Answer
The pH of this HCl solution is equal to 2.21.
Work Step by Step
1. Convert the volume to L:
$$Volume = 224 \space mL \times \frac{1 \space L}{1000 \space mL} = 0.224 \space L$$
2 . Convert the temperature to K:
$$T/K = 27.2 + 273.15 = 300.3 $$
3 . Find the amount of moles of this gas:
$$n = \frac{PV}{RT} = \frac{( 1.02 )( 0.224 )}{(0.0821)( 300.3 )}$$
$n = 0.00927 \space mol$
4. Calculate the concentration in 1.5 L:
$$M = \frac{9.27 \times 10^{-3}}{1.5} = 6.18 \times 10^{-3} \space M$$
5. Since $ HCl $ is a strong acid, all its concentration is going to produce $H_3O^+$:
$$[H_3O^+] = [ HCl ] = 6.18 \times 10^{-3} \space M$$
6. Calculate the pH:
$$pH = -log[H_3O^+] = -log( 6.18 \times 10^{-3} ) = 2.21 $$
