1.70
To find the pOH of a solution, you can use the formula pOH = -log[OH⁻]. Given that [OH⁻] = 1.41 × 10⁻¹³, calculate the pOH: pOH = -log(1.41 × 10⁻¹³) ≈ 12.85. Therefore, the pOH of the solution is approximately 12.85.
12.85 is the pOH.
1.70
1.70
The pOH can be calculated using the formula pOH = -log[OH-]. In this case, pOH = -log(9.0 x 10^-7) ≈ 6.05.
To find the concentration of hydroxide ions ([OH-]) in a solution when the pH is 4.0, you can use the formula pH + pOH = 14. Since the pH is 4.0, the pOH would be 14 - 4 = 10. To convert pOH to [OH-] concentration, use the formula [OH-] = 10^(-pOH). Thus, [OH-] = 10^(-10) = 1 x 10^(-10) M.
[OH-] = 1x10^-4.22 or more conventionally, [OH-] = 6.03x10^-5 M
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
The pH of a solution can be calculated using the formula pH = 14 - pOH. Given that the pOH is 3.31, we can subtract this value from 14 to find the pH. In this case, the pH of the solution would be approximately 10.69.
pH and pOH are a measure of the concentration of the hydronium ions and hydroxyl ions respectively in the solution. pH = -log[H+] pOH = -log[OH-] and they are related: pH + pOH = 14
D 6.04 Is the answer.
1.70