Question

Determine the [H+], pH and pOH of a solution with an [OH-] of 2.7 x 10^-7 M at 25°C.

Options:
Option 1: [H+]: 3.7 x 10^-8 M; pH: 7.43; pOH: 6.57
Option 2: [H+]: 3.7 x 10^-7 M; pH: 6.43; pOH: 7.57
Option 3: [H+]: 3.7 x 10^-6 M; pH: 5.43; pOH: 8.57
Option 4: [H+]: 3.7 x 10^-9 M; pH: 8.43; pOH: 5.57

Answer 1

To determine the [H+], pH, and pOH of a solution with an [OH-] of 2.7 x 10^-7 M at 25°C, we can use the equation pOH = -log[OH-]. Using this equation, we can calculate the pOH and then determine the pH using the equation pOH + pH = 14.00.

Step-by-step explanation:

To determine the [H+], pH, and pOH of a solution with an [OH-] of 2.7 x 10^-7 M at 25°C, we can use the equation:

pOH = -log[OH-]

Since pOH is given as 7.00 for a neutral solution, we can subtract the given [OH-] from 7.00 to find the pOH of the solution:

pOH = 7.00 - log(2.7 x 10^-7)

pOH ≈ 6.567

Using the equation pOH + pH = 14.00, we can calculate the pH:

pH = 14.00 - 6.567

pH ≈ 7.433

Therefore, the correct option is Option 1: [H+]: 3.7 x 10^-8 M; pH: 7.43; pOH: 6.57