The concentration of hydroxide ions (OH-) can be calculated from the pH using the formula: [OH-] = 10^(14 - pH). In this case, for a solution with a pH of 10, the concentration of OH- ions would be 10^(-4) M.
OH - A base. - log(1.5 X 10 -6 M) 14 - 5.8 = 8.2 pH =======
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
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.
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.
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
OH - A base. - log(1.5 X 10 -6 M) 14 - 5.8 = 8.2 pH =======
pH = -log10[H+] = -log10(0.001 mol/L )= -log10(10-3)= 3
7 or less
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
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
100 times. (10^2)
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.
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.
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
pH + pOH = 14. So pOH = 14 - 6 = 8 pOH = -log[OH-] [OH-] = 10-8 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.
[OH-] = 10-pOH = 10-(14-pH) = 10-(14-12.35) = 10-(1.65) = 0.0224 mol/L