Dilution and Intermolecular Forces in Chemistry

What is the initial concentration of the sodium sulfate solution in the example?

• 0.125 M

• 1 M

• 0.5 M

• 2 M

What is the target concentration for the new sodium sulfate solution?

• 1 M

• 0.125 M

• 0.5 M

• 2 M

What is the volume of the new solution we want to prepare?

• 100 mL

• 250 mL

• 1000 mL

• 500 mL

What is the intuition behind diluting a higher concentration solution to a lower concentration?

• Taking a larger volume of the original solution and adding solvent

• Taking a smaller volume of the original solution and adding solvent

• Adding less solvent

• Adding more solute

How do we calculate the number of moles needed in the final solution?

• By subtracting the volume from the molarity

• By dividing the volume by the molarity

• By multiplying the volume by the molarity

• By adding the volume and molarity

What is the formula for molarity?

• Number of moles of solute per liters of solution

• Number of milliliters of solution per moles of solute

• Number of liters of solution per moles of solute

• Number of moles of solute per milliliters of solution

How many moles of sodium sulfate are needed in the final solution?

• 0.125 moles

• 0.5 moles

• 0.0625 moles

• 1 mole

What volume of the original 1 M solution is required to achieve the desired concentration?

• 125 mL

• 250 mL

• 62.5 mL

• 500 mL

What is the final step to prepare the 0.125 M solution?

• Add 500 mL of the original solution

• Add more solute

• Add 62.5 mL of the original solution and fill up to 500 mL with water

• Add 62.5 mL of water

Why is it important to consider significant figures in the calculations?

• To ensure accuracy

• To reduce the volume of the solution

• To make the solution more concentrated

• To increase the number of moles