Calculating the Volume of HCl Used

Oct 13, 2025 by leolavanderia.com.br 112 views

Introduction

In chemistry, dilution is a crucial concept that involves the process of reducing the concentration of a solution by adding a solvent. This can be achieved by mixing a more concentrated solution with a solvent, resulting in a less concentrated solution. In this article, we will explore a scenario where a student is tasked with preparing a 50.0 mL sample of 1.80 M HCl by diluting a 3.00 M HCl solution. We will use the formula $M_1 V_1 = M_2 V_2$ to calculate the volume of 3.00 M HCl used by the student.

The Dilution Formula

The dilution formula is a fundamental concept in chemistry that allows us to calculate the volume of a solution required to achieve a specific concentration. The formula is given by:

M_1 V_1 = M_2 V_2

where:

$M_1$ is the initial concentration of the solution (in moles per liter, M)
$V_1$ is the initial volume of the solution (in liters, L)
$M_2$ is the final concentration of the solution (in moles per liter, M)
$V_2$ is the final volume of the solution (in liters, L)

Calculating the Volume of HCl Used

In this scenario, the student is tasked with preparing a 50.0 mL sample of 1.80 M HCl by diluting a 3.00 M HCl solution. We can use the dilution formula to calculate the volume of 3.00 M HCl used by the student.

First, we need to convert the initial and final volumes from milliliters (mL) to liters (L). We know that 1 L = 1000 mL, so:

V_1 = 3.00 \text{ M} \times 1.00 \text{ L} = 3.00 \text{ L}

V_2 = 50.0 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} = 0.0500 \text{ L}

Now, we can plug in the values into the dilution formula:

M_1 V_1 = M_2 V_2

3.00 \text{ M} \times 3.00 \text{ L} = 1.80 \text{ M} \times 0.0500 \text{ L}

9.00 \text{ M} \cdot \text{L} = 0.0900 \text{ M} \cdot \text{L}

To solve for $V_1$ , we can divide both sides of the equation by $M_1$ :

V_1 = \frac{M_2 V_2}{M_1}

V_1 = \frac{0.0900 \text{ M} \cdot \text{L}}{3.00 \text{ M}}

V_1 = 0.0300 \text{ L}

Now, we can convert the volume from liters (L) to milliliters (mL):

V_1 = 0.0300 \text{ L} \times \frac{1000 \text{ mL}}{1 \text{ L}} = 30.0 \text{ mL}

Conclusion

In this article, we used the dilution formula to calculate the volume of 3.00 M HCl used by a student to prepare a 50.0 mL sample of 1.80 M HCl. We found that the student used 30.0 mL of 3.00 M HCl to achieve the desired concentration.

Answer

The correct answer is:

C. 30.0 mL

This answer is based on the calculation we performed using the dilution formula. The student used 30.0 mL of 3.00 M HCl to prepare a 50.0 mL sample of 1.80 M HCl.

Introduction

In our previous article, we explored a scenario where a student is tasked with preparing a 50.0 mL sample of 1.80 M HCl by diluting a 3.00 M HCl solution. We used the dilution formula to calculate the volume of 3.00 M HCl used by the student. In this article, we will answer some frequently asked questions related to the dilution experiment.

Q&A

Q1: What is the dilution formula?

A1: The dilution formula is a fundamental concept in chemistry that allows us to calculate the volume of a solution required to achieve a specific concentration. The formula is given by:

M_1 V_1 = M_2 V_2

where:

$M_1$ is the initial concentration of the solution (in moles per liter, M)
$V_1$ is the initial volume of the solution (in liters, L)
$M_2$ is the final concentration of the solution (in moles per liter, M)
$V_2$ is the final volume of the solution (in liters, L)

Q2: How do I convert milliliters (mL) to liters (L)?

A2: To convert milliliters (mL) to liters (L), you can use the following conversion factor:

1 \text{ L} = 1000 \text{ mL}

For example, if you have 50.0 mL, you can convert it to liters (L) as follows:

V_2 = 50.0 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} = 0.0500 \text{ L}

Q3: What is the initial volume of the 3.00 M HCl solution?

A3: The initial volume of the 3.00 M HCl solution is 3.00 L.

Q4: What is the final volume of the 1.80 M HCl solution?

A4: The final volume of the 1.80 M HCl solution is 0.0500 L.

Q5: How do I calculate the volume of 3.00 M HCl used by the student?

A5: To calculate the volume of 3.00 M HCl used by the student, you can use the dilution formula:

M_1 V_1 = M_2 V_2

3.00 \text{ M} \times 3.00 \text{ L} = 1.80 \text{ M} \times 0.0500 \text{ L}

9.00 \text{ M} \cdot \text{L} = 0.0900 \text{ M} \cdot \text{L}

To solve for $V_1$ , you can divide both sides of the equation by $M_1$ :

V_1 = \frac{M_2 V_2}{M_1}

V_1 = \frac{0.0900 \text{ M} \cdot \text{L}}{3.00 \text{ M}}

V_1 = 0.0300 \text{ L}

Now, you can convert the volume from liters (L) to milliliters (mL):

V_1 = 0.0300 \text{ L} \times \frac{1000 \text{ mL}}{1 \text{ L}} = 30.0 \text{ mL}

Conclusion

In this article, we answered some frequently asked questions related to the dilution experiment. We provided explanations and examples to help you understand the concepts and calculations involved in the experiment.

Answer

The correct answer is:

C. 30.0 mL

This answer is based on the calculation we performed using the dilution formula. The student used 30.0 mL of 3.00 M HCl to prepare a 50.0 mL sample of 1.80 M HCl.