If a precipitation reaction occurs when a solution of one species is added to a solution of the other, enter the formula, including the state, of the soluble product. If there is no reaction, enter the formula and state of all ions in solution, separate by comma.
Al2(SO4)3(aq) + Mg(ClO4)2(aq) →
same procedure. see below.
To determine the soluble product or if no reaction occurs, we need to refer to the solubility rules. These rules outline which compounds are soluble and insoluble in water.
For the given reaction:
Al2(SO4)3(aq) + Mg(ClO4)2(aq)
We will break down the compounds into their respective ions:
Al2(SO4)3 dissociates into 2 Al^3+ ions and 3 SO4^2- ions.
Mg(ClO4)2 dissociates into 1 Mg^2+ ion and 2 ClO4^- ions.
Using the solubility rules:
1. All nitrates (NO3^-) are soluble.
2. Most sulfates (SO4^2-) are soluble, except for those of calcium (Ca^2+), strontium (Sr^2+), barium (Ba^2+), lead (Pb^2+), and silver (Ag^+).
3. Most chlorides (Cl-) are soluble, except for those of silver (Ag^+), lead (Pb^2+), and mercury (Hg2^2+).
4. Most perchlorates (ClO4-) are soluble.
From the solubility rules, we can identify that both Al^3+ and ClO4^- ions are soluble. However, Mg^2+ and SO4^2- ions are also soluble according to the solubility rules. So, no reaction occurs in this case.
Therefore, the formula and state of all ions in solution, separated by a comma, is:
Al^3+(aq), SO4^2-(aq), Mg^2+(aq), ClO4^-(aq)