anyone help me . .what volume of concentrated HCL solution whoch is 36% by mass and has a density of 1.179 g/ml , should be used to make 4.7 L of hcl solution with a pH of 1.8 ?
First you want to calculate the (HCl). That's
density x 1000 mL x (%/100) x 1/molar mass = M
1.179 x 1000 x 0.36 x (1/36.5) =11.6 M
Then c1v1 = c2v2
What H^+ do you want for pH = 1.8? That is 1.8 = -log(H^+) = about 0.0158
c = concn
v = volume
11.6 x v = 0.0158 x 4,700 mL
v = ? mL.
11.79
To calculate the volume of concentrated HCl solution needed, we need to follow these steps:
Step 1: Determine the concentration of HCl needed for the final solution.
The pH of 1.8 indicates that the final solution will be acidic. Since we want to use concentrated HCl solution, which is already highly acidic, we need to check if the pH requirement is within the range that the concentrated solution can achieve. HCl has a pH value close to 0 when it is in concentrated form. Therefore, a pH of 1.8 is achievable.
Step 2: Calculate the amount of HCl needed.
The concentration of the concentrated HCl solution is given as 36% by mass. This means that 36 g of HCl is present in 100 g of the solution.
We can calculate the mass of HCl needed for the final solution:
Mass of HCl = (Concentration of HCl (%)) x (Mass of HCl solution needed)
Let's denote the mass of HCl solution needed as M.
Thus,
36% x M = Mass of HCl
Step 3: Convert the mass of HCl to volume.
To convert the mass of HCl to volume, we need to use the density of the concentrated HCl solution, which is given as 1.179 g/ml.
Volume of HCl = (Mass of HCl) / (Density of HCl solution)
Step 4: Calculate the volume of concentrated HCl solution required.
The final solution volume needed is given as 4.7 L.
Now, let's calculate the volume of the concentrated HCl solution required:
Volume of concentrated HCl = (Volume of HCl) / (Final solution volume needed)
Following these steps, we can find the answer to your question.