determining [H+]

[205793570]

Hi, I am still confused on how to determine [H-]. the question states : Determine the [OH−] , pH, and pOH of a solution with a [H+] of 7.3×10−6 M at 25 °C.
can someone explain the steps? a simpler way to understand it?

[Omeed Kalan]

To get pH, use find the -log[H+], and then to find the pOH subtract the pH from 14. Then to find [OH], use 10^-(pOH).

[Caleb_Mei_1J]

Hey there!

Since you are given the hydrogen ion concentration [H+], you can determine the pH by using the formula pH = -log(H+). From there, you can determine the pOH which is 14 - pH. To determine the hydroxide ion concentration, you will use the formula 10^-pOH.

I hope this helps!

[Chris Korban 1D]

Since you need the PH and pOH you can just calculate either the pH or pOH and you can just use the equation pH+pOH=14 to solve for either equation

[Ryan Burchell 3D]

It gives you the concentration of the Hydrogen ions so you can find the pH by using -log[H+].

[bernal_maria1A]

Hi! I had a similar question! The help that I got was to

1. using the concentration of [H+] = 7.3×10−6, you use pH=-log[H+] or in this case pH=-log[7.3×10−6] to solve for pH
2. now that you have your PH, you can find pOH by simply doing : 14-pH= pOH (because pH and pOH should equal 14 together)
3. you find [OH-] by plugging in the given value of [H+] = 7.3×10−6 into the equation : 1.0×10−14=[H+][OH−] so 1.0×10−14 = [7.3×10−6][OH−] - solve for OH

[605537776]

the pH is the negative log of the hydronium concentration.