In a 1.2 M solution of KOH, a strong base, [H3O+] = _____, and [OH−] = _____.

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Let's analyze the situation step by step.

- The problem involves a 1.2 M solution of KOH, which is a strong base. Strong bases dissociate completely in water: KOH → K+ + OH−. Therefore, the concentration of hydroxide ions [OH−] equals the initial concentration of the base: [OH−] = 1.2 M.

- In aqueous solution at 25°C, the ion-product of water is Kw = [H3O+][OH−] ≈ 1.0 × 10−14. Since [OH−] is 1.2 M, we can solve for [H3O+]: [H3O+] = Kw / [OH−] ≈ (1.0 × 10−14) / (1.2) ≈ 8.3 × 10−15 M.

- Now, evaluate the given answer option: '8.3 × 10−15 M; 1.2 M'. This matches the calculated values for [H3O+] and [OH−], respectively, using the standard Kw value and the complete dissociation of KOH.

- Consider the logical consistency: if the base fully dissociates, [OH−] cannot be anything other than the original base concentration (assuming no significant autoionization effects beyond Kw). The hydronium ion concentration then remains governed by Kw, yielding the very small [H3O+] value calculated above.

- Since there are no alternative answer choices provided to compare, there is no need to critique other options. But conceptually, any correct response must pair [OH−] with the base concentration (1.2 M) and compute [H3O+] from Kw, yielding approximately 8.3 × 10−15 M.

- A common source of error would be misapplying Kw or assuming [H3O+] equals [OH−] for a strong base solution, which is incorrect here because the solution is highly basic and [H3O+] is determined by Kw divided by [OH−]. Also, confusing 1.0 × 10−14 with a different temperature or ionic strength would lead to an inaccurate [H3O+].

CHM-1020-LD01.2025SU PS II- Part I (Acids and Bases)

In a 1.2 M solution of KOH, a strong base, [H3O+] = _, and [OH−] = _.

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