Questions: Select all of the following reactions that produce a precipitate. Check all that apply. Note: Reference the Solubility of ionic compounds in water table for additional information. - BaCl2(aq) + H2SO4(aq) → - NaOH(aq) + HCl(aq) → - KCH3CO2(aq) + FeBr3(aq) → - Zn(s) + CuSO4(aq) → - KOH(aq) + Pb(CH3CO2)2(aq) → None of the above

Select all of the following reactions that produce a precipitate. Check all that apply. Note: Reference the Solubility of ionic compounds in water table for additional information. - BaCl2(aq) + H2SO4(aq) → - NaOH(aq) + HCl(aq) → - KCH3CO2(aq) + FeBr3(aq) → - Zn(s) + CuSO4(aq) → - KOH(aq) + Pb(CH3CO2)2(aq) → None of the above
Transcript text: Select all of the following reactions that produce a precipitate. Check all that apply. Note: Reference the Solubility of ionic compounds in water table for additional information. \begin{tabular}{|l|} \hline$\square \mathrm{BaCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow$ \\ \hline$\square \mathrm{NaOH}(a q)+\mathrm{HCl}(a q) \rightarrow$ \\ \hline$\square \mathrm{KCH}_{3} \mathrm{CO}_{2}(a q)+\mathrm{FeBr}_{3}(a q) \rightarrow$ \\ \hline$\square \mathrm{Zn}(s)+\mathrm{CuSO}_{4}(a q) \rightarrow$ \\ \hline $\mathrm{KOH}(a q)+\mathrm{Pb}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2}(a q) \rightarrow$ \\ \hline \end{tabular} None of the above
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Solution

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Solution Steps

Step 1: Identify the Reactions and Solubility Rules

To determine which reactions produce a precipitate, we need to apply solubility rules to the products of each reaction. A precipitate forms when an insoluble compound is produced in a reaction.

Step 2: Analyze Each Reaction

  1. Reaction 1: \(\mathrm{BaCl}_{2}(aq) + \mathrm{H}_{2}\mathrm{SO}_{4}(aq) \rightarrow \mathrm{BaSO}_{4}(s) + 2\mathrm{HCl}(aq)\)

    • \(\mathrm{BaSO}_{4}\) is insoluble in water, so a precipitate forms.

  2. Reaction 2: \(\mathrm{NaOH}(aq) + \mathrm{HCl}(aq) \rightarrow \mathrm{NaCl}(aq) + \mathrm{H}_{2}\mathrm{O}(l)\)

    • Both \(\mathrm{NaCl}\) and \(\mathrm{H}_{2}\mathrm{O}\) are soluble, so no precipitate forms.

  3. Reaction 3: \(\mathrm{KCH}_{3}\mathrm{CO}_{2}(aq) + \mathrm{FeBr}_{3}(aq) \rightarrow \mathrm{KBr}(aq) + \mathrm{Fe(CH}_{3}\mathrm{CO}_{2})_{3}(aq)\)

    • Both \(\mathrm{KBr}\) and \(\mathrm{Fe(CH}_{3}\mathrm{CO}_{2})_{3}\) are soluble, so no precipitate forms.

  4. Reaction 4: \(\mathrm{Zn}(s) + \mathrm{CuSO}_{4}(aq) \rightarrow \mathrm{ZnSO}_{4}(aq) + \mathrm{Cu}(s)\)

    • \(\mathrm{Cu}\) is a solid metal, but it is not considered a precipitate from a solution reaction. This is a single displacement reaction.

  5. Reaction 5: \(\mathrm{KOH}(aq) + \mathrm{Pb(CH}_{3}\mathrm{CO}_{2})_{2}(aq) \rightarrow \mathrm{KCH}_{3}\mathrm{CO}_{2}(aq) + \mathrm{Pb(OH)}_{2}(s)\)

    • \(\mathrm{Pb(OH)}_{2}\) is insoluble in water, so a precipitate forms.

Final Answer

The reactions that produce a precipitate are:

  • \(\mathrm{BaCl}_{2}(aq) + \mathrm{H}_{2}\mathrm{SO}_{4}(aq) \rightarrow \mathrm{BaSO}_{4}(s) + 2\mathrm{HCl}(aq)\)
  • \(\mathrm{KOH}(aq) + \mathrm{Pb(CH}_{3}\mathrm{CO}_{2})_{2}(aq) \rightarrow \mathrm{KCH}_{3}\mathrm{CO}_{2}(aq) + \mathrm{Pb(OH)}_{2}(s)\)

\[ \boxed{\text{Reactions 1 and 5 produce a precipitate.}} \]

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