Answer:
Step-by-step explanation:
To find the mole fraction of silver nitrate in the solution, you need to first find the molar mass of silver nitrate and then the number of moles of silver nitrate in the solution. Here's how you can do that:
Calculate the molar mass of silver nitrate:
AgNo3 has a molar mass of 169.87 g/mol
Calculate the mass of silver nitrate in the solution:
The solution is 12.0% by mass silver nitrate, so the mass of silver nitrate in 100 mL of the solution is:
mass of AgNO3 = 100 mL * 0.12 g/mL = 12 g
Calculate the number of moles of silver nitrate:
Number of moles of AgNO3 = mass of AgNO3 / molar mass of AgNO3
Number of moles of AgNO3 = 12 g / 169.87 g/mol = 0.0703 moles
Calculate the number of moles of the solvent (water) in the solution:
Since the density of the solution is 1.11 g/mL, the mass of 100 mL of the solution is 111 g. The mass of water in the solution is:
mass of water = 111 g - 12 g = 99 g
Since the molar mass of water is 18.015 g/mol, the number of moles of water in the solution is:
number of moles of water = 99 g / 18.015 g/mol = 5.49 moles
Calculate the mole fraction of silver nitrate:
The mole fraction of silver nitrate is the ratio of the number of moles of silver nitrate to the total number of moles in the solution:
mole fraction of AgNO3 = 0.0703 moles / (0.0703 moles + 5.49 moles) = 0.0127
So, the mole fraction of silver nitrate in the solution is 0.0127.