# In the laboratory you dilute 4.33 mL of a concentrated 3.00 M hydrobromic acid solution to a...

## Question:

In the laboratory you dilute 4.33 mL of a concentrated 3.00 M hydrobromic acid solution to a total volume of 150 mL. What is the concentration of the dilute solution?

## Number of moles:

In the word of chemistry, the number of moles is indicated by the product of the molarity of a chemical solution and the total volume of the chemical solution. The mathematical relation of the number of moles is shown below.

{eq}{\rm{Number}}\;{\rm{of}}\;{\rm{moles}} = {\rm{Molarity \times Volume}} {/eq}

Given data

• The volume of the concentrated hydrobromic acid solution is {eq}{V_h} = 4.33\;{\rm{mL}} = 4.33 \times {10^{ - 3}}\;{\rm{L}} {/eq}
• The molarity of the concentrated hydrobromic acid solution is {eq}{M_h} = 3\;{\rm{M}} {/eq}
• The total volume at which the diluted is {eq}{V_t} = 150\;{\rm{mL}} = 150 \times {10^{ - 3}}\;{\rm{L}} {/eq}

By sing the below relation, the number of mole is calculated as,

{eq}\begin{align*} n &= {M_h}{V_h}\\ &= \left( {3\;{\rm{M}}} \right)\left( {4.33 \times {{10}^{ - 3}}\;{\rm{L}}} \right)\\ &= 0.0129\;{\rm{mol}} \end{align*} {/eq}

By using the below relation concentration of the dilute solution is calculated as,

{eq}\begin{align*} M &= \dfrac{n}{{{V_t}}}\\ &= \dfrac{{\left( {0.0129\;{\rm{mol}}} \right)}}{{\left( {150 \times {{10}^{ - 3}}\;{\rm{L}}} \right)}}\\ &= 0.086\;{\rm{M}} \end{align*} {/eq}

Thus, the concentration of the dilute solution is 0.086 M.