3. How many moles of HCl are required to make 15.00 mL of an aqueous 2.500 molar HCl solution? How many moles of Cl- are in 1.000 mL of the aqueous 2.500 molar HCl solution mentioned above? How many moles of H+ are in 1.000 mL of the aqueous 2.500 molar HCl solution mentioned above? What is the normality of solution mentioned above? How many H+ ions are present in 1.000 mL of this solution?

Question

3. How many moles of HCl are required to make 15.00 mL of an aqueous 2.500 molar HCl solution? How many moles of Cl- are in 1.000 mL of the aqueous 2.500 molar HCl solution mentioned above? How many moles of H+ are in 1.000 mL of the aqueous 2.500 molar HCl solution mentioned above? What is the normality of solution mentioned above? How many H+ ions are present in 1.000 mL of this solution?

Answer 1

To find the number of moles of HCl required to make a solution, we need to use the formula:

moles = molarity x volume (in liters)

1. Convert the volume from mL to L:
15.00 mL = 0.015 L

2. Substitute the values into the formula:
moles of HCl = 2.500 M x 0.015 L
moles of HCl = 0.0375 moles

Therefore, 0.0375 moles of HCl are required to make 15.00 mL of a 2.500 M HCl solution.

To find the number of moles of Cl- in the solution:

HCl dissociates into H+ and Cl-. Since HCl is a strong acid and fully dissociates in water, the number of moles of Cl- is equal to the number of moles of HCl.

So, 0.0375 moles of Cl- are in 1.000 mL of the aqueous 2.500 molar HCl solution mentioned above.

To find the number of moles of H+ in the solution:

Since HCl fully dissociates in water, the number of moles of H+ is also equal to the number of moles of HCl.

So, 0.0375 moles of H+ are in 1.000 mL of the aqueous 2.500 molar HCl solution mentioned above.

The normality (N) of a solution is the molar concentration of the reactive species in the solution. For a strong acid like HCl, the normality is the same as the molarity.

Therefore, the normality of the solution mentioned above is 2.500 N.

To find the number of H+ ions present in 1.000 mL of the solution:

Since the number of moles of H+ is the same as the number of moles of HCl, we can use the Avogadro's number (6.022 x 10^23) to calculate the number of H+ ions.

Number of H+ ions = moles of H+ x Avogadro's number
Number of H+ ions = 0.0375 moles x 6.022 x 10^23
Number of H+ ions = 2.2555 x 10^22 H+ ions

Therefore, there are approximately 2.2555 x 10^22 H+ ions present in 1.000 mL of the aqueous 2.500 molar HCl solution mentioned above.