# In the laboratory, you dilute 2.51 mL of a concentrated 12.0 M hydrobromic acid solution to a...

## Question:

In the laboratory, you dilute {eq}\rm 2.51\ mL {/eq} of a concentrated {eq}\rm 12.0\ M {/eq} hydrobromic acid solution to a total volume of {eq}\rm 75.0\ mL {/eq}. What is the concentration of the dilute solution?

## Dilution:

Acids are used extensively in many chemical and biochemical experiments. They are usually available as concentrated solutions with very high molar concentrations. In order to prepare a solution of an appropriate lower solution, these concentrated acids can be diluted using the appropriate solvent.

## Answer and Explanation: 1

The dilution process can be expressed using the equation given below:

{eq}C_1V_1=C_2V_2\\ where:\\ C_1=initial\,concentration\\ V_1=initial\,volume\\ C_2=final\,concentration\\ V_2=final\,volume {/eq}

The concentration of the dilute solution (final concentration) can be determined by substituting the given values in the equation above. Thus, the concentration of the dilute solution is computed as follows:

{eq}C_2 = \frac{C_1V_1}{V_2}\\ C_2 = \frac{(12.0\,M)(2.51\,mL)}{75.0\,mL}\\ C_2 = \mathbf{0.402 \, M} {/eq}

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Chapter 8 / Lesson 5Want 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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