HCI (aq) is a strong acid. suppose you dissolved 0.0365 grams of HCI in water to give a final volume of 10.0 mL. what is the pH of this final solution. The molar mass of HCU is 36.5g /mole and the molar mass of water is 18.0g/mole
mols = grams/molar mass
M = mols/L solution
pH = -log(Molarity HCl)
I get pH = 1
To find the pH of the HCI solution, we need to determine the concentration of the H⁺ ions in the solution, which can be calculated using the formula:
Concentration (in mol/L) = amount of solute (in moles) / volume of solution (in L)
First, let's convert the mass of HCI to moles using its molar mass:
Moles of HCI = mass / molar mass
Moles of HCI = 0.0365 g / 36.5 g/mol = 0.001 mol
Now, let's convert the volume of the solution to liters:
Volume of solution = 10.0 mL = 10.0 mL / 1000 mL/L = 0.0100 L
Next, we can calculate the concentration of the H⁺ ions:
Concentration (in mol/L) = 0.001 mol / 0.0100 L = 0.100 mol/L
Since HCI completely dissociates in water, the concentration of the H⁺ ions is the same as the concentration of the HCI. Therefore, the concentration of H⁺ ions is 0.100 mol/L.
To find the pH of the solution, we can use the following formula:
pH = -log[H⁺]
Substituting the concentration of H⁺ into the formula:
pH = -log(0.100)
Using a scientific calculator, we can find that -log(0.100) is equal to 1.00.
Therefore, the pH of the final solution is 1.00.