What is the pH of a solution with [OH-] of 6.30 x 10-11 M?
[OH-] of 6.30 x 10-11 M?
pOH = -log(OH^-)
Then pH + pOH = 14. Plug in pOH and solve for pH.
To find the pH of a solution with a given hydroxide ion concentration, you need to use the relationship between hydroxide ions (OH-) and hydrogen ions (H+), which is governed by the equation:
OH- + H+ ↔ H2O
The concentration of OH- represents the basicity of the solution, while the concentration of H+ represents the acidity of the solution. The pH scale is a logarithmic scale that measures the acidity or basicity of a solution.
To find the pH, you can use the equation:
pOH = -log[OH-]
Since pOH + pH = 14 (at 25°C), you can rearrange the equation to solve for pH:
pH = 14 - pOH
Now, let's calculate the pOH and then the pH of the given solution.
Given: [OH-] = 6.30 x 10^-11 M
pOH = -log(6.30 x 10^-11)
= -log(6.30) - log(10^-11)
= -log(6.30) - (-11 x log(10))
= -log(6.30) + 11
≈ 10 + 11 (since the logarithm of a number close to 10 is approximately 1)
≈ 21
Therefore, the pOH of the given solution is approximately 21.
Now, use the equation pH = 14 - pOH to find the pH:
pH = 14 - 21
≈ -7
So, the pH of the solution with [OH-] of 6.30 x 10^-11 M is approximately -7.