Which is the pOH of an aqueous solution in which [OH–] = 0.00085M
Question
Which is the pOH of an aqueous solution in which [OH–] = 0.00085M
Solution
The pOH of a solution is calculated using the formula:
pOH = -log[OH-]
Given that the concentration of OH- ([OH-]) is 0.00085M, we can substitute this value into the formula:
pOH = -log(0.00085)
To calculate the pOH, you would use a calculator to find the value of the logarithm.
pOH ≈ 3.07
So, the pOH of the solution is approximately 3.07.
Similar Questions
If the pOH of a solution is , explain how to determine the pH of the solution.Answer text Question 3Rich text editor
The H⁺ concentration in an aqueous solution at 25 °C is 5.5 × 10⁻⁶ M. What is [OH⁻]?
Which is pOH?Multiple choice question.the value of the equilibrium constant expression for the ionization of a basethe value of the equilibrium constant expression for the ionization of a weak acidthe negative logarithm of the hydrogen ion concentration of a solutionthe negative logarithm of the hydroxide ion concentration of a solution
Which is the pH of an aqueous solution in which [H+] = 0.0055M?Multiple choice question.–2.262.26–3.003.00
The pH of a 0.001 M aqueous solution of sodium hydroxide will be:
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.