question help please

Question

If the [H+] was found in a lab sample to be 1.0 x 10-4 mol/L then calculate the pH and what pH of NaOH of equal volume and concentrate neutralize the acid?

Answer 1

pH = -log [H⁺]

The [H⁺] is given as 1.0x10^-4, so the pH is the negative log of this value.

Can you take the negative log?  You should get an answer of pH = 4

 

To reach neutrality (pH = 7), the [H⁺] will have to be lowered to 1.0x10^-7.  The reaction is H⁺ + OH^- ==> H₂O

What [OH^-] is required to make the [H⁺] 1.0x10^-7 if you begin with [H⁺] = 1.0x10^-4?  Then take pOH and then pH.