Question

Write complete ionic equation to show the reaction of aqueous hg2(no3)2 with aqueous sodium chloride to form solid hg2cl2 and aqueous sodium nitrate. express your answer as a chemical equation. identify all of the phases in your answer.

Answer 1

The complete ionic equation for the reaction of Hg2(NO3)2 with NaCl resulting in Hg2Cl2 and NaNO3 is Hg22+(aq) + 2Cl-(aq) → Hg2Cl2(s). Spectator ions like Na+ and NO3- are omitted.

Step-by-step explanation:

To write the complete ionic equation for the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate, first the reactants and products need to be represented in their ionic forms:

Hg22+(aq) + 2NO3-(aq) + 2Na+(aq) + 2Cl-(aq) → Hg2Cl2(s) + 2Na+(aq) + 2NO3-(aq)

Now, remove the spectator ions, which are the ions that do not participate in the creation of the precipitate. In this case, the sodium and nitrate ions are the spectator ions:

Hg22+(aq) + 2Cl-(aq) → Hg2Cl2(s)

This is the complete ionic equation showing the formation of the solid mercury(I) chloride precipitate from the aqueous ions.

Answer 2

First we start with our molecular equation to ensure all atoms are balanced in order to maintain the law of conservation of mass.

`Hg_2(NO_3)_2_(_a_q_) + NaCl_(_a_q_) \implies Hg_2Cl_2_(_s_) + NaNO_3_(_a_q_)`.

The equation is unbalanced since we have 1 Cl atom on left hand side as opposed to 2 on the right hand side and we have 2
`NO_3` molecules on left hand side and 1 on the right hand side. So we add a coefficient of 2 on both the
`NaCl` and
`NaNO_3`

`Hg_2(NO_3)_2_(_a_q_) + 2NaCl_(_a_q_) \implies Hg_2Cl_2_(_s_) + 2NaNO_3_(_a_q_)`

The reaction occurs between solutes that are soluble in water to give a solid as a precipitate. So the complete ionic equation will show the soluble compounds in their dissociated states as ions in water and the insoluble compound as a solid.

`2Hg^+_(_a_q_) + 2NO_3^-_(_a_q_) + 2Na^+_(_a_q_) + 2Cl^- _(_a_q_) \implies Hg_2Cl_2_(_s_) + 2Na^+_(_a_q_) + 2NO_3^-_(_a_q_)`