Question

An aqueous solution of sodium sulfide is allowed to react with an aqueous solution of magnesium chloride.The complete ionic equation contains which of the following species (when balanced in standard form)?a.Cl-(aq)b.2Na+(aq)c.2S2-(aq)d.Na+(aq)e.3Mg2+(aq)

Answer 1

Answer: The complete ionic equation contains $2Na^{+}(aq.)$ ions

Explanation:

Complete ionic equation is defined as the equation in which all the substance that are strong electrolyte are present in an aqueous are represented in the form of ions.

The chemical equation for the reaction of sodium sulfide and magnesium chloride is given as:

$Na_2S(aq.)+MgCl_2(aq.)\rightarrow 2NaCl(aq.)+MgS(s)$

Ionic form of the above equation follows:

$2Na^{+}(aq.)+S^{2-}(aq.)+Mg^{2+}(aq.)+2Cl^{-}(aq.)\rightarrow MgS(s)+2Na^+(aq.)+2Cl^-(aq.)$

The complete ionic equation for the above reaction follows:

$2Na^{+}(aq.)+S^{2-}(aq.)+Mg^{2+}(aq.)+2Cl^{-}(aq.)\rightarrow MgS(s)+2Na^+(aq.)+2Cl^-(aq.)$

Hence, the complete ionic equation contains $2Na^{+}(aq.)$ ions