Question #fc0a2

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Question #fc0a2

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Answer 1 · 2017-06-23T00:03:29

This reaction doesn't take place.

Explanation:

The thing to recognize here is that magnesium sulfate, ${MgSO}_{4}$ $"MgSO"_4$ , and sodium chloride, $NaCl$ $"NaCl"$ , the two potential products of the reaction, are soluble in water, which implies that they exist as ions in aqueous solution.

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This means that when you mix a solution of magnesium chloride and a solution of sodium sulfate, all the chemical species will exist as ions in solution, hence no reaction will take place.

The complete ionic equation would look like this

${Mg}_{(a q)}^{2 +} + 2 {Cl}_{(a q)}^{-} + 2 {Na}_{(a q)}^{+} + {SO}_{4 (a q)}^{2 -} \to {Mg}_{(a q)}^{2 +} + {SO}_{4 (a q)}^{2 -} + 2 {Na}_{(a q)}^{+} + 2 {Cl}_{(a q)}^{-}$ $"Mg"_ ((aq))^(2+) + 2"Cl"_ ((aq))^(-) + 2"Na"_ ((aq))^(+) + "SO"_ (4(aq))^(2-) -> "Mg"_ ((aq))^(2+) + "SO"_ (4(aq))^(2-) + 2"Na"_ ((aq))^(+) + 2"Cl"_ ((aq))^(-)$

Since all ions are spectator ions, i.e. they are present on both sides of the equation, you can say that you have

${MgCl}_{2 (a q)} + {Na}_{2} {SO}_{4 (a q)} \to N.R.$ $"MgCl"_ (2(aq)) + "Na"_ 2"SO"_ (4(aq)) -> "N.R."$

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Question #fc0a2

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