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Process is described for changing the concentration of solutions

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How do you clean concrete?

Muriatic acid (another name for HCl) is widely used for cleaning concrete and masonry surfaces. The acid must be diluted before use to get it down to a safer strength. Commercially available at concentrations of about 18%, this compound can be used to remove scales and deposits (usually composed of basic materials).


When additional water is added to an aqueous solution, the concentration of that solution decreases. This is because the number of moles of the solute does not change, while the volume of the solution increases. We can set up an equality between the moles of the solute before the dilution (1) and the moles of the solute after the dilution (2).


Since the moles of solute in a solution is equal to the molarity multiplied by the liters, we can set those equal.

M_1 \times L_1=M_2 \times L_2

Finally, because the two sides of the equation are set equal to one another, the volume can be in any units we choose, as long as that unit is the same on both sides. Our equation for calculating the molarity of a diluted solution becomes:

M_1 \times V_1 = M_2 \times V_2

Suppose that you have 100. mL of a 2.0 M solution of HCl. You dilute the solution by adding enough water to make the solution volume 500. mL. The new molarity can easily be calculated by using the above equation and solving for M_2 .

M_2=\frac{M_1 \times V_1}{V_2}=\frac{2.0 \text{ M} \times 100. \text{ mL}}{500. \text{ mL}}=0.40 \text{ M } HCl

The solution has been diluted by one-fifth since the new volume is five times as great as the original volume. Consequently, the molarity is one-fifth of its original value.

Another common dilution problem involves deciding how much of a highly concentrated solution is requires to make a desired quantity of solution of lesser concentration. The highly concentrated solution is typically referred to as the stock solution.

Sample Problem: Dilution of a Stock Solution

Nitric acid (HNO 3 ) is a powerful and corrosive acid. When ordered from a chemical supply company, its molarity is 16 M. How much of the stock solution of nitric acid needs to be used to make 8.00 L of a 0.50 M solution?

Step 1: List the known quantities and plan the problem.


  • stock HNO 3 = 16 M
  • V_2=8.00 \ \text{L}
  • M_2=0.50 \ \text{M}


  • \text{volume stock} \ \text{HNO}_3 \ (V_1)=? \ \text{L}

The unknown in the equation is V_1 , the volume of the concentrated stock solution.

Step 2: Solve.

V_1=\frac{M_2 \times V_2}{M_1}=\frac{0.50 \text{ M} \times 8.00 \text{ L}}{16 \text{ M}}=0.25 \text{ L}=250 \text{ mL}

Step 3: Think about your result.

250 mL of the stock HNO 3 needs to be diluted with water to a final volume of 8.00 L. The dilution is by a factor of 32 to go from 16 M to 0.5 M.

Dilutions can be performed in the laboratory with various tools, depending on the volumes required and the desired accuracy. The following images illustrate the use of two different types of pipettes. Figure below illustrates the use of two different types of pipettes. In the first figure, a glass pipette is being used to transfer a portion of a solution to a graduated cylinder. Use of a pipette rather than a graduated cylinder for the transfer improves accuracy. In the second Figure below , the student is using a micropipette , which is designed to quickly and accurately dispense small volumes. Micropipettes are adjustable and come in a variety of sizes.

Volumetric pipette.



  • A process is described for calculations of dilutions.


Read the material and work the problems at the link below:



  1. What does not change when additional water is added to a solution?
  2. What is a stock solution?
  3. How is a stock solution used?

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