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What is the complete ionic equation for [tex]\( H_2SO_4(aq) + CaI_2(aq) \rightarrow CaSO_4(s) + 2HI(aq) \)[/tex]?

A. [tex]\( 2H^{+} + SO_4^{2-} + Ca^{2+} + 2I^{-} \rightarrow Ca^{2+} + SO_4^{2-} + 2H^{+} + 2I^{-} \)[/tex]

B. [tex]\( H^{+} + SO_4^{2-} + Ca^{2+} + 2I^{-} \rightarrow CaSO_4 + H^{+} + I^{-} \)[/tex]

C. [tex]\( SO_4^{2-} + Ca^{2+} \rightarrow CaSO_4 \)[/tex]

D. [tex]\( 2H^{+} + SO_4^{2-} + Ca^{2+} + 2I^{-} \rightarrow CaSO_4 + 2H^{+} + 2I^{-} \)[/tex]

Sagot :

GinnyAnsweridn
To find the complete ionic equation for the reaction [tex]\(H_2SO_4(aq) + CaI_2(aq) \rightarrow CaSO_4(s) + 2 HI(aq)\)[/tex], we need to first break down all of the soluble strong electrolytes into their constituent ions and include spectator ions in the equation while the precipitate [tex]\(CaSO_4\)[/tex] will remain as a solid.

Let's start by dissociating each compound into its ions:

1. [tex]\(H_2SO_4(aq)\)[/tex] dissociates to [tex]\(2H^+(aq) + SO_4^{2-}(aq)\)[/tex]
2. [tex]\(CaI_2(aq)\)[/tex] dissociates to [tex]\(Ca^{2+}(aq) + 2I^-(aq)\)[/tex]
3. [tex]\(CaSO_4(s)\)[/tex] does not dissociate because it is a solid
4. [tex]\(2HI(aq)\)[/tex] dissociates to [tex]\(2H^+(aq) + 2I^-(aq)\)[/tex]

Now, we write the complete ionic equation, including all ions before and after the reaction:

Reactants:
[tex]\[2H^+ + SO_4^{2-} + Ca^{2+} + 2I^-\][/tex]

Products:
[tex]\[CaSO_4(s) + 2H^+ + 2I^-\][/tex]

Putting it all together:
[tex]\[2H^+ + SO_4^{2-} + Ca^{2+} + 2I^- \rightarrow CaSO_4(s) + 2H^+ + 2I^-\][/tex]

Now let's check the given choices:

A. [tex]\(2H^+ + SO_4^{2-} + Ca^{2+} + 2I^- \rightarrow Ca^{2+} + SO_4^{2-} + 2H^+ + 2I^-\)[/tex]

This choice shows all ions in both reactants and products but does not account for the formation of [tex]\(CaSO_4(s)\)[/tex], a solid precipitate. This is incorrect.

B. [tex]\(H^+ + SO_4^{2-} + Ca^{2+} + 2I^- \rightarrow CaSO_4 + H^+ + I^-\)[/tex]

This choice does not show all ions correctly and does not distinguish [tex]\(CaSO_4\)[/tex] as a solid appropriately. This is incorrect.

C. [tex]\(SO_4^{2-} + Ca^{2+} \rightarrow CaSO_4\)[/tex]

This choice is a net ionic equation, not a complete ionic equation. It excludes the spectator ions, which are needed for the complete ionic equation. This is incorrect.

D. [tex]\(2H^+ + SO_4^{2-} + Ca^{2+} + 2I^- \rightarrow CaSO_4(s) + 2H^+ + 2I^-\)[/tex]

This choice correctly shows all ions before and after the reaction, with [tex]\(CaSO_4(s)\)[/tex] distinguished as the precipitate formed.

Therefore, the correct complete ionic equation is given by:

[tex]\[2H^+ + SO_4^{2-} + Ca^{2+} + 2I^- \rightarrow CaSO_4(s) + 2H^+ + 2I^-\][/tex]

Hence, the correct answer is:
D. [tex]\(2H^+ + SO_4^{2-} + Ca^{2+} + 2I^- \rightarrow CaSO_4(s) + 2H^+ + 2I^-\)[/tex]
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