Exploring the World of Chemistry: Aluminum Nitrate Ions!
How can we determine the number of ions in a given mass of aluminum nitrate?
Let's dive into the world of chemistry and uncover the mystery behind aluminum nitrate ions. Are you ready?
Understanding the Calculation of Aluminum Nitrate Ions
Aluminum nitrate is a fascinating compound composed of aluminum ions and nitrate ions. To calculate the number of ions in a certain mass of aluminum nitrate, we need to follow a series of steps:
- Find the molar mass of aluminum nitrate (Al(NO3)3).
- Convert the given mass of aluminum nitrate to moles using the molar mass.
- Multiply the number of moles by the number of ions per formula unit.
By following these steps, we can uncover the secrets of aluminum nitrate ions and their presence in a specific mass of the compound.
Unlocking the Mystery: Calculating Aluminum Nitrate Ions
Aluminum nitrate (Al(NO3)3) is composed of aluminum ions (Al3+) and nitrate ions (NO3-). To determine the number of ions in 15.6 g of aluminum nitrate, we go through the following steps:
- Step 1: Molar mass of aluminum nitrate (Al(NO3)3):
- Aluminum (Al) has a molar mass of 26.98 g/mol.
- Nitrate (NO3-) has a molar mass of 62.01 g/mol.
- Step 2: Convert the given mass of aluminum nitrate to moles:
- Step 3: Multiply the number of moles by the number of ions per formula unit:
The total molar mass of aluminum nitrate is calculated as:
Molar mass of Al(NO3)3 = (1 x molar mass of Al) + (3 x molar mass of NO3-)
Molar mass of Al(NO3)3 = (1 x 26.98 g/mol) + (3 x 62.01 g/mol) = 213.0 g/mol
Number of moles = Given mass / Molar mass
Number of moles = 15.6 g / 213.0 g/mol = 0.0732 mol
Number of ions = Number of moles x Number of ions per formula unit
Number of ions = 0.0732 mol x (1 + 3) = 0.2928 mol
Therefore, there are approximately 0.2928 mol of ions in 15.6 g of aluminum nitrate. Isn't chemistry amazing?