# 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.

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.