Question

Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. Be sure to include the proper phases for all species within the reaction.

hg2so4(s) →

Answer 1

Mercury(I) sulfate (Hg2SO4) dissociates slightly in water to form Hg2^2+(aq) and SO4^2−(aq), but does not fully dissociate like strong electrolytes.

To complete the balanced dissociation equation for Hg2SO4 in aqueous solution, we need to remember that certain compounds do not fully dissociate in water. However, mercury(I) sulfate (Hg2SO4) is a slightly soluble compound and does dissociate slightly into ions in aqueous solution. The balanced dissociation for this compound would be:

Hg2SO4(s) → Hg2^2+(aq) + SO4^2−(aq)

Given that the dissociation is not 100%, the equation is written without the complete ionization as you would with strong electrolytes. If the question implies the dissociation should be considered as not occurring or negligible (since it's a slightly soluble salt), then the equation would end with 'NR' to mean 'no reaction'. However, without this implication, the slightly soluble salt should be shown dissociating as above.

So, Hg2SO4 does dissociate to a small extent into mercury(I) ions and sulfate ions in aqueous solution, but not completely.

Answer 2

Mercury(I) sulfate (Hg2SO4) is a sparingly soluble compound. When it dissociates in aqueous solution, it forms ions. The balanced dissociation equation for Hg2SO4 in aqueous solution would be as follows:

Hg2SO4(s) ⇌ 2Hg^2+(aq) + SO4^2-(aq)

Please note that the equilibrium arrow (⇌) indicates that this dissociation is a reversible reaction, and Hg2SO4 is sparingly soluble in water.