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What is the pOH of a solution with (OH-)1.4 10 -13?

Updated: 5/20/2022
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8y ago

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12.85

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Claudine Hermann

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Q: What is the pOH of a solution with (OH-)1.4 10 -13?
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What is the pOH of a solution with OH-1.4 10-13?

12.85 is the pOH.


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-] = 1.4 x 10-13?

12.85


What is the pOH of a solution with OH- 1.4 x 10-13?

12.85


A solution has a pOH of 4.5 What is the hydroxide ion concentration of this solution?

[H3O+] = 10-pH = 10-(14.0-pOH) = 10-(14-7.4) = 10-(6.6) = 2.5 x 10-7 mol/L


How do you calculate OH- with a ph of 1.12?

pH + pOH = 14. So pOH = 14 - 1.12 = 12.88 pOH = -log[OH-] [OH-] = 1.31 x 10-13 M


When was Alef Poh-ji born?

Alef Poh-ji was born on 1987-04-13.


How would OH- in an ammonia solution compare with OH- in a sodium hydroxide solution of a similar concentration?

Molar concentration in both base solutions NH3 and NaOH is assumed to be (equal) 0.1 mol Base/LWeak base like ammonia (NH3) with pKb = 9.2 and concentration (assumed) Cb = 0.1 (mol/L)pOH = 0.5*[pKb + pCb] = 0.5*[9.2 + 1.0] = 5.1 , hence [OH-] = 7.9*10-6pH = 14 - pOH = 8.9 hence [H+]= 1.3*10-9Strong base hydroxide (like from NaOH) with concentration (equally assumed) Cb = 0.1 (mol/L)pOH = 1.0 because [OH-] = 0.1pH = 13.0 hence [H+]= 1.0*10-13


How is the pH and poh of 0.1 M HCl?

pH = 1 HCl is a strong acid so fully dissociates, so the concentration of H+ is equal to that of the HCl and pH=-log[H+]


What is 10 to the negative 13 power multiply by 10 to the negative 33 power show solution?

It is: 1.0*10-46


What is the pH of a 1.0 10-3 M KOH solution?

[OH-] = 1x10^-3 M[H+][OH-] = 1x10^-14[H+] = 1x10^-14/1x10^-3 = 1x10^-11pH = -log 1x10^-11 = 11Done another way:pOH = -log [OH-] = -log 1x10^-3 = 3pH + pOH = 14pH = 14 - 3 = 11