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 = -log[H+]
[H+] = 2.51 x 10-6 M pH + pOH = 14.
So pOH = 14 - 5.6 = 8.4
pOH = -log[OH-]
[OH-] = 3.98 x 10-9 M
1/108.23 or ( 10-8.23 )
= 5.89 x 10-9 M OH-
OH - A base. - log(1.5 X 10 -6 M) 14 - 5.8 = 8.2 pH =======
pH=8
The higher the pH, the greater the concentration of Hydroxide (OH-) ions. So, the solution with the pH of 9 is your answer.
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
It depends on what the solution is. What affects the pH is the element. If there are more H+ ions in the solution you're referring to, the solution will be more acidic (lower pH). If there are more (OH)- ions in the solution, the solution will be more basic (higher pH).
OH - A base. - log(1.5 X 10 -6 M) 14 - 5.8 = 8.2 pH =======
pH=8
100 times. (10^2)
[OH-] = 3.31 log[OH-] = pOH = .51982 14-pOH = pH = 13.48
The concentration of H+ or OH-.
The higher the pH, the greater the concentration of Hydroxide (OH-) ions. So, the solution with the pH of 9 is your answer.
100,000 times more acidic
the concentration of OH ions in solutions
Adding a base will make the pH go up (increasing of OH- ions concentration).
Is always basic.
A solution with a pH greater than 7
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