Write the three chemical equations for the three equilibria that describe the fo

Question

Write the three chemical equations for the three equilibria that describe the formation of the three precipitates you listed in the table in question I. Interesting, we find that the exact same precipitate forms for a particular metal cation, regardless whether we use NaOh(aq), NH_3(aq), or Na_2CO_3(aq), as the precipitating reagent. And we name the resulting salt to reflect the anion that is present. That anion is (chemical formulation and charge) or (name). How can we explain the formation of that particular precipitate? Support your answer with chemical equation(s) showing why this anion is free in the solution.

Explanation / Answer

You need to mix two solutions, one containing the first part of the compound and the other containing the second part of the compound.

So for Al(OH)3 you need a soluble aluminium salt and a soluble hydroxide

When you look at solubility rules there are some patterns. Nitrates are all soluble as are alkali metal compounds.

So if we mix a solution of aluminium nitrate with say sodium hydroxide, aluminium hydroxide being insoluble will precipitate out and sodium nitrate remains in solution.
Al(NO3)3(aq) + 3NaOH(aq) ------> Al(OH)3(s) + 3NaNO3(aq).

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