Acid Base Equilibrium. Write equilibrium expressions for the following. HC 2 H 3 O 2(aq) + H 2 O (l) ⇌ C 2 H 3 O 2 - (aq) + H 3 O + (aq) NH 3(aq) + H 2 O (l) ⇌ NH 4 + (aq) + OH - (aq). Strong vs Weak Acid.
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A 0.25 M solution of acetic acid reacts with water to form hydronium and acetate ions. If the equilibrium constant (Ka) is 1.8x10-5
A 0.15 M solution of ammonia reacts with water to form hydroxide and ammonium ions. If the equilibrium constant (Kb) is 1.8x10-5
H2O(l) + H2O(l) ⇌ H3O+(aq) + OH-(aq)
% ionization = [H3O+]eq/ [HA]initial x 100%
Salts that Form Neutral Solutions
If Ka> Kb, pH will be acidic
Ka< Kb, pH will be basic
Ka= Kb, pH will be neutral
A 275 mL sample of 0.25 M methyl amine is
titrated with 0.35 M nitric acid. Calculate
A 120 mL sample of 0.50 M formic acid is titrated with 0.15 M calcium hydroxide. Determine
and 0.50 mol of sodium acetate in 2.0 L of water.
Calculate a) the pH of the original buffer.
b) the pH after the addition of 0.10 mol of OH- ignoring any volume changes.
c) the pH after the addition of 0.10 mol of H3O+ ignoring any volume changes.