Question

Write net ionic equations for the formation of (a) a precipitate when solutions of magnesium nitrate and potassium hydroxide are mixed. (b) two different precipitates when solutions of silver(I) sulfate and barium chloride are mixed.

Short answer

Question: Determine the net ionic equations for the following scenarios: (a) Magnesium nitrate is mixed with potassium hydroxide, and a precipitate forms. Write the net ionic equation for the formation of this precipitate. (b) Silver(I) sulfate is mixed with barium chloride, and two precipitates form. Write net ionic equations for the formation of these precipitates. Answer: (a) The net ionic equation for the formation of magnesium hydroxide precipitate is: Mg^{2+}(aq) + 2OH^-(aq) → Mg(OH)2(s) (b) The net ionic equations for the formation of silver chloride and barium sulfate precipitates are: - 2Ag^+(aq) + 2Cl^-(aq) → 2AgCl(s) (Silver chloride precipitate) - Ba^{2+}(aq) + SO4^{2-}(aq) → BaSO4(s) (Barium sulfate precipitate)

Step-by-step solution

Balanced chemical equation

Write the balanced chemical equation for the reaction between magnesium nitrate and potassium hydroxide. Mg(NO3)2(aq) + 2KOH(aq) → Mg(OH)2(s) + 2KNO3(aq)

Identify possible precipitates

Using solubility rules, identify possible precipitates. In this case, magnesium hydroxide (Mg(OH)2) is the precipitate as it is insoluble in water.

Write the ionic equation

Write the ionic equation for the reaction: Mg^{2+}(aq) + 2NO3^-(aq) + 2K^+(aq) + 2OH^-(aq) → Mg(OH)2(s) + 2K^+(aq) + 2NO3^-(aq)

Write the net ionic equation

Write the net ionic equation by eliminating spectator ions (2NO3^-(aq) and 2K^+(aq)): Mg^{2+}(aq) + 2OH^-(aq) → Mg(OH)2(s) (B) Silver(I) sulfate and barium chloride

Balanced chemical equation

Write the balanced chemical equation for the reaction between silver(I) sulfate and barium chloride. Ag2SO4(aq) + BaCl2(aq) → 2AgCl(s) + BaSO4(s)

Identify possible precipitates

Using solubility rules, identify possible precipitates. In this case, silver chloride (AgCl) and barium sulfate (BaSO4) are the precipitates since they are insoluble in water.

Write the ionic equation

Write the ionic equation for the reaction: 2Ag^+(aq) + SO4^{2-}(aq) + Ba^{2+}(aq) + 2Cl^-(aq) → 2AgCl(s) + BaSO4(s)

Write the net ionic equation for the first precipitate

Write the net ionic equation for the formation of silver chloride by eliminating spectator ions (SO4^{2-}(aq) and Ba^{2+}(aq)): 2Ag^+(aq) + 2Cl^-(aq) → 2AgCl(s)

Write the net ionic equation for the second precipitate

Write the net ionic equation for the formation of barium sulfate by eliminating spectator ions (2Ag^+(aq) and 2Cl^-(aq)): Ba^{2+}(aq) + SO4^{2-}(aq) → BaSO4(s)