You can purchase hydrochloric acid in a concentrated form that is 37.0 hcl by mass and has a density of 1.20g/mL. Describe how exactly you would prepare 2.85 L of 0.500 M HCL from the concentrated solution.

Calculate the molarity of the concentrated HCl. You made a typo and omitted the % after 37.

M HCl = 1000mL x 1.20g/mL x 0.37 x (1 mol/36.5g) = about 12.2M
Then mL1 x M1 = mL2 x M2
mL1 x 12.2M = 2850 mL x 0.500
Solve for mL 1 you need.
Take mL you've calculated, add to a 500 mL volumetric flask, add distilled water to the mark on the flask, mix thoroughly.

To prepare 2.85 L of 0.500 M HCl solution from the concentrated solution, follow these steps:

Step 1: Calculate the moles of HCl needed
To determine the number of moles required, use the equation: Molarity (M) = moles/volume (L). Rearrange the equation to solve for moles:
moles = Molarity × Volume

moles = 0.500 M × 2.85 L
moles = 1.425 mol

Step 2: Determine the volume of concentrated HCl required
To find the volume of concentrated HCl, use the equation: moles = mass/molar mass. Rearrange the equation to solve for mass:
mass = moles × molar mass

Since we know the concentration and density of the concentrated HCl, we can calculate the mass using the equation: mass = concentration × volume × density.

mass = 37.0% × 2.85 L × 1.20 g/mL
mass = 1.014 g

To convert grams to moles, divide by the molar mass of HCl (36.461 g/mol):
moles = 1.014 g / 36.461 g/mol
moles ≈ 0.028 mol

Step 3: Dilution process
To dilute the concentrated HCl, use the equation: M1V1 = M2V2, where M1 and V1 are the initial concentration and volume, and M2 and V2 are the final concentration and volume.

Since we know the initial volume (V1) and concentration (M1), and we want to prepare a 0.500 M HCl solution with a final volume of 2.85 L (V2), we can solve for the dilution volume (V1) using the equation:

V1 = (M2 × V2) / M1

V1 = (0.500 M × 2.85 L) / 37.0%
V1 ≈ 0.385 L

Step 4: Obtain the necessary amount of concentrated HCl
Measure approximately 0.385 L (or 385 mL) of the concentrated HCl using a graduated cylinder or a volumetric flask.

Step 5: Add distilled water to complete the 2.85 L volume
Pour the measured 0.385 L of concentrated HCl into a clean container. Then, add distilled water gradually while stirring until the total volume reaches 2.85 L.

Step 6: Mix well
Ensure that the solution is thoroughly mixed by stirring or swirling gently. This will ensure the complete distribution of HCl within the solution.

You have now prepared 2.85 L of 0.500 M HCl solution from the concentrated 37.0% HCl solution. Remember to handle concentrated HCl with care and wear appropriate personal protective equipment.

To prepare 2.85 L of a 0.500 M HCl solution from the concentrated solution with a density of 1.20 g/mL, follow these steps:

Step 1: Determine the amount of HCl needed.
To calculate the amount of HCl needed, we can use the formula:
Amount of solute (in moles) = Concentration (in M) * Volume (in liters)
In this case, the desired concentration is 0.500 M, and the desired volume is 2.85 L:
Amount of HCl = 0.500 mol/L * 2.85 L = 1.425 moles

Step 2: Calculate the mass of the concentrated HCl solution needed.
We know that the concentrated HCl solution has a concentration of 37.0% (or 37.0 g/100 mL) by mass and a density of 1.20 g/mL. We can use this information to calculate the mass needed:
Mass of concentrated HCl solution = Volume * Density = 2.85 L * 1.20 g/mL = 3.42 kg (or 3420 g)

Step 3: Determine the amount of actual HCl present in the concentrated solution.
To find the amount of HCl present in the concentrated solution, we need to consider its concentration (37.0% by mass) and molar mass (36.461 g/mol):
Amount of HCl = Concentration * Mass / Molar mass
Amount of HCl = 37.0% * 3420 g / 36.461 g/mol = 346.11 g / 36.461 g/mol ≈ 9.50 moles

Step 4: Dilute the concentrated solution to the desired volume.
To dilute the concentrated HCl solution to the desired volume of 2.85 L and desired concentration of 0.500 M, follow these steps:

a) Transfer the desired amount of concentrated HCl solution into a container. In this case, it is approximately 3.42 kg (or 3420 g).

b) Add distilled water to the container while stirring until the volume reaches 2.85 L.

c) Mix thoroughly to ensure proper dilution.

Step 5: Verify the concentration of the prepared solution.
You can use a pH meter or perform a titration to verify the concentration of the prepared HCl solution.

Note: Working with concentrated HCl requires caution. Always follow proper safety procedures, use appropriate protective equipment, and handle the chemical in a well-ventilated area.

94.94 mL