Dilution Concepts and Calculations

The video tutorial explains how to dilute a concentrated Kool-Aid solution to make it drinkable. It introduces the concept of molarity and demonstrates how to calculate the volume of concentrated syrup needed to achieve a desired dilution. The tutorial generalizes the dilution equation for any solution and applies it to a sulfuric acid example. Safety tips for handling acids are also provided.

Why is it necessary to dilute the concentrated Kool-Aid solution before serving?

• To make it more concentrated

• To increase the sugar content

• To reduce the sugar content to a drinkable level

• To change the color of the solution

What remains constant when a solution is diluted?

• The amount of solute

• The concentration of the solution

• The volume of the solution

• The temperature of the solution

How do you calculate the moles of solute in a solution?

• Moles = Molarity / Volume

• Moles = Volume x Temperature

• Moles = Volume / Molarity

• Moles = Molarity x Volume

What is the dilution equation used for calculating the volume of a concentrated solution?

• M1 / V1 = M2 / V2

• M1 + V1 = M2 + V2

• M1 x V1 = M2 x V2

• M1 - V1 = M2 - V2

In the Kool-Aid example, what is the volume of the concentrated syrup needed to achieve a 2 molar solution?

• 0.75 L

• 0.25 L

• 1.00 L

• 0.50 L

What is the molarity of the stock sulfuric acid solution used in the example?

• 0.5 molar

• 5 molar

• 12 molar

• 3 molar

How much of the 12 molar sulfuric acid is needed to make 0.5 L of a 3 molar solution?

• 0.500 L

• 0.375 L

• 0.250 L

• 0.125 L

What safety precaution is emphasized when diluting acids?

• Always add acid to water

• No specific precaution is needed

• Always add water to acid

• Mix acid and water simultaneously

What is the final volume of a 3 molar HCl solution made from 10 mL of 12 molar HCl?

• 20 mL

• 30 mL

• 40 mL

• 50 mL

What is the initial volume of the concentrated HCl solution in the example?

• 15 mL

• 10 mL

• 5 mL

• 20 mL