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pOH = -log [OH-], so pH = -log 9.0x10^-7pOH = 6.05 = 6.1 (to 2 significant figures)
What else can I help you with?
What is the pOH of a solution with OH- 1.410-13?
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.
What is the pOH of a solution with OH-1.4 10-13?
12.85 is the pOH.
What is the pOh solution with OH- 2.0X10-2?
To find the pOH from the hydroxide ion concentration (OH⁻), use the formula pOH = -log[OH⁻]. Given [OH⁻] = 2.0 × 10⁻² M, the calculation is pOH = -log(2.0 × 10⁻²) ≈ 1.70. Thus, the pOH of the solution is approximately 1.70.
If the pH of a solution is 4.0 what is the concentration of oh in the solution?
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.
What is the pOH of a solution with a (OH-) of 10-2?
1.70
What us the pOH of a solution with OH 9.0 10 -7?
The pOH can be calculated using the formula pOH = -log[OH-]. In this case, pOH = -log(9.0 x 10^-7) ≈ 6.05.
What is the pOH of a solution with (OH-)1.4 10 -13?
12.85
What is the pOH of a solution with OH 1.4 10-13?
12.85
What is poh of a solution with oh 2.0 10-2?
1.70
What is the poh of a solution with oh 2.0 10-2?
1.70
What is the OH- of a solution with pH 5.75?
The hydroxide ion concentration of a solution with pH 5.75 can be calculated using the formula [OH-] = 10^(-pOH). First, find the pOH by subtracting the pH from 14 (pOH = 14 - pH = 14 - 5.75 = 8.25). Then, calculate [OH-] = 10^(-8.25) ≈ 5.62 x 10^(-9) mol/L.
A solution of NaOH has OH- 1.9 x 10-6 What is the pOH of this solution?
5.7
