydronium ion and the hydroxide ion. The K value is
1.0x10-14
d. NaC2H3O2(s) ⇄ Na1+
(aq) + C2H3O2
1-
(aq) K=2.5x1045

check_circleExpert Solution
Step 1

The equilibrium constant is used to determine the extent of a reaction. The equilibrium constant (Keq) is greater than 103 for a fast reaction. The equilibrium constant (Keq) is smaller than 10-3 for the very slow reaction and for the reaction with moderate kinetic is in range of 103 to 10-3.

Step 2

For the reaction a. and c., the equilibrium constant is lower than 10-3. So, it is expected that the reactants are the predominating species. Ethanoic a...

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