Taking into account the definition of net ionic equation, a precipitate of SrSO₄ is formed when When an aqueous solution of strontium chloride is added to an aqueous solution of potassium sulfate, and the net ionic equation is:
Sr⁺²(aq) + SO₄⁻²(aq) → SrSO₄(s)
The net ionic equation is a chemical equation for a reaction that lists only the species that participate in the reaction.
In other words, an ionic equation is a chemical equation where electrolytes in aqueous solution are written as dissociated ions. Usually this is a salt dissolved in water.
The balanced equation will be:
SrCl₂(aq) + K₂SO₄(aq) → 2KCl(aq) + SrSO₄(s)
where (aq) means aqueous and (s) solid.
Taking into account that:
All Cl⁻, Br⁻ and I⁻ salts are soluble. All alkali metal salts are soluble. (for example, Li, Na, K salts)
Most sulfates are soluble, with the exception of Ba²⁺, Pb²⁺, Ag⁺ and Sr²⁺ sulfates.
The total ionic equation in separated aqueous solution will be:
Sr⁺²(aq) + 2 Cl⁻(aq) + 2 K⁺(aq) + SO₄⁻²(aq) → 2 K⁺(aq) + 2 Cl⁻(aq) + SrSO₄(s)
A spectator ion is an ion that appears both as a reactant and as a product in an ionic equation.
Spectator ions can be either cations (positively charged ions) or anions (negatively charged ions).
When writing a net ionic equation, spectator ions found in the original equation are ignored. Thus, the total ionic reaction is different from the net chemical reaction.
In this case, K⁺ and Cl⁻ are the spectator ions because they appear unchanged in both the product and the reagent. So these ions cancel out by writing the net ionic equation and you get:
Sr⁺²(aq) + SO₄⁻²(aq) → SrSO₄(s)
Since SrSO₄ is an insoluble salt, it will precipitate.
Finally, a precipitate of SrSO₄ is formed when When an aqueous solution of strontium chloride is added to an aqueous solution of potassium sulfate, and the net ionic equation is:
Sr⁺²(aq) + SO₄⁻²(aq) → SrSO₄(s)
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