Two aqueous solutions contain the ions indicated below (a)

Step 1 of 3

a) Sodium compounds are always soluble and chlorides most of the time. So, (the rest) limestone precipitate will form upon mixing the solutions.

Balanced molecular equation:

compound formulas can also be guessed counting the balls in the diagram

\(\mathrm{Na}_{2} \mathrm{CO}_{3}(a q)+\mathrm{CaCl}_{2}(a q)=2 \mathrm{NaCl}(a q)+\mathrm{CaCO}_{3}(s)\)

Total ionic equation:

(aq) compounds dissociate

\(\begin{array}{r} 2 \mathrm{Na}^{+}(a q)+\mathrm{CO}_{3}^{2-}(a q)+\mathrm{Ca}^{2+}(a q)+2 \mathrm{Cl}^{-}(a q)= \\ =2 \mathrm{Na}^{+}(a q)+2 \mathrm{Cl}^{-}(a q)+\mathrm{CaCO}_{3}(s) \end{array}\)

Cancel out unchanged ions.

Net ionic equation:

\(\mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}{ }^{2-}(a q) \longrightarrow \mathrm{CaCO}_{3}(s)\)

Result

\(\mathrm{Na}_{2} \mathrm{CO}_{3}+\mathrm{CaCl}_{2}=2 \mathrm{NaCl}+\underline{\mathrm{CaCO}_{3}}\)