The main ingredient of vinegar is acetic acid (HAc) that will dissociate into acetate (Ac^-) and hydrogen ion

(H⁺) in water: HAc < = > Ac^- (aq) + H⁺ (aq) . K_{HAc(room temp)} = 1.8x10^-5. If [HAc]_t = 0.001M, [Ac^-]_t =

0.0001M, and [H⁺] _t = 2x10^-4M, is the solution/system at its equilibrium?

(a) The system is at equilibrium (b) The system will never reach an equilibrium

(c) The system is not at its equilibrium. The system will shift toward the reactants side to reach a new

equilibrium.

(d) The system is not at its equilibrium. The system will shift toward the products side to reach a new

equilibrium.

(e) Need more conditions to decide the system’s status.

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Mo solve this HAC SHAC Y KHAC equal the react... View the full answer