Molarity of the solution that results when 71.3 g silver nitrate is dissolved in enough water to give a final volume of 757 mL.
To find the molarity of the solution, you need to know the number of moles of silver nitrate and the volume of the solution. Let's break down the steps to find the answer:
Step 1: Find the number of moles of silver nitrate.
To calculate the number of moles, we use the formula:
moles (mol) = mass (g) / molar mass (g/mol)
The molar mass of silver nitrate (AgNO3) can be calculated by adding up the atomic masses of its constituent elements:
Ag: 1 atom x 107.87 g/mol = 107.87 g/mol
N: 1 atom x 14.01 g/mol = 14.01 g/mol
O: 3 atoms x 16.00 g/mol = 48.00 g/mol
Adding the atomic masses together gives the molar mass of AgNO3: 107.87 g/mol + 14.01 g/mol + 48.00 g/mol = 169.88 g/mol
Now, let's calculate the number of moles:
moles of AgNO3 = 71.3 g / 169.88 g/mol ≈ 0.420 mol
Step 2: Find the volume of the solution in liters.
The volume given is 757 mL. To convert milliliters to liters, divide the volume by 1000:
volume (L) = 757 mL ÷ 1000 mL/L = 0.757 L
Step 3: Calculate the molarity.
Molarity (M) is defined as moles of solute per liter of solution:
Molarity (M) = moles of solute / volume of solution (L)
Molarity = 0.420 mol / 0.757 L ≈ 0.554 M
Therefore, the molarity of the solution is approximately 0.554 M when 71.3 g of silver nitrate is dissolved in enough water to give a final volume of 757 mL.