I need step by step directions im so confused!!!
A. [OH-]= 1.0•10^-2 M
B. [OH-]= 1.0•10^-11 M
A. [OH-]= 1.0•10^-2 M
B. [OH-]= 1.0•10^-11 M
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pH is the negative log of the concentration of the H+ ion.
Because you are given the concentrations of the OH- ion, you must find the pOH.
pH = 14 - pOH
So, take the negative log of your OH- concentration in part A.
-log(1.0*10^-2) = 2 (that is your pOH, NOT YOUR pH!)
To make it a pH, subtract your pOH value from 14. 14-2 = 12. Your pH is 12.
For part B, do the same thing!
The answer I got for B was a pH of 3.
Because you are given the concentrations of the OH- ion, you must find the pOH.
pH = 14 - pOH
So, take the negative log of your OH- concentration in part A.
-log(1.0*10^-2) = 2 (that is your pOH, NOT YOUR pH!)
To make it a pH, subtract your pOH value from 14. 14-2 = 12. Your pH is 12.
For part B, do the same thing!
The answer I got for B was a pH of 3.