Final answer:
To calculate the molarity of the silver(I) perchlorate solution, convert the given mass to moles using the molar mass of AgClO4 and divide by the volume of the solution. Assuming a 1 L flask was used, the concentration is approximately 0.423 M.
Step-by-step explanation:
To calculate the concentration of the silver(I) perchlorate solution prepared by a chemist, we first need to understand that concentration commonly refers to the molarity of a solution, which is the number of moles of solute per liter of solution (mol/L). However, the question does not specify the volume of the solution made, which is essential for calculating molarity. Assuming that '1.3x10² of silver(I) perchlorate' is meant to represent 1.3 x 10² grams (though it would be more precise if the units were clearly specified) and the volumetric flask used is of 1 L capacity, as per the information provided as a reference.
In this case, the concentration calculation would be:
- First, convert the mass of silver(I) perchlorate to moles using its molar mass:
Molar mass of AgClO4 (silver(I) perchlorate) = 207.87 (Ag) + 35.45 (Cl) + 4(15.999 (O)) = 207.87 + 35.45 + 63.996 = 307.316 g/mol
Number of moles of AgClO4 = (mass in grams) / (molar mass)
Number of moles of AgClO4 = (130) / (307.316) ≈ 0.423 moles
- Next, calculate the molarity:
Molarity (M) = (moles of solute) / (volume of solution in liters)
M = 0.423 moles / 1 L = 0.423 M
Therefore, the concentration of the silver(I) perchlorate solution is 0.423 M.
Please note that this calculation is based on the assumption of a 1 L volumetric flask; if a different flask size was used, the volume part of the molarity equation must be updated accordingly.