Exploring Molarity Concepts and Applications

Calculate the molarity of a solution containing 0.5 moles of sodium chloride (NaCl) dissolved in 2 liters of water.

• 0.25 M

• 0.5 M

• 1 M

• 2 M

If you have 3 moles of hydrochloric acid (HCl) in 1.5 liters of solution, what is the molarity?

• 1 M

• 2 M

• 3 M

• 4 M

A solution is made by dissolving 0.75 moles of glucose in 0.5 liters of water. What is the molarity of the solution?

• 0.75 M

• 1.5 M

• 2 M

• 3 M

Convert 500 mL of a 2 M solution of sulfuric acid (H₂SO₄) to liters and calculate the number of moles of solute present.

• 0.5 moles

• 1 mole

• 2 moles

• 4 moles

You have a 250 mL solution with a molarity of 3 M. How many moles of solute are in the solution?

• 0.25 moles

• 0.5 moles

• 0.75 moles

• 1 mole

A laboratory technician needs to prepare 1 liter of a 0.1 M potassium chloride (KCl) solution. How many moles of KCl are required?

• 0.01 moles

• 0.1 moles

• 1 mole

• 10 moles

If you dilute 1 liter of a 6 M solution to a final volume of 3 liters, what is the new molarity?

• 1 M

• 2 M

• 3 M

• 4 M

A chemist has a 0.5 M solution of acetic acid. If they need 0.25 moles of acetic acid, how much solution should they use?

• 0.25 L

• 0.5 L

• 0.75 L

• 1 L

How many liters of a 0.2 M solution are needed to obtain 0.4 moles of solute?

• 1 L

• 2 L

• 3 L

• 4 L

A solution contains 0.1 moles of solute in 250 mL of solution. What is the molarity?

• 0.1 M

• 0.2 M

• 0.3 M

• 0.4 M