Understanding Molality

What is the formula for calculating molality?

• Grams of solute divided by liters of solution

• Moles of solute divided by kilograms of solvent

• Grams of solute divided by kilograms of solvent

• Moles of solute divided by liters of solution

Which of the following is NOT a derived formula from the molality equation?

• Molality = moles of solute × kilograms of solvent

• Kilograms of solvent = moles of solute / molality

• Molality = moles of solute / kilograms of solvent

• Moles of solute = kilograms of solvent × molality

In the example with 0.15 moles of salt and 0.25 kg of water, what is the molality of the solution?

• 0.60 m

• 0.75 m

• 0.50 m

• 0.25 m

If a solution has a molality of 1.35 × 10^-4 m and 4.5 kg of solvent, how many moles of solute are present?

• 6.1 × 10^-4 moles

• 4.5 × 10^-4 moles

• 5.0 × 10^-4 moles

• 7.2 × 10^-4 moles

In the example with 6.5 moles of solute and a molality of 1.5 m, what is the mass of the solvent?

• 3.5 kg

• 6.0 kg

• 5.0 kg

• 4.3 kg

What is the first step in calculating molality when given grams of solute?

• Convert kilograms to moles

• Convert moles to kilograms

• Convert grams to moles

• Convert grams to kilograms

How do you convert 345 grams of water to kilograms?

• Multiply by 1000

• Divide by 1000

• Add 1000

• Subtract 1000

In the final example, what is the molality of the solution with 70.5 g of NaCl in 345 g of water?

• 3.54 m

• 2.50 m

• 4.00 m

• 1.75 m

What is the molar mass of NaCl used in the final example?

• 65 g/mol

• 60 g/mol

• 58 g/mol

• 55 g/mol

What does the lowercase 'm' stand for in the context of molality?

• Grams per kilogram

• Grams per liter

• Moles per kilogram

• Moles per liter