What is the molar mass of silver nitrate ?
The Correct Answer and Explanation is:
Correct Answer:
The molar mass of silver nitrate (AgNO₃) is 169.87 g/mol.
Explanation
The molar mass of a compound is the mass of one mole of that substance, expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms present in the chemical formula.
Silver nitrate has the chemical formula AgNO₃, meaning it consists of:
- 1 silver atom (Ag)
- 1 nitrogen atom (N)
- 3 oxygen atoms (O)
To determine the molar mass, we use the atomic masses from the periodic table:
- Silver (Ag) = 107.87 g/mol
- Nitrogen (N) = 14.01 g/mol
- Oxygen (O) = 16.00 g/mol
Now, we calculate: Molar Mass of AgNO₃=(1×107.87)+(1×14.01)+(3×16.00)\text{Molar Mass of AgNO₃} = (1 \times 107.87) + (1 \times 14.01) + (3 \times 16.00) =107.87+14.01+48.00=169.88 g/mol= 107.87 + 14.01 + 48.00 = \boxed{169.88\ \text{g/mol}}
(You may also see 169.87 g/mol depending on rounding conventions.)
Importance of Molar Mass:
Knowing the molar mass of silver nitrate is essential in chemistry for:
- Stoichiometry – determining how much of a substance is needed or produced in a chemical reaction.
- Concentration Calculations – converting between grams and moles when preparing solutions.
- Quantitative Analysis – calculating yields, limiting reagents, or titrations in labs.
Silver nitrate is a common reagent used in analytical chemistry, especially in precipitation reactions and in tests for halide ions. It’s also used in medicine for its antibacterial properties. Therefore, accurate molar mass is crucial in practical applications where precise measurement is required.
In summary, the molar mass of AgNO₃ is 169.87 g/mol, calculated by adding the atomic masses of silver, nitrogen, and oxygen atoms.
