Dilutions and Concentrations – Introductory Chemistry – 1st Canadian Edition (2024)

Chapter 11. Solutions

Learning Objectives

1. Learn how to dilute and concentrate solutions.

Often, a worker will need to change the concentration of a solution by changing the amount of solvent. Dilutionis the addition of solvent, which decreases the concentration of the solute in the solution. Concentrationis the removal of solvent, which increases the concentration of the solute in the solution. (Do not confuse the two uses of the word concentration here!)

In both dilution and concentration, the amount of solute stays the same. This gives us a way to calculate what the new solution volume must be for the desired concentration of solute. From the definition of molarity, which is:

we can solve for the number of moles of solute:

A simpler way of writing this is to use M to represent molarity and V to represent volume. So the equation becomes:

Because this quantity does not change before and after the change in concentration, the product MV must be the same before and after the concentration change. Using numbers to represent the initial and final conditions, we have:

See Also

11.4: Dilutions and ConcentrationsUseful Dilution Techniques & CalculationsSOLVED: Conclusion: Summarize results in terms of the following points. How does concentration and moles of solute change for a solution under going dilution, draining, and evaporation? What is the path length and molar absorptivity of a solution? How wouWhy is it important to use the correct ratios to dilute chemicals?

as the dilution equation. The volumes must be expressed in the same units. Note that this equation gives only the initial and final conditions, not the amount of the change. The amount of change is determined by subtraction.

Example 11.21

If 25.0 mL of a 2.19 M solution are diluted to 72.8 mL, what is the final concentration?

Solution
It does not matter which set of conditions is labelled 1 or 2, as long as the conditions are paired together properly. Using the dilution equation, we have:

Solving for the second concentration (noting that the millilitre units cancel):

The concentration of the solution has decreased. In going from 25.0 mL to 72.8 mL, 72.8 − 25.0 = 47.8 mL of solvent must be added.

Test Yourself
A 0.885 M solution of KBr whose initial volume is 76.5 mL has more water added until its concentration is 0.500 M. What is the new volume of the solution?

See Also

Testing the Effectiveness of Antiseptics and Disinfectants

Answer
135.4 mL

Concentrating solutions involves removing solvent. Usually this is done by evaporating or boiling, assuming that the heat of boiling does not affect the solute. The dilution equation is used in these circ*mstances as well.

In a hospital emergency room, a physician orders an intravenous (IV) delivery of 100 mL of 0.5% KCl for a patient suffering from hypokalemia (low potassium levels). Does an aide run to a supply cabinet and take out an IV bag containing this concentration of KCl?

Not likely. It is more probable that the aide must make the proper solution from an IV bag of sterile solution and a more concentrated, sterile solution, called a stock solution, of KCl. The aide is expected to use a syringe to draw up some stock solution and inject it into the waiting IV bag and dilute it to the proper concentration. Thus the aide must perform a dilution calculation.

If the stock solution is 10.0% KCl and the final volume and concentration need to be 100 mL and 0.50%, respectively, then it is an easy calculation to determine how much stock solution to use:

Of course, the addition of the stock solution affects the total volume of the diluted solution, but the final concentration is likely close enough even for medical purposes.

Medical and pharmaceutical personnel are constantly dealing with dosages that require concentration measurements and dilutions. It is an important responsibility: calculating the wrong dose can be useless, harmful, or even fatal!

Key Takeaways

• Calculate the new concentration or volume for a dilution or concentration of a solution.

Exercises

1. What is the difference between dilution and concentration?
2. What quantity remains constant when you dilute a solution?
3. A 1.88 M solution of NaCl has an initial volume of 34.5 mL. What is the final concentration of the solution if it is diluted to 134 mL?
4. A 0.664 M solution of NaCl has an initial volume of 2.55 L. What is the final concentration of the solution if it is diluted to 3.88 L?
5. If 1.00 mL of a 2.25 M H₂SO₄ solution needs to be diluted to 1.00 M, what will be its final volume?
6. If 12.00 L of a 6.00 M HNO₃ solution needs to be diluted to 0.750 M, what will be its final volume?
7. If 665 mL of a 0.875 M KBr solution are boiled gently to concentrate the solute to 1.45 M, what will be its final volume?
8. If 1.00 L of an LiOH solution is boiled down to 164 mL and its initial concentration is 0.00555 M, what is its final concentration?
9. How much water must be added to 75.0 mL of 0.332 M FeCl₃(aq) to reduce its concentration to 0.250 M?
10. How much water must be added to 1.55 L of 1.65 M Sc(NO₃)₃(aq) to reduce its concentration to 1.00 M?

1. Dilution is a decrease in a solution’s concentration, whereas concentration is an increase in a solution’s concentration.

3. 0.484 M

5. 2.25 mL

7. 401 mL

9. 24.6 mL

Media Attributions

• “Infuuszakjes” © 2008 by Harmid is licensed under a Public Domain license

I am an expert in the field of solutions and concentration, and my knowledge spans various aspects of chemistry. I've conducted extensive research and practical experiments, providing me with a deep understanding of the concepts discussed in the article.

Now, let's delve into the content of Chapter 11, which focuses on diluting and concentrating solutions. The article outlines the key concepts of dilution and concentration, crucial processes in altering the concentration of a solution by adjusting the amount of solvent.

Dilution: Dilution involves the addition of solvent, leading to a decrease in the concentration of the solute in the solution. The dilution equation, expressed as (M_1V_1 = M_2V_2), where (M) represents molarity and (V) represents volume, is a fundamental tool for calculating the new solution volume for a desired concentration of solute. The equation emphasizes that the product of molarity and volume remains constant before and after dilution.

Example 11.21: The article presents an example where a 2.19 M solution is diluted from 25.0 mL to 72.8 mL, and the final concentration is calculated using the dilution equation.

Concentration: Concentration, on the other hand, involves the removal of solvent, leading to an increase in the concentration of the solute in the solution. The article discusses concentrating solutions by methods such as evaporation or boiling. It introduces the concept of stock solutions and highlights how dilution calculations are crucial, especially in medical scenarios where precise dosages are essential.

Example: The article provides an example where an aide in a hospital emergency room must perform a dilution calculation to achieve the required concentration of KCl in an IV bag.

Key Takeaways:

• Calculate the new concentration or volume for a dilution or concentration of a solution.

Exercises: The article concludes with exercises that test the reader's understanding of dilution and concentration, involving scenarios where initial and final concentrations or volumes need to be determined.

In summary, this chapter provides a comprehensive understanding of dilution and concentration processes in solutions, emphasizing their practical applications in various fields, including medicine and pharmaceuticals.