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What is the pH of a solution whose OH1.5x10-6m?
OH - A base. - log(1.5 X 10 -6 M) 14 - 5.8 = 8.2 pH =======
What is the OH of a solution whose pH is 8.23?
The pH tells you the concentration of H+ ions in the solution according to this formula pH = -log [H+] (where the square brackets mean "the concentration of" whatever is inside the brackets) So, if you have the pH, you can find the concentration of H+ from this: [H+] = 10-pH If the pH is 5.00, then 10-5 = 1 x 10-5 M = 0.00001 moles per liter But that's [H+], not the concentration of [OH-]! But those two are related like this: [H+] * [OH-] = 10-14. So to find [OH-], we use: [OH-] = 10-14 / [H+] In this case, [OH-] = 1 x 10-9 M
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- in an ammonia solution if the pH is 10.20?
The OH- concentration in a solution can be calculated using the formula OH- = 10^(14 - pH). Therefore, for a solution with a pH of 10.20, the OH- concentration would be 10^(-3.8) M, or approximately 1.58 x 10^(-4) M.
Calculate the OH- of a solution that has a pH of 2.40?
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
What is the pH of a solution whose OH1.5x10-6m?
OH - A base. - log(1.5 X 10 -6 M) 14 - 5.8 = 8.2 pH =======
What is the pH of a soultion that has a h plus concentration of 0.001m?
pH = -log10[H+] = -log10(0.001 mol/L )= -log10(10-3)= 3
What is the pH of very acidic soultion?
7 or less
What is the OH of a solution whose pH is 8.23?
The pH tells you the concentration of H+ ions in the solution according to this formula pH = -log [H+] (where the square brackets mean "the concentration of" whatever is inside the brackets) So, if you have the pH, you can find the concentration of H+ from this: [H+] = 10-pH If the pH is 5.00, then 10-5 = 1 x 10-5 M = 0.00001 moles per liter But that's [H+], not the concentration of [OH-]! But those two are related like this: [H+] * [OH-] = 10-14. So to find [OH-], we use: [OH-] = 10-14 / [H+] In this case, [OH-] = 1 x 10-9 M
What is the pH of a solution with OH -?
Use this (at 25oC) : [OH-] = 10-(14-pH) ,so:[OH-] = 10-(14-5.75) = [OH-] = 10-8.25 = invlog(-8.25) = 5.6*10-9 mol/L
How many times more basic is a solution whose pH is 12 compared to a solution whose pH is 10?
100 times. (10^2)
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- in an ammonia solution if the pH is 10.20?
The OH- concentration in a solution can be calculated using the formula OH- = 10^(14 - pH). Therefore, for a solution with a pH of 10.20, the OH- concentration would be 10^(-3.8) M, or approximately 1.58 x 10^(-4) M.
Calculate the OH- of a solution that has a pH of 2.40?
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
If pH is 6 What is is OH?
pH + pOH = 14. So pOH = 14 - 6 = 8 pOH = -log[OH-] [OH-] = 10-8 M
What would be the pH of a solution with a hydroxide ion OH- concentration of 10-12 M?
The pH of a solution can be calculated using the formula: pH = -log[OH-]. Therefore, for a solution with [OH-] concentration of 10-12 M, the pH would be 12.
What is the OH- in an oven cleaning solution if the pH is 12.35?
[OH-] = 10-pOH = 10-(14-pH) = 10-(14-12.35) = 10-(1.65) = 0.0224 mol/L
