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Enter the net ionic equation for the reaction of AgNO3(aq)
with K2SO4(aq)
. Include phases. Refer to the solubility rules as necessary.

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quasarJose

Answer:

Explanation:

This is a typical double replacement or double decomposition reaction. In this kind of reaction, it involves the combination of ionic compounds which exchange their partners to form new compounds. Typical of these reaction is the formation of precipitates which are insoluble compounds.

The reaction equation is shown below:

 AgNO₃[tex](_{aq} )[/tex] + K₂SO₄[tex](_{aq} )[/tex] → 2KNO₃[tex](_{aq} )[/tex] + AgSO₄[tex](_{s}[/tex] )

From the rule of solubility:

  • All trioxonitrate(v) salts are soluble
  • Salts of silver sulfates are slightly soluble. This will form the precipitate in the solution.

We can write the ionic equation as:

      Ag⁺[tex](_{aq} )[/tex] + NO₃⁻[tex](_{aq} )[/tex] + 2K⁺[tex](_{aq} )[/tex] + SO₄²⁻[tex](_{aq} )[/tex] → AgSO₄[tex](_{s} )[/tex] + 2K⁺ + NO₃⁻[tex](_{aq} )[/tex]

The spectator ions or non-reactive ions are those ions that appears on both sides of the equation. These ions are the potassium and trioxonitrate ions. We cancel them out to give the net ionic equation of the reaction:

 Ag⁺[tex](_{aq} )[/tex] + SO₄²⁻[tex](_{aq} )[/tex] → AgSO₄[tex](_{s} )[/tex]

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