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Chapter 7: Problem 97

For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together. Indicate "none" if no precipitate will form.

Short Answer

Expert verified
In the first example reaction, the precipitate produced is BaSO鈧� (barium sulfate), and in the second example reaction, there is no precipitate formed.

Step by step solution

01

Write the balanced chemical equation.

First, we need to write the balanced chemical equation for the reaction between barium nitrate and sodium sulfate. Ba(NO鈧�)鈧�(aq) + Na鈧係O鈧�(aq) 鈫� BaSO鈧� + 2NaNO鈧�
02

Determine the solubility of the products.

We need to determine the solubility of BaSO鈧� and NaNO鈧� in water. By referring to the solubility rules mentioned in the analysis, we know that most nitrates are soluble, so NaNO鈧� is soluble in water. Most sulfates are soluble, except for those with certain cations such as barium. Therefore, BaSO鈧� is insoluble in water.
03

Identify the precipitate.

Since BaSO鈧� is insoluble in water, it will form a precipitate when the two reactants are mixed. So, the precipitate produced in this reaction is BaSO鈧�. Example 2: Mixing together aqueous solutions of potassium chloride (KCl) and ammonium nitrate (NH鈧凬O鈧�).
04

Write the balanced chemical equation.

First, we need to write the balanced chemical equation for the reaction between potassium chloride and ammonium nitrate. KCl(aq) + NH鈧凬O鈧�(aq) 鈫� KNO鈧� + NH鈧凜l
05

Determine the solubility of the products.

We need to determine the solubility of KNO鈧� and NH鈧凜l in water. By referring to the solubility rules mentioned in the analysis, we know that most nitrates are soluble, so KNO鈧� is soluble in water. Most chlorides are soluble, including those formed with ammonium, so NH鈧凜l is soluble in water.
06

Identify the precipitate.

Since both KNO鈧� and NH鈧凜l are soluble in water, no precipitate is formed in this reaction. Therefore, the answer is "none".

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Most popular questions from this chapter

Balance each of the following equations that describe synthesis reactions. a. \(\mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ca}(\mathrm{OH})_{2}(s)\) b. \(\mathrm{Fe}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s)\) c. \(\mathrm{P}_{2} \mathrm{O}_{5}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)\)

For the reaction \(16 \mathrm{Fe}(s)+3 \mathrm{~S}_{8}(s) \rightarrow 8 \mathrm{Fe}_{2} \mathrm{~S}_{3}(s),\) show how electrons are gained and lost by the atoms.

What salt would form when each of the following strong acid/strong base reactions takes place? a. \(\mathrm{HCl}(a q)+\mathrm{KOH}(a q) \rightarrow\) b. \(\mathrm{RbOH}(a q)+\mathrm{HNO}_{3}(a q) \rightarrow\) c. \(\mathrm{HClO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow\) d. \(\operatorname{HBr}(a q)+\operatorname{CsOH}(a q) \rightarrow\)

Balance each of the following oxidation-reduction reactions. a. \(\mathrm{Co}(s)+\mathrm{Br}_{2}(l) \rightarrow \mathrm{CoBr}_{3}(s)\) b. \(\mathrm{Al}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+\mathrm{H}_{2}(g)\) c. \(\mathrm{Na}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{NaOH}(a q)+\mathrm{H}_{2}(g)\) d. \(\mathrm{Cu}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{Cu}_{2} \mathrm{O}(s)\)

Balance each of the following equations that describe synthesis reactions. a. \(\mathrm{Fe}(s)+\mathrm{S}_{8}(s) \rightarrow \mathrm{FeS}(s)\) b. \(\mathrm{Co}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{Co}_{2} \mathrm{O}_{3}(s)\) c. \(\mathrm{Cl}_{2} \mathrm{O}_{7}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{HClO}_{4}(a q)\)
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