## Chemistry 12th Edition

$pH = 0.117$
1. Find the number of $HCl$ moles. molar mass $(HCl)$: 1.01 + 35.45 = 36.46g/mol $n(moles) = \frac{mass(g)}{molarmass(g/mol)}$ $n(moles) = \frac{18.4}{36.46} = 0.505$ 2. Now, calculate the concentration of $HCl$: $Concentration(M) = \frac{n(moles)}{Volume(L)}$ $C(M) = \frac{0.505}{0.662} = 0.763M$ 3. HCl is a strong acid, therefore: $[HCl] = [H^+] = 0.763M$ 4. Calculate the pH: $pH = -log[H^+] = -log(0.763) = 0.117$