Question

A solution contains one or more of the following ions: Hg2+2, Ba2+, and Fe2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no precipitate. When potassium carbonate is added to the remaining solution, a precipitate forms.What are the net ionic equations for the formation of each of the precipitates observed? Express your answers as chemical equations separated by a comma. Identify all the phases in your answer.

Answer 1

Answer:

Explanation:

Solubility is a measure of the ability of a given substance to dissolve in a liquid, that is, it describes the amount of solute that can be dissolved in a specific amount of solvent.  This occurs by solvation. Solvation is the process that involves the association of solvent molecules with molecules or ions of a solute. When the ions of a solvent dissolve, they are separated and surrounded by the molecules that form the solvent. The larger the size of the ion, the greater the number of molecules capable of surrounding it, so it is said that the ion is mostly solvated.

For a substance to dissolve in another the polarity of the molecules must be similar. For example, water is a polar compound and easily dissolves polar substances such as acids, hydroxides and inorganic salts and polar organic compounds. Although there are also exceptions. There are highly polar inorganic compounds that are insoluble in water, such as carbonates or sulphides.

Taking into account the aforementioned, the solubility rules were stated. One of these rules mentions that all chlorides (Cl-) are soluble except those of Hg₂²⁺, among others.  This means that by adding KCl to the mixture, the compound Hg₂Cl precipitates through the net ionic equation:

Hg₂²⁺ (aq) + Cl⁻ (aq) ⇒ Hg₂Cl (s)

Then the solution is filtered with the precipitate so that no more Hg₂²⁺ is present in the solution.

Another rule of solubility indicates that sulfates (SO₄²⁻) are all soluble except those of Ba²⁺, among others.  That is, between the sulfate and Ba²⁺ precipitate should form. But since it is indicated that potassium sulfate is added to the remaining solution without producing precipitate, it is possible to say that the sulfate is actually reacting with Fe²⁺. This, due to the solubility rule, is soluble with sulfate, producing no precipitate. So, since there is no precipitate, there is no net ionic equation. And there should be no Fe + 2 in the solution due to its reaction with sulfate.

Finally, another solubility rule indicates that all carbonates (CO₃²⁻), phosphates (PO₄³⁻), arsenates (As⁺⁵) and chromates (Cr₂O₄²⁻) are insoluble, except those of Group IA and those of NH₄⁺. Then  when potassium carbonate is added to the remaining solution, a precipitate is formed, product of the net ionic equation between Ba²⁺ and carbonate:

Ba²⁺ (aq) + CO₃²⁻ (aq) ⇒ BaCO₃ (s)

Answer 2

Net ionic equation :

2Cl⁻(aq) + Hg₂²⁺(aq) ---> Hg₂Cl₂(s)

CO₃²⁻(aq) + Ba²⁺(aq)---> BaCO₃(s)

Further explanation

There are two types of chemical reactions that may occur.

namely single-replacement reactions and double-replacement reactions.

Double-Replacement reactions. Happens if there is an ion exchange between two ion compounds in the reactant to form two new ion compounds in the product

To predict whether this reaction can occur or not is one of them, the precipitation reaction. A precipitation reaction occurs if two ionic compounds which are dissolved reacted to produce one of the products of the ion compound does not dissolve. Formation of these precipitating compounds that cause reactions can occur

Solubility Rules:

• 1. soluble compound

All compounds of Li +, Na +, K +, Rb +, Cs +, and NH4 +

All compounds of NO₃⁻ and C₂H₃O₂⁻

Compounds of Cl−, Br−, I− except Ag⁺, Hg₂²⁺, Pb²⁺

Compounds of SO₄²⁻ except Hg₂²⁺, Pb²⁺, Sr²⁺, Ba²⁺

• 2. insoluble compounds

Compounds of CO₃²⁻ and PO₄³⁻ except for Compounds of Li +, Na +, K +, Rb +, Cs +, and NH₄ +

Compounds of OH− except Compounds of Li +, Na +, K +, Rb +, Cs +, NH₄⁺, Sr²⁺, and Ba²⁺

A solution contains one or more of the following statements: Hg₂²⁺, Ba²⁺, and Fe²⁺

When potassium chloride (KCl) is added to the solution, a precipitate forms.

In accordance with the Solubility rules, all Cl-compounds are soluble compounds except Ag⁺, Hg₂²⁺, Pb²⁺. So the first reaction produces precipitated Hg₂Cl₂

net ionic reaction

2Cl⁻(aq) + Hg₂²⁺(aq) ---> Hg₂Cl₂(s)

Then potassium sulfate (K₂SO₄) is added to the remaining solution, producing no precipitate

Soutions only contain Ba²⁺, and Fe²⁺ ions

Because the reaction does not produce precipitated compounds, according to the Solubility rules, Compounds of SO₄²⁻ are soluble compounds except Hg₂²⁺, Pb²⁺, Sr²⁺, Ba², so the reaction with Ba²⁺ produces a precipitate, because producing no precipitate, then K₂SO₄ reacts with Fe²⁺ ions

K₂SO₄ (aq)+ Fe²⁺(aq) ---> FeSO₄ (aq) ---> there is no net ionic equation because all compounds dissolves

Potassium carbonate (K₂CO₃) is added to the remaining solution (containing Ba²⁺ ions), a precipitate forms

Because Compounds of CO₃²⁻ and PO₄³⁻ are insoluble compounds except for Compounds of Li +, Na +, K +, Rb +, Cs +, and NH₄ +, then  reaction between K₂CO₃ and Ba²⁺ produces a precipitate form

net ionic reaction:

CO₃²⁻(aq) + Ba²⁺(aq)---> BaCO₃(s)

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