In order to work out the change in pH, we have to first calculate the initial concentrations
of acetic acid and sodium acetate. We already know from Table 1 that the concentration of
sodium acetate is 3M. Plugging this into the Henderson-Hasselbalch equation, we can work
out the concentration of acetic acid. The Henderson-Hasselbalch equation is as follows:
pH = pKa + log [A–]/[HA], where [A–] is the acid concentration of the conjugate base, and [HA] is
the concentration of the acid. Plugging our values into this equation, we get 5.2 = 4.74 + log
[3]/[HA]. The concentration of acetic acid, therefore, works out to be 1M. In a 100mL solution, the
number of moles of sodium acetate and acetic acid works out to be 0.3 and 0.1 moles, respectively
without a calculator, how in the hell did they know that 10^.46 is about 3?
of acetic acid and sodium acetate. We already know from Table 1 that the concentration of
sodium acetate is 3M. Plugging this into the Henderson-Hasselbalch equation, we can work
out the concentration of acetic acid. The Henderson-Hasselbalch equation is as follows:
pH = pKa + log [A–]/[HA], where [A–] is the acid concentration of the conjugate base, and [HA] is
the concentration of the acid. Plugging our values into this equation, we get 5.2 = 4.74 + log
[3]/[HA]. The concentration of acetic acid, therefore, works out to be 1M. In a 100mL solution, the
number of moles of sodium acetate and acetic acid works out to be 0.3 and 0.1 moles, respectively
without a calculator, how in the hell did they know that 10^.46 is about 3?