Molarity and Solutions Concepts

The video tutorial introduces the concept of molarity, explaining how it is a measure of concentration expressed as moles of solute per liter of solution. It covers the definitions of solute, solvent, and solution, and demonstrates how to calculate molarity using examples with moles and grams. The tutorial also includes advanced problems involving molarity calculations with different substances, emphasizing the practical applications of these calculations in preparing solutions with specific concentrations.

What is the term for the substance that gets dissolved in a solution?

• Molarity

• Solvent

• Solute

• Solution

How is molarity expressed in terms of units?

• Liters per mole

• Grams per mole

• Moles per liter

• Grams per liter

If you have 1.25 moles of KCl in 1 liter of solution, what is the molarity?

• 2.5 M

• 1.3 M

• 0.8 M

• 1.25 M

What is the molarity of a solution with 0.65 moles of solute in 0.50 liters of solution?

• 0.8 M

• 1.3 M

• 1.25 M

• 1.4 M

How many moles of sodium fluoride are in 25.2 grams if the molar mass is 42.0 grams per mole?

• 1.3 moles

• 0.8 moles

• 1.25 moles

• 0.6 moles

To make a 1.4 M solution of ammonia in 2.5 liters, how many moles of ammonia are needed?

• 4.5 moles

• 3.5 moles

• 1.4 moles

• 2.5 moles

What is the molarity of a solution if 3.5 moles of NH3 are dissolved in 2.5 liters of water?

• 1.25 M

• 1.4 M

• 0.8 M

• 1.3 M

What is the mass of sodium chloride needed to make 4.5 liters of a 0.154 M solution?

• 40.5 grams

• 58.5 grams

• 25.2 grams

• 42.0 grams

What is the molar mass of sodium chloride used in the final problem?

• 42.0 grams per mole

• 58.5 grams per mole

• 25.2 grams per mole

• 40.5 grams per mole

What happens to the molarity of a solution if more solute is added?

• It becomes zero

• It increases

• It remains the same

• It decreases