Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning
ISBN 10: 1285199049
ISBN 13: 978-1-28519-904-7

Chapter 3 - Chemical Reactions - Questions for Review and Thought - Topical Questions - Page 148c: 42b

Answer

Acid and base used to form this ion, respectively, : $H_2SO_4$ and $Ca(OH)_2$, Complete ionic equation: $H^+(aq) + HS{O_4}^{-}(aq) + Ca^{2+}(aq) + 2OH^-(aq) -- \gt CaSO_4(s) + 2H_2O(l) $ Net ionic equation: $H^+(aq) + HS{O_4}^{-}(aq) + Ca^{2+}(aq) + 2OH^-(aq) -- \gt CaSO_4(s) + 2H_2O(l) $

Work Step by Step

1. Identify the ions of the salt: $(NaNO_2)$: $Ca^{2+}$ and $S{O_4}^{2-}$: To the cation, add hydroxide ions: $Ca(OH)_2$; this is the base. To the anion, add hydrogen ions: $H_2SO_4$; this is the acid. 2. Now, write the balanced overall equation between, which is: $Acid + Base -- \gt Salt + Water$ We already have the salt, so: $H_2S{O_4}(aq) + Ca(OH)_2(aq) -- \gt CaSO_4(s) + H_2O(l) $ ** Acording to table 3.1, $CaSO_4$ is not soluble in water. 3. Write the complete ionic equation. - For the completely dissociated/ionized compounds, separate them by their ions: $H^+(aq) + HS{O_4}^{-}(aq) + Ca^{2+}(aq) + OH^-(aq) -- \gt CaSO_4(s) + H_2O(l) $ * $H_2SO_4$ is a strong acid, but only for one of its hydrogens; therefore, it is totally dissociated in $H^+$ and $HS{O_4}^-$. * $Ca(OH)_2$ is a strong base, so it is completely ionized in water. Balance it: $H^+(aq) + HS{O_4}^{-}(aq) + Ca^{2+}(aq) + 2OH^-(aq) -- \gt CaSO_4(s) + 2H_2O(l) $ 4. Remove the repeated ions: $H^+(aq) + HS{O_4}^{-}(aq) + Ca^{2+}(aq) + 2OH^-(aq) -- \gt CaSO_4(s) + 2H_2O(l) $ This is the net ionic equation.
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