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Calculate the pH of a 0.10 M aqueous solution of sodium acetate…
Question
Calculate the pH of a 0.10 M aqueous solution of sodium acetate (CH3COONa). The ionization constant of acetic acid is Ka = 1.8 x 10^-5 and Kw = 1.0 x 10^-14. Give the answer rounded to three decimal places.
✓ Verified answer: 8.872checked by our engine — not a guess
Step-by-step solution
Acetate undergoes hydrolysis: CH3COO- + H2O <=> CH3COOH + OH-, with Kh = Kw/Ka = 1.0e-14/1.8e-5 = 5.556e-10.
For salt of conc C = 0.10 M, [OH-] = sqrt(Kh*C) = sqrt(5.556e-10 * 0.10) = sqrt(5.556e-11) = 7.454e-6 M.
pOH = -log10(7.454e-6) = 5.128.
pH = 14 - 5.128 = 8.872.
Final answer8.872
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