Acids and Bases - 3

Dissociations of weak acids and weak bases are considered reversible reactions.

• true

• false

K_a/K_{b =}

• [products]/[reactants]

• [reactants]/[products]

• [products]²/[reactants]

• [reactants]²/[products]

K_a/K_b<1 =

• the equilibrium favors the forward reaction thus more products are present

• considered a strong acid or strong base

• the equilibrium favors the reverse reaction thus more reactants are present

• considered a weak acid or weak base

K_a/K_b>1 =

• the equilibrium favors the forward reaction thus more products are present

• considered a strong acid or strong base

• the equilibrium favors the reverse reaction thus more reactants are present

• considered a weak acid or weak base

K_w =

• [H₃O⁺] [OH^-] [H₂O]

• ([H₃O⁺] [OH^-])/[H₂O]

• [H₂O] [OH^-]

• [H₃O⁺] [OH^-]

K_w =

• 1.0x10^-14, and is the equilibrium constant for water (water dissociation constant)

• 1.0x10^-7, and is the equilibrium constant for water (water dissociation constant)

• 1.0x10^-14, and is the concentration of OH^- under neutral conditions

• 1.0x10⁷, and is the concentration of H₃O⁺ under neutral conditions

[H₃O⁺]=[OH^-] =

• the solution is acidic

• the solution is neutral

• the solution is basic

[H₃O⁺]>[OH^-] =

• the solution is acidic

• the solution is neutral

• the solution is basic

[H₃O⁺]<[OH^-] =

• the solution is acidic

• the solution is neutral

• the solution is basic

pH =

• -log[H₃O⁺]

• log[H₃O⁺]

• -log[OH^-]

• -log([H₃O⁺][OH^-])