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?
Why don't you boil this down to exactly what you don't understand instead of using the shotgun approach.
To answer these questions, we need to use the formula:
Molarity (M) = moles of solute / volume of solution (in liters)
Let's solve each question step by step:
1. How many moles of HCl are required to make 15.00 mL of an aqueous 2.500 molar HCl solution?
To find the moles of HCl, we need to rearrange the formula:
moles of solute = Molarity × volume of solution (in liters)
Given:
Molarity (M) = 2.500 M
Volume of solution = 15.00 mL (which needs to be converted to liters)
First, convert the volume of solution to liters:
15.00 mL ÷ 1000 = 0.015 L
Now, let's substitute the values into the formula:
moles of HCl = 2.500 M × 0.015 L
moles of HCl = 0.0375 mol
Therefore, 0.0375 moles of HCl are required to make 15.00 mL of a 2.500 M HCl solution.
2. How many moles of Cl- are in 1.000 mL of the aqueous 2.500 molar HCl solution mentioned above?
Since HCl dissociates in water to form H+ and Cl- ions in equal amounts, the concentration of Cl- ions is the same as the HCl concentration.
Therefore, the number of moles of Cl- in 1.000 mL of the 2.500 M HCl solution would also be 0.0375 moles.
3. How many moles of H+ are in 1.000 mL of the aqueous 2.500 molar HCl solution mentioned above?
Since HCl dissociates in water to form H+ and Cl- ions in equal amounts, the concentration of H+ ions is also the same as the HCl concentration.
Therefore, the number of moles of H+ in 1.000 mL of the 2.500 M HCl solution would also be 0.0375 moles.
4. What is the normality of the solution mentioned above?
Normality (N) is a measure of the number of equivalents of solute per liter of solution. For an acid like HCl, its normality is equal to its molarity because HCl has a monoacidic behavior.
Therefore, the normality of a 2.500 M HCl solution would be 2.500 N.
5. How many H+ ions are present in 1.000 mL of this solution?
Since there is an equal number of moles of H+ ions and Cl- ions in a dissociated HCl molecule, the number of H+ ions is also equal to the number of moles of H+ ions calculated earlier.
In this case, the 1.000 mL of the 2.500 M HCl solution contains 0.0375 moles of H+ ions.