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.

ph=

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 1.3×10−6.

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×

ph=

Part F

Calculate the pH of a 0.10 M solution of HCl.

Express your answer numerically using two decimal places.

ph=

Answer 1

(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^-] = (K_b 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⁺] = (K_a 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