16. For parts of the free response queatlon th. Open with atiows, clearly thow the marthod used and the steps involved in arriving at your answers. You must siow your work to receive credit for your answer.
Examples and equations may be included in your answers where appropriate.
A student wishes to determine the concentration of $\mathrm{Ag}^{+}(a q)$ in a solution of $\mathrm{AgNO}_{3}(a q)$. The student combines $10.00 \mathrm{~mL}$ of $\mathrm{AgNO}_{3}(\mathrm{aq})$ with excess $\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})$ and observes the formation of a white precipitate. The formation of the precipitate is represented by the following equation.
$2 \mathrm{AgNO}_{3}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) ightarrow \mathrm{Ag}_{2} \mathrm{SO}_{4}(s)+2 \mathrm{NaNO}_{3}(a q)$
(a) Write the balanced net ionic equation for the precipitation reaction.
The student collects the precipitate by filtration and measures the mass of the filter paper and precipitate every 10 minutes as it dries. The student records the data in the following table.
\begin{tabular}{|c|c|}
\hline \multicolumn{1}{|c|}{ Mass of dry filter paper } & $0.88 \mathrm{~g}$ \
\hline Mass of filter paper and precipitate immediately after filtration & $4.82 \mathrm{~g}$ \
\hline Mass of filter paper and precipitate after 10 minutes & $4.37 \mathrm{~g}$ \
\hline Mass of filter paper and precipitate after 20 minutes & $4.01 \mathrm{~g}$ \
\hline Mass of filter paper and precipitate after 30 minutes & $3.79 \mathrm{~g}$ \
\hline
\end{tabular}
(b) Use the data above to calculate the number of moles of $\mathrm{Ag}_{2} \mathrm{SO}_{4}(s)$ (molar mass $311.8 \mathrm{~g} / \mathrm{mol}$ ) that precipitated.
(c) Calculate the concentration of $\mathrm{Ag}^{\dagger}(a q)$ in the original $10.00 \mathrm{~mL}$ solution of $\mathrm{AgNO}_{3}(a q)$.
(d) The concentration of $\mathrm{Ag}^{+}(a q)$ determined by the student is significantly higher than the actual concentration of $\mathrm{Ag}^{+}(\mathrm{aq})$ Based on the student's data table, identify an error in the experimental procedure that led to this result:
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Question

16. For parts of the free response queatlon th. Open with atiows, clearly thow the marthod used and the steps involved in arriving at your answers. You must siow your work to receive credit for your answer.
Examples and equations may be included in your answers where appropriate.
A student wishes to determine the concentration of $\mathrm{Ag}^{+}(a q)$ in a solution of $\mathrm{AgNO}_{3}(a q)$. The student combines $10.00 \mathrm{~mL}$ of $\mathrm{AgNO}_{3}(\mathrm{aq})$ with excess $\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})$ and observes the formation of a white precipitate. The formation of the precipitate is represented by the following equation.
$2 \mathrm{AgNO}_{3}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) ightarrow \mathrm{Ag}_{2} \mathrm{SO}_{4}(s)+2 \mathrm{NaNO}_{3}(a q)$
(a) Write the balanced net ionic equation for the precipitation reaction.
The student collects the precipitate by filtration and measures the mass of the filter paper and precipitate every 10 minutes as it dries. The student records the data in the following table.
\begin{tabular}{|c|c|}
\hline \multicolumn{1}{|c|}{ Mass of dry filter paper } & $0.88 \mathrm{~g}$ \
\hline Mass of filter paper and precipitate immediately after filtration & $4.82 \mathrm{~g}$ \
\hline Mass of filter paper and precipitate after 10 minutes & $4.37 \mathrm{~g}$ \
\hline Mass of filter paper and precipitate after 20 minutes & $4.01 \mathrm{~g}$ \
\hline Mass of filter paper and precipitate after 30 minutes & $3.79 \mathrm{~g}$ \
\hline
\end{tabular}
(b) Use the data above to calculate the number of moles of $\mathrm{Ag}_{2} \mathrm{SO}_{4}(s)$ (molar mass $311.8 \mathrm{~g} / \mathrm{mol}$ ) that precipitated.
(c) Calculate the concentration of $\mathrm{Ag}^{\dagger}(a q)$ in the original $10.00 \mathrm{~mL}$ solution of $\mathrm{AgNO}_{3}(a q)$.
(d) The concentration of $\mathrm{Ag}^{+}(a q)$ determined by the student is significantly higher than the actual concentration of $\mathrm{Ag}^{+}(\mathrm{aq})$ Based on the student's data table, identify an error in the experimental procedure that led to this result:
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Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Write the balanced net ionic equation**: The balanced net ionic equation for the precipitation reaction between $\mathrm{AgNO}_3$ and $\mathrm{Na}_2\mathrm{SO}_4$ involves the ions that form the precipitate. ‖ ‖ 2 ⋮ **Calculate the mass of $\mathrm{Ag}_2\mathrm{SO}_4$ precipitated**: Subtract the mass of the dry filter paper from the mass of the filter paper and precipitate after 30 minutes to find the mass of the precipitate. ‖ ‖ 3 ⋮ **Determine the number of moles of $\mathrm{Ag}_2\mathrm{SO}_4$**: Use the molar mass of $\mathrm{Ag}_2\mathrm{SO}_4$ to convert the mass of the precipitate to moles. ‖ ‖ 4 ⋮ **Calculate the concentration of $\mathrm{Ag}^+$**: Use the number of moles of $\mathrm{Ag}_2\mathrm{SO}_4$ to find the moles of $\mathrm{Ag}^+$, then divide by the volume of the $\mathrm{AgNO}_3$ solution to get the concentration. ‖ ‖ 5 ⋮ **Identify an error in the experimental procedure**: Analyze the data table for inconsistencies or trends that could indicate an error in the experimental procedure. ‖ ∻1 Answer∻ ⚹ $\mathrm{Ag}^+_{(aq)} + \mathrm{SO}_4^{2-}_{(aq)} ightarrow \mathrm{Ag}_2\mathrm{SO}_4_{(s)}$ ⚹ ∻2 Answer∻ ⚹ Number of moles of $\mathrm{Ag}_2\mathrm{SO}_4$ = $\frac{(3.79 \mathrm{~g} - 0.88 \mathrm{~g})}{311.8 \mathrm{~g/mol}}$ ⚹ ∻3 Answer∻ ⚹ Concentration of $\mathrm{Ag}^+$ = $\frac{ ext{moles of } \mathrm{Ag}_2\mathrm{SO}_4 imes 2}{0.01000 \mathrm{~L}}$ ⚹ ∻4 Answer∻ ⚹ Possible error: Incomplete drying of the precipitate, leading to an overestimation of the mass of $\mathrm{Ag}_2\mathrm{SO}_4$. ⚹ ∻Key Concept∻ ⚹ The net ionic equation represents the ions that participate directly in the reaction, forming the precipitate. ⚹ ∻Explanation∻ ⚹ The net ionic equation excludes spectator ions and shows the formation of the insoluble compound. ⚹ ∻Key Concept∻ ⚹ The number of moles of a compound is calculated by dividing its mass by its molar mass. ⚹ ∻Explanation∻ ⚹ This calculation is essential for stoichiometry, allowing us to relate mass to moles for chemical reactions. ⚹ ∻Key Concept∻ ⚹ The concentration of ions in a solution is determined by the number of moles of the ion divided by the volume of the solution. ⚹ ∻Explanation∻ ⚹ This relationship is used to find the molarity of a solution, which is a measure of its concentration. ⚹ ∻Key Concept∻ ⚹ Experimental errors can affect the accuracy of the results. ⚹ ∻Explanation∻ ⚹ Identifying potential errors helps in understanding discrepancies between expected and observed results.◊What is the chemical formula for Silver Sulfate (Ag2SO4)?⍭ Generate me a similar question◊⚹

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