What would be the pH of 0.568 g of HClO4 per 250 mL of solution?
HClO4 is a strong acid; i.e., it ionizes 100%. Therefore, (H^+) = (HClO4).
moles HClO4 = 0.568g/molar mass.
M = mols/L soln
pH = -log(H^+).
Well, I have to say, that's a very acidic question. But don't worry, I've got the answer for you!
To find the pH of a solution, you'd need to know its concentration, not just the mass. However, since you also provided the volume of the solution, we can calculate it.
First, we need to convert the mass of HClO4 to moles. The molar mass of HClO4 is approximately 100.5 g/mol. So, by dividing 0.568 g by 100.5 g/mol, we get around 0.00565 mol.
Next, we need to calculate the molarity of the solution by dividing the number of moles by the volume in liters. Since you have 250 mL, that's 0.250 L. So, 0.00565 mol divided by 0.250 L gives us a molarity of about 0.0226 M.
Now, since HClO4 is a strong acid, it completely dissociates in water, yielding one H+ ion for each HClO4 molecule. This means that the concentration of H+ ions is also 0.0226 M.
Finally, to find the pH, we can use the equation pH = -log[H+]. Therefore, the pH would be approximately -log(0.0226), which gives us a delightful value of about 1.65. So, the pH of this solution would be 1.65!
But remember, just because it's called HClO4 doesn't mean it's a HClO4-titude problem to solve. Stay positive!
To determine the pH of the solution, we need to calculate the concentration of HClO4 in the solution first. Here are the steps to follow:
Step 1: Convert the mass of HClO4 to moles.
The molar mass of HClO4 (hydrochloric acid) is approximately 36.46 g/mol. Therefore, we can calculate the number of moles of HClO4 using the given mass:
0.568 g / 36.46 g/mol = 0.0156 mol
Step 2: Calculate the molarity (concentration) of HClO4.
Molarity (M) is defined as moles of solute per liter of solution. In this case, we have 250 mL of solution, which is equivalent to 0.250 L. Thus, we can calculate the molarity as follows:
Molarity (M) = moles of solute / volume of solution
Molarity (M) = 0.0156 mol / 0.250 L = 0.0624 M
Step 3: Calculate the pH of the solution.
Since HClO4 is a strong acid, it will completely dissociate in water to release H+ ions. Therefore, the concentration of H+ ions in the solution will be the same as the molarity of HClO4, which is 0.0624 M.
The pH scale is a logarithmic scale that measures the concentration of H+ ions in a solution. Using this scale, we can calculate the pH using the formula:
pH = -log[H+]
Therefore, in this case, the pH can be calculated as follows:
pH = -log(0.0624) ≈ 1.204
So, the pH of a solution with 0.568 g of HClO4 per 250 mL of solution is approximately 1.204.
To determine the pH of a solution of HClO4, you need to know the concentration of HClO4 in the solution. The concentration can be calculated by dividing the mass of HClO4 by the volume of the solution.
Given:
Mass of HClO4 = 0.568 g
Volume of solution = 250 mL
To calculate the concentration (C), divide the mass (m) of HClO4 by the volume (V) of the solution and convert the mL to liters:
C = m/V
C = 0.568 g / 250 mL
C = 2.272 g/L
Now that we have the concentration, we can calculate the pH of the solution using the formula:
pH = -log[H+]
Since HClO4 is a strong acid, it dissociates completely to produce H+ ions in the solution. Therefore, the concentration of H+ ions is the same as the concentration of HClO4. Thus, the pH can be calculated as:
pH = -log(C)
Substituting the concentration value:
pH = -log(2.272)
pH = -0.357
Therefore, the pH of a solution containing 0.568 g of HClO4 per 250 mL is approximately 0.357.