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What is the net ionic equation of the following reaction?

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

A. [tex]\(H_2SO_4(aq) + CaI_2(aq) \rightarrow CaSO_4(s) + 2 HI(aq)\)[/tex]

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

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

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



Answer :

GinnyAnswer
To determine the net ionic equation for the given reaction:

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

we need to follow these steps:

1. Identify the spectator ions: Spectator ions are ions that do not participate in the actual reaction and remain unchanged on both sides of the equation. In this reaction, the ions [tex]\( 2 H^+ \)[/tex] and [tex]\( 2 I^- \)[/tex] appear on both sides of the equation without any change.

2. Remove the spectator ions: By eliminating [tex]\( 2 H^+ \)[/tex] and [tex]\( 2 I^- \)[/tex] from both sides of the equation, we simplify the reaction to:

[tex]\[ SO_4^{2-} + Ca^{2+} \rightarrow CaSO_4 \][/tex]

3. Write the net ionic equation: The simplified equation from which spectator ions have been removed represents the net ionic equation.

Thus, the net ionic equation for the given reaction is:

[tex]\[ SO_4^{2-} + Ca^{2+} \rightarrow CaSO_4 \][/tex]

Reviewing the provided options:
- Option A: Incorrect, it doesn't show the net ionic equation.
- Option B: Correct, it precisely matches our simplified reaction.
- Option C: Incorrect, it includes spectator ions.
- Option D: Incorrect, it includes spectator ions.

Therefore, the correct answer is:

[tex]\[ \boxed{2} \][/tex]

Represented as option B:

[tex]\[ SO_4^{2-} + Ca^{2+} \rightarrow CaSO_4 \][/tex]

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