Dilutions: Videos & Practice Problems

What is the primary purpose of performing a dilution on a solution?

What is a stock solution?

What visual change typically occurs in a solution as it is diluted?

If you have 100 mL of a 2 M solution and dilute it to 500 mL, what is the molarity of the diluted solution?

In the equation M₁V₁ = M₂V₂, what do M₁ and V₁ represent?

Which statement is true regarding M₁ and M₂ in a dilution process?

If you start with 200 mL of solution and add 300 mL of water, what is the final volume (V₂)?

A laboratory technician needs to prepare 1.0 L of a 0.50 M solution from a 2.0 M stock solution. How much stock solution is required?

Which of the following statements best describes the effect of dilution on molarity?

You have 250 mL of a 3.0 M solution. After adding 750 mL of water, what is the molarity of the new solution?

A chemist has 500 mL of a 4 M solution and needs to dilute it to 1 M. What will be the final volume of the solution?

Why does a solution's color become lighter as it is diluted?

If you have 150 mL of a solution and add 350 mL of solvent, what is the final volume?

A solution is diluted from 5 M to 1 M. What is the effect on the concentration of solute particles?

You need to prepare 2 L of a 0.2 M solution from a 1 M stock solution. How much stock solution should you use?

Why are stock solutions used in laboratories?

If 300 mL of a 6 M solution is diluted to 900 mL, what is the molarity of the diluted solution?

In the equation M₁V₁ = M₂V₂, what do M₂ and V₂ represent?

How does dilution affect the concentration of a solution?

You have 400 mL of a 5 M solution. After adding 600 mL of water, what is the molarity of the new solution?

A solution is diluted in two steps. First, $30.0\text{ mL}$ of a $4.50\text{ M}$ stock solution is diluted to $150.0\text{ mL}$. Then $20.0\text{ mL}$ of that diluted solution is further diluted to $250.0\text{ mL}$. What is the final molarity? Round to 3 decimal places.

A student has $45.0\text{ mL}$ of a $2.40\text{ M}$ solution and wants a final concentration of $0.600\text{ M}$. How many milliliters of water must be added? Round to 1 decimal place.

What volume of a $6.00\text{ M}$ stock $NaCl$ solution is needed to prepare $750.0\text{ mL}$ of a $0.480\text{ M}$ solution? Round to 2 decimal places.

A laboratory manual states that $18.0\text{ mL}$ of a stock solution was diluted to $250.0\text{ mL}$ to make a solution that is $0.216\text{ M}$. What was the molarity of the stock solution? Round to 2 decimal places.

To prepare $500.0\text{ mL}$ of a $0.0400\text{ M}$ solution, a student can use either a $0.200\text{ M}$ stock or a $2.00\text{ M}$ stock. If the better choice is the one requiring the larger measured aliquot, what aliquot volume should be transferred? Round to 1 decimal place.

A student intends to prepare $250.0\text{ mL}$ of a $0.200\text{ M}$ solution from a $1.00\text{ M}$ stock. By mistake, the student transfers $47.0\text{ mL}$ of stock and still dilutes to exactly $250.0\text{ mL}$. What concentration is actually obtained? Round to 3 decimal places.

How large must the final volume be if $85.0\text{ mL}$ of a $1.75\text{ M}$ solution is diluted until its concentration becomes $0.350\text{ M}$? Round to 1 decimal place.

A technician adds water to $0.125\text{ L}$ of a $1.80\text{ M}$ solution until the total volume is $825\text{ mL}$. What is the new molarity? Round to 3 decimal places.

A chemist uses $35.0\text{ mL}$ of a $1.50\text{ M}$ $NaOH$ stock solution and dilutes it to $500.0\text{ mL}$. If the molar mass of $NaOH$ is $40.00\text{ g/mol}$, what mass of $NaOH$ is present in the final diluted solution? Round to 2 decimal places.