- #1
Pengwuino
Gold Member
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In an experiment we did, we simply added 5ml of 0.1ml HCl into 20ml of a .5M solution of an unknown weak base. I'm not sure how we calculate the equilibrium constant though
We know the pH is 5.855 which means the pOH is 10^-(14-5.855) = 7.161 x 10^-9.
Now I'm a bit confused. Is the [HB+] concentration the same as the [OH-] concentration and is the equilibrium equation this?
[tex]Keq = \frac{{[HB][OH]}}{{}}[/tex]
We know the pH is 5.855 which means the pOH is 10^-(14-5.855) = 7.161 x 10^-9.
Now I'm a bit confused. Is the [HB+] concentration the same as the [OH-] concentration and is the equilibrium equation this?
[tex]Keq = \frac{{[HB][OH]}}{{}}[/tex]