Q8E
Question
How many moles of ionic species are present in \({\bf{1}}.{\bf{0}}{\rm{ }}{\bf{L}}\) of a solution marked \({\bf{1}}.{\bf{0}}M\) mercury (I) nitrate?
Step-by-Step Solution
VerifiedThere are \(3{\rm{M}}\)of ionic species in the solution, that is,\(1{\rm{M}}\)of \(Hg_2^{2 + }\)and \(2{\rm{M}}\)of\({\rm{NO}}_3^ - \).
Ionic species refers to the charged particles formed by the loss or gain of electrons. Compounds undergo dissociationand break down into smaller constituent ions.
- When an ionic species has a positive charge, it is called a cation.
- When an ionic species has a negative charge, it is called an anion.
The dissociation reaction is:
\({\bf{H}}{{\bf{g}}_{\bf{2}}}{\left( {{\bf{N}}{{\bf{O}}_{\bf{3}}}} \right)_{\bf{2}}} \to {\bf{Hg}}_{\bf{2}}^{{\bf{2 + }}}{\bf{ + 2NO}}_{\bf{3}}^{\bf{ - }}\)
1 M can be stated as:
\(1M = 1\frac{{mol}}{L}\)
If there is \(1\;{\rm{L}}\)of \(1{\rm{M}}\)solution of\({\rm{H}}{{\rm{g}}_2}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}\), there are \(3{\rm{M}}\)of ionic species in the solution consisting of \(1{\rm{M}}\)of\(Hg_2^{2 + }\)and \(2{\rm{M}}\)of\({\rm{NO}}_3^ - \).