Question

1.) Determine the [OH−] , pH, and pOH of a solution with a [H+] of 4.6×10−7 M at 25 °C.

[OH-]= ?

pH= ?

pOH= ?

2.) Determine the [H+][H+] , pH, and pOH of a solution with an [OH−][OH−] of 0.067 M0.067 M at 25 °C.   

[H+]= ?

pH= ?

pOH= ?

3.) Determine the [H+][H+] , [OH−][OH−] , and pOH of a solution with a pH of 8.858.85 at 25 °C.

[H+]= ?

pH= ?

pOH= ?

4.) Determine the [H+][H+] , [OH−][OH−] , and pH of a solution with a pOH of 4.744.74 at 25 °C.

[H+]= ?

pH= ?

pOH= ?

Answer 1

For aqueous solutions, the product of concentrations of OH- ion and H+ ion will be a constant and will be equal to 1×10^{-14 at 25 °C.}

[H+][OH-] = 1×10^-14 , ion-product constant of water

And pH is defined as negative of logarithm of concentration of H+

And pOH as negative logarithm of OH-

pH = -log [H+]

pOH = -log [OH-]

1)

2)

3)

4)