I am SO confused...
This one is easy. For conversions between H and OH, all you need to know that Kw=H x OH where Kw is the constant of water. That constant is 1 x 10^-14. So just solve for OH
1 x 10^-14 = 1.5 x 10^-5 X OH
divide 1 x 10^-14 by 1.5x10^-5 to get the answer
At 25°C, a solution has [H+] = 1.5 x 10-5. What is [OH-] for this solution?
As 2 water molecules collide with each other, an H+ is attracted from one of the water molecules to the other, as shown below.
H2O + H2O â H3O+1 + OH-1
The concentration of H3O+1 ions and OH-1 ions in an aqueous solution is determined by the equation below.
[H3O+1] * [OH-1] = 1 * 10^-14
[H3O+1] is the same as [H+]
(1 * 10^-5) * [OH-1] = 1 * 10^-14
[OH-1] = (1 * 10^-14) ÷ (1 * 10^-5) = 1 * 10^-9
I hope this helps!!
Remember that 14 = pH + pOH
And pH = -log [H+]
Does that help?
It is more complicated than that, but I am assuming this is in water and you are in grade 10. Wait until third year physical chemistry ;)
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This one is easy. For conversions between H and OH, all you need to know that Kw=H x OH where Kw is the constant of water. That constant is 1 x 10^-14. So just solve for OH
1 x 10^-14 = 1.5 x 10^-5 X OH
divide 1 x 10^-14 by 1.5x10^-5 to get the answer
At 25°C, a solution has [H+] = 1.5 x 10-5. What is [OH-] for this solution?
As 2 water molecules collide with each other, an H+ is attracted from one of the water molecules to the other, as shown below.
H2O + H2O â H3O+1 + OH-1
The concentration of H3O+1 ions and OH-1 ions in an aqueous solution is determined by the equation below.
[H3O+1] * [OH-1] = 1 * 10^-14
[H3O+1] is the same as [H+]
(1 * 10^-5) * [OH-1] = 1 * 10^-14
[OH-1] = (1 * 10^-14) ÷ (1 * 10^-5) = 1 * 10^-9
I hope this helps!!
Remember that 14 = pH + pOH
And pH = -log [H+]
Does that help?
It is more complicated than that, but I am assuming this is in water and you are in grade 10. Wait until third year physical chemistry ;)