Calculating Molarity: Concepts and Practice Problems

What are the two main components of a solution?

• Acid and base

• Solvent and solute

• Liquid and gas

• Metal and non-metal

Why is water considered a universal solvent?

• It is found in all chemical laboratories

• It dissolves more substances than any other liquid

• It is the only liquid that can dissolve gases

• It is a liquid at room temperature

What does a concentrated solution contain?

• A small amount of solute

• No solute at all

• A large amount of solute

• Only liquid solvents

What is the formula for molarity?

• Liters of solution over moles of solute

• Grams of solute over liters of solution

• Moles of solute over liters of solution

• Moles of solvent over grams of solute

How do you convert grams to moles for molarity calculations?

• Multiply by the molar mass

• Add the molar mass

• Subtract the molar mass

• Divide by the molar mass

What does the term 'molarity' refer to in chemistry?

• The concentration of a solution

• The temperature of a solution

• The volume of a solvent

• The weight of a solution

What is the molarity of a solution made by dissolving 11.5 grams of NaOH in 1.50 liters of water?

• 0.2875 M

• 0.192 M

• 1.50 M

• 11.5 M

How do you convert milliliters to liters in molarity calculations?

• Divide by 100

• Multiply by 1000

• Divide by 1000

• Multiply by 100

What is the molarity of a solution prepared by dissolving 1.56 grams of gaseous HCl in water to make a 26.8 milliliter solution?

• 0.0427 M

• 1.56 M

• 1.60 M

• 26.8 M

To prepare a 0.200 M solution of K2Cr2O7, how many grams of the solid should be weighed out for one liter of solution?

• 294 grams

• 1 liter

• 58.5 grams

• 0.200 grams