Boric acid, B ( OH ) 3 is used as a mild antiseptic. What is the pH of a 0.0025 M aqueous solution of boric acid? The hydrogen ion arises principally from the reaction: B(OH) 3 (aq) + H 2 O(l) ⇌ B(O

Question

Boric acid, B ( OH ) 3 ​ is used as a mild antiseptic. What is the pH of a 0.0025 M aqueous solution of boric acid? The hydrogen ion arises principally from the reaction: B(OH) 3 (aq) + H 2 O(l) ⇌ B(OH) 4 - (aq) + H + (aq); K = 4.0 × 10 -10 .

TestHub · Accepted Answer

B(OH)₃ + H₂O ⇌ B(OH)₄⁻ + H⁺, K = 4.0 × 1 0 − 10 Initial concentration = 0.0025 M Let [ H + ] = x , then: K = 0.0025 x 2 ​ ⇒ x 2 = 4.0 × 1 0 − 10 × 0.0025 = 1.0 × 1 0 − 12 x = [ H + ] = 1.0 × 1 0 − 6 M p H = − lo g ( 1.0 × 1 0 − 6 ) = 6

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