Perpare 500ml of 1M HCl solution from a bottle of concentrated 37%(W/W) HCL stock with a density of 1.19g/ml.
37%= 37/100 x 100
therefore mass is 37g
molarity = mol/vol
1= mol/0.5
mol=0.5
mass of Hcl needed = molxmr
mass = 0.5 x 36.5
mass = 18.25g
Oh, so you want to prepare a 1M HCl solution? Haha, well, let's get cracking!
You'll need to use the concentrated 37% HCl stock, which has a density of 1.19g/mL. Now, to calculate the amount of HCl we'll need, we'll need to do some math gymnastics.
First, let's figure out the mass of the HCl in the concentrated solution. Since it's 37% W/W, that means it contains 37g of HCl per 100g of solution. So for a total of 500mL, the mass of HCl would be approximately 37g/100g x 500mL = 185g.
Now, to calculate the amount of concentrated HCl we'll need to dilute to make a 1M solution, we'll have to use the formula Molarity = Moles/Volume. We know the desired molarity is 1M, and we have a total volume of 500mL. So, rearranging the formula, we can calculate the number of moles we need: Moles = Molarity x Volume = 1M x 0.5L = 0.5 moles.
Finally, we'll need to calculate the mass of HCl needed to get the desired moles. The molar mass of HCl is approximately 36.5g/mol. So the mass will be: Mass = Moles x Molar Mass = 0.5 moles x 36.5g/mol = 18.25g.
So, to summarize, you'll need approximately 18.25g of the concentrated 37% HCl stock to prepare your 500mL 1M HCl solution. Just be careful not to splash it in your eyes!
To prepare 500ml of 1M HCl solution from a bottle of concentrated 37% (W/W) HCl stock with a density of 1.19g/ml, you will need to follow these steps:
1. Calculate the mass of HCl needed:
- The percentage concentration of the stock solution is 37% (W/W), which means it contains 37g HCl in 100g of the solution.
- So, the mass of HCl in the stock solution is (37g/100g) x 500ml = 185g
2. Calculate the volume of the stock solution needed:
- To find the volume, divide the mass of HCl needed by the density of the stock solution:
Volume = Mass / Density = 185g / 1.19g/ml ≈ 155.46ml
3. Dilute the stock solution to the desired concentration:
- Take a clean container and measure 155.46ml of the concentrated HCl stock solution using a graduated cylinder or pipette.
- Add water to bring the total volume up to 500ml.
Now you have prepared 500ml of 1M HCl solution from the concentrated 37% (W/W) HCl stock solution.
To prepare 500ml of 1M HCl solution from a bottle of concentrated 37% (W/W) HCl stock with a density of 1.19g/ml, you will need to follow these steps:
1. Determine the mass of HCl needed:
- Calculate the mass of HCl in the concentrated solution:
Mass = % concentration x Volume x Density
Mass = 37% x 500ml x 1.19g/ml
Mass = 0.37 x 500 x 1.19
Mass = 222.65g
2. Convert the mass of HCl to moles:
- Use the molar mass of HCl (36.5g/mol):
Moles = Mass / Molar mass
Moles = 222.65g / 36.5g/mol
Moles = 6.1mol
3. Calculate the volume of the concentrated solution needed:
- Use the molarity equation: Molarity = Moles / Volume
- Rearrange the equation to isolate Volume:
Volume = Moles / Molarity
Volume = 6.1mol / 37mol/L (since you want 1M HCl)
Volume ≈ 0.165 L (165ml)
4. Dilute the concentrated solution to obtain 500ml of 1M HCl:
- Transfer the 165ml of concentrated HCl into a container.
- Add distilled water to reach a total volume of 500ml.
Note: When working with strong acids like HCl, always remember to exercise caution and wear appropriate protective equipment, such as gloves and safety glasses.
Your 0.5 mol HCl needed and 18.25 g needed are correct but it's the long way of going about it. However, you have no connection between this work and the 37 g/100 that you have in the stock. You can complete your work by
mass = volume x density or
18.25 = volume x 1.19 or volume = 15.336 mL (and I know that's too many sig figures) of the stock BUT since that is only 37% pure, then
15.336/0.37 = about 41.4 mL of the stock you want to take.
The easier way to work this is to 1. Determine the molarity of the stock.
2. Use the dilution formula.
1.
M of the stock.
1.19 g/mL x 1000 mL x 0.37 = g HCl in 1000 mL. Then g/36.5 = about 12 M but you can be more accurate than that.
2. mL1 x M1 = mL2 x M2
500*1 = mL2 x 12.06M
mL2 = about 41 mL