pH of acids, bases and salts

Exercise 15

    

Calculate the volume of a 38 % ($\rho_S=$ 1.1886 $\frac{g}{mL}$) solution $S$ of chlorhydric acid that must be diluted in a volumetric flask $j$ of 1000 $mL$ in order to obtain a solution with $pH$ = 1.38

$HCl$: strong acid Final solution: $c$ $=$ $10^{-pH}$ = $10^{-1.38}$ = 0.01 $\frac{mol}{L}$ $n_{HCl}$ = $c_{HCl}\cdot V_{j}$ = 0.01$\cdot$1 = 0.01$\;mol$ The initial concentrated solution had the same number of moles: Initial solution $S$: $m_{HCl}$ = $n_{HCl}\cdot M_{HCl}$ = 0.01$\cdot$36.47 = 0.365$\;g$ $m_S$ = $\frac{m_{HCl}\cdot 100}{\%_S}$ = $\frac{0.365\cdot 100}{38}$ = 0.961$\;g$ $V_S$ = $\frac{m_S}{\rho_S}$ = $\frac{0.365}{1.1886}$ = 0.307$\;mL$