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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 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.
What is the OH- in a solution with a pOH of 4.22?
The concentration of OH- ions in a solution with a pOH of 4.22 is 5.24 x 10^-5 M.
What is the pOH of a solution with OH 1.4 10 13?
The pOH of a solution with an OH- concentration of 1.4 x 10^-13 M is 1.85. This is calculated by taking the negative logarithm of the OH- concentration, which is -log(1.4 x 10^-13) = 12.85, then subtracting it from 14 to find the pOH: 14 - 12.85 = 1.85.
What is the pOH of a solution with OH 2.0 x 10-2?
1.7
What is the pOH of a solution with OH-1.4 10-13?
12.85 is the pOH.
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 is poh of a solution with oh 2.0 10-2?
1.70
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 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
What is the pOH of a solution with OH- 2.0 x 10-2?
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
What is the pOH of a solution with [OH-] = 1.4 x 10-13?
12.85
What is the pOH of a solution with OH- 1.4 x 10-13?
12.85
