Part B Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2. Expre
ID: 947346 • Letter: P
Question
Part B
Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2.
Express your answer numerically using two decimal places.
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Part C
Calculate the pH of a 0.10 M solution of NaOH.
Express your answer numerically using two decimal places.
ph=
Part D
Calculate the pH of a 0.10 M solution of hydrazine, N2H4. Kb for hydrazine is 1.3×106.
Express your answer numerically using two decimal places.
ph=
Part E
Calculate the pH of a 0.10 M solution of hypochlorous acid, HOCl. Ka of HOCl is 3.5×
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Part F
Calculate the pH of a 0.10 M solution of HCl.
Express your answer numerically using two decimal places.
ph=
Explanation / Answer
(B)Ba(OH)2 -------> Ba2+ + 2OH-
[OH-] = 2 x 0.10 = 0.20M
We know that,
pH = - Log[H+]
(or) pH = 14 + Log[OH-]
pH = 14 + log (0.20)
pH = 14 - 0.70
pH = 13.30
(C) NaOH ------> Na+ + OH-
[OH-] = 0.10M
pH = 14 + Log(0.10)
pH = 14 - 1
pH = 13.00
(D) [OH-] = (Kb x C)1/2
[OH-] = (1.3 x 10-6 x 0.10)1/2
[OH-] = 0.36 x 10 -3 M
therefore, pH = 14 + Log(0.36x10-3)
pH = 10.56
(E) [H+] = (Ka xC )1/2
[H+] = (3.5 x 10-8 X 0.10)1/2
[H+] = 0.59 x 10-4 M
pH = - Log (0.59 x 10-4)
pH = 4.23 M
(F) pH = - Log[H+]
pH = - Log (0.10)
pH = 1.00