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law and the rate constant for the reaction.

PLEASE HELP!!!!.
A buffer solution was prepared by mixing 150.00 mL of 1.1341 mol/L of CH3COOH
and 100.00 mL of 0.831 mol/L of barium acetate. Determine the pH of the buffer
solution after the addition of 10.00 mL of 0.010 mol sulphuric acid. Kc for acetic acid
is 1.8 x 10-5

Respuesta :

onyebuchinnaji

The pH of the buffer solution after the addition of sulfuric acid is determined as 4.43.

Initial moles of acid and base

The initial moles of acid and base conjugate is determined as follows;

n = CV

na₁ = (150 x 1.1341)/1000

na₁ = 0.17 mol

nb₁ = (100 x 0.831)/1000

nb₁ = 0.083 mol

Number of moles of the acid added

H₂SO4  ⇄ 2H²⁺  + SO₄²⁻

na₂ = (10 x 0.01)/1000

na₂ = 0.0001 mol

Final number of moles of the acid and base

nb = 0.083 - 2(0.0001) = 0.0829 mol

na = 0.17 + 2(0.0001) = 0.1702 mol

pH of the buffer solution

[tex]Ka = \frac{[CH_3COO][H^+]}{[CH_3COOH]} \\\\1.8\times 10^{-5} = \frac{0.0829(H^+)}{0.1702} \\\\H^+ = \frac{(1.8 \times 10^{-5})(0.1702)}{0.0829} \\\\H^+ = 3.696 \times 10^{-5}\\\\pH = -Log [H^+]\\\\pH = -Log (3.696 \times 10^{-5})\\\\pH = 4.43[/tex]

Thus, the pH of the buffer solution after the addition of sulfuric acid is determined as 4.43.

Learn more about buffer solutions here: https://brainly.com/question/8676275

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