What is the pH of a solution whose [H3O+] is 9.2× 10^−9 M?
What's wrong with pH = -log(H3O^+)?
What is the pH of a solution whose [H3O+] is 1 X 10 -6 M?
To determine the pH of a solution with a given concentration of hydronium ions ([H3O+]), you can use the formula:
pH = -log[H3O+]
In this case, the concentration of hydronium ions is 9.2× 10^−9 M. Plugging this value into the formula:
pH = -log[9.2×10^−9]
Now, let's calculate the pH:
pH = -log(9.2×10^-9)
Using a scientific calculator or logarithmic table, you can find the logarithm of the concentration:
log(9.2×10^-9) ≈ -8.04
Finally, apply the negative sign to the result to obtain the pH:
pH ≈ -(-8.04) ≈ 8.04
Therefore, the pH of the solution with a concentration of [H3O+] of 9.2× 10^−9 M is approximately 8.04.
To find the pH of a solution, we can use the formula:
pH = -log[H3O+]
Given that the [H3O+] is 9.2× 10^−9 M, we can substitute this value into the formula:
pH = -log(9.2× 10^−9)
To evaluate this calculation using a calculator or scientific calculator, follow these steps:
1. Enter 9.2× 10^−9 into the calculator.
2. Take the negative logarithm of the value entered: -log(result).
The resulting value will give you the pH of the solution.
Note: The logarithm function used in this calculation is typically denoted as log10 or simply log, and it represents the base-10 logarithm.