A solution of silver perchlorate (AgClO4) is made by dissolving 40.4 g of pure silver perchlorate and diluting it to exactly 140 ml. What is the solutions molarity?

Can you just go through the steps of what I need to do? I'm so confused. Thanks

a. determine the mole mass of AgClO4

b. then determine the moles of silver perchlorate. 40.4/molmass

c. then divide by liters of solution (0.140)

Molarity=moles/volumeinLiters

1.413mol/L

Sure! I'll walk you through the steps to find the molarity of the silver perchlorate solution.

Step 1: Calculate the number of moles of silver perchlorate (AgClO4) dissolved:
To do this, you need to know the molar mass of AgClO4, which can be calculated by adding up the atomic masses of each element in the compound. The atomic masses of silver (Ag), chlorine (Cl), and oxygen (O) are 107.87 g/mol, 35.45 g/mol, and 16.00 g/mol, respectively.

Molar mass of AgClO4 = (Ag: 1 x 107.87 g/mol) + (Cl: 1 x 35.45 g/mol) + (O: 4 x 16.00 g/mol)
= 107.87 g/mol + 35.45 g/mol + 64.00 g/mol
= 207.32 g/mol

Now, you need to convert the given mass of pure silver perchlorate (40.4 g) to moles using the formula:

Number of moles = Given mass / Molar mass
= 40.4 g / 207.32 g/mol
≈ 0.1952 mol

Step 2: Calculate the volume of the solution in liters:
The given volume is 140 ml, but molarity requires the volume to be expressed in liters. So, convert the volume to liters by dividing it by 1000 (since there are 1000 ml in 1 liter):

Volume (in liters) = 140 ml / 1000
= 0.140 L

Step 3: Calculate the molarity:
Finally, use the formula for molarity, which is defined as moles of solute divided by liters of solution:

Molarity (M) = Moles of solute / Volume of solution (in liters)
= 0.1952 mol / 0.140 L
≈ 1.394 M

So, the molarity of the silver perchlorate solution is approximately 1.394 M.