0
- log(1 X 10^-5 M)
= 5
14 - 5
= 9 pH
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Wiki User
∙ 12y ago
Wiki User
∙ 6y agoThe pH is 10.
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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
Prepare 5 M NaOH of pH 12?
na+oh +25=53 ph+poh=2.3
What is the pH of a solution with a oh of 3.31 00000000 M?
[OH-] = 3.31 log[OH-] = pOH = .51982 14-pOH = pH = 13.48
PH level when OH- equals 2.3 x 10-3 M?
-log(2.3 X 10^-3 M) = 2.6 14 - 2.6 = 11.4 pH ( OH - )
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
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
Given that you have a H3O concentration of 0.0034 M what is the OH-?
[H3O+][OH-] = Kw = 1x10^-14[OH-] = 1x10^-14/0.0034 = 1x10^-14/3.4x10^-3[OH-] = 2.9x10^-12 M
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 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 H3O in a solution of OH- 1x10-12M?
- log(1 X 10 -12 M) = 12 pH -----------------------very little room for H3O
What is the pH of 1x10-3 H?
- log(1 X 10 -3 M H +) = 3 pH =====
Prepare 5 M NaOH of pH 12?
na+oh +25=53 ph+poh=2.3
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
Express the hydroxide and hydronium ion concentrations in pure water at 25C?
[H3O+] = 1x10^-7 M = hydronium ion concentration[OH-] = 1x10^-7 M = hydroxide ion concnetration
How big is 10 microns?
A micron (µm), presumably referring to a Micrometre is one millionth of a meter (1x10-6 m ). Thus, making 10 microns (1x10-5 m). A micron (µm), presumably referring to a Micrometre is one millionth of a meter (1x10-6 m ). Thus, making 10 microns (1x10-5 m).
What is the concentration of OH ions in a HCl solution whose hydrogen ion concentration is 2.7M?
1.0 * 10-4 is the OH- concentration[H30+] = 10(-pH) = 10-10 = 1.0 * 10-10 M[OH-] = (Kw) / [H30+] = (1.0 * 10-14) /(1.0 * 10-10) = 1.0 * 10-4 MShortcut:The pH and pOH values must add up to equal pKw, which value is 14.0 (at 25o).Given the pH of 10, you simply subtract 10 from the required 14 to get -4. Insert the -4 into the concentration format (1.0*10x) to get 1.0*10-4
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
