How would you prepare 100.0 mL of 0.07500 M AgNO3 solution starting with pure solute?
molarity = # moles/L and
moles = grams/molar mass.
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To prepare a 100.0 mL of 0.07500 M AgNO3 solution starting with pure solute, you will need to follow these steps:
Step 1: Determine the required amount of AgNO3.
The concentration (Molarity) is defined as moles of solute per liter of solution. Therefore, you need to calculate the moles of AgNO3 required for the desired concentration.
Molarity (M) = moles of solute / volume of solution (in liters)
Rearranging the formula, moles of solute = Molarity × volume of solution (in liters)
moles of AgNO3 = 0.07500 M × 0.1000 L
Step 2: Calculate the mass of AgNO3 needed.
To determine the mass of AgNO3 required, you need to use its molar mass. The molar mass of AgNO3 is obtained by adding up the atomic masses of its constituent elements.
The molar mass of AgNO3 = atomic mass of Ag + atomic mass of N + 3 × atomic mass of O
The molar mass of AgNO3 = (107.87 g/mol) + (14.01 g/mol) + 3 × (16.00 g/mol)
Step 3: Prepare the solution.
Once you have calculated the mass of AgNO3 needed, you can prepare the solution by dissolving the calculated amount of AgNO3 in a small volume of water. After the solute has dissolved, add more solvent (water) to reach a final volume of 100.0 mL.
It's important to note that when working with concentrated acids or bases, appropriate safety precautions should be taken, including the use of gloves, goggles, and a fume hood if necessary.