## Chemistry: Atoms First (2nd Edition)

1. Calculate the $[H_3O^+]$ necessary to reach pH = 1.50 $[H_3O^+] = 10^{-pH}$ $[H_3O^+] = 10^{- 1.5}$ $[H_3O^+] = 3.162 \times 10^{- 2}M$ 2. Since $HCl$ is a strong acid: $[HCl] = [H_3O^+] = 3.162 \times 10^{- 2}M$ 3. Use the dilution equation to find the necessary volume of the 12M HCl solution: $C_1 * V_1(L) = C_2 * V_2(L)$ $0.03162* 1.6= 12 * V_2$ $0.050592 = 12 * V_2$ $V_2 = 0.004216L = 4.216ml$