The molarity of a concentrated acid is 1.15M .what volume of HCl is required to make 1l of 0.1M HC

You need 0.1 moles for 1L of diluted acid.

The concentrated acid has 1.15 moles per liter.

So, you need 0.1/1.15 = 0.087 liters of the concentrate.

or, 87 ml

To determine the volume of the concentrated acid (1.15M HCl) required to make 1L of 0.1M HCl, we can utilize the formula:

M1V1 = M2V2

where:
M1 = molarity of the concentrated acid
V1 = volume of the concentrated acid
M2 = desired final molarity
V2 = desired final volume

Let's substitute the given values into the formula and solve for V1:

(1.15M)(V1) = (0.1M)(1L)

V1 = (0.1M)(1L) / 1.15M
V1 = 0.0869565 L

Therefore, approximately 0.087 liters (or 87 milliliters) of the concentrated acid is required to make 1L of 0.1M HCl.

To find the volume of the concentrated acid required to make 1 liter of 0.1M HCl, you can use the formula:

M1 x V1 = M2 x V2

Where:
- M1 is the molarity of the concentrated acid
- V1 is the volume of the concentrated acid
- M2 is the desired molarity of the HCl solution
- V2 is the final volume of the HCl solution

In this case, you are given:
- M1 = 1.15 M (molarity of the concentrated acid)
- V1 = ?
- M2 = 0.1 M (desired molarity of the HCl solution)
- V2 = 1 L (final volume of the HCl solution)

Substituting these values into the formula, we get:

1.15 M x V1 = 0.1 M x 1 L

Now, let's solve for V1:

V1 = (0.1 M x 1 L) / 1.15 M
V1 = 0.0869 L or 86.9 mL

Therefore, you would need approximately 86.9 mL of the concentrated acid to make 1 liter of 0.1M HCl.