Calculate the hydronium ion, [ H30+], and hydroxide ion, [OH-], concentrations for a

0.0117 M HCl Solution.

[H3O+] = 0.0117 M

[OH-] = 8.5 * 10^-13 M

Explanation:

Step 1: Data given

Concentration of HCl = 0.0117 M

Step 2:

HCl is a strong acid

pH of a strong acid = - log[H+] = - log[H3O+]

[H3O+] = 0.0117 M

pH = - log (0.0117)

pH = 1.93

pOH = 14 - 1.93 = 12.07

pOH = - log[OH+] = 12.07

[OH-] = 10^-12.07 = 8.5 * 10^-13

Or

Kw / [H3O+] = [ OH-]

10^-14 / 0.0117 = 8.5*10^-13