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Chapter 8: Problem 68

Aqueous solutions of sodium sulfide and iron(III) nitrate are combined. (a) Does a precipitation reaction occur? Explain. (b) If it does, write a net ionic equation for the reaction.

Short Answer

Expert verified
Yes, a precipitation reaction occurs when aqueous solutions of sodium sulfide and iron(III) nitrate are combined, forming insoluble iron(III) sulfide. The net ionic equation for the reaction is: \(\text{Fe}^{3+} + 3 \: \text{S}^{2-} \rightarrow \text{Fe}_{2}\text{S}_{3}\)

Step by step solution

01

Determine if a precipitation reaction occurs

Using the solubility rules, we can predict if a reaction will occur by checking if any of the products formed are insoluble. When sodium sulfide (Na2S) and iron(III) nitrate (Fe(NO3)3) react, their ions will exchange, producing sodium nitrate (NaNO3) and iron(III) sulfide (Fe2S3). According to the solubility rules, nitrates are generally soluble, and sulfides of transition metals, like iron, are generally insoluble. Therefore, a precipitation reaction will occur, as iron(III) sulfide is insoluble.
02

Write the balanced molecular equation

Now that we know a reaction will occur, we can write the balanced molecular equation for the reaction. The balanced equation is: \(2 \: \text{Na}_{2}\text{S} + \text{Fe}(\text{NO}_{3})_{3} \rightarrow 4 \: \text{NaNO}_{3} + \text{Fe}_{2}\text{S}_{3}\)
03

Write the complete ionic equation

Next, we will write the complete ionic equation by dissociating all strong electrolytes into their respective ions: \(2 \: (2 \: \text{Na}^{+} + \text{S}^{2-}) + (\text{Fe}^{3+} + 3 \: \text{NO}_{3}^{-}) \rightarrow 4 \: (\text{Na}^{+} + \text{NO}_{3}^{-}) + \text{Fe}_{2}\text{S}_{3}\)
04

Write the net ionic equation

Finally, we will write the net ionic equation by eliminating the spectator ions (Na⁺ and NO₃⁻). We are left with: \(\text{Fe}^{3+} + 3 \: \text{S}^{2-} \rightarrow \text{Fe}_{2}\text{S}_{3}\) So, the net ionic equation for the reaction between aqueous sodium sulfide and iron(III) nitrate is: \(\text{Fe}^{3+} + 3 \: \text{S}^{2-} \rightarrow \text{Fe}_{2}\text{S}_{3}\)

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Most popular questions from this chapter

Sulfur dioxide and water are formed when hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{~S}\), reacts with oxygen gas. Write the balanced equation for the reaction.

Consider the ionic bonds between \(\mathrm{Na}^{+}\) ions and \(\underline{\mathrm{Cl}}^{-}\) ions in \(\mathrm{NaCl}(\mathrm{s}) .\) Why must energy be added to break these bonds (in other words, what is the added energy used for)?

Balance this chemical equation by inspection: \(\mathrm{Fe}_{2} \mathrm{O}_{3}+\mathrm{C} \rightarrow \mathrm{Fe}+\mathrm{CO}_{2}\)

When a precipitate forms in water, the water often becomes warmer. What is the source of the heat energy that warms the water?

Acids produce ions when dissolved in water, and bases produce ions when dissolved in water.
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