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What is the OH- in a solution with a pOH of 4.22?
[OH-] = 1x10^-4.22 or more conventionally, [OH-] = 6.03x10^-5 M
What is the pOH of a solution with OH 2.0 x 10-2?
1.7
What is the pH of a 10-5 m of koh solution?
The pH of a 10^-5 M KOH solution would be around 9. For a given concentration of a strong base like KOH, the pH can be calculated using the formula pH = 14 - pOH. Given that pOH = -log[OH-] and [OH-] = 10^-5 M in this case, pOH = 5. Therefore, pH = 14 - 5 = 9.
What is the OH- of a pOH of 9.29?
If your given pH or pOH, you can also find [H+] or [OH-] use antilog
If the pH of a solution is 10.7, what would the pOH be?
The pOH is 6,4.
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.
What is the pH of a 0.0110 M solution of Ba OH2?
The pH of a 0.0110 M solution of Ba(OH)2 can be calculated by finding the hydroxide ion concentration, which is double the concentration of the Ba(OH)2 solution. Therefore, [OH-] = 2 * 0.0110 M = 0.0220 M. From this, you can calculate the pOH using the formula -log[OH-], and then convert pOH to pH using the relation pH + pOH = 14.
What is the OH- in a solution with a pOH of 4.22?
[OH-] = 1x10^-4.22 or more conventionally, [OH-] = 6.03x10^-5 M
How do you calculate OH- with a ph of 1.12?
To calculate the concentration of hydroxide ions (OH-) from a given pH value, you can use the formula: [OH-] = 10^(-pH). For a pH of 1.12, the concentration of hydroxide ions would be [OH-] = 10^(-1.12) = 0.079 moles per liter.
What is the pOH of a solution with (OH) 9.0 107?
To find the pOH of a solution, you can use the formula pOH = -log[OH⁻]. Given that the hydroxide ion concentration [OH⁻] is 9.0 × 10⁻⁷ M, the pOH can be calculated as follows: pOH = -log(9.0 × 10⁻⁷) ≈ 6.05. Thus, the pOH of the solution is approximately 6.05.
What is the pOH of the solution with (oH-)2.010 -2?
To find the pOH of a solution, you can use the formula pOH = -log[OH⁻]. Given that the concentration of hydroxide ions [OH⁻] is 2.010 × 10⁻² M, you would calculate pOH as follows: pOH = -log(2.010 × 10⁻²) ≈ 1.69. Thus, the pOH of the solution is approximately 1.69.
What is the pOH of a solution with OH 2.0 x 10-2?
1.7
What is the pH of a 10-5 m of koh solution?
The pH of a 10^-5 M KOH solution would be around 9. For a given concentration of a strong base like KOH, the pH can be calculated using the formula pH = 14 - pOH. Given that pOH = -log[OH-] and [OH-] = 10^-5 M in this case, pOH = 5. Therefore, pH = 14 - 5 = 9.
What is the OH- of a pOH of 9.29?
If your given pH or pOH, you can also find [H+] or [OH-] use antilog
If the pH of a solution is 10.7, what would the pOH be?
The pOH is 6,4.
What is the OH in a solution with a pOH of 4.22?
[OH-] = 1x10^-4.22 or more conventionally, [OH-] = 6.03x10^-5 M
PH level when OH- equals 2.3 x 10-3 M?
The pH level when [OH-] equals 2.3 x 10^-3 M can be calculated using the equation: pOH = -log[OH-]. Given [OH-] = 2.3 x 10^-3 M, pOH = -log(2.3 x 10^-3) ≈ 2.64. Since pH + pOH = 14, pH = 14 - pOH = 14 - 2.64 ≈ 11.36.
