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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
What is the OH- in an ammonia solution if the pH is 10.20?
Use this (at 25oC) : [OH-] = 10-(14-pH) ,so:[OH-] = 10-(14-10.20) = [OH-] = 10-3.80 = invlog(-3.80) = 1.6*10-4 mol/L
How much NaOH is needed to prepare 546 mL of solution with a pH of 10.00?
pH=10, so pOH=14-10=4 [OH]=10^-pOH [OH]=10^-4 [OH]=0.0001
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 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 very acidic soultion?
7 or less
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
What is the OH- in an ammonia solution if the pH is 10.20?
Use this (at 25oC) : [OH-] = 10-(14-pH) ,so:[OH-] = 10-(14-10.20) = [OH-] = 10-3.80 = invlog(-3.80) = 1.6*10-4 mol/L
How much NaOH is needed to prepare 546 mL of solution with a pH of 10.00?
pH=10, so pOH=14-10=4 [OH]=10^-pOH [OH]=10^-4 [OH]=0.0001
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
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 pH is a soultion of sodium chloride in pure water?
it has neither an acidic nor an alkaline pH, it is neutral at pH 7
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 pH is 6 What is is OH?
pH + pOH = 14. So pOH = 14 - 6 = 8 pOH = -log[OH-] [OH-] = 10-8 M
