Final answer:
The reaction of dilute potassium hydroxide with barium chloride forms a precipitate of barium hydroxide and a solution of potassium chloride. The net ionic equation for this reaction is Ba2+(aq) + 2OH-(aq) → Ba(OH)2(s), omitting the spectator ions K+ and Cl-.
Step-by-step explanation:
When dilute potassium hydroxide is added to a solution of barium chloride, a double displacement reaction occurs, forming barium hydroxide, a precipitate, and potassium chloride in solution. The molecular equation for this reaction is:
BaCl2(aq) + 2KOH(aq) → Ba(OH)2(s) + 2KCl(aq)
The complete ionic equation shows all strong electrolytes as ions:
Ba2+(aq) + 2Cl−(aq) + 2K+(aq) + 2OH−(aq) → Ba(OH)2(s) + 2K+(aq) + 2Cl−(aq)
By removing the spectator ions, which are the potassium ions (K+) and the chloride ions (Cl−), we can write the net ionic equation:
Ba2+(aq) + 2OH−(aq) → Ba(OH)2(s)