what are the products formed, including the correct phases, when mixing together aqueous solutions of…

what are the products formed, including the correct phases, when mixing together aqueous solutions of magnesium nitrate and sodium hydroxide?\n○ mg(oh)₂(s) + 2 nano₃(s)\n○ mg(oh)₂(s) + 2 na⁺(aq) + 2 no₃⁻(aq)\n○ mg(oh)₂(aq) + 2 nano₃(aq)\n○ mg²⁺(aq) + 2 no₃⁻(aq) + 2 na⁺(aq) + 2 oh⁻(aq)

what are the products formed, including the correct phases, when mixing together aqueous solutions of magnesium nitrate and sodium hydroxide?\n○ mg(oh)₂(s) + 2 nano₃(s)\n○ mg(oh)₂(s) + 2 na⁺(aq) + 2 no₃⁻(aq)\n○ mg(oh)₂(aq) + 2 nano₃(aq)\n○ mg²⁺(aq) + 2 no₃⁻(aq) + 2 na⁺(aq) + 2 oh⁻(aq)

Answer

Explanation:

Step1: Write the chemical reaction

The reaction between magnesium nitrate ($\ce{Mg(NO3)2}$) and sodium hydroxide ($\ce{NaOH}$) is a double - displacement reaction. The general form of a double - displacement reaction is $\ce{AB + CD\rightarrow AD+CB}$. For $\ce{Mg(NO3)2(aq)+2NaOH(aq)\rightarrow Mg(OH)2(s) + 2NaNO3(aq)}$

Step2: Analyze the solubility

According to solubility rules:

  • Hydroxide salts ($\ce{OH^{-}}$) are generally insoluble. Magnesium hydroxide ($\ce{Mg(OH)2}$) is insoluble in water, so it forms a solid (precipitate), denoted as (s).
  • Nitrate salts ($\ce{NO3^{-}}$) are generally soluble. Sodium nitrate ($\ce{NaNO3}$) is soluble in water, so it exists in the aqueous state, denoted as (aq). Sodium ions ($\ce{Na^{+}}$) and nitrate ions ($\ce{NO3^{-}}$) are spectator ions in the net ionic equation, but in the full ionic equation, they are in the aqueous state.

Answer:

$\ce{Mg(OH)2(s)+2NaNO3(aq)}$