Please prepare 0.5L of 1.2M HCl in 50% (v/v) aqueous methanol.
The details of HCl are as follows:
Hydrochloric acid:
Purity : 36%-38%
Density : 1.18g/mL
Physical state : liquid
Molecular weight : 36.42 g/mol
Describe the procedures and apparatus you need to use for the solution preparation. Explain your answer.
- can you help me? I'm so sorry. I don't have any idea how to do this :(
Oh, don't worry, my friend! I'm here to help and add a little fun to the process! Let's get started on making that solution.
First, let's calculate the amount of HCl needed to prepare 0.5L of a 1.2M solution. Remember, Molarity (M) is defined as moles of solute per liter of solution.
So, for a 1.2M solution, we need 1.2 moles of HCl per liter. Since we need only 0.5L, we'll need 0.6 moles of HCl.
Now, let's calculate the volume of the concentrated HCl needed. We know that the purity of HCl is 36%-38%. Taking the average, let's assume it's 37%.
Since the density of HCl is 1.18 g/mL, we can calculate the mass of HCl needed for 0.6 moles using its molecular weight of 36.42 g/mol. The mass would be 0.6 moles * 36.42 g/mol = 21.85 grams.
To find the volume, divide the mass by the density:
Volume = mass / density
Volume = 21.85 g / 1.18 g/mL = 18.51 mL
So, we need approximately 18.51 mL of 37% HCl to prepare the solution.
Now, let's move on to preparing the solution. Here are the steps:
1. Take a clean, dry beaker or flask that can hold at least 0.5L of liquid.
2. Measure 18.51 mL of the 37% HCl using a pipette or a measuring cylinder, and add it to the beaker/flask.
3. Add approximately 450 mL of aqueous methanol to the beaker/flask. Make sure to use 50% (v/v) aqueous methanol, which means equal volumes of methanol and water.
4. Use a stirring rod to mix the contents of the beaker/flask thoroughly. Be gentle, no need to stir like you're in a hurricane!
5. Once everything is mixed properly, you can now add water to bring the total volume up to 0.5L. Again, be gentle with your stirring!
And voila! You now have your 0.5L of 1.2M HCl in 50% (v/v) aqueous methanol. Just remember to handle the HCl with caution, wear appropriate safety gear, and work in a well-ventilated area. Safety first, my friend!
I hope that helped, and I hope I managed to make you smile along the way. If you have any more questions, feel free to ask!
No problem! I'm here to help you. Let's break down the process step-by-step:
1. Determine the amount of HCl needed:
The concentration of HCl required is 1.2M, and you want to prepare 0.5L of this solution. Using the formula: Molarity (M) = Moles (mol) / Volume (L), we can rearrange to find the number of moles needed:
Moles (mol) = Molarity (M) x Volume (L)
Moles (mol) = 1.2M x 0.5L = 0.6 moles
2. Calculate the quantity of HCl needed:
The molecular weight of HCl is given as 36.42 g/mol. Using the formula: Mass (g) = Moles (mol) x Molecular weight (g/mol), we can find the mass of HCl required:
Mass (g) = 0.6 moles x 36.42 g/mol = 21.85 g
3. Determine the amount of 36-38% HCl needed:
The purity of HCl is given as 36-38%. Assuming the average purity of 37%, we can calculate the required amount of 37% HCl solution using the formula: Mass of HCl (g) = Mass of 37% HCl (g) x (100 / % purity):
Mass of 37% HCl (g) = 21.85 g x (100 / 37) = 59.05 g
4. Prepare the HCl solution:
To prepare 0.5L of the 1.2M HCl solution using 37% HCl, you would follow these steps:
a. Measure 59.05 g of 37% HCl using a balance.
b. Transfer the measured HCl into a suitable container.
c. Rinse the container with a small amount of distilled water to ensure all the HCl is transferred.
d. Fill the container with distilled water up to approximately 400 mL.
e. Once the HCl is dissolved, add methanol to achieve a 50% (v/v) ratio.
Apparatus needed:
- Balance to measure the mass of HCl
- Suitable container to hold the solution (such as a beaker or a volumetric flask)
- Graduated cylinder or pipette to measure the volumes accurately
- Distilled water for dilution
- Methanol for achieving a 50% (v/v) ratio
- Safety equipment such as gloves, goggles, and a lab coat to handle the corrosive HCl safely.
Please note that hydrochloric acid can be hazardous, so it's essential to follow proper safety precautions while working with it. If you are not familiar with laboratory procedures, it's advisable to seek guidance from a trained professional.
Sure, I can help you with that. Preparing a solution of 0.5L of 1.2M HCl in 50% (v/v) aqueous methanol requires a step-by-step procedure and specific equipment. Here's how you can do it:
1. Calculate the mass of HCl needed:
The molarity (M) of a solution is calculated using the formula:
Molarity (M) = moles of solute / volume of solution (in L)
Rearrange the equation to find the moles of solute:
Moles of solute = Molarity (M) x Volume of solution (in L)
In this case, the volume of the solution is 0.5 L and the desired molarity is 1.2 M.
Moles of HCl = 1.2 M x 0.5 L = 0.6 moles
To find the mass of HCl needed, use the molecular weight of HCl:
Mass of HCl = Moles of HCl x Molecular weight of HCl
Mass of HCl = 0.6 moles x 36.42 g/mol = 21.85 g
2. Measure and dissolve HCl in methanol:
To obtain a 50% (v/v) aqueous methanol solution, you need equal volumes of methanol and water. In this case, you require 0.25 L of methanol.
Use a balance to measure out 21.85 g of pure HCl.
Note: Be sure to handle HCl with extreme care as it is highly corrosive and can cause burns. Wear appropriate protective equipment and work in a well-ventilated area.
Next, pour the 0.25 L of methanol into a suitable container. Slowly add the measured HCl to the methanol, stirring gently until the HCl is completely dissolved.
3. Prepare the 50% (v/v) aqueous methanol solution:
To achieve a 50% (v/v) aqueous methanol solution, you need to combine an equal volume of water with the methanol-HCl mixture. In this case, you require 0.25 L of water.
Use a graduated cylinder to measure out 0.25 L of water.
Mix the water and methanol-HCl solution together in a clean, dry container, ensuring thorough mixing. The resulting solution will be your desired 0.5L of 1.2M HCl in 50% (v/v) aqueous methanol.
Note: It's essential to follow appropriate safety precautions while handling chemicals. Be sure to wear gloves, goggles, and work in a well-ventilated area. Also, make sure to check the compatibility of the container with the chemicals being used.
I hope this explanation helps you with the solution preparation. Let me know if you have any further questions!