5) How many mL of 1M HCl is used to make the following dilutions?

a) 100mL of 0.1M HCl =
b) 250mL of 0.5M HCl=
c) 10ml of 0.01M HCl=

36.64 is the molar mass of hcl do I divide that into ml?

Use the dilution formula for these.

c1v1 = c2v2
c = concn
v = volume

for a.
100 mL x 0.1M = ? mL x 1M
Solve for ?mL of the 1M.

b.
250 mL x 0.5M = ? mL x 1 M
Solve for ?mL of 1 M.

a) 10ml

b) 125ml

To calculate the amount of 1M HCl required to make a desired dilution, you need to use the concept of molarity and the equation:

(M₁)(V₁) = (M₂)(V₂)

Where:
M₁ = initial molarity
V₁ = initial volume
M₂ = final molarity
V₂ = final volume (desired dilution volume)

a) To make 100mL of 0.1M HCl:
M₁ = 1M
V₁ = ? (unknown)
M₂ = 0.1M
V₂ = 100mL

Using the equation: (1M)(V₁) = (0.1M)(100mL)
Rearranging the equation to solve for V₁, we have:
V₁ = (0.1M)(100mL) / 1M
V₁ = 10 mL

b) To make 250mL of 0.5M HCl:
M₁ = 1M
V₁ = ? (unknown)
M₂ = 0.5M
V₂ = 250mL

Using the equation: (1M)(V₁) = (0.5M)(250mL)
Rearranging the equation to solve for V₁, we have:
V₁ = (0.5M)(250mL) / 1M
V₁ = 125 mL

c) To make 10mL of 0.01M HCl:
M₁ = 1M
V₁ = ? (unknown)
M₂ = 0.01M
V₂ = 10mL

Using the equation: (1M)(V₁) = (0.01M)(10mL)
Rearranging the equation to solve for V₁, we have:
V₁ = (0.01M)(10mL) / 1M
V₁ = 0.1 mL

As for the molar mass of HCl, 36.64 g/mol is the correct value. However, it is unrelated to the calculations for volume and molarity. The molar mass is used to convert grams to moles or vice versa, but when determining the volume of a solution, you only need to work with the molarity and required volumes.