How do I prepare 100mL of 10g/L HCl from concentrated HCl(37%HCl, density 1.19g/mL)
Is it 2.28mL of conc HCl dilute to 100mL with water?
Please show the calculation steps.
M 37% HCl is
1.19 g/mL x 1000 mL x 0.37/36.46 = 12.08M
M 10g/L is
10/36.46 = 0.274 M
Then use the dilution formula of
c1v1=c2v2.
My answers is 2.268 which rounds to 2.28 mL. I suspect the only difference is in what we used for the molar mass HCl
37% HCl is 0.37g/g
to prepare 100mL of 10g/L HCl solution you need 1g of HCl
then the volume of 37% HCl is
1g/(0.37g/g x 1.19g/mL)=2.27mL
is this refer to pharmacopia
suppose you dissolve 10 grams of HCl gas in 250 ml of water initially at 25 C, what till the final temperature of the solution be?
Well, well, well, it seems like we have a chemistry question on our hands. Don't worry, I'm here to add a little laughter to the equation!
To prepare 100mL of a 10g/L HCl solution, we need to dilute the concentrated HCl (37%HCl, density 1.19g/mL). Let's calculate the amount of concentrated HCl we'll need.
First, we need to find the mass of HCl in the desired 100mL solution. Since we want a concentration of 10g/L, we can go ahead and say we need 10g of HCl in our final solution.
To find the volume of concentrated HCl required, we can use the equation:
Volume (V1) × Concentration (C1) = Volume (V2) × Concentration (C2)
Where V1 and C1 are the initial volume and concentration (concentrated HCl) and V2 and C2 are the final volume and concentration (desired solution).
Plugging the values into the equation, we have:
V1 × 37%HCl = 100mL × 10g/L
Now, let's solve for V1:
V1 = (100mL × 10g/L) / 37%HCl
V1 ≈ 2.70mL
So, to prepare 100mL of a 10g/L HCl solution, you'll need approximately 2.70mL of concentrated HCl.
Now, go ahead and add that to 97.30mL of water (100mL - 2.70mL), and you've got yourself a funny little HCl solution! Just be sure to handle it with care, because chemistry jokes tend to be a little bit acidic!
To prepare 100mL of a 10g/L (or 10%) HCl solution from concentrated HCl (37% HCl, density 1.19g/mL), we need to calculate the volume of concentrated HCl required and then dilute it with water to reach a total volume of 100mL.
The first step is to calculate the amount of HCl needed in grams. This can be done using the formula:
Amount (g) = Volume (L) × Concentration (g/L)
Given that we want to prepare a 100mL (or 0.1L) solution and the concentration required is 10g/L, we can calculate the amount of HCl required as follows:
Amount (g) = 0.1 L × 10 g/L = 1 g
Next, we need to determine the volume of concentrated HCl needed to provide 1g of HCl. To do this, we divide the mass of HCl by the density of the concentrated HCl:
Volume (mL) = Amount (g) ÷ Density (g/mL)
Plugging in the values, we get:
Volume (mL) = 1 g ÷ 1.19 g/mL ≈ 0.84 mL
So, approximately 0.84 mL of concentrated HCl is required.
Finally, we need to dilute the concentrated HCl to a total volume of 100mL by adding water. This means that the volume of water needed will be:
Volume of water (mL) = Total volume (mL) - Volume of concentrated HCl (mL)
Plugging in the values, we get:
Volume of water (mL) = 100 mL - 0.84 mL ≈ 99.16 mL
Therefore, in order to prepare 100mL of a 10g/L HCl solution, you will need approximately 0.84 mL of concentrated HCl to be diluted with approximately 99.16 mL of water.
Please note that these calculations are approximate and may vary slightly depending on the accuracy of the measurements and the specific concentration of the concentrated HCl solution you have. It is always advisable to double-check the calculations and use caution when handling concentrated chemicals.