What is the molar mass of Ag3PO4?
Understand the Problem
The question is asking for the molar mass of the compound silver phosphate, represented by the chemical formula Ag3PO4. To find the molar mass, we need to sum the atomic masses of all the atoms present in the formula: three silver (Ag) atoms, one phosphorus (P) atom, and four oxygen (O) atoms.
Answer
The molar mass of silver phosphate is \( 418.58 \, \text{g/mol} \).
Answer for screen readers
The molar mass of silver phosphate (Ag3PO4) is ( 418.58 , \text{g/mol} ).
Steps to Solve
- Identify Atomic Masses
Find the atomic masses of each element in the compound Ag3PO4. The atomic masses are approximately:
- Silver (Ag): 107.87 g/mol
- Phosphorus (P): 30.97 g/mol
- Oxygen (O): 16.00 g/mol
- Calculate Silver's Contribution
Since there are three silver atoms, we multiply the atomic mass of silver by 3: $$ \text{Mass of Ag} = 3 \times 107.87 , \text{g/mol} = 323.61 , \text{g/mol} $$
- Calculate Phosphorus's Contribution
There is one phosphorus atom, so we take the atomic mass of phosphorus directly: $$ \text{Mass of P} = 1 \times 30.97 , \text{g/mol} = 30.97 , \text{g/mol} $$
- Calculate Oxygen's Contribution
There are four oxygen atoms, so we multiply the atomic mass of oxygen by 4: $$ \text{Mass of O} = 4 \times 16.00 , \text{g/mol} = 64.00 , \text{g/mol} $$
- Sum All Contributions
Now we add all the contributions together to find the total molar mass of silver phosphate: $$ \text{Total Molar Mass} = \text{Mass of Ag} + \text{Mass of P} + \text{Mass of O} $$ Substituting the values: $$ \text{Total Molar Mass} = 323.61 , \text{g/mol} + 30.97 , \text{g/mol} + 64.00 , \text{g/mol} = 418.58 , \text{g/mol} $$
The molar mass of silver phosphate (Ag3PO4) is ( 418.58 , \text{g/mol} ).
More Information
The molar mass is important in chemical calculations, as it allows for the conversion between grams and moles. For silver phosphate, knowing the molar mass helps in stoichiometric calculations in chemical reactions.
Tips
- Failing to multiply the atomic mass by the correct number of atoms for each element.
- Forgetting to add all the contributions together to get the final total mass.