---
title: "A student performs a gravimetric analysis to determine the mass percent of silver in an alloy. A \\(2.00 \\text{ g}\\) sample of the alloy is completely dissolved in excess concentrated \\(\\text{HNO}_3\\text{(aq)}\\). An excess of \\(\\text{NaCl(aq)}\\) is added to the solution, causing all of the silver to precipitate as \\(\\text{AgCl(s)}\\). The precipitate is collected on filter paper, washed, and dried to constant mass. The experimental data and molar masses are shown in the tables below.  | Measurement | Mass | | :— | :— | | Mass of alloy sample | \\(2.00 \\text{ g}\\) | | Mass of dry filter paper | \\(0.800 \\text{ g}\\) | | Mass of filter paper \\(+\\) dry \\(\\text{AgCl(s)}\\) | \\(2.235 \\text{ g}\\) |  | Substance | Molar Mass (\\(\\text{g/mol}\\)) | | :— | :— | | \\(\\text{Ag}\\) | \\(108.0\\) | | \\(\\text{Cl}\\) | \\(35.5\\) | | \\(\\text{AgCl}\\) | \\(143.5\\) |  Based on the data, what is the mass percent of \\(\\text{Ag}\\) in the alloy sample?"
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date_modified: "2026-09-28T11:59:49+00:00"
---

# A student performs a gravimetric analysis to determine the mass percent of silver in an alloy. A \(2.00 \text{ g}\) sample of the alloy is completely dissolved in excess concentrated \(\text{HNO}_3\text{(aq)}\). An excess of \(\text{NaCl(aq)}\) is added to the solution, causing all of the silver to precipitate as \(\text{AgCl(s)}\). The precipitate is collected on filter paper, washed, and dried to constant mass. The experimental data and molar masses are shown in the tables below.

| Measurement | Mass |
| :— | :— |
| Mass of alloy sample | \(2.00 \text{ g}\) |
| Mass of dry filter paper | \(0.800 \text{ g}\) |
| Mass of filter paper \(+\) dry \(\text{AgCl(s)}\) | \(2.235 \text{ g}\) |

| Substance | Molar Mass (\(\text{g/mol}\)) |
| :— | :— |
| \(\text{Ag}\) | \(108.0\) |
| \(\text{Cl}\) | \(35.5\) |
| \(\text{AgCl}\) | \(143.5\) |

Based on the data, what is the mass percent of \(\text{Ag}\) in the alloy sample?

A student performs a gravimetric analysis to determine the mass percent of silver in an alloy. A \(2.00 \text{ g}\) sample of the alloy is completely dissolved in excess concentrated \(\text{HNO}_3\text{(aq)}\). An excess of \(\text{NaCl(aq)}\) is added to the solution, causing all of the silver to precipitate as \(\text{AgCl(s)}\). The precipitate is collected on filter paper, washed, and dried to constant mass. The experimental data and molar masses are shown in the tables below.

| Measurement | Mass |
| :--- | :--- |
| Mass of alloy sample | \(2.00 \text{ g}\) |
| Mass of dry filter paper | \(0.800 \text{ g}\) |
| Mass of filter paper \(+\) dry \(\text{AgCl(s)}\) | \(2.235 \text{ g}\) |

| Substance | Molar Mass (\(\text{g/mol}\)) |
| :--- | :--- |
| \(\text{Ag}\) | \(108.0\) |
| \(\text{Cl}\) | \(35.5\) |
| \(\text{AgCl}\) | \(143.5\) |

Based on the data, what is the mass percent of \(\text{Ag}\) in the alloy sample?

- **A.** \(54.0\%\)
- **B.** \(71.8\%\)
- **C.** \(84.1\%\)
- **D.** \(95.4\%\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123457/*