Calculate the pH of each of the following solutions: 2.8 times 10^-4 M Ba(OH)_2

Question

Calculate the pH of each of the following solutions: 2.8 times 10^-4 M Ba(OH)_2 5.2 times 10^-4 M HNO_3. The pOH of a strong base solution is 1.88 at 25 degree C. Calculate the concentration of the base (a) if the base is KOH and (b) if the base is Ba(OH)_2 Which of the following diagrams best representation a strong acid, such as HCl, dissolved in water? Which represents a weak acid? Which represents a very weak acid? (The hydrated proton is shown as a hydronium ion. Water molecules are omitted for clarity.)

Explanation / Answer

15.18 a)   [OH-] = 2 x [Ba(OH)2] = 2 x 2.8 x 10-4 N = 5.6 x 10-4 N

            pH = 14 - pOH = 14 - {-log[OH-] }

                = 14 + log [ 5.6 x 10-4 N]

               = 10.75

          pH = 10.75

b) [H+] = [HNO3 ] = 5.2 x 10-4 M = 5.2 x 10-4 N

          pH = - log [H+] = - log [5.2 x 10-4] = 3.28

          pH = 3.28

15.23 Given that pOH = 1.88

               [OH-] = 10-pOH = 10-1.88 = 0.013 N

a) [KOH] = [OH-] = 0.013 N = 0.013 M

b) [Ba(OH)2] = [OH-] = 0.013 N

    [Ba(OH)2] = [OH-] /2 = 0.013 / 2 = 0.0065 M

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