What is the molar mass of (NH_(4))_(3)PO_(4) ? Keep three places after the decimal (the thousandths place). square g/mol

To find the molar mass of \((NH_{4})_{3}PO_{4}\), we need to sum the molar masses of all the atoms in the compound.<br /><br />1. **Calculate the molar mass of \(NH_{4}\):**<br /> - Nitrogen (N): \(14.01 \, \text{g/mol}\)<br /> - Hydrogen (H): \(1.01 \, \text{g/mol}\)<br /><br /> For \(NH_{4}\):<br /> \[<br /> 14.01 \, \text{g/mol} + 4 \times 1.01 \, \text{g/mol} = 14.01 \, \text{g/mol} + 4.04 \, \text{g/mol} = 18.05 \, \text{g/mol}<br /> \]<br /><br />2. **Calculate the molar mass of \((NH_{4})_{3}\):**<br /> \[<br /> 3 \times 18.05 \, \text{g/mol} = 54.15 \, \text{g/mol}<br /> \]<br /><br />3. **Calculate the molar mass of \(PO_{4}\):**<br /> - Phosphorus (P): \(30.97 \, \text{g/mol}\)<br /> - Oxygen (O): \(16.00 \, \text{g/mol}\)<br /><br /> For \(PO_{4}\):<br /> \[<br /> 30.97 \, \text{g/mol} + 4 \times 16.00 \, \text{g/mol} = 30.97 \, \text{g/mol} + 64.00 \, \text{g/mol} = 94.97 \, \text{g/mol}<br /> \]<br /><br />4. **Add the molar masses of \((NH_{4})_{3}\) and \(PO_{4}\):**<br /> \[<br /> 54.15 \, \text{g/mol} + 94.97 \, \text{g/mol} = 149.12 \, \text{g/mol}<br /> \]<br /><br />Therefore, the molar mass of \((NH_{4})_{3}PO_{4}\) is \(149.120 \, \text{g/mol}\).