Calculate the volume of a 32 % ($\rho_S=$ 1.1934 $\frac{g}{mL}$) solution $S$ of nitric acid
that must be diluted in a volumetric flask $j$ of 250 $mL$ in order to obtain a solution with $pH$ = 2.96
$HNO_3$: strong acid
Final solution:
$c$ $=$ $10^{-pH}$ =
$10^{-2.96}$ =
0.19 $\frac{mol}{L}$
$n_{HNO_3}$ =
$c_{HNO_3}\cdot V_{j}$ =
0.19$\cdot$0.25 =
0.0475$\;mol$
The initial concentrated solution had the same number of moles:
Initial solution $S$:
$m_{HNO_3}$ =
$n_{HNO_3}\cdot M_{HNO_3}$ =
0.0475$\cdot$63.02 =
2.993$\;g$
$m_S$ =
$\frac{m_{HNO_3}\cdot 100}{\%_S}$ =
$\frac{2.993\cdot 100}{32}$ =
9.353$\;g$
$V_S$ =
$\frac{m_S}{\rho_S}$ =
$\frac{2.993}{1.1934}$ =
2.508$\;mL$
