A 0.01 M solution of a HBrO is 4.0% ionized. is the PH value of this acid? (Log4 = 0.6)
To find the pH value of a solution, we need to calculate the concentration of hydrogen ions (H+) in the solution. Given that the HBrO solution is 4.0% ionized, it means that 4.0% of the initial concentration of HBrO has dissociated into H+ and BrO- ions.
Let's calculate the concentration of H+ ions in the solution:
1. Start with the initial concentration of HBrO, which is 0.01 M.
2. Since the solution is 4.0% ionized, only 4.0% of the HBrO has dissociated into H+ ions. Thus, the concentration of H+ ions is 4.0% of 0.01 M.
Concentration of H+ = 4.0% × 0.01 M = 0.04 × 0.01 M = 0.0004 M.
Now, let's calculate the pH of the solution using the relationship between pH and the concentration of H+ ions:
pH = -log10[H+]
Given that log4 = 0.6, we can rearrange the equation to solve for [H+]:
[H+] = 10^(-pH)
Substituting the value of pH into the equation:
[H+] = 10^(-0.6)
Using logarithmic properties, we can rewrite this equation as:
[H+] = 1 / 10^(0.6)
Calculating the value:
[H+] ≈ 1 / 2.5119
[H+] ≈ 0.3981 (approximately)
Therefore, the concentration of H+ ions in the solution is approximately 0.3981 M.
Now, we can calculate the pH using this concentration:
pH = -log10(0.3981)
Using a scientific calculator, calculate the negative logarithm of 0.3981:
pH ≈ 0.4
Therefore, the pH value of the HBrO solution is approximately 0.4.