Statement I: An aqueous solution having pH 6.8 must be acidic.<br><br>Statement II: An aqueous solut — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

- Statement I is incorrect: An aqueous solution having pH 6.8 is neutral at temperatures where neutral water's pH is 6.8 (such as around 37°C where Kw = 2.5 × 10^-14). Thus, a pH of 6.8 does not always represent an acidic solution.<br>- Statement II is correct: By definition, neutral water has [H+] = [OH-] = sqrt(Kw). An acidic solution is one where [H+] > [OH-], which mathematically means [H+] > sqrt(Kw) at any temperature.