What is the molarity of the diluted solution when 0.50 L of a 0.360 M solution of H3PO4 is...

Question:

What is the molarity of the diluted solution when 0.50 L of a 0.360 M solution of {eq}H_3PO_4 {/eq} is diluted to a final volume of 3.00 L?

Diluting a Solution:

The dilution process is achieved by adding more solvent to an existing stock solution. In a dilute solution, the solute particles remain more separated compared to the stock solution. So, the concentration of a stock solution is reduced during dilution.

Answer and Explanation: 1

According to the law of dilution, we can write:

{eq}\rm C_iV_i=C_fV_f {/eq}

  • {eq}\rm C_i\;and\;C_f {/eq} represent the initial and final concentrations of a solution, respectively.
  • {eq}\rm V_i\;and\;V_f {/eq} represent the initial and final volumes of a solution, respectively.

Given (for {eq}\rm H_3PO_4 {/eq} solution):

{eq}\rm C_i=0.360\;M\\ \rm V_i=0.50\;L\\ \rm V_f=3.00\;L {/eq}


Substituting the above values, we get:

{eq}\rm 0.360\;M\times 0.50\;L=C_f\times 3.00\;L\\ \rm \Rightarrow C_f=0.060\;M {/eq}


Hence, the molarity of the diluted solution is 0.060 M.


Learn more about this topic:

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Calculating Dilution of Solutions

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Chapter 8 / Lesson 5
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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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