What is the pH of each of the following aqueous solutions? (a) 0.036 M HCl WebAssign will check your answer for the correct number of significant figures. 1.44 Correct: Your answer is correct. (b) 0.17 M KOH WebAssign will check your answer for the correct number of significant figures. 13.23 Correct: Your answer is correct. (c) 0.19 M Ba (OH) 2

(a) 0.036 M HCl

[HCl] = 0.036 M

As HCl is a strong acid, it will completely dissociate and produce H + ions.

[ H+] = M

pH = - log [ H+]

pH = - log[0.036]

pH = - (-1.444)

pH = 1.44

(b) 0.17 M KOH

pH + pOH = 14

pH = - log10[H+], and pOH = 14-pH

pH = 14 - pOH

pH = 14 - (-log10 (0.17))

pH = 14 - (0.77) = 13.23

(c) 0.19 M Ba (OH) 2

[H+] [OH-] = 1.0*10-14M

[OH-] = 2 * 0.19 = 0.38M

[H+] = 2.63 * 10-14M

pH = - log10 ([H+])

pH = - log10 (2.63 * 10-14) = 13.58.