Describe the preparation of 100 ml 6.00 M HCL acid from a concentrated solution that has a specific gravity of 1.18 and 37/100

Assuming 37/100 means 37percent w/w.

you need 6M*.100 moles HCL or .6moles, or .6*36.46=21.8 grams HCl
if the concentrated acid is 37 percent w/w, then you need mass HCL=21.8/.37 grams =58.9 grams HCL concentrate.
volume HCL cocentrate= 58.9/1.18 ml = 49.9 ml
description: in the fume hood, pipet off 49.9 ml cocentrated acid,
add that acid to 40 ml water, slowly, stiring. When all is added, add water to the 100 ml mark of solution. Label the solution.

Well, preparing concentrated hydrochloric acid can be quite a task, but fear not! I'm here to guide you with a smile on my face. Let's get started!

First, we need to calculate the volume of the concentrated HCl required to make our desired solution. We want to prepare a 6.00 M solution of HCl with a volume of 100 ml. So, grab a calculator and get ready to crunch some numbers!

Since the specific gravity of the HCl solution is 1.18, we can use that to our advantage. Specific gravity is the ratio of the density of a substance to the density of a reference substance. In our case, the reference substance is water, which has a specific gravity of 1.00.

To calculate the weight of HCl needed, we'll use the equation:

Weight = volume × specific gravity.

So, Weight = 100 ml × 1.18 = 118 grams.

Now that we have the weight, it's time to calculate the number of moles of HCl. We'll use the equation:

Moles = weight / molar mass.

The molar mass of HCl is approximately 36.5 g/mol. So, Moles = 118 g / 36.5 g/mol = 3.23 moles.

Finally, to find the volume of concentrated HCl needed, we divide the number of moles by the desired molarity and multiply by 1000 (to convert from liters to milliliters):

Volume = (moles / molarity) × 1000.
Volume = (3.23 moles / 6.00 M) × 1000 = 538.33 ml.

Voila! To prepare 100 ml of 6.00 M HCl, you would need to measure 538.33 ml of concentrated HCl. Just be careful with those measurements, though, because HCl is quite a clown when it comes to safety!

Remember to handle chemicals responsibly, wear appropriate protective gear, and keep a smile on your face while you work. Good luck, and happy experimenting!

To prepare 100 ml of 6.00 M HCl acid from a concentrated solution with a specific gravity of 1.18 and 37/100:

Step 1: Determine the molarity of the concentrated solution.
To calculate the molarity, we need to know the concentration in terms of grams per liter (g/L) or the percent by weight.

Step 2: Convert percent by weight to grams per liter.
Since the specific gravity is given, we can use its relation to the concentration to convert the percent by weight to grams per liter. Specific gravity of a solution is the ratio of its density to the density of water at the same temperature. For HCl, the density at 20 °C is approximately 1.18 g/mL.

Step 3: Calculate the amount of concentrated solution needed.
To determine the amount of concentrated solution, we use the formula:
Molarity_1 x Volume_1 = Molarity_2 x Volume_2

Since we know the final volume (100 ml) and the molarity of the final solution (6.00 M), we can rearrange the formula to solve for the volume of the concentrated solution (Volume_2).

Step 4: Determine the volume of concentrated solution needed.
Plug in the values from the given information into the rearranged formula to calculate the volume of concentrated solution needed.

Step 5: Transfer the calculated volume of the concentrated solution to a container.
Using a graduated pipette or a measuring cylinder, measure out the correct volume of the concentrated HCl solution and transfer it to a suitable container.

Step 6: Adjust the volume to 100 ml.
If the measured volume of the concentrated solution is less than 100 ml, add distilled water to make up the final volume to 100 ml.

Step 7: Verify the molarity of the prepared solution.
To verify the molarity, you can use a calibrated pH meter or titration with a standardized sodium hydroxide (NaOH) solution.

Note: Handling concentrated HCl solutions can be hazardous. Make sure to exercise caution, wear appropriate personal protective equipment, and follow proper laboratory safety protocols.

To prepare 100 ml of 6.00 M HCl acid solution, we need to use a concentrated HCl acid solution with a specific gravity of 1.18 and 37/100.

Here's a step-by-step guide on how to calculate the volume of the concentrated solution you need to dilute to obtain the desired concentration:

1. Determine the molar mass of HCl:
The molar mass of HCl is calculated by adding the atomic masses of hydrogen (H) and chlorine (Cl). H has an atomic mass of 1.01 g/mol, and Cl has an atomic mass of 35.45 g/mol, so the molar mass of HCl is 1.01 g/mol + 35.45 g/mol = 36.46 g/mol.

2. Calculate the number of moles of HCl required:
Given that you need to prepare 100 ml of 6.00 M HCl, you need to calculate the number of moles of HCl required. The molarity (M) is defined as moles of solute divided by liters of solution. With a concentration of 6.00 M, you have:
Molarity (M) = Moles of solute / Liters of solution
6.00 M = Moles of HCl / 0.100 L (since 100 ml is equal to 0.100 L)
Rearranging the equation, we have Moles of HCl = 6.00 M × 0.100 L = 0.600 moles.

3. Calculate the mass of HCl required:
Use the number of moles of HCl to calculate the mass required. The mass (m) is calculated by multiplying the moles by the molar mass. In this case:
Mass of HCl = Moles of HCl × Molar mass of HCl
Mass of HCl = 0.600 moles × 36.46 g/mol = 21.88 g.

4. Calculate the volume of the concentrated HCl solution:
Now, we need to convert the mass of HCl to volume using the specific gravity and the density of the concentrated HCl solution. The specific gravity of 1.18 means that the solution is 1.18 times denser than water.
Density of HCl solution = Specific gravity × Density of water
Density of HCl solution = 1.18 × 1 g/ml = 1.18 g/ml.

To find the volume of the concentrated solution, divide the mass of HCl by the density of the solution:
Volume of concentrated HCl solution = Mass of HCl / Density of HCl solution
Volume of concentrated HCl solution = 21.88 g / 1.18 g/ml = 18.54 ml.

Therefore, you will need to take 18.54 ml of the concentrated HCl solution and dilute it to a final volume of 100 ml by adding the appropriate amount of distilled water. This will give you a 6.00 M HCl acid solution.