What is the molar mass of silver nitrate?

The molar mass of silver nitrate (AgNO₃) can be calculated by adding the atomic masses of each element in the compound. Silver nitrate consists of silver (Ag), nitrogen (N), and oxygen (O). To find the molar mass, we need to know the atomic masses of these elements, which are approximately: silver (107.87 g/mol), nitrogen (14.01 g/mol), and oxygen (16.00 g/mol). Since there are three oxygen atoms in silver nitrate, we will multiply the atomic mass of oxygen by three.

Calculating the Molar Mass

Let's break it down step by step:

• Silver (Ag): 1 atom × 107.87 g/mol = 107.87 g/mol
• Nitrogen (N): 1 atom × 14.01 g/mol = 14.01 g/mol
• Oxygen (O): 3 atoms × 16.00 g/mol = 48.00 g/mol

Adding It All Together

Now, we simply add these values together to find the total molar mass of silver nitrate:

107.87 g/mol (Ag) + 14.01 g/mol (N) + 48.00 g/mol (O) = 169.88 g/mol

The Final Result

Therefore, the molar mass of silver nitrate is approximately 169.88 g/mol. This value is essential in various applications, such as stoichiometry in chemical reactions, where knowing the exact molar mass helps in calculating the amounts of reactants and products involved.

Practical Implications

Understanding the molar mass of compounds like silver nitrate is crucial in fields such as chemistry, biology, and environmental science. For instance, in a laboratory setting, if you need to prepare a solution of silver nitrate, knowing its molar mass allows you to accurately measure the required amount to achieve a desired concentration.