pH + pOH = 14.
So pOH = 14 - 6 = 8
pOH = -log[OH-]
[OH-] = 10-8 M
pH and pOH are logarithmic functions. pH 3 has pOH = 11pH 9 has pOH = 5.The difference in [OH-] is 6 which on a log scale means 10^6 or 1 million times more OH- at pH 9 compared to pH 6.
OH - A base. - log(1.5 X 10 -6 M) 14 - 5.8 = 8.2 pH =======
Depends on the pH, at low pH (below pH 7), the H+ ion concentration is greater, and high pH the OH- ion concentration is greater
pH= -log[H+] pH + pOH = 14 pOH = 14 - pH pOH= -log[OH], so the antilog of -pOH will give you the OH concentration.
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
pH and pOH are logarithmic functions. pH 3 has pOH = 11pH 9 has pOH = 5.The difference in [OH-] is 6 which on a log scale means 10^6 or 1 million times more OH- at pH 9 compared to pH 6.
OH - A base. - log(1.5 X 10 -6 M) 14 - 5.8 = 8.2 pH =======
[OH-] = 3.31 log[OH-] = pOH = .51982 14-pOH = pH = 13.48
Depends on the pH, at low pH (below pH 7), the H+ ion concentration is greater, and high pH the OH- ion concentration is greater
pH= -log[H+] pH + pOH = 14 pOH = 14 - pH pOH= -log[OH], so the antilog of -pOH will give you the OH concentration.
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
Higher concentration.pH is an abbreviation for potential Hydrogen. When the pH value is below 7 on the 0-14 scale, an aqueous solution is considered to be acidic. If the pH value of an aqueous solution is above 7, it is considered to be alkaline or base. When pH is at 7, it is neutral.Below 7.0: Acidic (higher H+ concentration, lower OH- concentration H+ < OH-)Exactly 7.0: Neutral (equal H+ and OH- concentrations H+ = OH-)Above 7.0: Alkaline (lower H+ concentration, higher OH- concentration H+ > OH-)The scale is considered a logarithmic scale, where 2 adjacent values increase or decrease 10 fold. (ex. a pH of 7 is 10x less acidic than a pH of 6, whereas a pH of 4 is 100x more acidic than a pH of 6).
ph = LOG[OH-] so.... Ph= LOG[0.170] =0.76955 H+OH = 14 so 14- 0.76955 = 13.23
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
pH depends on ions H+ or OH-.
As pH increases H+ ions concentration decreases means OH- ions concentration increases . If pH increases from 8 to 13 , OH- ions concentration increases.
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