Calculate the final concentration of the solution in a 50.0 mL sample of a 2.50 M KCl solution,...

Question:

Calculate the final concentration of the solution in a 50.0 mL sample of a 2.50 M KCl solution, diluted with water to 0.400 L.

The Concentration of Solution:

The concentration of the solution is taken as the total number of moles of the solute that is dissolved in a given amount of solvent. One unit of concentration is molarity. The molarity is computed by getting the ratio of the number of moles of the solute with the total volume of the solution. Higher molarity means a more concentrated solution.

Answer and Explanation: 1

To solve for the final concentration of the KCl, we need to determine first the number of moles present in the 50.0 mL sample.

{eq}\rm moles\,KCl = 2.50\,M \times 0.0500\,L \\ moles\,KCl = 0.125\,moles {/eq}

Now, to solve for the final concentration, we just need to divide the total number of moles by the total volume of the solution.

{eq}\rm [KCl]=\dfrac{0.125\,moles}{(0.0500+0.400)\,L}\\ [KCl]=0.278\,M {/eq}


Learn more about this topic:

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Calculating Dilution of Solutions

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Chapter 8 / Lesson 5
93K

Want to know how to calculate dilution factor? See dilution equations, the dilution formula, and learn how to dilute acid and how to dilute a solution.


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