Question
Using the following salts listed below, calculate the moles of acid and conjugate base needed to make $V = \pu{100 mL}$ of $c = \pu{0.50 M}$, $pH \in 6.5, 6.7, 6.8$ phosphate buffer solutions. ($\mathrm pK_\mathrm a(\ce{H2PO4}) = 6.64$)
Molas masses of salts:
- $\ce{KH2PO4} = 136.09 ~\pu{g/mol}$
- $\ce{NaH2PO\cdot H2O} = \pu{137.99 g/mol}$
- $\ce{Na2HPO4 \cdot 7H2O} = \pu{268.09 g/mol}$
- $\ce{K2HPO4} = \pu{174.2 g/mol}$
I tried using the Henderson-Hasselbalch equation but I am stuck at the point where I have found the base-acid ratio and I need to find the moles of the acid and the moles of the base.
$$ \mathrm pH = \mathrm pK_\mathrm a + \log\left(\frac{[\text{Conjugate base}]}{[\text{Acid}]}\right)\\ n = \pu{100 ml} \times \pu{0.5 M} =\pu{ 0.05 mol} $$
For pH 6.5: $$ 6.5 = 6.64 + \log\frac{[B]}{[A]}\\ \frac{[B]}{[A]} = 0.72 $$ Here I got the base-acid ratio as 0.72 but what should I do next? I tried looking up for solutions and a person suggests using $A + B = 0.05$ But how do I know what A and B are just by knowing the ratio is 0.72?