If you're working in a chemistry lab, it's essential to know how to calculate a dilution.

The Tocris dilution calculator is a useful tool which allows you to calculate how to dilute a stock solution of known concentration. Enter C 1, C 2 & V 2 to calculate V 1. Concentration 1 femtomolar picomolar nanomolar micromolar millimolar molar Volume 1 nanoliter microliter milliliter liter.

Review of Dilution, Concentration, and Stock Solutions

1. » Dilution Calculator - Percent. Initial Data. Concentration Before Dilution (C1)% Volume Before Dilution (V1) Concentration After Dilution (C2).
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3. Oct 08, 2013  A serial dilution is a series of sequential dilutions used to reduce a dense culture of cells to a more usable concentration. Each dilution will reduce the concentration of bacteria by a specific.

A dilution is a solution made by adding more solvent to a more concentrated solution (stock solution), which reduces the concentration of the solute. An example of a dilute solution is tap water, which is mostly water (solvent), with a small amount of dissolved minerals and gasses (solutes).

An example of a concentrated solution is 98 percent sulfuric acid (~18 M). The primary reason you start with a concentrated solution and then dilute it to make a dilution is that it's very difficult—and sometimes impossible—to accurately measure solute to prepare a dilute solution, so there would be a large degree of error in the concentration value.

Use the law of conservation of mass to perform the calculation for the dilution:

Dilution Example

As an example, say you need to prepare 50 milliliters of a 1.0 M solution from a 2.0 M stock solution. Your first step is to calculate the volume of stock solution that is required.

To make your solution, pour 25 ml of stock solution into a 50 ml volumetric flask. Dilute it with solvent to the 50 ml line.

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Avoid This Common Dilution Mistake

It's a common mistake to add too much solvent when making the dilution. Make sure you pour the concentrated solution into the flask and then dilute it to the volume mark. Do not, for example, mix 250 ml of concentrated solution with 1 liter of solvent to make a 1-liter solution.

Real-life chemists in real-life labs don’t make every solution from scratch. Instead, they make concentrated stock solutions and then make dilutions of those stocks as necessary for a given experiment.

Definition of binary numbers. To make a dilution, you simply add a small quantity of a concentrated stock solution to an amount of pure solvent. The resulting solution contains the amount of solute originally taken from the stock solution but disperses that solute throughout a greater volume. Therefore, the final concentration is lower; the final solution is less concentrated and more dilute.

How do you know how much of the stock solution to use and how much of the pure solvent to use? It depends on the concentration of the stock and on the concentration and volume of the final solution you want. You can answer these kinds of pressing questions by using the dilution equation, which relates concentration (C) and volume (V) between initial and final states:

C₁V₁ = C₂V₂

You can use the dilution equation with any units of concentration, provided you use the same units throughout the calculation. Because molarity is such a common way to express concentration, the dilution equation is sometimes expressed in the following way, where M₁ and M₂ refer to the initial and final molarity, respectively:

M₁V₁ = M₂V₂

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For example, how would you prepare 500. mL of 0.200 M NaOH(aq) from a stock solution of 1.5 M NaOH?

Start by using the dilution equation,

Serial Dilution Calculator Molarity

M₁V₁ = M₂V₂

The initial molarity, M₁, comes from the stock solution and is therefore 1.5 M. The final molarity is the one you want in your final solution, which is 0.200 M. The final volume is the one you want for your final solution, 500. mL, which is equivalent to 0.500 L. Using these known values, you can calculate the initial volume, V₁:

The calculated volume is equivalent to 67 mL. The final volume of the aqueous solution is to be 500 mL, and 67 mL of this volume comes from the stock solution. The remainder, 500 mL – 67 mL = 433 mL, comes from pure solvent (water, in this case). So to prepare the solution, add 67 mL of 1.5 M stock solution to 433 mL water. Mix and enjoy!

Try another problem: What is the final concentration in molarity of a solution prepared by diluting 2.50 mL of 3.00 M KCl(aq) up to 0.175 L final volume?

You can use the dilution equation,

M₁V₁ = M₂V₂

Dilution Concentration Calculator

In this problem, the initial molarity is 3.00 M, the initial volume is 2.50 mL or 2.50 x 10^–3 L and the final volume is 0.175 L. Use these known values to calculate the final molarity, M₂:

So, the final concentration in molarity of the solution is

Serial Dilution Calculation A Level Biology

4.29 x 10^–2M