Asolution 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.

Net ionic equation :

2Cl⁻(aq) + Hg₂²⁺(aq) ---> Hg₂Cl₂(s)

CO₃²⁻(aq) + Ba²⁺(aq)---> BaCO₃(s)

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:

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⁺

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)

the net ionic equation  

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calculate how many grams of ammonia can be produced from 4.21 grams of

n2 + 3h2 = 2nh3

my answer:

25.0g n2 x (1 mol/ 28.0gn2) x (2 mol nh3/ 1 mol n2) x (17.0g nh3/ 1 molnh3) = 30.36g n2

25.0g h2 x (1 mol h2/ 2.00g h2) x (2 mol nh3/ 3 mol h2) x (17.0g nh3/ 1 mol nh3) = 141.67g h2

lr = n2

c, liquids evaporate, creating a gas