Q. What is the molar mass of \(\text{AgNO}_3\)?

Q: What is the molar mass of \mathrm{AgNO_3} ?

\mathrm{AgNO_3} molar mass \approx 107.87 + 14.01 + 3(16.00) = 169.88 \, \mathrm{g/mol} (about 169.9 \, \mathrm{g/mol}).

Q: What atomic masses should be used for the calculation?

Use standard atomic masses: \mathrm{Ag} \approx 107.87 , \mathrm{N} \approx 14.01 , \mathrm{O} \approx 16.00 \, \mathrm{g/mol} .

Q: Why does oxygen get multiplied by 3 in \mathrm{AgNO_3} ?

The subscript in \mathrm{NO_3} indicates three oxygen atoms per formula unit, so you add 3 \times 16.00.

Q: What is the molar mass of \mathrm{Ag^+} and how does it relate?

\mathrm{Ag^+} molar mass is the atomic mass of Ag: \approx 107.87 \, \mathrm{g/mol} . For \mathrm{AgNO_3} , add \mathrm{NO_3} mass as well.

Answer

To find the molar mass of silver nitrate, \( \text{AgNO}_3 \), add the atomic masses of its atoms: \( \text{Ag} \), \( \text{N} \), and \( \text{O} \) (three oxygens).

\[
\text{Molar mass} = M(\text{Ag}) + M(\text{N}) + 3M(\text{O})
\]

Using typical atomic masses \( M(\text{Ag}) \approx 107.87 \, \text{g/mol} \), \( M(\text{N}) \approx 14.01 \, \text{g/mol} \), and \( M(\text{O}) \approx 16.00 \, \text{g/mol} \):

\[
107.87 + 14.01 + 3(16.00) = 107.87 + 14.01 + 48.00 = 169.88 \, \text{g/mol}
\]

Final result: \( \text{AgNO}_3 \) has a molar mass of \( 169.88 \, \text{g/mol} \) (about \( 169.9 \, \text{g/mol} \)).

Detailed Explanation

To find the molar mass of silver nitrate, \( \text{AgNO}_3 \), follow these steps.

Step 1: Identify the atoms in the formula.

\(\text{AgNO}_3\) contains:

1 atom of Ag (silver)
1 atom of N (nitrogen)
3 atoms of O (oxygen)

Step 2: Write the atomic masses you will use.

Use standard atomic (periodic table) values:

Ag: \(107.87\ \text{g/mol}\)
N: \(14.01\ \text{g/mol}\)
O: \(16.00\ \text{g/mol}\)

Step 3: Multiply each atomic mass by how many of each atom are in the formula.

Compute each contribution:

Silver contribution: \(1 \times 107.87 = 107.87\ \text{g/mol}\)
Nitrogen contribution: \(1 \times 14.01 = 14.01\ \text{g/mol}\)
Oxygen contribution: \(3 \times 16.00 = 48.00\ \text{g/mol}\)

Step 4: Add all the contributions to get the molar mass.

Sum them:

\[
\text{Molar mass of } \text{AgNO}_3 = 107.87 + 14.01 + 48.00
\]
\[
\text{Molar mass of } \text{AgNO}_3 = 169.88\ \text{g/mol}
\]

Final Answer:

The molar mass of \( \text{AgNO}_3 \) is \( \boxed{169.88\ \text{g/mol}} \).

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General Chemistry FAQs

What is the molar mass of \( \mathrm{AgNO_3} \) ?

\( \mathrm{AgNO_3} \) molar mass \( \approx 107.87 + 14.01 + 3(16.00) = 169.88 \, \mathrm{g/mol} \) (about \(169.9 \, \mathrm{g/mol}\)).

What atomic masses should be used for the calculation?

Use standard atomic masses: \( \mathrm{Ag} \approx 107.87 \), \( \mathrm{N} \approx 14.01 \), \( \mathrm{O} \approx 16.00 \, \mathrm{g/mol} \).

How do you set up the molar mass expression for \( \mathrm{AgNO_3} \)?

\( M = 1(\mathrm{Ag}) + 1(\mathrm{N}) + 3(\mathrm{O}) = 107.87 + 14.01 + 3(16.00) \).

Why does oxygen get multiplied by 3 in \( \mathrm{AgNO_3} \)?

The subscript in \( \mathrm{NO_3} \) indicates three oxygen atoms per formula unit, so you add \(3 \times 16.00\).

What is the molar mass of \( \mathrm{Ag^+} \) and how does it relate?

\( \mathrm{Ag^+} \) molar mass is the atomic mass of Ag: \( \approx 107.87 \, \mathrm{g/mol} \). For \( \mathrm{AgNO_3} \), add \( \mathrm{NO_3} \) mass as well.

What is the molar mass of the \( \mathrm{NO_3^-} \) portion?

\( M(\mathrm{NO_3^-}) = 14.01 + 3(16.00) = 62.01 \, \mathrm{g/mol} \). Combine with Ag: \(107.87 + 62.01 = 169.88 \, \mathrm{g/mol}\).

AgNO3 molar mass is 169.87 g/mol.
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