Acetic acid has a Ka of 1.75x10^-5. The weak acid approximation (for this class) would be allowed for which of the following initial concentrations of acetic acid? a. 1.75E^-6
b. 1.75E^-5
c. 0.00175
d. 0.0175
e. 0.175

e. 0.175

Explanation:

The equilibrium constant of a reaction is the value of its reaction quotient when at equilibrium. The equilibrium concentration of a product or reactant depends on the initial concentrations and equilibrium constant of the reactants and products.

The weak acid approximation depends on the initial concentration and equilibrium constant (). The farther the initial concentration and equilibrium constant are from one another, the more likely the approximation would be valid.

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation: