How many milliliters of an aqueous solution of 0.172 M silver fluoride is needed to obtain 12.1 grams of the salt?
12.1 grams is how many moles?
Moles=Molarity*volume
you are given molarity as .172, so solve for volume (in liters)and convert to ml
To solve this problem, we need to use the concept of molarity, which is defined as the number of moles of solute per liter of solution.
Step 1: Calculate the molar mass of silver fluoride (AgF)
The molar mass of silver (Ag) is 107.87 g/mol, and the molar mass of fluorine (F) is 18.99 g/mol. To calculate the molar mass of silver fluoride, we add the molar masses of Ag and F:
Molar mass of AgF = Molar mass of Ag + Molar mass of F = 107.87 g/mol + 18.99 g/mol = 126.86 g/mol
Step 2: Convert the mass of silver fluoride to moles
To convert the mass of silver fluoride (12.1 grams) to moles, divide the mass by the molar mass:
Moles of AgF = Mass of AgF / Molar mass of AgF = 12.1 g / 126.86 g/mol
Step 3: Use the molarity formula to find the volume
The molarity (M) is defined as moles of solute per liter of solution. Rearranging the formula, we get:
Volume of solution (in liters) = Moles of solute / Molarity
In this problem, we are given the molarity of the solution (0.172 M) and the moles of solute from Step 2. Plugging these values into the formula, we have:
Volume of solution (in liters) = Moles of AgF / Molarity = (12.1 g / 126.86 g/mol) / 0.172 mol/L
Step 4: Convert the volume to milliliters
Finally, to convert the volume from liters to milliliters, multiply by 1000:
Volume of solution (in milliliters) = Volume of solution (in liters) * 1000
Plug in the values and calculate to get the final answer.