QQuestionChemistry
QuestionChemistry
Calculate the molar mass of the compound containing Ag+ and SO^42− ions.
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Identify the ions in the compound
The compound contains silver (Ag+) and sulfate (SO4^{2 -}) ions. This suggests we're dealing with silver sulfate (Ag^2SO4).
Step 3:: Determine the number of atoms of each element
- Silver (Ag): 2 atoms - Sulfur (S): 1 atom - Oxygen (O): 4 atoms
Step 4:: Look up the atomic masses
- Oxygen (O): $$m_{O} = 16.00 \mathrm{~g/mol}
- Sulfur (S): m_{S} = 32.07 \mathrm{~g/mol}
Step 5:: Calculate the molar mass by summing the masses of all atoms
\begin{align}
\text{Molar Mass} &= (2 \times m_{Ag}) + (1 \times m_{S}) + (4 \times m_{O}) \ &= (2 \times 107.87) + (1 \times 32.07) + (4 \times 16.00) \ &= 215.74 + 32.07 + 64.00 \ &= 311.81 \mathrm{~g/mol} \end{align}
Final Answer
The molar mass of Ag^2SO^4 is 311.81 \mathrm{~g/mol}.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students